In $$Fe{(CO)}_{5}$$, the $$Fe-C$$ bond possess:

both $$\sigma$$ and $$\pi$$ characters

MCQ Questions for Class 11 Medical Chemistry Chemical Bonding And Molecular Structure Quiz 14

Diatomic molecule has a dipole moment of 1.2 D.If its bond is

$1.0 \mathring{A}$ , what fraction of an electronic charge exists on each atom?

0%
11 %
0%
20 %
0%
25 %
0%
15 %

The acid containing S-O-O-S bond is

0%
$H_2SO_5$
0%
$H_2S_2O_7$
0%
$H_2S_2O_6$
0%
$H_2S_2O_8$

The increasing order of dipole moment is

0%
$C{H_3}I < C{H_3}Br < C{H_3}CI < C{H_3}F$
0%
$C{H_3}F < C{H_3}CI < C{H_3}Br < C{H_3}I$
0%
$C{H_3}I < C{H_3}Br < C{H_3}F < C{H_3}CI$
0%
$C{H_3}I < C{H_3}F < C{H_3}Br < C{H_3}CI$

$Fe{(CO)}_{5}$ , the

$Fe-C$ bond possess:

0%
$\sigma$ -character only
0%
$\pi$ -character only
0%
both $\sigma$ and $\pi$ characters
0%
ionic character

In which of the following molecules number of lone pairs and bond pairs on central atom are not equal?

0%
$H_2O$
0%
$I^-_3$
0%
$O_2F_2$
0%
$SCl_2$

Carbon has a Covalency of 2 in CO and 4 in

$C{O_2}$ and

$C{H_4}$ .

Its valency in

${C_2}{H_2}\,$ is :

0%
3
0%
4
0%
2
0%
1

Coordinate bond is not present in

0%
$BF_{4}^{-}$
0%
$CO_{3}^{2-}$
0%
$AlCl_{4}^{-}$
0%
$Any\ of\ these$

${ PO }_{ 4 }^{ 3- }$ ion, the formal charge on each oxygen atom and

$P-O$ bond order respectively.

0%
$-0.75, 0.6$
0%
$-0.5, 1.0$
0%
$-0.75, 1.25$
0%
$-3.0, 1.5$

Which of the following statement is wrong:

0%
Hybridisation is the mixing of atomic orbitals prior to their combining into molecular orbitals
0%
$sp^2$ hybrid orbital are formed from two p atomic orbitals and one s atomic orbital
0%
$dsp^2$ hybrid orbitals are all at $90^o$ to one another
0%
$sp^3d^2$ hybrid orbitals are directed towards the corners of a regular tetrahedron

Physical properties of compound depend on:

0%
primary forces present in the compound
0%
secondary forces present in the compound
0%
bond angle of the molecule
0%
shape of the molecule

C-H bond distance is longest in __________ .

0%
$C_2H_2$
0%
$C_2H_4$
0%
$C_2H_6$
0%
$C_3H_6$

For the following geometry, which of the ineqquality is/are correct ?

0%
${ \theta }_{ 1 }^{ ' }<{ \theta }_{ 1 }$
0%
${ \theta }_{ 2 }<{ \theta }_{ 2 }^{ ' }$
0%
${ \theta }_{ 1 }<{ \theta }_{ 1 }^{ ' }$
0%
${ \theta }_{ 2 }>{ \theta }_{ 2 }^{ ' }$

Compound having zero dipole moment is

0%
${\text{C}}{{\text{H}}_{\text{3}}}{\text{Cl}}$
0%
${\text{C}}{{\text{H}}_{\text{2}}}{\text{C}}{{\text{l}}_{\text{2}}}$
0%
${\text{CHC}}{{\text{l}}_{\text{3}}}\;$
0%
${\text{CC}}{{\text{l}}_{\text{4}}}$

Of the following molecules, the one, which has permanent dipole moment, is-

0%
$\mathrm { SiF } _ { 4 }$
0%
$\mathrm { BF } _ { 3 }$
0%
$\mathrm { PF } _ { 3 }$
0%
$\mathrm { PF } _ { 5 }$

Which element has variable covalency ?

0%
F
0%
I
0%
H
0%
O

Which of the following element shows maximum valency?

0%
Carbon
0%
Barium
0%
Nitrogen
0%
Sulphur

Arrange the following compounds in decreasing order of their dipole moment.

${\text{C}}{{\text{H}}_{\text{3}}} - {\text{C}}{{\text{H}}_{\text{2}}} - \;{\text{N}}{{\text{O}}_{\text{2}}}\;$

${\text{C}}{{\text{H}}_{\text{3}}} - {\text{C}}{{\text{H}}_{\text{2}}} - \;{\text{N}}{{\text{H}}_{\text{2}}}\;$

III

${\text{C}}{{\text{H}}_{\text{3}}} - {\text{C}}{{\text{H}}_{\text{2}}} - \;{\text{F}}\;$

${\text{C}}{{\text{H}}_{\text{3}}} - {\text{C}}{{\text{H}}_{\text{2}}} - \;{\text{CN}}$

0%
$IV > III > I > II$
0%
$IV > I > III > II$
0%
$I > III > IV > II$
0%
$I > IV > III > II$

In which of the following the experimental dipole moment is more than what is expected from theory

0%
0%
0%
0%
All of these

Find the correct option.

0%
${ NH }_{ 3 }<{ NF }_{ 3 }$ (Dipole moment)
0%
${ CO }<{ CO }_{ 2 }$ [C-O bond length]
0%
${ NH }_{ 2 }^{ - }>{ NH }_{ 4 }^{ + }$ (Bond angle)
0%
${ I }_{ 3 }^{ - }<{ N }_{ 3 }^{ - }$ [lone pairs]

Correct order of dipole moment is :
1) I = II = III 2) I < II < III
3) I > II > III 4) II < III < I

0%
1
0%
2
0%
3
0%
4

Number of sigma bonds in

$CH_{4}$ is:

0%
4
0%
2
0%
3
0%
5

In which of the following pairs , the hybridisation of central atmos is same but molecular geometry is not the same ?

0%
${ SO }_{ 3 },{ CO }_{ 3 }^{ 2- }$
0%
${ SO }_{ 3 }^{ 2- },{ NH }_{ 3 }$
0%
${ PCl }_{ 5 },{ POCl }_{ 3 }$
0%
${ XeF }_{ 2 },{ ICl }_{ 3 }$

Which theory is useful to determine geometrical structure of molecules ?

0%
Molecular orbital theory
0%
VSEPR theory
0%
Resonance theory
0%
Quantam mechanics

Number of

$(\sigma)-$ bonds present in

$\mathrm{CH}_{4}$ is:

0%
4
0%
3
0%
2
0%
1

Which type of bond is present in

$Xe$ molecules ?

0%
Covalent
0%
Ion-dipole
0%
Van der Waals
0%
Dipole-dipole

Which of the following statement is incorrect?

0%
The tendency to attract bonded pair of the electron in case of hybrid orbitals follows the order: $sp > sp^2 > sp^3$
0%
Alkali metals generally have negative value of electron gain enthalpy
0%
$Cs^+(g)$ releases more energy upon gain of an electron than $Cl(g)$
0%
The electronegativity values for $2$ p-series elements is less than that for $3$ p-series elements on account of small size and high inter electronic configuration

Bond distance in HF is

$9.17\times10^{-11}\ m$ . The dipole moment of

$HF$ is

$6.104\times10^{-30}$ .The percent ionic character in

$HF$ will be: (electron charge

$=1.60\times10^{-19}$ C)

0%
$61.0\%$
0%
$38.0\%$
0%
$35.5\%$
0%
$41.5\%$

In the following i.

$N_2 \rightarrow N^+_2 \quad ii. O_2 \rightarrow O^+_2 ;\quad$ the electrons respectively are removed from

0%
$( {\sigma } 2 p_z)\ and\ ( \pi^* 2p_y\ or\ \pi^* 2 p_x )$
0%
$( \pi^* 2 p_x )\ and\ ( \pi^* 2p_y\ or\ \pi^* 2 p_x )$
0%
$( \pi^* 2 p_y )\ and\ ( \pi^* 2p_y\ or\ \pi^* 2 p_x )$
0%
$( \pi^* 2 p_z)\ and\ ( \pi^* 2p_y\ or\ \pi^* 2 p_x )$

The sum of

$\sigma$ and

$\pi$ -bonds present in the given molecule is

0%
26
0%
28
0%
29
0%
30

Number of lone pair present in each molecule of

$H_2O , NH_3$ and

$C_2H_4$ respectively.

0%
$1, 2, 1$
0%
$2, 1, 0$
0%
$1, 1, 1$
0%
$2, 1, 2$

Which of the following represent

$sp - sp - sp^2 - sp - sp^2 - sp^3$ hybridization from left to right order?

0%
$CH_2= CH - C = \overset{H}{\overset{|}{C}} - C \equiv N$
0%
$CH \equiv C - CH = C = CH-CH_3$
0%
$N \equiv C - \overset{H}{\overset{|}{C}} - \underset{H}{\underset{|}{C}} - CH - CH_3$
0%

Explanation

Carbon having single bond is

$sp^3$ hybridised, carbon with double bond is

$sp^2$ hybridised and the carbon having triple bond is

$sp$ hybridised.

In option B

$CH$ is

$sp$ hybridised,

$C$ is

$sp$ hybridised,

$CH$ is

$sp^2$ hybridised,

$C$ is

$sp$ hybridised,

$CH$ is

$sp2$ hybridised and

$CH_3$ is

$sp^3$ hybridised.

A molecule

$(X)$ has (i) four sigma bonds formed by the overlap of

$sp^{2}$ and

$s$ orbitals; (ii) one sigma bond formed by

$sp^{2}$ and

$sp^{2}$ - orbitals and (iii) one

$\pi-bond$ formed by

$p_{z}$ and

$p_{z}$ orbitals. Which of the following is

$X$ ?

0%
$C_{2}H_{6}$
0%
$C_{2}H_{5}Cl$
0%
$C_{2}H_{2}Cl_{2}$
0%
$C_{2}H_{4}$

Select the correct statement :

0%
If molecule has any polar bond, then it is always polar
0%
Solubility of noble gases increases in water down the group when their size increases because London dispersion force increases
0%
First ionization energy of Al is greater than that of gallium
0%
$XeF^{ \oplus}_5$ has disorted octahedral geometry

In which of the following, the number of orbital dipoles is equal to the numebr of bonds moments?

0%
$PCl_3$
0%
$SO_3$
0%
$O_3$
0%
$H_2O$

The number and types of bonds between two carbon atoms in calcium carbide is:

0%
one sigma, two pi
0%
one sigma, one pi
0%
tow sigma, one pi
0%
two sigma, two pi

Arrange the following compounds in order of increasing dipole moments,
Toluene (I), m-dichlorobenzene (II), o -dichlorobenzene (III), & p-dichlorobenzene (IV)

0%
I < IV < II < III
0%
IV < I < II < III
0%
IV < I < III < II
0%
IV < II < I < III

Explanation

Order of dipole moment of the given compounds is:

$\mathrm{p-dichloro \ benzene < Toluene < m-dichloro \ benzene < o-dichloro \ benzene}$

Hence, Option "B" is the correct answer.

Find out the similarities between

$I_2Cl_6$ and

$Al_2Cl_6 .$

0%
Both have $3\ C -4e^-$ bond
0%
Both have $sp^3$ hybridization for the central atom
0%
Both are non planar
0%
All are correct

Explanation

$I_2Cl_6$

Hybridization of each

$I : sp^3 d^2$

Planar structure

2 bonds are of

$3C -4e^-$

4 bonds are of

$2C - 2 e^-$

$Al_2Cl_6$

Hybridization of each

$Al : sp^3$

Non-polar structure

2 bonds are of

$3C - 4e^-$

4 bonds are of

$2C - 2e^-$

1584183_1721723_ans_cc1da2713baf49fab323634cea05a9aa.png

Back bonding always changes

0%
bond angle
0%
hybridisation of central atom
0%
planarity
0%
bond length

What will be the value of formal charge of individual atom of

$O_3$ molecule :-

0%
+1, +1, +1
0%
0, +1, -1
0%
0, 0, 0
0%
+2, -2, 0

Which bond properties are consistent with one another?

0%
Bond order- Higher, Bond length- Shorter, Vibrational frequency- higher
0%
Bond order- Higher, Bond length- longer, Vibrational frequency - lower
0%
Bond order- Lower, Bond length - shorter, Vibrational frequency- lower
0%
Bond order- Lower, Bond length- longer, Vibrational frequency - higher

Which type of bond is present in

$[ BeF_2]_n$ polymer ?

0%
$3C-2e^-$
0%
$3C-4e^-$
0%
$2C-3e^-$
0%
None of these

Select the correct statement(s):

0%
the tendency of polymerization of the oxyanions lies in the sequence:

$SiO^{4-}_4 > PO^{3-}_4 > SO^{2-}_4> ClO^{2-}_4$
0%
the molecular structure of $S_4N_4H_4$ and $S_4N_4F_4$ are different
0%
the bond strength of P-O linkage is maximum in $OPF_3$ compared to all other analogous halogen compounds
0%
The structural geometries of $NO ^+_2$ and $NO_2$ are different

An example of molecule having a three center bond is:

0%
$NH_3$
0%
$H_3 BO_3$
0%
$NaBH_4$
0%
$B_2H_6$

Explanation

A three-center two-electron bond is an electron deficient chemical bond where three atoms share two electrons. The combination of three atomic orbitals form three molecular orbitals: one bonding, one non-bonding, and one anti-bonding.

The two electrons go into the bonding orbital, resulting in a net bonding effect and constituting a chemical bond among all three atoms. In many common bonds of this type, the bonding orbital is shifted towards two of the three atoms instead of being spread equally among all three. The simplest example of a 3c-2e bond is in the

$B_2H_6$ . Hence correct answer is option D.

1560872_1725874_ans_b653e1f78cb741a4a669e900d0e1f821.png

Which of the following sets of the molecule(s) is/are having a V-shape but different hybridization?

0%
$SnCl_2$ and $H_2O$
0%
$SO_2$ and $NO^+_2$
0%
$BF^-_2$ and $SCl_2$
0%
$OF_2$ and $SCl_2$

In V.B.T., the idea of hybridization was required to explain which of the following facts:

0%
The equivalence of the bonds in most of the com-pounds
0%
The stereochemistry of the molecules
0%
The better overlapping of the orbitals
0%
None of these

The bond order of

$O_2^+$ is:

0%
$1$
0%
$1.5$
0%
$2.5$
0%
$3$

Explanation

Hint: Bond order can be calculated by using molecular orbital theory.

Step 1: Determination of Bond Order :

Total number of electrons in $O_2=16$ but due to a positive charge one electron is deducted and thus,

the total number of electrons in ${O_2}^+ = 15$

Molecular orbital configuration can be written as,

$(\sigma 1s)^2 <(\sigma\ast 1s)^2< (\sigma 2s)^2< (\sigma\ast 2s)^2< (\sigma 2pz)^2< (\pi 2px)^2 \approx (\pi 2py)^2< (\pi\ast 2px)^1 \approx (\pi\ast 2py)^0$

$\ast \ -$ mark represent the electron is present in anti-bonding molecular orbital.

Bond order can be defined as:

$Bond\ Order = \dfrac{Number\ of\ electrons\ in\ B.M.O\ –\ Number\ of\ electrons\ in\ A.B.M.O.}{2}$

( where, B.M.O. - Bonding Molecular Orbital, A.B.M.O - Anti-bonding Molecular Orbital )

${O_2}^+$ has $10$ bonding electrons and $5$ antibonding electrons.

So, the bond order is $\dfrac{10-5}{2}=2.5$ .

Final Step: Correct Answer - (C) $2.5$ .

Select the correct statement(s):

0%
Para-dihydroxy benzene is polar while para-dimethy benzene is non-polar
0%
Dipole moment of $NH_3$ is larger than that of $NF_3$
0%
The direction of dipole moment in $CO$ is from $C$ to oxygen
0%
All are incorrect

Choose the incorrect statement:

0%
All $S-F$ bond length are identical in $SF_4.$
0%
All $Cl-F$ bond length are identical in $ClF_3 .$
0%
All $\angle FClF$ angles are identical in $ClF_3.$
0%
All possible angle in $BF_2Cl$ are $120^0 .$

Which of the following molecules/ions are all the bonds not equal?

0%
$SF_4$
0%
$SiF_4$
0%
$XeF_4$
0%
$BF_4^-$

Explanation

$SF_4 ,$ the central aton S has

$sp^d$ -hybridization. Thus it contains two axial and two equatorial bonds to give a see-saw structure .
1584342_1722149_ans_a0557e2b67ec48b8a4345710b5cf9702.png

1584342_1722149_ans_a0557e2b67ec48b8a4345710b5cf9702.png

Which are the correct statements for

$NO_2$ ?

0%
It is paramagentic and dimerizes to $N_2O_4$
0%
$N_2O_4$ is plannar and diamagnetic
0%
$NO_2$ is linear containing an odd number of electrons
0%
$N-O$ bonds in $NO_2$ are of different lengths

CBSE Questions for Class 11 Medical Chemistry Chemical Bonding And Molecular Structure Quiz 14 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

CBSE Questions for Class 11 Medical Chemistry Chemical Bonding And Molecular Structure Quiz 14 - MCQExams.com

0:0:3

Practice Class 11 Medical Chemistry Quiz Questions and Answers

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