Class 12 Engineering Chemistry - Coordination Compounds

Match each coordination compound in List-I with an appropriate pair of characteristics from List-II. ( $en = H_2HCH_2CH_2NH_2$ ; Atomic numbers: $Ti =22, Cr=24; Co=27; Pt = 78$ )

(P)

$[Cr(NH_3)_4Cl_2]Cl \rightarrow$ Paramagnetic and exhibits cis-trans isomerism
(Q)

$[Ti(H_2O)_5Cl](NO_3)_2 \rightarrow$ Paramagnetic and exhibits ionization isomerism
(R)

$[Pt (en)(NH_3)Cl]NO_3 \rightarrow$ Diamagnetic and exhibits ionization isomerism
(S)

$[Co (NH_3)_4 (NO_3)_2] NO_3 \rightarrow$ Diamagnetic and exhibits cis-trans isomerism

Blue-green is the complimentary color of red spectral color.
If true enter 1, else enter 0.

The correct answer is 1.

Blue-green is the complimentary color of red spectral color.

Orange is the complimentary colour of blue spectral colour.
If true 1 else 0.

Here, it can be seen that,

Name the series of lines in the hydrogen spectrum which lies in the ultra-violet region :

The Lyman series is a hydrogen spectral series of transitions and resulting ultraviolet emission lines of the hydrogen atom as an electron goes from

$n \geq 2$ to

$n = 1$ (where

$n$ is the principal quantum number) the lowest energy level of the electron.

Haemoglobin is a complex of $Fe(II)$ bound to porphyrin rings.
If true enter 1, else enter 0.

The correct answer is 1.

Haemoglobin is a complex of

$Fe(II)$ bound to porphyrin rings.

A porphyrin molecule can coordinate to a metal using the four nitrogen atoms as electron-pair donors and hence, is a polydentate ligand. This porphyrin ring consists of four pyrrole molecules cyclically linked together (by bridges) with the iron ion bound in the center.

Discuss briefly giving an example in each case the role of coordination compound in biological system.

Chlorophyll which is a green coloured pigment, that plays an important role in photosynthesis is a complex of magnesium. In chlorophyll, the Mg is coordinated to porphyrin ring.
Hemoglobin which is a iron(+2) complex carries oxygen to different parts of our body.
A complex of cobalt metal i.e, $B_{12}$ Vitamin, is involved in the metabolism of every cell in our body.

What type of isomerism is exhibited the complex $[Co(NH_3)_5Cl]SO_4$ ?

The given compound

$[Co(NH_3)_5Cl]SO_4$ shows ionisations isomerism due to two possible ionising groups.

The isomers are

$[Co(NH_3)_5Cl]SO_4\Leftrightarrow [Co(NH_3)_5SO_4]Cl$

Identify the type of Isomerism existing in between the following compounds.
$\left[ {Co\left( {N{H_3}} \right)s\,N{O_2}} \right]$ and $\left[ {Co\left( {N{H_3}} \right)s\,ON{O_2}} \right]C{l_2}$

LINKAGE ISOMERS as nitrate is a ambidentate ligand. It is a monodentate ligand having two donating sites, in complex 1 N- donates lone pair and in complex 2 oxygen donates hence they are Linkage isomers of each other.
The isomers formed due to ambidentate ligand are called as Linkage Isomers.

How many isomeric forms are possible for the octahedral complex, $[Rh(en)_{2}(NO_{2})(SCN)]^{+}$ ?

1376915_1290872_ans_5a03b91d160f4d40b107e37fcf194e43.jpg

What is the use of coordination compounds for purification of water Medical and catalyst

1.Purification of water: EDTA is a complex which is used for the determination of hardness of water

2.Medical uses: There are many coordination compounds that are used for medical treatment and one such complex is cis-platin. It is used in the cases of cancer tumors

3.Uses of coordination compounds also find there application in catalyst. These days they are popular in polymer industry as well.

Indicate the types of isomerism exhibited by the following complex and draw the structure of this isomer.
$[Co(NH_3)_5(NO_2)](NO_3)_2$

$[Co(NH_{3})_{5} (NO_{2})](NO_{3})_{2}$

The given compound can exhibit only linkage isomerism due to the presence of ambidentate ligand

$(-NO_{2})$

The complex in the left in the picture is

$[Co(NH_{3})_{5}(NO_{2})](NO_{2})_{2}$ .

The complex in the right in the picture is

$[Co(NH_{3})_{5}(ONO)](NO_{2})_{2}$ .

So, the number of possible isomers is=2

1166833_1105179_ans_b541f06ab7604b76b99d7479403f5205.png

How are the hybrid orbitals arranged in the molecules?

Hybridisation is the inter mixing of two or more different orbitals to get the hybrid orbitals of all having same size and energy.

$\rightarow$ Based on the number of hybrid orbitals they will arrange in the molecule.

$3$ trigonal.

4-tetrahydral etc and shapes can be changed in the presence of lone pair.

Match the given pairs.

The complex of the type

$\displaystyle \left [ Ma_{2}b_{2}c_{2} \right ]^{n\pm }$ shows geometrical as well as optical isomerism. Except one, other geometrical isomers are optically inactive.
The complex of the type

$\displaystyle \left [ Ma_{3}b_{2}c \right ]^{n\pm }$ shows three geometrical isomers.
The complex of the type

$\displaystyle \left [ Ma_{2}bcde \right ]^{n\pm }$ has total 15 space isomers.
The complex of the type

$\displaystyle \left [ M\left ( AB \right )_{3} \right ]^{n\pm }$ has four optically active isomers.

The primary valency of a central metal ion in a complex is satisfied with _______ .

Primary valency is basically the oxidation state of the metal ion forming the complex and most metals basically have a positive charge, so it has to balanced by anions.

According to Werner's coordination theory, there are _____ kinds of valency - _ and ____.

According to Warner's theory, the central metal atom in coordination compounds shows two types of valency.

They are the primary and secondary valency. The primary valency relates to the oxidation state and the secondary valency relates to the coordination number.

Match column-I with column-II

$[Co(NH_3)_4Cl_2]$ shows geometrical isomerism.

$[Co(en)_3]Cl_2$ shows optical isomerism.

$[Co(en)_2(NO_2)Cl]SCN$ shows optical isomerism, ionization isomerism and geometrical isomerism.

$[Co(NH_3)_6][Cr(CN)_6]$ shows coordination isomerism.

In $[Fe(H_2O)_6]Cl_3$ , six $H_2O$ are joined by primary valency (PV) and three $Cl$ are joined by secondary valency (SV).
If true enter 1, else enter 0.

The correct answer is 1.

$[Fe(H_2O)_6]Cl_3$ : Three

$Cl$ joined by primary valency(PV) and six

$H_2O$ joined by secondary valency(SV).

The primary valancies are normally ionisable and are satisfied by negative ions.

The secondary valancies are non-ionisable which are satisfied by negative ions or neutral molecules. The secondary valency is equal to the coordination number and is fixed for a metal.

Match column-I with column

$Na_2[Pt(SCN)_2(ox)_2]$ shows linkage isomerism, geometrical isomerism and optical isomerism.

$[CrCl_2(NH_3)_4]NO_3$ shows geometrical isomerism and Ionization isomerism.

$[Pt(NO_2)(Gly)(NH_3)]$ shows linkage isomerism and geometrical isomerism.

$K_3[Fe(OH)_2(C_2O_4)_2]$ shows geometrical isomerism and optical isomerism.

Vitamin $B_{12}$ is a complex of cobalt. If true enter 1, else enter 0.

Vitamin

$B_{12}$ is a complex of cobalt. It is cyanocobalamin

$(C_{63}H_{88}CoN_{14}O_{14}P)$ . Its main sources are meat, fish, egg, milk etc. Its deficincy is responsible for pernicious anaemia.

Match the following.

The coordination compound

$[Co(en)_{2}Cl_{2}]Cl$ exhibits optical isomerism and geometrical isomerism.
The coordination compound

$[Co(en)_{2}(NO_{2})Cl]SCN$ exhibits optical isomerism, ionization isomerism and geometrical isomerism.
The coordination compound

$[Co(NH_{3})_{6}][Cr(F)_{6}]$ exhibits coordination isomerism.

What is hybridisation?

$\bf{Hint:}$ Two different energy orbitals form an equal energy orbitals.

$\bf{Explanation:}$

Hybridization is a process in which two or more than two orbitals of different energies undergoes mixing to form new set of hybrid orbitals.

For example : Hybridization in

$CH_{4}$ molecule.
Here, mixing of one

$s$ and three

$p$ orbital will result in

$sp^3$ hybrid orbital.

For the complex $[NiCl_{4}]^{2-}$ , write
(i) the IUPAC name (ii) the hybridization type (iii) the shape of the complex.
(Atomic no. of $Ni = 28$ )

1. Nickel(II) chloride
2. Here nickel is in +2 oxidation state and the ion has the electronic configuration

$3d^8$ . Each

$Cl^-$ ion donates a pair of electrons. The compound is paramagnetic, since, it contains two unpaired electrons.
3. In tetrahedral complexes, one s and three p orbitals are hybridised to form four equivalent orbitals oriented tetrahedrally.

Name the following coordination entities and draw the structures of their steroisomers:
(i) $[Co(en)_2Cl_2]^+ (en=ethane - 1, 2-diamine)$
(ii) $[Cr(C_2O_4)_3]^{3-}$
(iii) $[Co(NH_3)_3Cl_3]$
(Atomic number $Cr=24, Co=27$ )

(i)

$[Co(en)_2Cl_2]^+$ : dichoridobis (ethylenediamine) cobalt (III) ion (as 2 chlorine atoms are there di chloro, 2- ethylene diamine groups represent bis (en) .

(ii)

$[Cr(C_2O_4)_3]^{3-}$ : Trioxalatochromate (III) ion (as 3 oxylate groups represents (tri oxylatato))
(iii)

$[Co(NH_3)_3Cl_3]$ : triamminetrichloridocobalt (III) ( as three ammino and three chloine atoms represent tri ammine tri chloro )

Write the IUPAC names of the following coordination compounds:
(i) $[Cr(NH_3)_3Cl_3]$
(ii) $K_3[Fe(CN)_6]$
(iii) $[CoBr_2(en)_2]^{+}$ , (en = ethylenediamine)

IUPAC names of the compounds are

(i)

$[Cr{ ({ NH }_{ 3 }) }_{ 3 }{ Cl }_{ 3 }]$ = triamminetrichlorochromium (III)

(ii)

${ K }_{ 3 }[Fe{ (CN) }_{ 6 }]$ = Potassium hexacyanoferrate (III)

(iii)

${ [Co{ Br }_{ 2 }{ (en) }_{ 2 }] }^{ + }$ = Dibromidobis(ethane-1,2-diamine)cobalt (III) ion

Write the name, the structure and the magnetic behavior of each one of the following complexes:
(i) $[Pt (NH_3) Cl (NO_2)]$
(ii) $[Co(NH_3)_4Cl_2] Cl$
(iii) $Ni (CO)_4$
(At. Nos. $Co = 27, Ni = 28, Pt = 78$ )

(i) Amminechloronitrito platinum (II) ,Square planner , DM

(ii)Tetraammine dichloro cobalt (III) chloride, Ocahedral, DM

(iii)Tetracarbonyl nickel (o) , Tetrahedral, DM

(i) Write the IUPAC name of the complex $\left[ Cr{ \left( N{ H }_{ 3 } \right) }_{ 4 }{ Cl }_{ 2 } \right] Cl$ .
(ii) What type of isomerism is exhibited by the complex ${ \left[ Co{ \left( en \right) }_{ 3 } \right] }^{ 3+ }$ ?
( $en=$ ethane-1, 2-diamine)
(iii) Why is ${ \left[ Ni{ Cl }_{ 4 } \right] }^{ 2- }$ paramagnetic but $\left[ Ni{ \left( CO \right) }_{ 4 } \right]$ is diamagnetic?
( $Cr=24, Co=27, Ni=28$ )

(i) The IUPAC name of the complex

$[Cr(NH_3)_4Cl_2]Cl$ is Tetraamminedichlorochromium(III) chloride.

(ii) The complex

$[Co(en)_3]^{3+}$ exhibits optical isomerism. Its optical isomers are shown in the image.

(iii) In

$[NiCl_4]^{2-}$ , the oxidation state of Ni is +2. Chloride is a weak field ligand and does not cause pairing up of electrons against the Hund's rule of maximum multiplicity. As a result, two unpaired electrons are present in the valence d-orbitals of Ni which impart paramagnetic character to the complex. On the other hand, carbonyl is a strong field ligand and causes pairing up of electrons against the Hund's rule of maximum multiplicity. As a result, no unpaired electrons are present and hence, the complex is diamagnetic.

Write the types of isomerism exhibited by the following complexes.
(i) $[Co(NH_{3})_{5}Cl]SO_{4}$
(ii) $[Co(en)_{3}]^{3+}$
(iii) $[Co(NH_{3})_{6}] [Cr(CN)_{6}]$

(i) Ionisation isomerism

(ii) Optical isomerism(see diagram)

(III) Coordination isomerism

The electron pairs involved in hybridisation and not involved in bonding are called ___________.

Lone pairs

The pair of electrons involve in bonding are called as bond pair. And the pair of electron surrounding the central atom which belongs to central atom but not involved in bonding are called as lone pair of electrons.

Name the types of isomerism shown by the following pairs of compounds:
(i) $[CoCl(H_2O)(NH_3)_4Cl_2]$ and $[CoCl_2(NH_3)_4]Cl\cdot H_2O$
(ii) $[Pt(NH_3)_4][PtCl_6]$ and $[Pt(NH_3)_4Cl_2][PtCl_4]$

(i) Hydrate isomerism.
(ii) Coordination isomerism.

How does ${ K }_{ 2 }\left[ Pt{ Cl }_{ 4 } \right]$ get ionized when dissolved in water? Will it form precipitate when $AgN{ O }_{ 3 }$ solution is added to it? Give a reason for your answer.

$\displaystyle { K }_{ 2 }\left[ Pt{ Cl }_{ 4 } \right]$ is a coordination compound with complex ion

$\displaystyle \left[ Pt{ Cl }_{ 4 } \right]^{2-}$ .
When

$\displaystyle { K }_{ 2 }\left[ Pt{ Cl }_{ 4 } \right]$ is dissolved in water, the complex ion

$\displaystyle \left[ Pt{ Cl }_{ 4 } \right]^{2-}$ will retain its identity.

$\displaystyle { K }_{ 2 }\left[ Pt{ Cl }_{ 4 } \right] \rightarrow 2K^+ + \left[ Pt{ Cl }_{ 4 } \right]^{2-}$
However when

$\displaystyle AgNO_3$ is added to

$\displaystyle { K }_{ 2 }\left[ Pt{ Cl }_{ 4 } \right]$ , grey precipite of

$\displaystyle Pt { Cl }_{ 2 }\left( AgN{ O }_{ 3 } \right) \left( S \right)$ is obtained.

$\displaystyle { K }_{ 2 }Pt{ Cl }_{ 4 }+2AgN{ O }_{ 3 }\rightarrow 2KCl\left( aq \right) +Pt { Cl }_{ 2 }\left( AgN{ O }_{ 3 } \right) \left( S \right)$

What are the dark lines seen in the solar spectrum called?

Dark lines of solar spectrum are called Fraunhofer lines.

Illustrate with example, the difference between a double salt and coordination compound.

Double salts are those molecular or addition compounds which exist in a solid state but dissociate into constituents ions when dissolved in water Ex. Mohr salt

$FeS{ O }_{ 4 }{ \left( N{ H }_{ 4 } \right) }_{ 2 }S{ O }_{ 4 }\cdot 6{ H }_{ 2 }O$ .
Coordination compounds are those molecular or addition compounds which retained their identity in aqueous solution and shows property entirely different from their constituent ions. Ex. Potassium ferrocyanide

${ K }_{ 4 }\left[ Fe{ \left( CN \right) }_{ 6 } \right]$ .

(i) What type of isomers are $\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 5 }Br \right] { SO }_{ 4 }$ and $\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 5 }{ SO }_{ 4 } \right] Br$ ? Give a chemical test to distinguish between them.
(ii) Write the structures of optical isomers of the complex ion ${ \left[ Co{ (en) }_{ 2 }{ Cl }_{ 2 } \right] }^{ + }$

(i)

$\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 5 }Br \right] { SO }_{ 4 }$ and

$\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 5 }{ SO }_{ 4 } \right] Br$ are Ionization isomer

$I$

$II$
When the two isomers are treated with slightly acidic

$Ba{Cl}_{2}$ solution

$\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 5 }Br \right] { SO }_{ 4 }$ produces white ppt.

$(Ba{SO}_{4})$ but

$\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 5 }{ SO }_{ 4 } \right] Br$ does not.
(ii) Optical Isomers of

${ \left[ Co{ (en) }_{ 2 }{ Cl }_{ 2 } \right] }^{ + }$

Explain co-ordination and ionisation isomeristmes with a suitable example for each.

(i) Co-ordination isomerism : In a bimetallic complex, die distribution of ligands between the two co-ordination spheres can differ, giving rise to isomers called the co-ordination isomers. This phenomenon is called as co-ordination isomerism. This isomerism is explained by the following pairs of complexes Where the complex cation and anion have different metal centres.
a)

$\underset{Cobalt(III)}{\underset{Hextunmine}{[CO^{III}(NH_3)_6]}} \,\,\,\,\, \underset{Chromate(III)}{\underset{Hertacyano}{[Cr(CN)_6]}}$
and

$\underset{Chromium(III)}{\underset{Hextunmine}{[Cr^{III}(NH_3)_4]}} \,\,\,\,\, \underset{Cobatate(III)}{\underset{Hertacyano}{[CO^{III}(CN)_6]}}$
b)

$\underset{Platinum (II)}{\underset{Tetraammine}{[Pt^{II}(NH_3)_4] }} \,\,\,\,\, \underset{Cuparate (II)}{\underset{Tetrachloro}{[CuCl_4]}}$
and

$\underset{Copper (II)}{\underset{Tetraammine}{[Cu(NH_3)_4] }} \,\,\,\,\, \underset{Platinate (II)}{\underset{Tetrachloro}{[PtCl_4]}}$
In the above isomers, the interchange ligands in the co-ordination spheres of cationic and anionic parts takes place and leads to obtain co-ordination isomerism.
ionisation isomerism: Co-ordination compounds containing the same molecular formula but rotating various ions in solution are called ionisation isomers. This property is known as ionisation isomerism.
In this type ofisomerism the diffarontearises from the interchange of groups within or outside the co-ordination sphere.
E.g, : This type of isomerism is furnished by the red-violet

$[Co(NH_3)_5Br]SO_4$
pentaamminebromocobat (III) sulphate

$[CO(NH_3)_5SO_4]Br$
pentaamminesulphatocobalt (III) bromide
Red violet isomer gives sulphate, ion and red isomer furnishes bromide ion in solution.

Explain the difference between a double-salt and a complex, giving an example in each case.

Double salts exist in solid state but dissociate into constituent ions on dissolution in water. They lose their identity in aqueous solution. Mohr's salt

$\displaystyle FeSO_4 \cdot (NH_4)_2SO_4 \cdot 6H_2O$ is a double salt. The aqueous solution of this salt gives the test of

$\displaystyle Fe^{2+}$ ,

$\displaystyle NH_4^+$ and

$\displaystyle SO_4^{2-}$ ions.

On the other hand complexes ( or coordination compounds) retain their identity in aqueous solutions and show properties which are different from those of constituent ions. For example, ferrocyanide ion

$\displaystyle [Fe(CN)_6]^{4-}$ is a complex ion and it retains its identity in solution. It does not dissociates to give

$\displaystyle Fe^{2+}$ ions and

$\displaystyle CN^-$ ions. Hence, the aqueous solution of , ferrocyanide ion

$\displaystyle [Fe(CN)_6]^{4-}$ will not give test of

$\displaystyle Fe^{2+}$ ions and

$\displaystyle CN^-$ ions.

Explain the applications of coordination compounds in the field of metal purification giving an example :

Mond process for refining nickel metal:
Nickel is heated in a stream of CO to form nickel tetra carbonyl complex which is highly volatile.

$\displaystyle Ni+4CO \xrightarrow {330-350 K} Ni(CO)_4$
Nickel tetra carbonyl is heated at high temperature. It decomposes to give pure nickel.

$\displaystyle Ni(CO)_4 \xrightarrow {450-470K} Ni+4CO$

Explain coordination and ionisation isomerism with example.

(i) Coordination isomerism:

Coordination isomerism involves the intercharge of ligands in the coordination spheres of cationic and anionic parts and is observed in a bimetallic complex in which the distribution of ligands between the two coordination spheres can vary. Different complexes have same molecular formula.
For example,

$\displaystyle [Co(NH_3)_6][Cr(CN)_6]$ and

$\displaystyle [Cr(NH_3)_6][Co(CN)_6]$ are coordination isomers. In

$\displaystyle [Co(NH_3)_6][Cr(CN)_6]$ , ammonia ligands are bound to cobalt and cyano ligands are bound to chromium. And in

$\displaystyle [Cr(NH_3)_6][Co(CN)_6]$ ammonia ligands are bound to chromium and cyano ligands are bound to cobalt.

(ii) Ionisation isomerism.

Ionisation isomerism involves coordination compounds having the same molecular formula but gives different ions in solution. It involves exchange of ions inside and outside the coordination sphere.
For example

$\displaystyle [Co(NH_3)_5SO_4]$ Br and

$\displaystyle [Co(NH_3)_5Br]SO_4$ are ionisation isomers.

$\displaystyle [Co(NH_3)_5SO_4]$ Br gives

$\displaystyle [Co(NH_3)_5SO_4]^++Br^-$ ions in the solution whereas

$\displaystyle [Co(NH_3)_5Br]SO_4$ gives

$\displaystyle [Co(NH_3)_5Br]^{2+}+SO_4^{2-}$ ions in the solution.

Write a note on Haemoglobin.

Haemoglobin in the red blood cells carries oxygen from the lungs to the tissues. It delivers the oxygen molecule to myoglobin in the tissues. When the oxygen has been released for cell respiration, haemoglobin. Loses its bright red colour and becomes purple. It then combines with the waste carbond dioxide produced by the cells and deposits in the lungs so that the gas can be exhaled. Both haemoglobin and myoglobin having the same structure excepting the fact that myoglobin is a monomer and heamoglobin is a tetramer. Both are iron-porphyrin complex called heme group in which iron is in +2 oxidation state. The working part of haemoglobin is a heme group containing an

$Fe^{2+}$ cation coordinated to four nitrogen atoms of porphyrin group and one nitrogen atom of histidine group. The sixth octahedral site is available to bind oxygen molecule.

Classify the following into homoleptic & heteroleptic complexes?
i) $K_4[Fe(CN)_6]$
ii) $[Co(NH_3)_5(CO_3)]Cl$
iii) $K_2[Zn(OH)_4]$
iv) $[Pt(NH_3)_2Cl(NO_2)]$

In homoleptic complex, only one type of ligand is present.
In heteroleptic complex, more than one type of ligands are present.
(i)

$\displaystyle K_4[Fe(CN)_6]$ and (iii)

$\displaystyle K_2[Zn(OH)_4]$ are homoleptic complexes.
(ii)

$\displaystyle [Co(NH_3)_5(CO_3)]Cl$ and (iv)

$\displaystyle [Pt(NH_3)_2Cl(NO_2)]$ are heteroleptic complexes.

Explain the violet colour of $[Ti(H_2O)_6]^{3+}$ complex on basis of the crystal field theory?

In the complex

$\displaystyle [Ti(H_2O)_6]^{3+}$ , the Ti atom has oxidation state of

$\displaystyle+3$ . Its outer electronic configuration is

$\displaystyle 3d^1$ . It has one unpaired electron. This unpaired electron is excited from

$\displaystyle t_{2g}$ level to

$\displaystyle e_g$ level by absorbing yellow light and hence appears violet coloured.

Explain Werner's theory of coordinate compounds with suitable examples?

Werner's theory of coordinate compounds-

$1893$ , Werner was the first to propose correct structures for coordination compounds containing complex ions, in which a central transition metal atom is surrounded by neutral or anionic ligands.

Postulates of Werner's Theory-

The central metal or the metal atoms in coordination compounds show two types of valency. They are the primary and secondary valency.
The primary valency relates to the oxidation state and the secondary valency relates to the coordinate number.
The number of secondary valences is fixed for every metal atom. It means that the coordination number is fixed.
The metal atom works towards satisfying both its primary and secondary valencies. Primary valency is satisfied by negative ion whereas secondary valences are satisfied by negative ion or by neutral molecules.

Example-

In , the coordination number of cobalt is $6$ and $N{H}_{3}$ molecule satisfy all the $6$ secondary valencies while Chloride ions satisfy the $3$ primary valencies. These are non-directional in character. These chloride ions instantaneously precipitate on the addition of silver nitrate. Thus the total number of ions are $4$ , i.e., three chloride ions and one complex ion.
In $Co{Cl}_{3}.4N{H}_{3}$ , two chloride ions exhibit the dual behaviour of satisfying both Primary and Secondary Valencies. The compound gives a precipitate with silver nitrate corresponding to only one ${Cl}^{-}$ ion and the total number of ions is $2$ . Hence, we can formulate it as $\left[ Co{Cl}_{2} {\left( N{H}_{3} \right)}_{4} \right]Cl$ .

(a) Give the postulates of Werner's theory of co-ordination compounds.
(b) Differentiate between chemical reactions and nuclear reactions.

(a) Postulates of Werner's theory:
1) Every metal atom has two types of valencies
(i) Primary valency or ionisable valency
(ii) Secondary valency or non ionisable valency
2) The primary valency corresponds to the oxidation state of the metal ion.
The primary valency of the metal ion is always satisfied by negative ions.
3) Secondary valency corresponds to the coordination number of the metal ion or atom. The secondary valencies may be satisfied by either negative ions or neutral molecules.
4) The molecules or ion that satisfy secondary valencies are called ligands.
5) The ligands which satisfy secondary valencies must project in definite directions in space. So the secondary valencies are directional in nature whereas the primary valencies are non-directions in nature.
6) The ligands have unshared pair of electrons. These unshared pair of electrons are donated to central metal ion or atom in a compound. Such compounds are called coordination compounds.
Werner's representation
Werner represented the first member of the series

$[Co(NH_3)6]Cl_3$ as follows. In this representation, the primary valency (dotted lines) are satisfied by the three chloride ions. The six secondary valencies (solid lines) are satisfied by the six ammonia molecules.

Chemical reaction	Nuclear reaction
(i) In a chemical reaction, the nuclei of the atoms taking part remain unaffected only the electrons in the extra nuclear part of the atoms take part in the chemical process.	In nuclear reaction, the nuclei of the atoms interact with other nuclei or lighter particles or photons resulting in the formation of new nuclei and one or more lighter particles.
(ii) These reactions involve some loss, gain or overlap of outer orbital electrons of the reactant atoms.	These reactions involve emission of alpha, beta and gamma particles from the nucleus.
(iii) A chemical reaction is balanced info mass only.	Nuclear reaction is balanced in terms of both mass and energy.
(iv) The energy changes in chemical reaction is very much less than the nuclear reaction.	The energy changes are far exceed than the energy changes in chemical reactions.
(v) In this reaction, the energy is expressed in terms of kilojoules per mole.	In this reaction, the energy is expressed in MeV per individual nucleus.
(vi) No new element is produced since nucleus is unaffected.	New elements/isotope may be produced during this reaction.
(viii) These reaction are affected by change n temperature and pressure.	These reactions are not affected by temperature and pressure.
(ix) For this reaction law of conservation of mass hold good.	For this reaction, law of mass does not hold good.
(x) The atomic number of the element does not change.	The atomic number of the element changes.

Explain Werner's theory of co-ordination compounds?

Central metal atom shows two types of valencies:
(i) Primary (principal) valency. It represents oxidation number of the metal. It is non directional and usually written outside the coordination sphere. It does not give the idea of geometry of the coordination compounds. It is shown by dotted line.
(ii) Secondary (auxillary valence). It represents coordination number of metal.
The metal atom tries to satisfy both its valencies. It is directional and usually written inside the coordination sphere. It gives definite geometry to coordination compounds. It is shown by solid line.

Write the IUPAC name of following compounds :
(A) $K_3[Fe(CN)_6$
(B) $[Co(NH_3)_6]Cl_3$

IUPAC name :
(A) Potassium hexacyano ferrate (III)
(B) Hexammine cobalt chloride (III)

Draw Werner's structure of the following:
(a) $CoCl_{3} . 6NH_{3}$
(b) $CoCl_{3} . 5NH_{3}$
(c) $CoCl_{3} . 4NH_{3}$
(d) $CoCl_{3} . 3NH_{3}$

The Werner's structures are as shown.

Write any two postulates of Werner's theory of coordination compounds.

Postulates of werner's theory of Co-ordination compounds:
(1) Most of the metallic elements exhibits two types of valence: (i) Primary valence or principal valence and (ii) secondary valence
(2) Every metal tends to satisfy both of its primary and secondary valences.
(3) Every metal has a fixed number of secondary valence
(4) The secondary valence is always directed towards fixed positions in space.

What is Zeise's Salt and Ferrocene? Explain with structure?

$\text {Zeise's salt}$ is

$K [PtCl_3 (\eta^2-C_2H_4)]$ . The structure of the Zeise's salt is shown in the figure. This salt was prepared by Danish pharmacist Zeise in 1830 . It is one of the compound of transition metals which was prepared earlier. The plane of ethylene molecule and the

$C = C$ axis are perpendicular to the expected bond direction of the central atom.

$\text {Ferrocene}$ This is an orange-yellow compound. It is an organometallic compound with formula

$Fe(C_5H_5)_2$ . The structure of Ferrocene is shown in the given figure.

How do 'd' orbitals split in an octahedral crystal field?

According to Crystal Field Theory, as a ligand approaches the metal ion, the electrons in the d-orbitals and those in the ligand repel each other due to repulsion between like charges. Thus the d-electrons closer to the ligands will have a higher energy than those further away which results in the d-orbitals splitting in energy.

The most common type of complex is octahedral; here six ligands form an octahedron around the metal ion. In octahedral symmetry the d-orbitals split into two sets with an energy difference, where the ${ d }_{ xy }{ d }_{ yz }{ d }_{ zx }$ orbitals will be lower in energy than the ${ d }_{ { z }^{ 2 } }{ d }_{ { x }^{ 2 }-{ y }^{ 2 } }$ , which will have higher energy, because the former group is farther from the ligands than the latter and therefore experience less repulsion.

What types of isomer are $[Co(NH_3)_5 Br] SO_4$ and $[Co(NH_3)_5 SO_4] Br$ ?

$\displaystyle [Co(NH_3)_5 Br] SO_4$ and

$\displaystyle [Co(NH_3)_5 SO_4] Br$ are ionisation isomers. In aqueous solution, they undergo dissociation to form different ions.

$\displaystyle [Co(NH_3)_5 Br] SO_4$ on dissociation in aqueous solution gives

$\displaystyle [Co(NH_3)_5 Br]^{2+}$ and

$\displaystyle SO_4^{2-}$ ions.

$\displaystyle [Co(NH_3)_5 Br] SO_4 \rightarrow [Co(NH_3)_5 Br]^{2+}+ SO_4^{2-}$

Whereas

$\displaystyle [Co(NH_3)_5 SO_4] Br$ on dissociation in aqueous solution gives

$\displaystyle [Co(NH_3)_5 SO_4] ^+$ and

$\displaystyle Br^-$ ions.

$\displaystyle [Co(NH_3)_5 SO_4] Br \rightarrow [Co(NH_3)_5 SO_4] ^++Br^-$

Number of $Cl^{-}$ ions satisifying both primary and secondary valency are in $CoCl_{3}5NH_{3}$ .

Here,

$\left[ {Co{{\left( {N{H_3}} \right)}_5}cl} \right]c{l_2}$

$1\,cl$ shows dual behavior because

$5NH_3$ satisfy valency and remaining

$1$ secondary valency satisfy by

$cl$ .

Define primary and secondary valency of metal ions proposed by werner theory?

According to Werners theory each coordinate complex compound exhibits two types of valencies.The are a) primary valency and b) secondary valency. Primary valencies are satisfied by only negative charge and it is equal to oxidation state of central metal ion.

Secondary valencies are satisfied by either negative charge or neutral species and it is equal to the coordinate number. Primary valencies are denoted by dotted lines and ionisible. Secondary valenices are denoted by dark or straight lines and non ionisible.

For the complex ion $[Fe(CN)_6]^{3-}$ , state:
(i) the type of hybridisation.
(ii) the magnetic behaviour.
(iii) the oxidation number of the central metal atom.

$[Fe(CN)_6]^{ -3 }$ complex

$CN$ is a strong field ligand therefore will form low spin complex by using inner 3d-orbitals. Since it has octahedral geometry as there are 6 ligands, so its hybridization will be

$d^2sp^3$ .

The central metal has oxidation number

$+3$ calculated as:

$x+6\times(-1)=-3$

Fe has

$4s^23d^6$ configuration and therefore

$Fe^{ 3+ }$ will be

$3d^5$ . Upon pairing it has one unpaired electron that makes it paramagnetic complex.

Write primary and secondary valency of $Co$ in $[Co(Nn_{3})_{6}]Cl_{3}$ ?

Primary valence is 3. Since, 3 chloride ligands are present, the oxidation number of Co is +3.
Secondary valence is 6. Since, 6 ammonia ligands are present, the co -ordination number of Co is 6.

Write the name and draw the structures of each of the following complex compounds.
(i) $\left[ Co{ \left( N{ H }_{ 3 } \right) }_{ 4 }{ \left( { H }_{ 2 }O \right) }_{ 2 } \right] { Cl }_{ 2 }$
(ii) $\left[ Pt{ \left( N{ H }_{ 3 } \right) }_{ 4 } \right] \left[ \left( NiC{ l }_{ 4 } \right) \right]$

1131594_795720_ans_f444eef17863432ca2fc88d0b219e889.png

Predict whether the following molecules are isostructural or not. Justify your answer
(i) $N{Me}_{3}$ (ii) $N{(Si{Me}_{3})}_{3}$

i) R.E.F image

{No back bonding since no empty orbital in carbon}

ii) R.E.F image

{Planar due to back-bonding from N: to 3d - of si}

1132298_874693_ans_52a19dea1128485c919cb1da1e11fc01.png

Explain hybridisation, geometry and magnetic property of $[Ni(CN)_4]^{2-}$ ion using Valence Bond Theory(VBT). [Atomic number of Ni is $28$ ].

Ni atom has electronic configuration

$[Ar]3d^84s^2$ .

$Ni^{2+}$ ion has electronic configuration

$[Ar]3d^84s^0$ . Hybridisation involved is

$dsp^2$ . Geometrical shape is square planar

Magnetic property is diamagnetic as all electrons are paired.

Chlorophyll contains 2.68% of $Mg$ by weight. Then the number of $Mg$ atom in 2.00 g of chlorophyll is:
(Atomic mass of $Mg = 24$ )

Total mass of chlorophyll

$=2g$

$\%$ of

$Mg$ in chlorophyll

$=2.68\%$

$\Rightarrow$ mass of

$Mg$ in 2g of chlorophyll

$=2\times \cfrac{2.68}{100}$

Nuumber of magnesium atom

$\left(\cfrac{0.00536}{24}\right)\times \left(6.023 \times 10^{23}\right)$

$=1.345\times 10^{20}$ atoms.

Give two examples of Complex compound.

Examples of complex compound include potassium ferrocyanide

$\displaystyle K_4[Fe(CN)_6]$ and potassium ferricyanide

$\displaystyle K_3[Fe(CN)_6]$ . Other examples include pentaamine chloro cobalt(III) chloride

$\displaystyle [Co(NH)_5Cl]Cl_2$ and dichlorobis (ethylenediammine) platinum(IV) nitrate

$\displaystyle [Pt(en)_2Cl_2] (NO_3)_2$ .

Define Hybridization.

Orbital hybridization is the concept of mixing atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., then the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory.
For example, in the ethane molecule, the bonding picture according to valence orbital theory is very similar to that of methane. Both carbons are $sp^{3}$ -hybridized, meaning that both have four bonds arranged with tetrahedral geometry.

960241_1039622_ans_8e44100c073c422bb52de579c09b67fa.png

Write formula of the following compound:
(i) dichloridobis (ethylene diamine) cobalt (III) ion.
(ii) sodiumethylenediaminetetraacetatonickelate (II)
(iii) hexaammineplatinum (IV) chloride

(i)

$[Co(en)_2Cl_2]^{3+}$

(ii)

$Na_2[Ni (EDTA)]$

(iii)

$[Pt(NH_3)_6]Cl_4$

${ \left[ Co{ \left( N{ H }_{ 3 } \right) }_{ 6 } \right] }^{ 3+ }$ is a yellowish orange colored compound.

${ \left[ Ti{ \left( { H }_{ 2 }O \right) }_{ 6 } \right] }^{ 3+ }$ is a violet compound.

${ \left[ Ni{ \left( { H }_{ 2 }O \right) }_{ 6 } \right] }^{ 2+ }$ is a green compound.

${ \left[ Ni{ \left( { H }_{ 2 }O \right) }_{ 4 }\left( en \right) \right] }^{ 2+ }\left( aq \right)$ is a pale blue compound.

The complex studied by Werner had a composition corresponding to the formula $Pt{Cl}_{4}.2KCl$ . From electrical conductance measurements, he determined that each formula unit contained three ions. He also found that silver nitrate did not give a precipitate of $AgCl$ with this complex. Write a formula for this complex that agrees with this information.

Since

$AgCl$ precipitate is not formed with this complex, this implies that

$Cl^-$ ions are not free and are inside the coordination sphere.

Also, it contains

$3$ ions. Therefore, the possible formula of this complex is

$K_2[PtCl_6]$ .

What is coordination compound ?

A coordination complex is the product of a lewis acid-base reaction, in which the neutral molecules or anions (or ligands) bond to the central metal atom by coordinate or covalent bond. And the compound having these coordination complex are called Coordination Compounds.

Which of the following can show coordination isomerism?
(i) $\left[ Cu{ \left( { NH }_{ 3 } \right) }_{ 4 } \right] \left[ Pt{ Cl }_{ 4 } \right]$ (ii) ${ \left[ Fe{ \left( { NH }_{ 3 } \right) }_{ 6 } \right] }_{ 2 }{ \left[ Pt{ (CN) }_{ 6 } \right] }_{ 3 }\quad$
(iii) $\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 6 } \right] \left[ Cr{ \left( { C }_{ 2 }{ O }_{ 4 } \right) }_{ 3 } \right]$ (iv) $\left[ Pt{ (en) }_{ 3 } \right] { \left( { SO }_{ 4 } \right) }_{ 2 }$

Coordination isomerism is a form of structural isomerism in which the composition of the complex ion varies. In a coordination isomer the total ratio of ligand to metal remains the same, but the ligands attached to a specific metal ion change.
i) In

$\left[ Cu\left( NH_{ 3 } \right) _{ 4 } \right] \left[ PtCl_{ 4 } \right]$ complex , both anion and cation can be metal complex ions which yields an isomer and this type of isomerism is referred to as coordination isomerism.
conclusion: hence the first(i) complex will show the coordination isomerism.

What is crystal field splitting energy? Draw a figure to show spitting of degenerate orbitals in an octahedral crystal field?

Crystal field stabilization energy:

It is the energy of

$e^-$ configuration in the ligand field minus the energy of the

$e^-$ configuration in isotropic field.

$CFSE=\triangle E=E_{ligand field}- E_{isotropic field}$

$CFSE$ depends on-

Geometry that changes the d-orbital splitting pattern.
Number of d- $e^-s$
Spin Pairing energy
Ligand character via spectrochemical series.

(Refer to Image)

1020662_1099443_ans_794545978e664184b91dfc17d258bc60.PNG

What is the Primary and Secondary Valence of $PtCl_{2}.2NH_{3}$ ?

Primary valency is the number of ions required to satisfy the charge on the metal ion.

Secondary valency is the number of ions of molecules that are coordinated to the metal ion.

Coordination number of

$Pt$ in

$PtCl_2.2NH_3$ is

$4$ , which are satisfied by

$2Cl$ and

$2NH_3$ . Hence, it does not have any primary valency and has

$4$ secondary valency.

Indicate the types of isomerism exhibited by the following complex and draw the structure of this isomer.
$[Pt(NH_3)(H_2O)Cl_2]$

In the given Complex geometrical cis - trans isomer can exist as shown in the image.
1074317_1105180_ans_58ee2aa3145140c390cbada6e24a35ef.png

What is the major product in this reaction.

Here

$Br$ has higher leaving capability than

$Cl$ . So on treatment with

$NaI$ ,

${ I }^{ \left( - \right) }$ substitutes

${ Br }^{ \left( - \right) }$ throng nucleophilic substitution.

1162882_1096200_ans_5f5f453db4904d45b60ba5b43b532778.png

What is the hybridization of central atom in following? $PH_3, PH_{4}^+,$

(i)

$PH_3 \longrightarrow \cfrac {Valence\quad e^-\quad of\quad central\quad atom+ Number\quad of\quad univalent\quad atom+ \pm charge}{2}$

$\Rightarrow \cfrac {5+3}{2}=4$

$\therefore sp^3$

(Refer to Image 1)

(ii)

$PH_4^+ \longrightarrow \cfrac {5+4-1}{2}=4=sp^3$

(Refer to Image 2)

1100595_1093770_ans_9465ae67e6994b3e9e917b77360174b4.png

On the basis of Werner's theory explain, why cobalt amine complex, $CoCl_{ 3 }{ 4NH }_{ 3 }$ when treated with ${ Ag }{ NO }_{ 3 }$ solution precipitates only one ${ Cl }^{ - }$ ion even though there are three ${ Cl }^{ - }$ ions?

In this compound, two

$Cl^-$ ions exhibit dual behavior of satisfying both primary and secondary valancies. These chloride ions do not get precipitated the

$D^-$ ion remained would get attached to the central metal atom via only secondary valency thus, it gets precipitated upon treatment with

$AgNO_3$ solution.
1057320_1126515_ans_e509d6186ecb402c96cd4a0300f01986.PNG

What is EAN? Write it's formula.

EAN is called as effective atomic number. It represents the total number of electrons surrounding the metal atom in a complex.It is composed of the electrons of metal and the corresponding ligands attached to that metal.It is calculated as:

EAN = Atomic number of the metal +(Number of ligands x electrons donated by each ligand) - positive oxidation state of the metal.

Explain the bonding on $CoCl_{ 2 }.3N{ H }_{ 3 }$ and $CoCl_{ 2 }.5N{ H }_{ 3 }$ structure on the basis at Werner's theory.

$CoCl_3.5NH_3$ complex

_____________________

Co-ordination number of

$Co$ is

$6$ . One remaining position is occupied by

$Cl^-$ ion.

$Cl^-$ ion exhibits the dual behaviour as it has a primary as well as secondary valency.

(Refer to Image)

Number of

$Cl^-$ ions precipitated=

$2$

Total number of ions=

$3$

Formula=

$[CoCl(NH_3)_5]Cl_2$

$CoCl_3.3NH_3$ complex

_____________________

$3 Cl^-$ ions satisfy primary as well as secondary valency. No

$Cl^-$ ion will be precipitated on the addition of

$AgNO_3$ at room temperature.

$\therefore$ Complex behave as neutral non-conducting molecule.

(Refer to Image 2)

1212640_1127463_ans_0ff60ff26ba7401682b9dce57cc5de2b.png

If the value of C.F.S.E. for ''Ni" is $\triangle _{ o }$ then what is the CFSE value Pd?

On going from

$3d$ to

$4d$ sense,

CFSE increase by

$50$ %

$3d=$ given,

$Ni$ has CFSE

$=\triangle$

$4d=$ CFSE of

$Pd=\triangle_0+(1/2)\triangle_0=1.5\triangle_0$

What is IUPAC name of $K_{3}\left [ Fe\left ( CN \right )_{5}NO \right ]$ ?

$K_3[Fe(CN)_5NO]$

$CN-$ Cyano

$NO-$ Nitrito-N

The name of the complex compound will be (IUPAC name)

Potassium pentacyanonitrito-N-ferrate(III)

Write the formula of the following complexes.
Bis (ethnylene diammine) dichloro iridium (III) ion

The formula of Bis (ethnylene diammine)dichloro iridium (III) ion is

$[Ir(en)_2 Cl_2]^{+}$ .

Write the formula of the following complexes.
Tris (ethylene diammine) cobalt (II) sulphate

Tris(ethylene diammine) cobalt (III) sulphate

Tris indicates three ligands of ethylene diammine which is a neutral ligand, and cobalt is the central metal with oxidation number +2

ethylene diammine

$\Rightarrow C_2H_8N_2$

Hence, the formula is:

$[Co(C_2H_8N_2)_3]SO_4$

What is coordinate bond?

Discuss briefly giving an example in each case the role of coordination compound medicinal chemistry.

Coordination compounds are major components in drug designing and synthesis of drugs. The major example is certain compounds of platinum. For example, cis-platin. It is a drug for cancer. These are used for inhibiting the growth of tumors.

Write the possible stereo isomers of the following complexes and identify the type :-
a) $[co(NH_3)_3Cl_3]$
b) $[pt(gly)_2]$
c) $[cr (en)_3]$

1015207_1143602_ans_63f35b7b5f434cefb1943f8f9ce64b51.png

Draw the isomer of $[Pt({ { NH }_{ 3 } })_{ 3 }{ Cl }_{ 3 }]$ , $[Co({ { NH }_{ 3 } })_{ 5 }{ Cl }{ SO }_{ 4 }]$ .

1351507_1141078_ans_030ef88c754c4bc987f2227a02409254.jpg

What is the nomenclature of $\left[ { CoCl }_{ 2 }({ NH }_{ 3 })_{ 4 } \right] ^{ + }$ ?

The IUPAC name of the given compound is tetraaminedichloro cobalt(III).

What is the primary valency of $[Co (NH_3)_4 Cl_2] Cl_2$ ?

The primary valency is the oxidation no. of the central metal atom and it is +4 .

what is the formula of potassium amminetrichlorido platinate(ii)

The formula of potassium amminetrichloridoplatinate(II) is

$K[Pt(NH_3)Cl_3]$ .

Differentiate between primary and secondary valencies?

Primary valency	Secondary valency
Primary valency is equal to the Oxidation number of central ion.	Secondary valency is equal to the coordination number of central metal ion.
It is non directional	It is directional
It is ionisable	It is non ionisable

write down the formulae of given compound
tetra amine zinc(II) nitrate

The formula of tetra amine zinc(II) nitrate is

$[Zn(NH_3)_4](NO_3)_2$

Draw the structure of $ClO_3^-$ .

1120194_1191564_ans_37b219caad16458cba1d369bd8363e85.PNG

Write down the $IUPAC$ name of the complex $[Pt (en)_2CI_2]^{2+}$ . What type of isomerism is shown by this complex.

1305777_1216505_ans_10b7ce07261046dd8e393a1c980e5170.PNG

write the formulae for Trioxalato cobaltate(III)ion

The formula of the compound trioxalatocobaltate(III) ion is

$[Co(C_2O_4)_3]^{3-}$ .

what is the formula of tetrakis(pyridine) platinum(ii) tetraphenyl borate(iii)

The formula of the compound tetrakis(pyridine)platinum(II)tetraphenylborate(III) is

$[Pt(py)_4][B(Ph)_4]_2$ .

$Cl_3^{^ - },Br_3^{^ - },ICl_2^{^ - },IBr_2^{^ - }\,including\,I_3^{^ - }$ . In these ions, one of the halogen atom (in case of similar atom) or halogen atom large in size undergoes $s{p^3}d$ -hybridization giving a liner shape with three lone pairs at equation positions.

$Geometry \to$ trigonal bipyramidal

$Shape \to$ liner

1381025_1265085_ans_52257f50e6444abb8fe83534d0a0ab3f.jpg

What is Hybridization ?

1351506_1291920_ans_3750111011414aaebc67dde8e14d34bc.jpg

On the basis of the following observations made with aqueous solutions. assign secondary valences to metals in the following compounds :
Formula Moles of AgCl precipitated per mole of the compounds with excess AgNO,
$\left( i \right)\,PdC{l_2}.4N{H_3}$ 2
$\left( {ii} \right)\,NiC{l_2}.6{H_2}O$ 2
$\left( {iii} \right)\,PtC{l_4}.2HCl$ 0
$\left( {iv} \right)\,CoC{l_3}.4N{H_3}$ 1
$\left( v \right)\,PtC{l_2}.2N{H_3}$ 0

(i) Secondary 4 (ii) Secondary 6 (iii) Secondary 6 (iv) Secondary 6 (v) Secondary 4

Name the type of isomerism exhibited by the following isomers : $[Cr(NH_3)_6][Co(CN_6)]$ and $[Co(NH_3)_6][Cr(CN)_6]$

Coordination Isomerism

Find sum of possible value of 'n' for which complex having formula: $[Pt(NH_{3})_{2}Cl_{2}]_{n}$ can exit.

the value of n=1

What is the hybridization of each in $CH_{2}=c=CH_{2}$ ?

1305243_1607142_ans_3013ccae18634e9db43ebf50703d02ed.jpg

select the correct state of hybridization at $X_1, X_2, X_3 and X_4$
$X_1$ $X_2$ $X_3$ $X_4$
(a) $sp^2$ $sp$ $sp^2$ $sp^3$
(b) $sp^3$ $sp^2$ $sp$     $sp$
(c) $sp^2$ $sp^2$    $sp$ $sp^3$
(d) $sp^3$ $sp^2$     $sp^2$       $sp$

1359797_1585237_ans_8996c5def79f4a169e22be5a10296e6e.jpeg

What is denticity?

1356808_1588986_ans_88186a249fc24422a4eb99b79c36c8fe.jpg

Draw all of the isomers of boht tetrahedral and square planar complexes which have unidentate ligands of type A and two unidentate ligands of type B.

Draw all of the isomers of an octahedral complex which has three identical bidentate ligands.

Describe the methods by which the presence of complex ions may be detected in solution.

What methods could be used to distinguish between cis and trans isomer of a complex?

Draw energy level diagrams and indicate the occupancy of the orbitals in the following complexes :
(a) $d^6$ octahedral, low-spin
(b) $d^9$ octahedral with tetragonal elongation
(c) $d^8$ square planar
(d) $d^6$ tetrahedral.

Calculate in units $\triangle_0$ the difference in crystal field stabilization energy between complexes (a) and (b) assuming that the ligands are strong field ligands.

$octshedral - 2.4 \triangle_0 , tetrahedral - 0.27 \triangle_0 , difference - 2.13 \triangle_0$

What are the geometric arrangements of $sp^3d^2, sp^3d$ and $dsp^2$ hybrid orbitals?

Match the metals of List $I$ with the biological organic of List $II$

1) Iron is present in haemoglobin - a red pigment of blood cells.

2) Zinc is present in the eyes of certain animals.

3) Manganese, iron and copper are present in chloroplasts.

4) Calcium and phosphorus are present in the teeth and bones of animals.

5) Some of the best sources of chromium are broccoli, liver and brewer's yeast. Potatoes, whole grains, seafood and meats also contain chromium.

Hence the correct match is :

A) Chromium - Prawns

B) Iron - Chloroplasts, Haemoglobin

C) Zinc - Eyes of cat and cows

D) Calcium - Bones

Hence the correct answer is : A - 4 , B - 1 , 2 , C - 3 , D - 5

Name the metal present in haemoglobin.

The heme group (a component of the hemoglobin protein) is a metal complex, with iron as the central metal atom, that can bind or release molecular oxygen.

Describe hybridization in the case of $PCl_5$ and $SF_6$ . The axial bonds are longer as compared to equatorial bonds in $PCl_5$ whereas in $SF_6$ both axial bonds and equatorial bonds have the same bond length. Explain .

1896967_1723547_ans_3d2d3e1583044769a0e933c7e22844e4.jpg

Find the number of total possible coordination isomers in $[Pt(NH_3)_4][Cu(Cl)_4]$ .

The number of total possible coordination isomers in

$[Pt(NH_{3})_{4}][Cu(Cl)_{4}]$ is 4.

These include coordination isomers

$[Pt(Cl)_{4}][Cu(NH_{3})_{4}]$

$[Cu(NH_{3})_{3}Cl][Pt(Cl)_{3}NH_{3}]$

$[Pt(NH_{3})_{3}Cl][Cu(Cl)_{3}NH_{3}]$

$[Pt(NH_{3})_{4}][Cu(Cl)_{4}]$

Hence , correct answer is 4 .

Give the electronic configuration of the following complexes on the basis of crystal field splitting theory.
$[CoF_6]^{3-}, [Fe(CN)_6]^{4-}$ and $[Cu(NH_3)_6]^{2+}$ .

$[CoF_6]^{3-}, Co^{3+}\rightarrow (d^6)\rightarrow t^4_{2g}e^2_g$

$[Fe(CN)_6]^{4-}, Fe^{2+}\rightarrow (d^6)\rightarrow t^6_{2g}e^0_g$ ,

$[Cu(NH_3)_6]^{2+}, Cu^{2+}\rightarrow (d^9)\rightarrow t^6_{2g}e^3_g$ .

In $SF_4$ atom has $sp^x d$ hybridisation.What is the value of x?

1559943_1727102_ans_abd4971eb43249dba3529c9197fe4eb9.jpg

$NiCl_2$ in the presence of dimethyl glycoxime (DMG) gives a complex which precipitates in the presence of $NH_4OH$ , giving a bright red color.
Draw its structure and show H bonding.

Structure of the complex is given above.
1925885_1727678_ans_4d9be9a8033547289818a8acef1155c9.JPG

Write the formulae of the following complex.
Pentamminechlorocobalt(III) ion.

$\text{The formulae of the Pentamminechlorocobalt(III) ion. is } [Co(NH_3)_5Cl]^{2+}$
1925646_1727618_ans_d3c4eaabc2e446b79fe5ab6841efb628.png

The number of orbitals involved in the hybridization of $XeF_2$ is:

1728225_1727095_ans_1d38eb848f5d4f9da41673514520748e.jpg

A complex of the type $[M(AA)_2X_2]^{n+}$ is known to be optically active. What does this indicate about the structure of the complex? Give one example of such complex.

An optically active complex of the type

$[M(AA)_2X_2]^{+n}$ indicates cis-octahedral structure.

e.g., cis -

$[Pt(en_2Cl_2]^{2+}$ or cis -

$[Cr(en)_2Cl_2]^+$ .

Match the complexes in List-I with their stereoproperties in List-II:

(A) is optically inactive and show facial form.

(B) shows facial and trans form and is optically inactive

(D) is Cis shows facial form, and trans shows meridian form and is inactive.

Draw the structure of geometrical isomers of $[Pt(gly)_2]$ where $gly \to NH_2CH_2COO^-$ .

1573950_1731674_ans_21f00c5a853745d1b2278c0d15cabf16.jpg

Match the hybridization in List-I with its reference in complex compounds List-II:

$A \rightarrow (iii)(iv), \ B \rightarrow (ii)(iv), \ C \rightarrow (i), \ D \rightarrow (i)$

What type of isomers are the following ?
$[Co(py)_2(H_2O)_2Cl_2]Cl$ and $[Co(py)_2(H_2O)Cl_3]H_2O$

1669414_1729808_ans_49cc7bd35e004df4b6462dd413da038c.jpg

Write the formulae of the following complexes:
Potassium ethylenediamine tetraacetate ferrate (II)

The formula of the complexes:

Potassium ethylenediamine tetraacetate ferrate(II) is

$K_2[Fe(EDTA)]$ .

A certain complex ion has the formula $[M(en)_2Br_2]^+$ where $M$ is the metal ion and en = ethylene diamine. How many isomers are possible for this?

1575567_1731706_ans_1b4f9b90523b4f4bb42af62dafba4c00.jpg

Write down the names of crystal structures in which the following elements are present.

$Sc,\ Ti,\ V,\ Cr,\ Mn,\ Fe,\ Co,\ Ni,\ Cu,\ Zn.$

1728149_1732034_ans_bf4b4b8b7f184f7aafefb19ba5778251.jpg

The EAN of each $Mn(Z=25)$ in $Mn_2(CO)_{10}$ is $36$ . What is the structure of this complex?

Structure of

$(Mn)_2CO_{10}$

EAN of carbonyl compounds = z(Atomic number) + no. of electron donated + 1M-M delta bond

It is given that in

$(Mn)_2CO_{10}$ EAN =36

By equating we get the number of electron donated = 10

1575536_1731682_ans_4d5dbab2109d403293a8f35f92cd08ad.jpg

The decahydrate form of sodium carbonate i.e. washing soda on standing in air effloresces and crumbles to powder. The number of water molecule (s) present in the compound formed is

$Na_{2}CO_{3}\cdot10H_{2}O\xrightarrow[-9H_{2}O]{effloresces}Na_{2}CO_{3}\cdot{H}_{2}O$ (monohydrate)

Ans-

$1$

Account for the following:
Give the formula and describe the structure of a noble species which is isostructural with $IBr_{2}^{-}$ .

Total number of lone pairs around central atom

$I$ , is 3.

Total number of bond pairs around central atom

$I$ , is 2.
Therefore, according to

$VSEPR$ theory,

$IBr_{2}^{-}$ , should be linear.
Now a noble gas compound having

$10$ electrons in the valence shell of central atom is

$XeF_{2} (8 + 2 \times 1 = 10)$ . As it has

$2$ bond pairs and

$3$ lone around

$Xe$ therefore like

$IBr_{2}^{-}, XeF_{2}$ is also linear.

1638684_1778532_ans_ccdfd92391f140fe9388757d6a1f9af3.png

$CO^{3-}$ ion is bound to one $Cl$ , one $NH_3$ molecule and two bidentate ethylene molecule.
Write the formula, name and magnetic behaviour of the above coordination entity.

Formula:

$[Co(NH_3)Cl(en)_2]^{2+}$

Name of the complex : Amminechloridobis ( ethane-1, 2-diamime) - cobalt (III) ion

Magnetic behaviour: Diamagnetic

Name a complex used in treatment of cancer.

Cisplatin

$\left\{cis-[Pt(NH_{3})_{2}Cl_{2}])\right\}$ is used in the treatment of cancer.

$Ni^{2+}$ ion is bound to two water molecules and two oxalate ions.
Write the formula, name and magnetic behaviour of the above coordination entity.

Formula:

$[Ni(H_2O)_2(ox)_2]^{2-}$

Name of the complex:

$Diaquadioxalatonickelate (II) ion$

Magnetic behaviour:

$Paramagnetic$

What are crystal fields?

The ligands especially anionic (or polar neutral ligands) has around them negatively charged field because of which they are called crystal field.

Write the formula of the following :
Tetraammineaquachloridocobalt (III) nitrate

The chemical formula of the above compound is

$[Co(NH_3)_4(H_2O)Cl](NO_3)_2$

What type of isomerism is shown by the following complex:
$[Co(NH_{3})_{6}][Cr(CN)_{6}]$

The complex

$[Co(NH_{3})_{6}][Cr(CN)_{6}]$ shows Coordinate isomerism.

Giving a suitable example for each, explain the following:
Crystal field splitting

$\textbf{Crystal field splitting}$ : When the ligands approach the central metal ion, the electrons in the

$d-$ orbital of central metal ion will be repelled by the ion pairs of the ligands. Because of these interactions the degeneracy of

$d-$ orbitals of the metal ion is lost and these split into two sets of orbital having different energies. This is known as crystal field splitting e.g., for

$d^4$ , configuration is

$t_{2g}^3 , e_g^1$ , in the presence of weak field ligand.

What type of isomerism is exhibited by the following complex:
$[Co(NH_{3})_{5}SO_{4}]Cl$

The complex

$[Co(NH_{3})_{5}SO_{4}]Cl$ shows Ionisation isomerism.

A coordination compound with the molecular formula $CrCl_{3}.4H_{2}O$ precipitates $AgCl$ with $AgNO_{3}$ solution. Its molar conductivity is found to be equivalent to two ions. What is the structural formula and name of the compound?

It is given that molar conductivity is equivalent to two ions

Total two ions mean one ionizable ion and one complex ion.

∴ Formula is $[Co(H_2O)_4Cl_2]Cl$

Name of the complex: tetraaquadichloridocobalt (III) chloride

What type of isomerism is shown by the complex $[Cr(H_2 O)_6]Cl_3$ ?

Hydration isomerism is shown by the complex

$[Cr(H_2O)_6]Cl_3$ .

Name the following coordinates entity and describe its structure
$[Fe(CN)_6]^{4-}$
(Atomic Number: $Fe=26$ )

IUPAC Name:

$Hexacyanoferrate(II)$ ion;

$Fe^{2+}(3d^6)$

$d^2 sp^3$ hybdrisation in

$[Fe(CN)_6]^{4-}$ leads to octahedral structure.

Write the state of hybridisation, shape and IUPAC name of the complex $[CoF_6]^{3-}$ .

IUPAC name: Hexafluoridocobaltate

$(III)$ ion

Hybridisation

$=sp^3d^2$

Shape= Octahedral

1642334_1779275_ans_f8c87589fbcb437caf16ea6f2b914dab.png

What is meant by crystal field splitting energy? On the basis of crystal field theory, write the electronic configuration of $d^4$ in terms of $t_{2g}$ and $e_g$ in an octahedral field when
$\Delta_0 < P$

The difference of energy between two sets of degenerated orbitals after crystal field splitting is known as crystal field splitting energy.

Electronic configuration of

$d^4$ if

$\Delta_0 < P$ is

$t_{2g}^3 e_g^1$

What type of isomerism is shown by $[Co(NH_3)_5 ONO]Cl_2$ ?

The above complex shows Linkage isomerism and the linkage isomer is

$[Co (NH)_3 NO_2]Cl_2$

What type of isomerism is shown by the complex $[Co(NH_3)_5 (SCN)]^{2+}$ ?

$[Co(NH_3)_5 (SCN)]^{2+}$ shows Linkage isomerism and the linkage isomer is

$[Co(NH_3)_5 (NCS)]^{2+}$

What is meant by crystal field splitting energy? On the basis of crystal field theory, write the electronic configuration of $d^4$ in terms of $t_{2g}$ and $e_g$ in an octahedral field when
$\Delta_0 > P$

The difference of energy between two sets of degenerated orbitals after crystal field splitting is known as crystal field splitting energy.

Electronic configuration of

$d^4$ if

$\Delta_0 > P$ is

$t_{2g}^4 e_g^0$

What type of isomerism is shown by the complex $[Co(NH_3)_6] [Cr(CN)_6]$ ?

$[Co(NH_3)_6] [Cr(CN)_6]$ shows Coordination isomerism.

Name the following coordinates entities and describe their structures
$[Ni(CN)_4]^{2-}$
(Atomic Numbers: $Ni=28$ )

IUPAC Name: Tetracyanonickelate

$(II)$ ion;

$Ni^{2+}(3d^8)$

$dsp^2$ hybdrisation in

$[Ni(CN)_4]^{2-}$ leads to square planar structure.

1642340_1779280_ans_8b94a45d9e774394a161401554cbefd7.png

Using valence bond theory explain the $[Co(NH_3)_6]^{3+}$ in relation to the term given below:
Type of hybridisation

Hybridisation:

$d^2sp^3$

1642398_1779305_ans_2d28581245fa4311b0f5ff466fcb9258.png

Answer the following question:
On the basis of crystal field theory, write the electronic configuration for $d^4$ ion, if $\Delta_0 < P$ .

$\Delta_0 < P$ , the fourth electron enters in one of the two

$e_g$ orbitals giving the configuration

$t_{2g}^3 e_g^1$ .

Described for the following complex ion, the type of hybridisation, shape and magnetic property:
$[NiCl_4]^{2-}$

The central metal Ni undergoes

$sp^3$ hybridisation due to which the structure of the complex becomes tetrahedral.

It is paramagnetic due to the presence of unpaired

$e^-$ in d orbitals.

1645925_1779349_ans_f8eae690a9e1432c813bc6648617597b.png

Described for the following complex ion, the type of hybridisation, shape and magnetic property:
$[Fe(H_2 O)_6]^{2+}$

The shape of the complex is Octahedral because of

$sp^3 d^2$ hybridisation. It is Paramagnetic, as there are four unpaired electrons present in the complex ion.
1645913_1779346_ans_ec1b532042984cbaae455d566185387a.png

1645913_1779346_ans_ec1b532042984cbaae455d566185387a.png

Explain the following with two examples:
Coordination entity

$\textbf{Coordination entity}$ : A coordinate entity constitute a central metal atom ot ion bonded to a fixed of number of molecules or ion (ligands).

e.g,

$[Co(NH_3)_3 Cl_3], [Fe(CN)_6]^{4-}, [Cu(NH_3)_4]^{2+}$ .

$[Co(NH_2)_6]^{3+}$

The central atom Co is

$d^2 sp^3$ hybridised which leads to octahedral geometry. The complex is Diamagnetic, as there is no unpaired electron present in the complex.
1645914_1779348_ans_20a92bca5a594339978876f4ec996347.png

1645914_1779348_ans_20a92bca5a594339978876f4ec996347.png

Indicate the types of isomerism exhibited by the following complex and draw the structures of the isomers:
$K[Cr(H_2O)_2(C_2O_4)_2]$

Both geometrical (cis-trans) and optical isomers for cis-form can exist.
1642433_1779317_ans_ca2c2cb7690c4a55b45603da5129be4c.png

Answer the following question:
On the basis of crystal field theory, write the electronic configuration for $d^4$ ion if $\Delta_0 < P$ .

$\Delta_0 < P$ then fourth electrons enters one of the

$e_g$ orbitals giving the configuration

$t_{2g}^3 e_g^1$

Answer the following question:
Define crystal field splitting. On the basis of crystal field theory, write the electronic configuration for $d^{4}$ ion if $\Delta_0 < P$ .

When ligand approaches a transition metal ion, the

$d-$ orbital split int two sets, one with lower energy and the other with higher energy. The difference between the two sets of orbital is called crystal field splitting energy.
If

$\Delta_0 < P$ , the fourth electrons one of the

$e_g$ giving the configuration

$t_{2g}^3 e_g^1$ ,

Answer the following question:
Name two complexes which are used in medicines.

1. The platinum complex,

$cis-[Pt(NH_3)_2Cl_2]$ known as cisplatin is used in the treatment of cancer.
2.

$Ca-EDTA$ complex is used in the treatment of lead poisoning.

Write all the possible isomers of $[Co(NH_3)_5(SCN)]Cl$

$[Co(NH_3)_5(SCN)]Cl, [Co(NH_3)_5(NCS)]Cl, [Co(NH_3)_5Cl]SCN, [ Co(NH_3)_5Cl]NCS$ .

$MA_5B$ type complexes do not show geometrical or optical isomerism.

Indicate the types of isomerism exhibited by the following complex and draw the structures of the isomers:
$[Pt(NH_3)(H_2O)Cl_2]$

The complex

$[Pt(NH_3)(H_2O)Cl_2]$ shows Geometrical isomerism.
1642429_1779316_ans_4cabe9f9945945beb334019e0051343d.png

A metal ion $M^{n+}$ having $d^4$ valence electronic configuration combines with three bidentate ligands to form a compound. Assuming $\Delta_0 > P$ :
Name the type of isomerism exhibited by this complex.

The complex shows Optical isomerism.

$CoSO_4Cl.5NH_3$ exists in two isomeric forms $'A'$ and $'B'$ . Isomer $'A'$ reacts with $AgNO_3$ to give white precipitate, but does not react with $BaCl_2$ . Isomer $'B'$ gives white precipitate with $BaCl_2$ but does not react with $AgNO_3$ . Answer the following question:
Name the type of isomerism involved.

The isomerism involved in the above phenomenon is Ionisation isomerism.

What is the hybridization of each carbon in $H_2C=C=CH_2$ ?

The given structure is of

$C_3H_4$ in which all three carbon atoms are linked to each other by double bonds. Carbons are marked as C1. C2 and C3. C1 and C3 are

$sp^2$ hybridized because of having

$3\sigma$ and

$1\pi$ bonds. C2 has

$2\sigma$ bonds and

$2\pi$ bonds it is

$sp$ hybridized.

$H_2\overset{C1}C=\overset{C2}C=\overset{C3}CH_2$

A metal ion $M^{n+}$ having $d^4$ valence electronic configuration combines with three bidentate ligands to form a compound. Assuming $\Delta_0 > P$ :
What type of hybridisation will $M^{n+}$ ion have?

As there are three bidentate ligands to combine, therefore hybridisation will be

$d^2 sp^3$ .

$CoSO_4Cl.5NH_3$ exists in two isomeric forms $'A'$ and $'B'$ . Isomers $'A'$ reacts with $AgNO_3$ to give white precipitate, but does not react with $BaCl_2$ . Isomer $'B'$ gives white precipitate with $BaCl_2$ but does not react with $AgNO_3$ . Answer the following questions:
Identify $'A'$ and $'B'$ and write their structural formulae.

$A=[Co(NH_3)_5 SO_4]Cl$

$B=[Co(NH_3)_5Cl]SO_4$

Answer the following question:
Give the electronic configuration of the $d-$ orbitals of $Ti$ in $[Ti(H_2O)_6]^{3+}$ ion in an octahedral crystal field.

$[Ti(H_2O)_6]^{3+}$ ion,

$Ti$ in

$+3$ oxidation state. Thre is one electron in

$d-$ orbital and the electronic configuration is

$t_{2g}^1 e_g^0$ .

Explain, how is the electronegativity of carbon atoms related to their state of hybridization in an organic compound?

Since s-electrons are more strongly attached by the nucleus than p-electrons, therefore, electronegativity increases as the s-character of the hybridized orbital increases, i.e., in the order:

$sp^3<sp^2<sp.$

Explain the following:
Low spin octahedral complex of nickel are not known.

For the formation of low spin complex, electrons present in

$3d$ electrons of

$Ni^{2+}$ should pair up. This will produce only one empty

$d$ orbital. Hence,

$d^2 sp^3$ hybridisation in nickel is not possible to form low spin octahedral complex.
1645957_1779382_ans_f914b055ce654466aa1f9300a3696784.png

1645957_1779382_ans_f914b055ce654466aa1f9300a3696784.png

Give the structure of the following compounds.
2-Hydroxycyclopentanecarbaldehyde

1717603_1797114_ans_a73f603148154dcd9427732520a7f34b.png

Explain the following term with example.
Structural isomerism

Structural isomerism or constitutional isomerism is a form of isomerism in which molecules have the same molecular but different arrangement of the atoms in space. Different arrangements may be in bonding patterns and atomic organization

For example :

$CH_{3} OCH_{3} \ and\ CH_{3}CH_{2}OH$ are structural isomers.

Column-I and Column-II contains four entries each. Entries of Column-I are to be matched with one or more than one entries of Column-II. Each entry of Column-I may have the matching with one or more than one entries of Column-II.

Sodium nitroprusside- $Na_{2}[Fe(CN)_{5}NO]$

$Hyb.^{n} - d^{2}sp^{3};$

$\mu = 0;$

$octahedral,$

$NO^{+}$ ligand

Brown ring $[\overset {+I}{Fe}(H_{2}O)_{5}NO]^{2+}$

$Hyb^{n}.\rightarrow sp^{3}d^{2};$

$octahedral,$

$m = 3.89\ BM,$

$NO^{+} ligand$

Complex formed during extraction of $Ag$ is $[Ag(CN)_{2}]^{-}$

$Hyb^{n}. - sp^{3}d^{2};$

$octahedral,$

$m = 3.89\ BM,$

$NO^{+}$ ligand

Complex formed during extraction of $Ag$ is $[Ag(CN)_{2}]^{-}$

$Hyb^{n} - d^{2}sp^{3}; octahedral, \mu = 0$ .

Brown colour of the complex $[Fe(H_{2}O)_{5}(NO)]SO_{4}$ is due to C.T. spectrum which causes momentary change in oxidation state. Find out oxidation state of $Fe$ in this complex.

$\overset {+1}{[Fe}(H_{2}O)_{5}(NO)]SO_{4}$

So, the oxidation state of Iron in given complex is +1.

Calculate the magnetic moment of $Ni^{2+}$ ion.

Configuration of d orbitals for

$Ni^{2+}$ is

$3d^8$ so the number of unpaired electrons are two therefore the magnetic moment of

$Ni^{2+}$ given by

$\mu = \sqrt{n(n + 2)}$

$= \sqrt{2 (2 + 2)}$

$= \sqrt{8} = 2\sqrt{2}$

$= 2 \times 1.414 = 2.828$ B.M.

Explain the hybridization of the central metal atom in the complex $[Ni(CN)_4]^{2-}$ with the help of diagram.

$[Ni(CN)_4]^{2-}$

Electronic configuration of

$Ni : [Ar] 4s^2 3d^8$

Electronic configuration of

$Ni^{2+} : [Ar] 4s^0 3d^8$

Outer electronic configuration of

$Ni^{2+}$ (Refer Fig.1)

Pairing of electrons takes place in the presence of strong field ligand

$CN^-$ . Thus , one

$3d$ orbital becomes vacant.

(Refer Fig.2) As the hybridization involved is

$dsp^2$ , we get square planar complex. As there are no unpaired

electrons the complex is diamagnetic.

1744960_1831356_ans_9c6540cbf049424a89069ab4ee5ab4b1.png

What is hybridization ?

Hybridization is a process where two or more atomic orbital of comparable energy of valency shell of an atom mix to form the same number of new orbital of the same energy.

What is meant by hybridisation of atomic orbitals? Describe $sp, sp^2$ and $sp^3$ hybridixation with examples.

Hybridization is the phenomenon of intermixing of orbitals slightly different energies so as to redistribute their energies and to give new set of orbitals of equivalent energy and shape. The atomic orbitals taking part in hybridisation are called hybrid orbitals. These hybrid orbitals have minimum repulsion between their electron pairs and thus are more stable. Only orbitals of almost similar energies and belonging to same atom and ion under go hybridization. Th number of hybrid orbitals produced ie equal to the number of pure orbitals mixed during hybridization. The type of hybridisation indicates the geometry of the molecules. Only atomic orbitals participate in hybridisation. Electron's present in them do not take part.

(a)

$sp$ hybridisation: The type of hybridisation involves the mixing of one

$s$ and one

$p$ orbital resulting in the formation of two equivalent

$sp$ hybrid orbitals. Each

$sp$ hybrid orbital has

$50\% s-$ character and

$50\% p-$ character. Such a molecules in which the central atom is

$sp-$ hybridised and linked directly two other central atoms possesses linear geometry.

This type of hybridisation is also known as diagonal hybridisation. The bond angle is

$180^o$ .

(b)

$sp^2$ hybridisation: In this hybridisation, there is involvement of one

$s$ and two

$p$ orbitals in order to form three equivalent

$sp^2$ hybridized orbitals. The three hybrid orbitals so formed are oriented in a plane at maximum distance to form an angle of

$120^o$ between the hybrid orbitals. The hybrid orbitals are oriented in a trigonal planar arrangement.

(c)

$sp^3$ hybridisation: In this type of hybridisation, there is mixing of one

$s-$ orbital and three

$p-$ orbitals of the valence shell to form four

$sp^3$ hybrid orbital equivalent energies and shape. There is

$25\% s-$ character and

$75\% p-$ character in each

$sp^3$ hybrid orbital. This hybridisation has tetrahedral geometry.

What will be geometry of complexes having hybridization $sp^3$ and $dsp^2$ . Give an example of each.

The geometry of complex having hybridization

$sp^3$ will be tetrahedral and geometry for

$dsp^2$ hybridization will be square planar.

e.g.,

$[NiCl_4]^{2-}$ having tetrahedral geometry and hybridization will be

$sp^3$ and

$[Pt(CN)_4]^{2-}$ having square planar geometry and hybridization will be

$dsp$ on central atom.

How many structural isomers can you draw for pentane?

Step 1: Structural isomers

Structural isomers are compounds having the same molecular formula but different arrangements of atoms.

As the name suggests 'pent' means five, thus pentane has five carbon atoms.

The molecular formula of pentane is

$C_5 H_{12}$

Step 2: Structural isomers of pentane

Three structural isomers of pentane are:

n-pentane
Iso-pentane (methyl butane)
Neo-pentane (dimethyl propane)

Final Step: Pentane has three structural isomers.

Define Hybridization.

Hybridization is a process where two or more atomic orbital of comparable energy of valency shell of an atom mix to form the same number of new orbital of the same energy.

The valence atomic orbital on carbon in silver acetylide is .................hybridized.

The valence atomic orbital on carbon in silver acetylide is sp hybridized.

This carbon has two bonding domains and zero lone pairs.

$H−C≡C^{-} Ag^{+}$

Hence , The valence atomic orbital on carbon in silver acetylide is

$sp$ hybridized .

The maximum number of stereoisomers possible for the ion $[\overset {IV}{Pd}(NH_{3})_{2}(H_{2}O)_{2}Br_{2}]^{2+}$ is :

Six stereoisomers (optical and geometrical) are possible for

$[\overset {IV}{Pd}(NH_{3})_{2}(H_{2}O)_{2}Br_{2}]^{2+}$ .

They are as follows:
(1) to (5) are geometrical isomers; (5) and (6) are optical isomers.

Match the complex in List-I with the type of isomerism given in List-II.

Complex	Isomerism
$[Co(NH_3)_4Cl_2]$	Geometrical
$cis[Co(en)_2Cl_2]$	Optical
$[Co(en)_2(NO_2)Cl]SCN$	Ionisation
$[Co(NH_3)_6][Cr(CN)_6]$	Coordination

Match the complex in List-I with its corresponding property(ies) given in List-II.

Complex	Isomerism
$[Cr(NO_2)_2(NH_3)_2Cl_2]$	Geometrical, Linkage
$[Cr(NH_3)_4Cl_2]Br$	Ionisation, Geometrical
$[Cr(en)_3]^{3+}$	Optical
$[Pt(NH_3)_2Cl_2][Cu(CN)_4]$	Coordination, Linkage

Column $\displaystyle -$ I Column $\displaystyle -$ II
( where AB $\displaystyle \rightarrow$ Unsym. bidentate ligand having no chiral center, a, b, c, d & e $\displaystyle \rightarrow$ monodentate ligands )

The complex of the type

$\displaystyle \left [ Ma_{2}bcde \right ]^{n\pm }$ contains 3 optically inactive isomers.
The complex of the type

$\displaystyle \left [ Ma_{2}b_{2}c_{2} \right ]^{n\pm }$ contains 6 stereo( space ) isomers and 2 optically active isomers.
The complex of the type

$\displaystyle \left [ Ma_{3}bcd \right ]^{n\pm }$ contains 3 optically inactive isomers, 4 geometrical isomers and 2 optically active isomers.
The complex of the type

$\displaystyle \left [ M\left ( AB \right )c_{2}d_{2} \right ]^{n\pm }$ contains 4 geometrical isomers and 6 stereo( space ) isomers.

Column I Column II

The complex

$\displaystyle \left [ Ni\left ( gly \right )_{3} \right ]^{-}$ has four optically active isomers and is paramagnetic in nature as it contains unpaired electrons.
The complex

$\displaystyle \left [ FeBr_{2}Cl_{2}\left ( NO_{2} \right )\left ( OH \right ) \right ]^{4-}$ has four optically active isomers and eight stereo isomers. It is paramagnetic complex as it contains unpaired electrons.
The complex

$\displaystyle \left [ IrCl_{2}\left ( gly \right )_{2} \right ]^{-}$ contains eight stereo isomers and is diamagnetic in nature due to presence of all paired electrons.
The complex

$\displaystyle \left [ Co\left ( CN \right )_{2}\left ( NO_{2} \right )_{2}\left ( NH_{3} \right )\left ( py \right ) \right ]^{-}$ has four optically active isomers, and eight stereo isomers. It is diamagnetic in nature as all the electrons are paired.

Match the complexes in List 1 with their properties in List 2.

A) The complex

$\displaystyle \left [ CoCl_{3}\left ( NH_{3} \right )_{3} \right ]$ shows geometrical isomerism in the form of facial and meridional isomerism.
B) The complex

$\displaystyle \left [ Cr\left ( OX \right )_{3} \right ]^{3-}$ shows optical isomerism, due to the presence of molecular asymmetry. It shows two optically active isomers which are a pair of enantiomers.
C) The complex

$\displaystyle \left [ CrCl_{2}\left ( OX \right )_{2} \right ]$ shows geometrical as well as optical isomerism.
The cis form is optically active whereas, the trans form is optically inactive. It has two optically active isomers.
D) The complex

$\displaystyle \left [ RhCl_{3}\left ( Py \right )_{3} \right ]$ shows geometrical isomerism in the form of facial and meridional isomerism.

There are ............... electron in $t_{2g}$ orbitals in $[CoF_6]^{3-}$ .

$[CoF_6]^{3-}$ , the central cobalt atom has +3 oxidation state and has electronic configuration

$3d^6$ . Since, fluoride is a weak ligand, the electrons will prefer to go to

$e_g$ level than pair up. Hence, the outer electronic configuration will be

$t_{2g}^{4}e_g^2$ .

$[CoF_6]^{3-}$ has 4 electrons in

$t_{2g}$ orbitals.

Match the column.

(A) The complex

$[M(AA)_3]$ shows optical isomerism.
(B) The complex

$[M(AA)_2b_2]$ shows optical isomerism.
It has only one cis and one trans isomer.
In this complex, any cis isomer is optical active.
(C) The complex

$[M(AA)b_2c_2]$ shows optical isomerism.
It has only one cis and two trans isomers.
(D) The complex

$[M(AA)b_2cd]$ shows optical isomerism.
It has four geometrical isomers.
In this complex any cis isomer is optical active.

Write the sum of geometrical isomers in [Pt(H $_2$ N - CH(CH $_3$ ) - COO $^-$ ) $_2$ ] complex and stereoisomers of [Pt(gly) $_3$ ] $^+$ complex.

Total number of geometrical isomers in [Pt(H

$_2$ N - CH(CH

$_3$ ) - COO

$^-$ )

$_2$ ] = 4
Total number of stereo isomers in [Pt(gly)

$_3$ ]

$^+$ = 4
Sum of geometrical isomers and stereo isomers of given complexes = 8
Thus, the sum of geometrical isomers in [Pt(H

$_2$ N - CH(CH

$_3$ ) - COO

$^-$ )

$_2$ ] complex and stereoisomers of [Pt(gly)

$_3$ ]

$^+$ complex is 8.

Match the complex (in Column I) with the type of isomerism (in Column II) (unitary match).

(A) The complex

$[Co(NH_3)_4Cl_2]$ shows geometrical isomerism.
(B) The complex

$cis[Co(en)_2Cl_2]$ shows optical isomerism.
(C) The complex

$[Co(en)_2(NO_2)Cl]SCN$ shows ionization isomerism.
(D) The complex

$[Co(NH_3)_6][Cr(CN)_6]$ shows coordination isomerism.

Find the total number of possible structural isomers of the compound $[\overset{II}{Cu}(NH_3)_4]\overset{II}{[Pt}Cl_4].$

The total number of possible structural isomers of the compound

$[\overset{II}{Cu}(NH_3)_4]\overset{II}{[Pt}Cl_4]$ is 4.

These include coordination isomers

$[Cu(NH_3)_4][PtCl_4]$ ,

$[Cu(NH_3)_3Cl][PtCl_3(NH_3)]$ ,

$[Pt(NH_3)_3Cl][CuCl_3(NH_3)]$ ,

and

$[Pt(NH_3)_4][CuCl_4]$

Explain the bonding in coordination compounds in terms of Werners postulates.

Postulates of Werner's coordination theory:
(1) Metal shows primary valence (ionizable, oxidation number) and secondary valence (non ionizable, coordination number).

(2) Coordination number (secondary valence) is fixed for every metal.
(3) Negative ions satisfy primary valence and negative ions or neutral molecules satisfy secondary valence.
(4) Secondary valencies are directional in nature and determine stereochemistry of complex.

$S^{2-}+Na_2[Fe(CN)_5NO]\longrightarrow$ Complex is having violet/purple coloration(X)
The total number of possible isomers for complex X is ......... provided the ambident behavior of $CN^-$ is not considered.

$S^{2-}+Na_2[Fe(CN)_5NO]\longrightarrow Na_2[Fe(CN)_5NOS]^{2-}$ The Complex is having violet/purple coloration.
The total number of possible isomers for complex is 3 provided the ambident behavior of

$CN^-$ is not considered.

Specify the oxidation numbers of the metals in the following coordination entities:
(i) $[Co(H_{2}O)(CN)(en)_{2}]^{2+}$ (ii) $[CoBr_{2} (en)_{2}]^{+}$ (iii) $[PtCl_{4}]^{2-}$ (iv) $K_{3} [Fe(CN)_{6}]$ (v) $[Cr(NH_{3})_{3}Cl_{3}]$

Let X be the oxidation number of metal in the complex.
(i)

$\displaystyle X + 0 + (-1) + 2(0) = +2 \\ X = +3$
(ii)

$\displaystyle X + 2(-1) +2(0) = +1 \\ X = +3$
(iii)

$\displaystyle X + 4(-1) = -2 \\ X = +2$
(iv)

$\displaystyle 3(+1) +X + 6(-1) = 0 \\ X = +3$
(v)

$\displaystyle X + 3(0) +3(-1) = 0 \\ X =+3$

What is the oxidation state of Co in the complex $[CoCl_2(en)_2]^+$ ?

[Note: Ethylenediamine (en) $=H_2N-CH_2-CH_2-NH_2$ ]

Ethylenediamine is a neutral ligand and chloride has a

$-1$ charge associated with it.

Let's assume oxidation state of Cobalt

$=x$ and, that of

$Cl^-=-1$

Then,

$x + 2\times({-1})= +1\Longrightarrow\ x=+3$

Hence, the oxidation state of Co is +3.

List various types of isomerism possible for coordination compounds, giving an example of each.

Various types of isomerism possible for coordination compounds, alongwith an example of each are as shown.

Aqueous copper sulphate solution (blue in colour) gives:
(i) a green precipitate with aqueous potassium fluoride and
(ii) a bright green solution with aqueous potassium chloride. Explain these experimental results.

Aqueous copper sulphate solution is blue in colour due to presence of

$\displaystyle [Cu(H_2O)_4] ^{2+}$ ions.
(i) It reacts with KF to form green coloured

$\displaystyle [CuF_4]^{2-}$ .

$\displaystyle [Cu(H_2O)_4] ^{2+} + 4 F^- \rightarrow [CuF_4]^{2-}$

It reacts with KCl to form bright green coloured

$\displaystyle [CuCl_4]^{2-}$ .

$\displaystyle [Cu(H_2O)_4] ^{2+} + 4 Cl^- \rightarrow [CuCl_4]^{2-}$
In both examples, the weak field ligand water is replaced by fluoride and chloride ions.

What is the coordination entity formed when excess of aqueous $KCN$ is added to an aqueous solution of copper sulphate? Why is it that no precipitate of copper sulphide is obtained when $H_{2}S(g)$ is passed through this solution?

Copper sulphate reacts with excess

$KCN$ to form

$\displaystyle [Cu(CN)_4]^{2-}$ .
Cyanide ion is strong field ligand and forms highly stable complex ion and does not ionize to give

$\displaystyle Cu^{2+}$ ions. When

$\displaystyle H_2S$ gas is passed, free

$\displaystyle Cu^{2+}$ are not available to form

$CuS$ precipitate.

Amongst the following, the most stable complex is:
(i) $[Fe(H_{2}O)_{6}]^{3+}$ (ii) $[Fe(NH_{3})_{6}]^{3+}$ (iii) $[Fe(C_{2}O_{4})_{3}]^{3-}$ (iv) $[FeCl_{6}]^{3-}$

$\displaystyle [Fe(C_{2}O_{4})_{3}]^{3-}$ is a metal chelate. Hence, it is most stable.

Draw all the isomers (geometrical and optical) of:
(i) $[CoCl_{2} (en)_{2}]^{+}$ (ii) $[Co(NH_{3})Cl(en)_{2}]^{2+}$ (iii) $[Co(NH_{3})_{2}Cl_{2} (en)]^{+}$

Discuss briefly giving an example in each case the role of coordination compounds in:
(i) biological systems (ii) medicinal chemistry and (iii) analytical chemistry (iv) extraction/metallurgy of metals.

(i) Biological systems
Several naturally occurring biologically important compounds are coordination compounds.
Thus, chlorophyll is a coordination compound containing Mg(II) ions. It is green pigment present in plants and is used in photosynthesis.
(ii) Medicinal chemistry
To remove metal poisoning, complexing agents are used, cis platin

$\displaystyle [PtCl_2(NH_3)_2]$ is used in cancer chemotherapy.
(iii) Analytical chemistry
Complex formation is used in qualitative scheme of analysis. In group I analysis, silver ion is separated from the precipitate of

$\displaystyle AgCl, Hg_2Cl_2$ and

$\displaystyle PbCl_2$ . Aqueous ammonia is added to the ppt. AgCl dissolves due to formation of soluble complex.

$\displaystyle AgCl + 2NH_3 \rightleftharpoons [Ag(NH_3)_2]Cl$
(iv) Extraction/metallurgy of metals
Metals such as gold and silver are extracted by complex formation technique. Cyanide process is used for extraction of silver and gold from its ore.

$\displaystyle Ag_2S + 4NaCN \rightarrow 2Na[Ag(CN)_2] + Na_2S$

$\displaystyle 2Na[Ag(CN)_2] + Zn \rightarrow Na_2[Zn(CN)_4] + 2Ag$

Draw figure to show the splitting of d orbitals in an octahedral crystal field.

The splitting of

$d-$ orbitals in an octahedral crystal field is as shown.

Amongst the following ions which one has the highest magnetic moment value?
(i) $[Cr(H_{2}O)_{6}]^{3+}$ (ii) $[Fe(H_{2}O)_{6}]^{2+}$ (iii) $[Zn(H_{2}O)_{6}]^{2+}$

(i)

$\displaystyle [Cr(H_2O)_6]^{3+} : 3d^3 :$ 3 unpaired electrons
(ii)

$\displaystyle [Fe(H_2O)_6]^{2+} : 3d^6 :$ 4 unpaired electrons. has maximum magnetic moment.
(iii)

$\displaystyle [Zn(H_2O)_6]^{2+} : 3d^{10} :$ 0 unpaired electrons and is diamagnetic.

(i) What are the postulates of Werner's theory?
(ii) Write the IUPAC names fo ${K}_{3}\left[Fe{\left(CN\right)}_{6}\right]$ , $\left[Co{\left(N{H}_{3}\right)}_{6}\right]{Cl}_{3}$ .

i) $\text{Postulates of Werner’s theory}$ :

Every metal atom has two types of valencies

i)Primary valency or ionisable valency

ii)Secondary valency or non ionisable valency

The primary valency corresponds to the oxidation state of the metal ion.The primary valency of the metal ion is always satisfied by negative ions.
Secondary valency corresponds to the coordination number of the metal ion or atom. The secondary valencies may be satisfied by either negative ions or neutral molecules.
The molecules or ion that satisfy secondary valencies are called ligands.
The ligands which satisfy secondary valencies must project in definite directions in space. So the secondary valencies are directional in nature whereas the primary valencies are non-directional in nature.
The ligands have unshared pair of electrons. These unshared pair of electrons are donated to central metal ion or atom in a compound. Such compounds are called coordination compounds.

(ii) ${K}_{3}\left[Fe{\left(CN\right)}_{6}\right]$ is Potassium hexacyanoferrate(III).

$\left[Co{\left(N{H}_{3}\right)}_{6}\right]{Cl}_{3}$ .is Hexamminecobalt (III) chloride.

Rules of hybridization say that hybrid orbitals form only sigma bonds. However, unsaturated hydrocarbons like (ethylene and acetylene) possess multiple bonds between carbons.

Rules of hybridization say that hybrid orbitals from only sigma bonds. This statement is true but ethylene and acetylene form multiple bonds.

In the case of ethylene, it shows

$sp^2$ hybridization. Thus, only two p-orbital takes part in hybridization and form a sigma bond.

The one unhybridized p-orbital lie perpendicular to

$sp^2$ hybrid orbital and form a double bond with unhybridized p-orbital of other carbon atoms by lateral sharing of electrons.

Similarly, in acetylene, two p-orbitals remain unhybridized and form two

$\pi$ bonds with each other.

Write the formula of the following coordination compound.
Iron(III) hexacyanoferrate(II).

The formula of the complex anion hexacyanoferrate(II) is

$[Fe(CN)_6]^{-4}$ . The oxidation number of iron is

$+2$ and each cyanide ion has

$-1$ charge. Hence, the net charge on the complex anion is

$+2+6(-1)=-4$ .
-4 charge on complex anion will be balanced by +3 charge on

$Fe^{3+}$ cation when 4

$Fe^{3+}$ cations combine with 3

$[Fe(CN)_6]^{-4}$ complex anions.
The formula of the coordination compound Iron(III) hexacyanoferrate(II) is

$Fe_4([Fe(CN)_6])_3$
Note: In the name Iron(III) hexacyanoferrate(II), the numbers in parenthesis in roman numerals indicates the oxidation number of iron atoms.

Define linkage and ionisation isomerism?

Linkage isomerism.
The same ligand is bonded to central metal atom or ion through different atoms. The molecular formula of linkage isomers is same but they differ in linkage of the ligand to central metal atom. Yellow coloured

$\displaystyle [Co(NH_3)_5NO_2]Cl_2$ and red coloured

$\displaystyle [Co(NH_3)_5ONO]Cl_2$ are linkage isomers.

Ionisation isomerism (ion-ion exchange isomerism).
There is exchange of ions inside and outside the coordination sphere. The molecular formula of ionisation isomers is same but different ions are produced in solution.

$\displaystyle [Co(NH_3)_5SO_4]Br$ and

$\displaystyle [Co(NH_3)_5Br]SO_4$ are ionisation isomers.

$Co.{ Cl }_{ 3 }.5{ NH }_{ 3 }{ H }_{ 2 }O$ is a pink solid, the solution of this salt is also pink and formed $3$ mol of $AgCl$ with silver nitrate solution. On heating pink solid, it loses one water molecule and forms purple solid having same ratio of $Co:{ NH }_{ 3 }:Cl$ as that of pink solid. The purple solid when dissolved in water and treated with silver nitrate forms $1$ mol of $AgCl$ . Draw the structures and name of the pink and purple solids.

The given pink solid is $[Co(NH_3)_5(H_2O)]Cl_3$ . The name of this complex is Pentaamineaquacobalt (III) Chloride. The purple solid is $[Co(NH_3)_5]Cl_3$ . The name of this complex is Pentaaminechlorocobalt (III) Chloride.Since the first complex, as given forms $3$ moles of $AgCl$ with $AgNO_3$ so it must have $3$ ionizable $Cl^-$ ions and in second complex there are $2$ ionizable $Cl^-$ ions.

1001464_819312_ans_5c903c7053c6411a87703e07e6b0e7b7.PNG

Match each coordination compound in List-I with an appropriate of characteristics from List-II. ( $en={ H }_{ 2 }HC{ H }_{ 2 }C{ H }_{ 2 }N{ H }_{ 2 }$ ; Atomic numbers: Ti = 22, Cr = 24; Co = 27; Pt = 78)
List I List II
A $\left[ Cr{ \left( { NH }_{ 3 } \right) }_{ 4 }{ Cl }_{ 2 } \right] Cl$ 1 Paramagnetic and exhibits ionization isomerism
B $\left[ Ti{ \left( { H }_{ 2 }O \right) }_{ 3 }Cl \right] { \left( { NO }_{ 3 } \right) }_{ 2 }$ 2 Diamagnetic and exhibits cis-trans isomerism
C $\left[ Pt\left( en \right) { \left( N{ H }_{ 3 } \right) }Cl \right] { NO }_{ 3 }$ 3 Paramagnetic and exhibits cis-trans isomerism
D $\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 4 }{ \left( { NO }_{ 3 } \right) }_{ 2 } \right] { NO }_{ 3 }$ 4 Diamagnetic and exhibits ionization isomerism

REF.Image

$A\rightarrow Cr^{+3}\Rightarrow x=2=+1\Rightarrow \boxed {x=3}$

$B\rightarrow Ti^{+3}\Rightarrow x-1=2\Rightarrow \boxed {x=3}$

$C\rightarrow Pt^{+4}\Rightarrow x-2-1=1\Rightarrow \boxed {x=4}$

$d\rightarrow Co^{+3}\Rightarrow x-2=1 \Rightarrow \boxed {x=3}$

$A\rightarrow 2$

$B\rightarrow 1$

$C\rightarrow 1$

$D\rightarrow 2$

$H_{2}O$ is weak ligand.

1442137_881326_ans_b7597757826046d49d44f271359b182d.png

What is meant by complex compound? Describe the main points of Werner's theory.

Coordination compound, any of a class of substances with chemical structures in which a central metal atom is surrounded by nonmetal atoms or groups of atoms, called ligands, joined to it by chemical bonds.

Werner theory describes the structure and formation of complex compounds or coordination compounds.

Main points of Werner’s Theory:

1.The central metal or the metal atoms in coordination compounds show two types of valency. They are the primary and the secondary valency.

2. The primary valency relates to the oxidation state and the secondary valency relates to the coordinate number.

3. The number of secondary valences is fixed for every metal atom. It means that the coordination number is fixed.

4. The metal atom works towards satisfying both its primary and secondary valencies. A negative ion satisfies the primary valency. On the other hand, a negative ion or neutral molecules satisfy secondary valencies.

5. The secondary valencies point towards a fixed position in space thus have definite geometry of the compound thus its directional.

On the basis of the following observations made with aqueous solutions, assign secondary valences to metals in the following compounds:
Formula Moles of $AgCl$ precipitated per mole of the compounds with excess $AgNO_3$
(i) $PdCl_2.4NH_3$ $2$
(ii) $NiCl_2.6H_2O$ $2$
(iii) $PtCl_4.2HCl$ $0$
(iv) $CoCl_3.4NH_3$ $1$
(v) $PtCl_2.2NH_3$ $0$

Moles of

$AgCl$ precipitated per mole of the compound is equal to the primary valences of the metal.

So,

(i)

$PdCl_2.4NH_3$ with

$2$ moles of

$AgCl$ precipitated means secondary valence of

$Pd$ is

$4\Rightarrow [Pd(NH_3)_4]Cl_2$

(ii)

$NiCl_2.6H_2O$ with

$2$ moles of

$AgCl$ precipitated means secondary valence of

$Ni$ is

$6\Rightarrow [Ni(H_2O)_6]Cl_2$

(iii)

$PtCl_4.2HCl$ with

$0$ moles of

$AgCl$ precipitated means secondary valence of

$Pt$ is

$6\Rightarrow [PtCl_4(HCl)_2]$

(iv)

$CoCl_3.4NH_3$ precipitates

$1$ mole of

$AgCl$ . So, secondary valence of

$Co$ is

$6\Rightarrow [Co(NH_3)_4Cl_2]Cl$

(v)

$PtCl_2.2NH_3$ precipitates

$0$ mole of

$AgCl$ . So, secondary valence of

$Pt$ is

$4\Rightarrow [PtCl_2(NH_3)_2]$

Which of the following is ore stable and why? ${ \left[ Co{ \left( { NH }_{ 3 } \right) }_{ 3 } \right] }^{ 3+ }$ and ${ \left[ Co{ \left( en \right) }_{ 3 } \right] }^{ 3+ }$ . Name the following coordination compound and draw its possible structures $\left[ { Co }Cl_{ 2 }{ \left( en \right) }_{ 2 } \right] Cl$

${ \left[ Co{ \left( en \right) }_{ 3 } \right] }^{ 3+ }$ is more stable than

${ \left[ { Co\left( { NH }_{ 3 } \right) }_{ 6 } \right] }^{ 3+ }$

Because in complex compounds, the complex compound which has more chelation is stable than a compound which has chelation. Polydentate ligands and bidentate ligands have more chelation than monodentate ligand. Hence,

${ \left[ { Co\left( en \right) }_{ 3 } \right] }^{ 3+ }$ which has a bidentate ligand is more stable than

${ \left[ Co{ \left( { NH }_{ 3 } \right) }_{ 6 } \right] }^{ 3+ }$ which has a monodentate ligand.

Chelation :- It is a type of bond in complex compounds where there is a formation of two or more separate co-ordinate bonds between a polydentate ligand and metal atom.

$\left[ { { CoCl } }_{ 2 }{ \left( en \right) }_{ 2 } \right] Cl$ is known as Dichloro bis(ethylenediamine) cobalt (III) chloride structure of

$\left[ { { CoCl } }_{ 2 }{ \left( en \right) }_{ 2 } \right] Cl$ .

980732_1078071_ans_e7b7e248920d41dfbff680b95447f8e6.jpg

What is Werner's Theory

The important postulates of Werner's theory is :

1. The metal atom shows two types of valency a) primary valency and b) secondary valency.

2. The primary valency relates to the oxidation state and the secondary valency relates to the coordination number of the central metal atom

3. Secondary valency is fixed for the metal.

4. The metal atom works to satisfy both its valency.

What is the change in colour of potassium dichromate when aq. KOH is added in it .

Orange colour changes to yellow

$C{r_2}{O_7}^{2 - } + 2O{H^ - } \to 2Cr{o_4}^{2 - } + {H_2}O$

Orange Yellow

Explain, on the basis of crystal filed splitting in case of $[Ni(H_{2}O)_{6}]^{2+}, [Ni(H_{2}O)_{4}en]^{2+}$ and $[Ni(H_{2}O)_{2}(en)_{2}]^{2+}$ ions.

1337787_1317561_ans_66541031248f423f9907a0dd1a146791.jpg

Co-ordinates complexes involving $F^-$ ions are more stable than those having $CI^-$ & $Br^-$ ions?

1337876_1311599_ans_67d280c2d5d24b40b5da8f7fa6e430df.jpg

What is the hydrate isomerism? Explain with in example?

Solvate isomers or hydrate isomerism are the isomers which have the same composition but differ with reference to the number of solvent ligand molecules as well as the counter ion in the crystal lattice.

For example $[Cr(H_2O)_6]Cl_3$ is violet colored, $[CrCl(H_2O)_5]Cl_2H_2O$ is blue-green, and $[CrCl_2(H_2O)_4]Cl_2H_2O$ is dark green.

Total number of cis $N-Mn-Cl$ bond angles (that is, $Mn-N$ and $Mn-Cl$ bonds in cis position) present in a molecule of cis $[Mn(en)_2Cl_2]$ complex is ______.
$(en=NH_2CH_2CH_2NH_2)$

There are 6

$N-Mn-Cl$ bonds present in

$]Mn(en)_2Cl_2]$ .
1307444_1633386_ans_33fc4a2b23644b6db416d1c46963d4b3.png

Show by means of a diagram how the pattern of d orbital splitting changes as an octahedral complex undergoes tetragonal distortion and eventually becomes a square planar complex.

1555421_1713342_ans_7cb1285814404b6f8d869a282a934f84.jpg

Given that the maximum absorption in the d-d peak for $[ Ti(H_2O)_6]^{3+}$ occurs at $20300cm^{-1}$ predict where the peaks will occurs for $[Ti(CN)_6]^{3-}$ and $[Ti(Cl)_6]^{3-}$

1555427_1713350_ans_82c1ef3a44bf441d8bb24d1dec7ea327.jpg

Write the formula for each of the following complexes :
(a) tetraamminecopper (II) sulphate
(b) potassium tetracyanonickelate (0)
(c) bis (cyclopentadiehyl)iron(II)
(d) tetrathicyanato -N-zinc (II)
(e) diamminebis (ethylenediamine) cobalt (III) chloride
(f) tetraammineddithiocyanatochromium (III)
(g) potassium tetraoxomanganate (VII)
(h) potassium terioxalatoalumminate (III)
(i) tetrapyridineplatinum (II) tetrachloroplatinate (II)

The sum of primary and secondary valencies of chromium in the complex $CrCl_3\cdot 6NH_3$ is?

Primary valency = oxidation state

secondary valency = Number of molecule co-ordinate to central atom

In the molecule

$CrCl_{3}.6NH_{3}$

Cr is +3 state . Hence Primary valency = 3

six(6)

$NH_{3}$ is co-ordinate with central atom. Hence , secondary valency = 6

Sum = 3 + 6 = 9

Hence , correct answer is 9 .

Find the total number of possible isomers of $[CrCl_3(NH_3)_3]$ .

1970626_1722779_ans_3d71291405134463b7d5079c2c1867bb.jpg

Find the number of isomeric forms in which $[Co(NH_3)_4Cl_2]^+$ ion can occur.

Two isomeric forms cis and trans are possible for

$[Co(NH_{3})Cl_{2}]^{+}$ .

Hence , correct answer is 2.

Find the total number of possible isomers of $[CrCl_2(CN)(NH_3)en]$ .

1979911_1725246_ans_bf580ee4497b4bd7a3e0a616f4f61896.jpg

The number of total possible stereoisomers for $[Pd(NH_2-CH(CH_3)-CO^-_2)_2]$ is?

1970633_1725763_ans_0e2b095d22da434fa0b55ee2f1314578.jpg

Find the total number of possible isomers of $[ZnCl_2F_2]^{2-}$ .

1970634_1725765_ans_262d583ad88d480c8a21f63828afcf5f.jpg

Write the sum of geometrical isomer in $[Ma_2b_2c_2]$ complex and stereoisomers in $[M(AB)_3]$ complex.

1970629_1725312_ans_b50b78098a984048a583ec499ed0874c.jpg

Find the total number of isomer of $[Be(gly)_2]$ .

1970632_1725755_ans_bf70aee4ca1b4d5da61030950ca9faa1.jpg

How many maximum atom(s) is/are present in same of plane of $Cr(CO)_6?$

1900887_1725770_ans_4038cfdb1c3a4b6dae5bccc1d0754831.jpeg

Match the column:

a) REF. IMAGE 1

i) Bent structure

ii)

$sp^3$ hybridization

iii) planar

iv)

$\mu \neq 0$ , polar

b) REF. IMAGE 2

i) Tetrahedral structure

ii) Nonplanar

iii)

$sp^3$ - hybridization

iv)

$\mu \neq 0$

v) Nonpolar

c) REF. IMAGE 3

$sp^3 d$ hybridization

ii)

$dz^2$ is involved in hybridization

iii) Linear, planar

iv)

$\mu \neq 0$ , Nonpolar

d) REF. IMAGE 4

$sp^3 d^2$ - hybridization

ii)

$d_{x^2-y^2}, d_{z^2}$ orbitals are involved in hybridization

iii) Nonplanar

iv)

$\mu \neq 0$ nonpolar

e) REF. IMAGE 5

$sp^3$ hybridization

ii) Bent structure

iii) planar

iv)

$\mu \neq 0$ , polar

1549402_1726369_ans_d7e7ad865d8d422d81dc73ef779e1e1c.JPG

A coordination compound $CrCl_3\cdot 4H_2O$ precipitates silver chloride when treated with silver nitrate. The molar conductance of its solution corresponds to a total of two ions. Write structural formula of the compound and name it.

Since precipitates of silver chloride when treated with silver nitrate so there is chloride ion outside the complex. Since only two ions are formed so there is only 1 chloride ion outside the complex. So, structural formula of the compound and name is :

$[Co(H_2O)_4Cl_2]Cl$ and Tetraaquadichloridocobalt(III) chloride.

Arrange the following complexes in the increasing order of conductivity of their solution:
$[Co(NH_3)_3Cl_3],\ [Co(NH_3)_4Cl_2]Cl, \ [Co(NH_3)_6]Cl_3,\ [Cr(NH_3)_5Cl]Cl_2$ .

Complex which give more ions on dissolution is more conducting.

$[Co(NH_3)_6]Cl_3 > [Cr(NH_3)_5Cl]Cl_2 > [Co(NH_3)_4Cl_2]Cl > [Co(NH_3)_3Cl_3]$

$CoSO_4Cl_5NH_3$ exists in two isomeric forms 'A' and 'B'. Isomer 'A' reacts with $AgNO_3$ to give white precipitate, but does not react with $BaCl_2$ . Isomer 'B' gives white precipitate with $BaCl_2$ but does not react with $AgNO_3$ . Answer the following question.
Identify 'A' and 'B' and write their structural formulas.

1980268_1727105_ans_37c8e1e02c044a21b98d3359e16ba20b.jpg

$AgCl$ dissolves in excess of $KCN$ solution to give the ________ complex compound.

$AgCl$ dissolves in excess of

$KCN$ solution to give the

$K[Ag(NH)_2]$ complex compound.

$AgCl+2KCN\rightarrow K[Ag(CN)_2]+KCl$ .

$S^{2-}+Na_2[Fe(CN)_5NO]\rightarrow$ Complex is having violet/purple coloration (X).
The total number of possible isomers for complex X is.....provided the ambient behaviour of $CN^{-}$ is not considered.

1902276_1728774_ans_3fb952470be84c84b99e402df0075887.jpg

What type of isomers are the following ?
$[(CO)_5MnSCN]$ and $[(CO)_5MnNCS]$

Linkage isomerism occurs with ambidentate ligands that are capable of coordinating in more than one way.
The best known cases involve the monodentate ligands:

$SCN^-$

$/$

$NCS^-$ and

$NO_2^-$

$/$

$ONO^-$ . The only difference is what atoms, the molecular ligands use to attach to the central ion. The ligand(s) must have more than one donor atom, but bind to ion in only one place. So these are linkage isomers.

What type of isomers are the following ?
$[Co(en)_3][Cr(CN)_6]$ and $[Cr(en)_3][Co(CN)_6]$

1669413_1729805_ans_2197bfa8364d43dd8ad4005f411e6546.jpg

Describe a simple chemical test that would allow you to distinguish between the compounds, $[Co(NH_3)_5Br]SO_4$ and $[Co(NH_3)_5SO_4]Br$ .

$[Co(NH_3)_5Br] SO_4$ is red-violet. An aqueous solution gives a white precipitate of

$BaSO_4$ and

$BaCl_2$ solution. In contrast

$[Co(NH_3)_5SO_4] Br$ is red. A solution of this complex does not give a positive sulphate test with

$BaCl_2$ .

What type of isomers are the following ?
$[Co(NH_3)_5NO_3]SO_4$ and $[Co(NH_3)_5SO_4]NO_3$

The isomers which form different ions in solution, although, they have same the composition, are called ionization isomers. In the former, the nitrate ion is coordinated to the

$Co^{3+}$ ion and the sulfate ion is outside the coordination sphere; in the latter the sulfate ion occurs within the coordination sphere, and the nitrate ion is outside it. Hence it is ionization isomers.

Explain the geometry and magnetic nature of the following complex ion on the basis of valence band theory: $[MnCl_4]^{2-}$

2039910_1729822_ans_8afac39295ae483aaa4358534a952266.jpg

What are the main features of the ligand field theory?

The Ligand field theory (LFT) describes the bonding, orbital arrangement, and other characteristics of coordination complexes. It represents an application of molecular orbital theory to transition metal complexes. A transition metal ion has nine valence atomic orbitals: five nd, one (n+1)s, and three (n+1)p orbitals.

How many different structures are possible for each of the following complex ions ?
$[Co (NH_3)_4(H_2O)_2]^{3+}$

1736980_1731685_ans_30c35e632fad4eb89e2692444185f277.png

How many different structures are possible for each of the following complex ions ?
$[Co (NH_3)_3(H_2O)_3]^{3+}$

1736981_1731686_ans_fee121c0bfa245e49884549f75c67c69.png

How many different structures are possible for each of the following complex ions ?
$[Co(NH_3)_5H_2O]^{3+}$

1962278_1731683_ans_031aa144ca9d48a88bc403403a807416.jpg

Describe at least three applications of coordination compounds.

Three applications of coordination compounds:

1. Zinc-complex enzymes like carbonic anhydrase important to buffering reactions in blood.

2. Copper-complex enzymes important to iron storage and producing pigments in hair, skin, and eyes.

3. Nickel-complex enzymes as part of the enzymes urease and hydrogenase.

How many different structures are possible for each of the following complex ions ?
$[Co(NH_3)_2(H_2O)_4]^{3+}$

1737008_1731687_ans_1e568eb2c5c443a78ae919d8cda7f5fe.png

How many maximum atoms lie in the same plane in the structure of methylenesuphurtetrafluoride $(CH_{2}SF_{4})$ ?

$\text{Structure of }CH_2SF_4\text{ bond involving a p-orbital of carbon atom must lie in the equatorial plane of}$

$\text{the molecule.}$

$Six\text{ atoms i.e., 2H atoms, C, S.and both equatorial F-atoms lie in one plane.}$
1865066_1746514_ans_b2913631a3f748db9df2c2e257a003cb.png

How many isomers of the complex, $[Pt \left ( NH_{3} \right )_{2}\left ( SCN \right )_{2}]$ are possible ?

Answer:

The complex

$[Pt(NH_3)_2(SCN)_2]$ forms two stereoisomers,

Since

$SCN$ is ambidentate ligand

$2$ or more donor atoms are present they joined to the central metal atom as

$-NCS$ of

$-SCN$ both will form cis and trans isomers so total

$4$ isomers are possible from this complex.

How many geometrical isomers are possible for each of the following complexes? Draw the structure of each isomer: Pt(NH3)2(SCN)2

What are the products and type of isomers when $Br_2$ adds to:

The products are as shown in the figure:

cis-Compound + trans-Addition of

$Br_2 \rightarrow (\pm)$ Product.

1672069_1768439_ans_d8e2b2bc3a064c1991ff81194df1e395.png

Define hybridisation.

Hybridisation is a concept of mixing atomic orbitals into new hybrid orbitals which are generally of lower energy and suitable for the pairing of electrons to form chemical bonds in valence bond theory.

Hybridization helps to predict the shape and geometry of molecule and way bonding happens in that.

What are the postulates of Werner's theory of coordination compounds?

Werner propounded his theory of coordination compounds. The main postulates are:

1) In coordination compounds metals show two types of valences primary and secondary.

2) The primary valences are normally ionisable and are satisfied by negative ions.

3) The secondary valences are non-ionisable. They are satisfied by neutral molecules or negative ions. The secondary valence is equal to the coordination number and is fixed for a metal.

4) The ions/groups bound by the secondary linkages to the metal have characteristic spatial arrangements corresponding to different coordination numbers.

Give two examples of complex compounds.

Examples of complex compounds are chlorophyll, hemoglobin, cyanocobalamine.

Name the main metal present in the following:
(a) Haemoglobin
(b) Chalk
(c) Chlorophyll
(d) Chocolate wrappers

The main metal present are:

(a) Iron

(b) Calcium
(c) Magnesium
(d) Aluminium

Draw the mirror image of $[CO(en)_2Cl_2]^+$

The mirror image of

$[CO(en)_2Cl_2]^+$ exhibits geometrical isomerism.
1744895_1831332_ans_a6aabe2d512943e2947f9be4c55208f7.png

What is $CFSE$ of complex ion $[FeF_{6}]^{4-}$ in terms of $\Delta _O$ ?

1771214_1819219_ans_e5cd6098e9a046dcb8c25436159a07a3.jpg

Explain the importance of coordination compounds in extraction of metals.

$KCN$ is used to extract silver from

$Ag_2S$ in the form of cynide complex and then reducing it with zinc as show by the following equations :

$4KCN + Ag_2S \rightarrow 2K[Ag(CN)_2] + K_2S$

$2K[Ag(CN)_2] + Zn \rightarrow K_2[Zn(CN)_4] + 2Ag$

	List I		List II
A	$\left[ Cr{ \left( { NH }_{ 3 } \right) }_{ 4 }{ Cl }_{ 2 } \right] Cl$	1	Paramagnetic and exhibits ionization isomerism
B	$\left[ Ti{ \left( { H }_{ 2 }O \right) }_{ 3 }Cl \right] { \left( { NO }_{ 3 } \right) }_{ 2 }$	2	Diamagnetic and exhibits cis-trans isomerism
C	$\left[ Pt\left( en \right) { \left( N{ H }_{ 3 } \right) }Cl \right] { NO }_{ 3 }$	3	Paramagnetic and exhibits cis-trans isomerism
D	$\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 4 }{ \left( { NO }_{ 3 } \right) }_{ 2 } \right] { NO }_{ 3 }$	4	Diamagnetic and exhibits ionization isomerism

Formula	Moles of $AgCl$ precipitated per mole of the compounds with excess $AgNO_3$
(i) $PdCl_2.4NH_3$	$2$
(ii) $NiCl_2.6H_2O$	$2$
(iii) $PtCl_4.2HCl$	$0$
(iv) $CoCl_3.4NH_3$	$1$
(v) $PtCl_2.2NH_3$	$0$

Coordination Compounds - Class 12 Engineering Chemistry - Extra Questions

Match each coordination compound in List-I with an appropriate pair of characteristics from List-II. (en=H2HCH2CH2NH2en = H_2HCH_2CH_2NH_2; Atomic numbers: Ti=22,Cr=24;Co=27;Pt=78Ti =22, Cr=24; Co=27; Pt = 78)

Blue-green is the complimentary color of red spectral color.If true enter 1, else enter 0.

Orange is the complimentary colour of blue spectral colour.If true 1 else 0.

Name the series of lines in the hydrogen spectrum which lies in the ultra-violet region :

Haemoglobin is a complex of Fe(II)Fe(II) bound to porphyrin rings.If true enter 1, else enter 0.

Discuss briefly giving an example in each case the role of coordination compound in biological system.

What type of isomerism is exhibited the complex [Co(NH3)5Cl]SO4[Co(NH_3)_5Cl]SO_4?

Identify the type of Isomerism existing in between the following compounds. [Co(NH3)sNO2]\left[ {Co\left( {N{H_3}} \right)s\,N{O_2}} \right] and [Co(NH3)sONO2]Cl2\left[ {Co\left( {N{H_3}} \right)s\,ON{O_2}} \right]C{l_2}

How many isomeric forms are possible for the octahedral complex, [Rh(en)2(NO2)(SCN)]+[Rh(en)_{2}(NO_{2})(SCN)]^{+}?

What is the use of coordination compounds for purification of water Medical and catalyst

Indicate the types of isomerism exhibited by the following complex and draw the structure of this isomer.[Co(NH3)5(NO2)](NO3)2[Co(NH_3)_5(NO_2)](NO_3)_2

How are the hybrid orbitals arranged in the molecules?

Match the given pairs.

The primary valency of a central metal ion in a complex is satisfied with _______ .

According to Werner's coordination theory, there are _______ kinds of valency - _____ and ______.

Match column-I with column-II

In [Fe(H2O)6]Cl3[Fe(H_2O)_6]Cl_3, six H2OH_2O are joined by primary valency (PV) and three ClCl are joined by secondary valency (SV).If true enter 1, else enter 0.

Match column-I with column

Vitamin B12B_{12} is a complex of cobalt. If true enter 1, else enter 0.

Match the following.

What is hybridisation?

For the complex [NiCl4]2−[NiCl_{4}]^{2-}, write(i) the IUPAC name (ii) the hybridization type (iii) the shape of the complex.(Atomic no. of Ni=28Ni = 28)

Name the following coordination entities and draw the structures of their steroisomers:(i) [Co(en)2Cl2]+(en=ethane−1,2−diamine)[Co(en)_2Cl_2]^+ (en=ethane - 1, 2-diamine)(ii) [Cr(C2O4)3]3−[Cr(C_2O_4)_3]^{3-}(iii) [Co(NH3)3Cl3][Co(NH_3)_3Cl_3](Atomic number Cr=24,Co=27Cr=24, Co=27)

Write the IUPAC names of the following coordination compounds:(i)[Cr(NH3)3Cl3][Cr(NH_3)_3Cl_3](ii)K3[Fe(CN)6]K_3[Fe(CN)_6](iii)[CoBr2(en)2]+[CoBr_2(en)_2]^{+}, (en = ethylenediamine)

Write the name, the structure and the magnetic behavior of each one of the following complexes:(i) [Pt(NH3)Cl(NO2)][Pt (NH_3) Cl (NO_2)](ii) [Co(NH3)4Cl2]Cl[Co(NH_3)_4Cl_2] Cl(iii) Ni(CO)4Ni (CO)_4(At. Nos. Co=27,Ni=28,Pt=78Co = 27, Ni = 28, Pt = 78)

Write the types of isomerism exhibited by the following complexes.(i) [Co(NH3)5Cl]SO4[Co(NH_{3})_{5}Cl]SO_{4}(ii) [Co(en)3]3+[Co(en)_{3}]^{3+}(iii) [Co(NH3)6][Cr(CN)6][Co(NH_{3})_{6}] [Cr(CN)_{6}]

The electron pairs involved in hybridisation and not involved in bonding are called ___________.

Name the types of isomerism shown by the following pairs of compounds:(i) [CoCl(H2O)(NH3)4Cl2][CoCl(H_2O)(NH_3)_4Cl_2] and [CoCl2(NH3)4]Cl⋅H2O[CoCl_2(NH_3)_4]Cl\cdot H_2O(ii) [Pt(NH3)4][PtCl6][Pt(NH_3)_4][PtCl_6] and [Pt(NH3)4Cl2][PtCl4][Pt(NH_3)_4Cl_2][PtCl_4]

How does K2[PtCl4]{ K }_{ 2 }\left[ Pt{ Cl }_{ 4 } \right] get ionized when dissolved in water? Will it form precipitate when AgNO3 AgN{ O }_{ 3 } solution is added to it? Give a reason for your answer.

What are the dark lines seen in the solar spectrum called?

Illustrate with example, the difference between a double salt and coordination compound.

Explain co-ordination and ionisation isomeristmes with a suitable example for each.

Explain the difference between a double-salt and a complex, giving an example in each case.

Explain the applications of coordination compounds in the field of metal purification giving an example :

Explain coordination and ionisation isomerism with example.

Write a note on Haemoglobin.

Classify the following into homoleptic & heteroleptic complexes?i) K4[Fe(CN)6]K_4[Fe(CN)_6]ii) [Co(NH3)5(CO3)]Cl[Co(NH_3)_5(CO_3)]Cliii) K2[Zn(OH)4]K_2[Zn(OH)_4]iv) [Pt(NH3)2Cl(NO2)][Pt(NH_3)_2Cl(NO_2)]

Explain the violet colour of [Ti(H2O)6]3+[Ti(H_2O)_6]^{3+} complex on basis of the crystal field theory?

Explain Werner's theory of coordinate compounds with suitable examples?

(a) Give the postulates of Werner's theory of co-ordination compounds.(b) Differentiate between chemical reactions and nuclear reactions.

Explain Werner's theory of co-ordination compounds?

Write the IUPAC name of following compounds :(A) K3[Fe(CN)6K_3[Fe(CN)_6(B) [Co(NH3)6]Cl3[Co(NH_3)_6]Cl_3

Draw Werner's structure of the following:(a) CoCl3.6NH3CoCl_{3} . 6NH_{3}(b) CoCl3.5NH3CoCl_{3} . 5NH_{3}(c) CoCl3.4NH3CoCl_{3} . 4NH_{3}(d) CoCl3.3NH3CoCl_{3} . 3NH_{3}

Write any two postulates of Werner's theory of coordination compounds.

What is Zeise's Salt and Ferrocene? Explain with structure?

How do 'd' orbitals split in an octahedral crystal field?

What types of isomer are [Co(NH3)5Br]SO4[Co(NH_3)_5 Br] SO_4 and [Co(NH3)5SO4]Br[Co(NH_3)_5 SO_4] Br?

Number of Cl−Cl^{-} ions satisifying both primary and secondary valency are in CoCl35NH3CoCl_{3}5NH_{3}.

Define primary and secondary valency of metal ions proposed by werner theory?

For the complex ion [Fe(CN)6]3−[Fe(CN)_6]^{3-}, state:(i) the type of hybridisation.(ii) the magnetic behaviour.(iii) the oxidation number of the central metal atom.

Write primary and secondary valency of CoCo in [Co(Nn3)6]Cl3[Co(Nn_{3})_{6}]Cl_{3}?

Predict whether the following molecules are isostructural or not. Justify your answer(i) NMe3N{Me}_{3} (ii) N(SiMe3)3N{(Si{Me}_{3})}_{3}

Explain hybridisation, geometry and magnetic property of [Ni(CN)4]2−[Ni(CN)_4]^{2-} ion using Valence Bond Theory(VBT). [Atomic number of Ni is 2828].

Chlorophyll contains 2.68% of MgMg by weight. Then the number of MgMg atom in 2.00 g of chlorophyll is:(Atomic mass of Mg=24Mg = 24)

Give two examples of Complex compound.

Define Hybridization.

Write formula of the following compound:(i) dichloridobis (ethylene diamine) cobalt (III) ion.(ii) sodiumethylenediaminetetraacetatonickelate (II)(iii) hexaammineplatinum (IV) chloride

What is coordination compound ?

What is crystal field splitting energy? Draw a figure to show spitting of degenerate orbitals in an octahedral crystal field?

What is the Primary and Secondary Valence of PtCl2.2NH3PtCl_{2}.2NH_{3}?

Indicate the types of isomerism exhibited by the following complex and draw the structure of this isomer.[Pt(NH3)(H2O)Cl2][Pt(NH_3)(H_2O)Cl_2]

What is the major product in this reaction.

What is the hybridization of central atom in following? PH3,PH+4,PH_3, PH_{4}^+,

On the basis of Werner's theory explain, why cobalt amine complex, CoCl_{ 3 }{ 4NH }_{ 3 }CoCl_{ 3 }{ 4NH }_{ 3 } when treated with { Ag }{ NO }_{ 3 }{ Ag }{ NO }_{ 3 } solution precipitates only one { Cl }^{ - }{ Cl }^{ - } ion even though there are three { Cl }^{ - }{ Cl }^{ - } ions?

What is EAN? Write it's formula.

Explain the bonding on CoCl_{ 2 }.3N{ H }_{ 3 }CoCl_{ 2 }.3N{ H }_{ 3 } and CoCl_{ 2 }.5N{ H }_{ 3 }CoCl_{ 2 }.5N{ H }_{ 3 } structure on the basis at Werner's theory.

If the value of C.F.S.E. for ''Ni" is \triangle _{ o }\triangle _{ o } then what is the CFSE value Pd?

What is IUPAC name of K_{3}\left [ Fe\left ( CN \right )_{5}NO \right ]K_{3}\left [ Fe\left ( CN \right )_{5}NO \right ]?

Write the formula of the following complexes.Bis (ethnylene diammine) dichloro iridium (III) ion

Write the formula of the following complexes.Tris (ethylene diammine) cobalt (II) sulphate

What is coordinate bond?

Discuss briefly giving an example in each case the role of coordination compound medicinal chemistry.

Write the possible stereo isomers of the following complexes and identify the type :- a) [co(NH_3)_3Cl_3][co(NH_3)_3Cl_3]b) [pt(gly)_2][pt(gly)_2]c) [cr (en)_3][cr (en)_3]

Draw the isomer of [Pt({ { NH }_{ 3 } })_{ 3 }{ Cl }_{ 3 }][Pt({ { NH }_{ 3 } })_{ 3 }{ Cl }_{ 3 }], [Co({ { NH }_{ 3 } })_{ 5 }{ Cl }{ SO }_{ 4 }][Co({ { NH }_{ 3 } })_{ 5 }{ Cl }{ SO }_{ 4 }] .

What is the nomenclature of \left[ { CoCl }_{ 2 }({ NH }_{ 3 })_{ 4 } \right] ^{ + }\left[ { CoCl }_{ 2 }({ NH }_{ 3 })_{ 4 } \right] ^{ + } ?

What is the primary valency of [Co (NH_3)_4 Cl_2] Cl_2[Co (NH_3)_4 Cl_2] Cl_2 ?

what is the formula of potassium amminetrichlorido platinate(ii)

Differentiate between primary and secondary valencies?

write down the formulae of given compoundtetra amine zinc(II) nitrate

Match each coordination compound in List-I with an appropriate pair of characteristics from List-II. ( $en = H_2HCH_2CH_2NH_2$ ; Atomic numbers: $Ti =22, Cr=24; Co=27; Pt = 78$ )

Blue-green is the complimentary color of red spectral color.
If true enter 1, else enter 0.

Orange is the complimentary colour of blue spectral colour.
If true 1 else 0.

Haemoglobin is a complex of $Fe(II)$ bound to porphyrin rings.
If true enter 1, else enter 0.

What type of isomerism is exhibited the complex $[Co(NH_3)_5Cl]SO_4$ ?

Identify the type of Isomerism existing in between the following compounds.
$\left[ {Co\left( {N{H_3}} \right)s\,N{O_2}} \right]$ and $\left[ {Co\left( {N{H_3}} \right)s\,ON{O_2}} \right]C{l_2}$

How many isomeric forms are possible for the octahedral complex, $[Rh(en)_{2}(NO_{2})(SCN)]^{+}$ ?

Indicate the types of isomerism exhibited by the following complex and draw the structure of this isomer.
$[Co(NH_3)_5(NO_2)](NO_3)_2$

According to Werner's coordination theory, there are _____ kinds of valency - _ and ____.

In $[Fe(H_2O)_6]Cl_3$ , six $H_2O$ are joined by primary valency (PV) and three $Cl$ are joined by secondary valency (SV).
If true enter 1, else enter 0.

Vitamin $B_{12}$ is a complex of cobalt. If true enter 1, else enter 0.

For the complex $[NiCl_{4}]^{2-}$ , write
(i) the IUPAC name (ii) the hybridization type (iii) the shape of the complex.
(Atomic no. of $Ni = 28$ )

Name the following coordination entities and draw the structures of their steroisomers:
(i) $[Co(en)_2Cl_2]^+ (en=ethane - 1, 2-diamine)$
(ii) $[Cr(C_2O_4)_3]^{3-}$
(iii) $[Co(NH_3)_3Cl_3]$
(Atomic number $Cr=24, Co=27$ )

Write the IUPAC names of the following coordination compounds:
(i) $[Cr(NH_3)_3Cl_3]$
(ii) $K_3[Fe(CN)_6]$
(iii) $[CoBr_2(en)_2]^{+}$ , (en = ethylenediamine)

Write the name, the structure and the magnetic behavior of each one of the following complexes:
(i) $[Pt (NH_3) Cl (NO_2)]$
(ii) $[Co(NH_3)_4Cl_2] Cl$
(iii) $Ni (CO)_4$
(At. Nos. $Co = 27, Ni = 28, Pt = 78$ )

Write the types of isomerism exhibited by the following complexes.
(i) $[Co(NH_{3})_{5}Cl]SO_{4}$
(ii) $[Co(en)_{3}]^{3+}$
(iii) $[Co(NH_{3})_{6}] [Cr(CN)_{6}]$

Name the types of isomerism shown by the following pairs of compounds:
(i) $[CoCl(H_2O)(NH_3)_4Cl_2]$ and $[CoCl_2(NH_3)_4]Cl\cdot H_2O$
(ii) $[Pt(NH_3)_4][PtCl_6]$ and $[Pt(NH_3)_4Cl_2][PtCl_4]$

How does ${ K }_{ 2 }\left[ Pt{ Cl }_{ 4 } \right]$ get ionized when dissolved in water? Will it form precipitate when $AgN{ O }_{ 3 }$ solution is added to it? Give a reason for your answer.

Classify the following into homoleptic & heteroleptic complexes?
i) $K_4[Fe(CN)_6]$
ii) $[Co(NH_3)_5(CO_3)]Cl$
iii) $K_2[Zn(OH)_4]$
iv) $[Pt(NH_3)_2Cl(NO_2)]$

Explain the violet colour of $[Ti(H_2O)_6]^{3+}$ complex on basis of the crystal field theory?

(a) Give the postulates of Werner's theory of co-ordination compounds.
(b) Differentiate between chemical reactions and nuclear reactions.

Write the IUPAC name of following compounds :
(A) $K_3[Fe(CN)_6$
(B) $[Co(NH_3)_6]Cl_3$

Draw Werner's structure of the following:
(a) $CoCl_{3} . 6NH_{3}$
(b) $CoCl_{3} . 5NH_{3}$
(c) $CoCl_{3} . 4NH_{3}$
(d) $CoCl_{3} . 3NH_{3}$

What types of isomer are $[Co(NH_3)_5 Br] SO_4$ and $[Co(NH_3)_5 SO_4] Br$ ?

Number of $Cl^{-}$ ions satisifying both primary and secondary valency are in $CoCl_{3}5NH_{3}$ .

For the complex ion $[Fe(CN)_6]^{3-}$ , state:
(i) the type of hybridisation.
(ii) the magnetic behaviour.
(iii) the oxidation number of the central metal atom.

Write primary and secondary valency of $Co$ in $[Co(Nn_{3})_{6}]Cl_{3}$ ?

Predict whether the following molecules are isostructural or not. Justify your answer
(i) $N{Me}_{3}$ (ii) $N{(Si{Me}_{3})}_{3}$

Explain hybridisation, geometry and magnetic property of $[Ni(CN)_4]^{2-}$ ion using Valence Bond Theory(VBT). [Atomic number of Ni is $28$ ].

Chlorophyll contains 2.68% of $Mg$ by weight. Then the number of $Mg$ atom in 2.00 g of chlorophyll is:
(Atomic mass of $Mg = 24$ )

Write formula of the following compound:
(i) dichloridobis (ethylene diamine) cobalt (III) ion.
(ii) sodiumethylenediaminetetraacetatonickelate (II)
(iii) hexaammineplatinum (IV) chloride

What is the Primary and Secondary Valence of $PtCl_{2}.2NH_{3}$ ?

Indicate the types of isomerism exhibited by the following complex and draw the structure of this isomer.
$[Pt(NH_3)(H_2O)Cl_2]$

What is the hybridization of central atom in following? $PH_3, PH_{4}^+,$

On the basis of Werner's theory explain, why cobalt amine complex, $CoCl_{ 3 }{ 4NH }_{ 3 }$ when treated with ${ Ag }{ NO }_{ 3 }$ solution precipitates only one ${ Cl }^{ - }$ ion even though there are three ${ Cl }^{ - }$ ions?

Explain the bonding on $CoCl_{ 2 }.3N{ H }_{ 3 }$ and $CoCl_{ 2 }.5N{ H }_{ 3 }$ structure on the basis at Werner's theory.

If the value of C.F.S.E. for ''Ni" is $\triangle _{ o }$ then what is the CFSE value Pd?

What is IUPAC name of $K_{3}\left [ Fe\left ( CN \right )_{5}NO \right ]$ ?

Write the formula of the following complexes.
Bis (ethnylene diammine) dichloro iridium (III) ion

Write the formula of the following complexes.
Tris (ethylene diammine) cobalt (II) sulphate

Write the possible stereo isomers of the following complexes and identify the type :-
a) $[co(NH_3)_3Cl_3]$
b) $[pt(gly)_2]$
c) $[cr (en)_3]$

Draw the isomer of $[Pt({ { NH }_{ 3 } })_{ 3 }{ Cl }_{ 3 }]$ , $[Co({ { NH }_{ 3 } })_{ 5 }{ Cl }{ SO }_{ 4 }]$ .

What is the nomenclature of $\left[ { CoCl }_{ 2 }({ NH }_{ 3 })_{ 4 } \right] ^{ + }$ ?

What is the primary valency of $[Co (NH_3)_4 Cl_2] Cl_2$ ?

write down the formulae of given compound
tetra amine zinc(II) nitrate

Draw the structure of $ClO_3^-$ .

Write down the $IUPAC$ name of the complex $[Pt (en)_2CI_2]^{2+}$ . What type of isomerism is shown by this complex.

Name the type of isomerism exhibited by the following isomers : $[Cr(NH_3)_6][Co(CN_6)]$ and $[Co(NH_3)_6][Cr(CN)_6]$

Find sum of possible value of 'n' for which complex having formula: $[Pt(NH_{3})_{2}Cl_{2}]_{n}$ can exit.

What is the hybridization of each in $CH_{2}=c=CH_{2}$ ?

select the correct state of hybridization at $X_1, X_2, X_3 and X_4$
$X_1$ $X_2$ $X_3$ $X_4$
(a) $sp^2$ $sp$ $sp^2$ $sp^3$
(b) $sp^3$ $sp^2$ $sp$ $sp$
(c) $sp^2$ $sp^2$ $sp$ $sp^3$
(d) $sp^3$ $sp^2$ $sp^2$ $sp$

What are the geometric arrangements of $sp^3d^2, sp^3d$ and $dsp^2$ hybrid orbitals?

Match the metals of List $I$ with the biological organic of List $II$

Describe hybridization in the case of $PCl_5$ and $SF_6$ . The axial bonds are longer as compared to equatorial bonds in $PCl_5$ whereas in $SF_6$ both axial bonds and equatorial bonds have the same bond length. Explain .

Find the number of total possible coordination isomers in $[Pt(NH_3)_4][Cu(Cl)_4]$ .

Give the electronic configuration of the following complexes on the basis of crystal field splitting theory.
$[CoF_6]^{3-}, [Fe(CN)_6]^{4-}$ and $[Cu(NH_3)_6]^{2+}$ .

In $SF_4$ atom has $sp^x d$ hybridisation.What is the value of x?

$NiCl_2$ in the presence of dimethyl glycoxime (DMG) gives a complex which precipitates in the presence of $NH_4OH$ , giving a bright red color.
Draw its structure and show H bonding.

Write the formulae of the following complex.
Pentamminechlorocobalt(III) ion.

The number of orbitals involved in the hybridization of $XeF_2$ is:

A complex of the type $[M(AA)_2X_2]^{n+}$ is known to be optically active. What does this indicate about the structure of the complex? Give one example of such complex.

Draw the structure of geometrical isomers of $[Pt(gly)_2]$ where $gly \to NH_2CH_2COO^-$ .

What type of isomers are the following ?
$[Co(py)_2(H_2O)_2Cl_2]Cl$ and $[Co(py)_2(H_2O)Cl_3]H_2O$

Write the formulae of the following complexes:
Potassium ethylenediamine tetraacetate ferrate (II)

A certain complex ion has the formula $[M(en)_2Br_2]^+$ where $M$ is the metal ion and en = ethylene diamine. How many isomers are possible for this?

Write down the names of crystal structures in which the following elements are present.

$Sc,\ Ti,\ V,\ Cr,\ Mn,\ Fe,\ Co,\ Ni,\ Cu,\ Zn.$

The EAN of each $Mn(Z=25)$ in $Mn_2(CO)_{10}$ is $36$ . What is the structure of this complex?

Account for the following:
Give the formula and describe the structure of a noble species which is isostructural with $IBr_{2}^{-}$ .

$CO^{3-}$ ion is bound to one $Cl$ , one $NH_3$ molecule and two bidentate ethylene molecule.
Write the formula, name and magnetic behaviour of the above coordination entity.

$Ni^{2+}$ ion is bound to two water molecules and two oxalate ions.
Write the formula, name and magnetic behaviour of the above coordination entity.

Write the formula of the following :
Tetraammineaquachloridocobalt (III) nitrate

What type of isomerism is shown by the following complex:
$[Co(NH_{3})_{6}][Cr(CN)_{6}]$

Giving a suitable example for each, explain the following:
Crystal field splitting

What type of isomerism is exhibited by the following complex:
$[Co(NH_{3})_{5}SO_{4}]Cl$

A coordination compound with the molecular formula $CrCl_{3}.4H_{2}O$ precipitates $AgCl$ with $AgNO_{3}$ solution. Its molar conductivity is found to be equivalent to two ions. What is the structural formula and name of the compound?

What type of isomerism is shown by the complex $[Cr(H_2 O)_6]Cl_3$ ?

Name the following coordinates entity and describe its structure
$[Fe(CN)_6]^{4-}$
(Atomic Number: $Fe=26$ )

Write the state of hybridisation, shape and IUPAC name of the complex $[CoF_6]^{3-}$ .

What is meant by crystal field splitting energy? On the basis of crystal field theory, write the electronic configuration of $d^4$ in terms of $t_{2g}$ and $e_g$ in an octahedral field when
$\Delta_0 < P$

What type of isomerism is shown by $[Co(NH_3)_5 ONO]Cl_2$ ?