$K_4\left[Fe{\left(CN\right)}_6\right]$

  $\left[Co{\left(N{H}_3\right)}_6\right]C{l}_3$

 $\left[Cu{\left(N{H}_3\right)}_4\right]C{l}_2$

  $\left[Ni{\left(CO\right)}_4\right]$

The former is an example of a basic compound, while the latter is an amphoteric compound

The former is an example of an amphoteric compound, while the latter is a basic compound

The former is an example of a double salt, while the latter is a coordination compound

The former is an example of a coordination compound, while the latter is a double salt

) 3, 6

) 3, 2

) 2, 2

) 1, 3

3

2

1

0

Weak field ligands cause higher splitting in the d orbitals than strong field ligands.

Weak field ligands cause lower splitting in the d orbitals than strong field ligands.

Strong field ligands did not form a complex with metal ion.

None of the above.

The heat of formation between the two levels (${\mathrm{e}}_{\mathrm{g}}$ and ${\mathrm{t}}_{2\mathrm{g}}$)

The combined pairing energy of the two levels (${\mathrm{e}}_{\mathrm{g}}$ and ${\mathrm{t}}_{2\mathrm{g}}$) 

The combined energy of the two levels (${\mathrm{e}}_{\mathrm{g}}$ and ${\mathrm{t}}_{2\mathrm{g}}$) 

The energy difference between the two levels (${\mathrm{e}}_{\mathrm{g}}$ and ${\mathrm{t}}_{2\mathrm{g}}$) 

Electrons in the 3d orbitals remain unpaired in ${\left[\mathrm{Ni}{\left(\mathrm{CN}\right)}_4\right]}^{2-}$

Electrons in the 3d orbitals remain unpaired in [Cr(NH₃)₆]³⁺

Electrons in the 3p orbitals remain unpaired in [Cr(NH₃)₆]³⁺

Electrons in the 3p orbitals remain unpaired in ${\left[\mathrm{Ni}{\left(\mathrm{CN}\right)}_4\right]}^{2-}$

There are paired electrons in [Ni(H₂O)₆]²⁺ while all electrons are unpaired in [Ni(CN)₄]^2–

There are unpaired electrons in [Ni(H₂O)₆]²⁺ while all electrons are paired in [Ni(CN)₄]^2–

There are unpaired electrons in [Ni(H₂O)₆]²⁺ and [Ni(CN)₄]^2–

None of the above.

Higher lattice energy value of [Fe(CN)₆]^4– as compared to [Fe(H₂O)₆]²⁺

Higher CFSE value of [Fe(CN)₆]^4– as compared to [Fe(H₂O)₆]²⁺

Lower CFSE value of [Fe(CN)₆]^4– as compared to [Fe(H₂O)₆]²⁺

Lower lattice energy value of [Fe(CN)₆]^4– as compared to [Fe(H₂O)₆]²⁺

The metal-carbon bonds in metal carbonyls have both σ and π characters.

The metal-carbon bonds in metal carbonyls have only σ character.

The metal-carbon bonds in metal carbonyls have only π character.

The metal-carbon bonds in metal carbonyls have only hydrogen bonding.

The greater proportion of products.

The greater proportion of reactants

Lesser concentration of catalyst at equilibrium

4 . All of the above

 $[\mathrm{Ni}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6{]}^{2+}$ < $[\mathrm{Ni}{\left({\mathrm{NH}}_3\right)}_6{]}^{2+}$ < $[\mathrm{Ni}{\left({\mathrm{NO}}_2\right)}_6{]}^{4-}$

 $[\mathrm{Ni}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6{]}^{2+}$ > $[\mathrm{Ni}{\left({\mathrm{NH}}_3\right)}_6{]}^{2+}$ > $[\mathrm{Ni}{\left({\mathrm{NO}}_2\right)}_6{]}^{4-}$

 $[\mathrm{Ni}{\left({\mathrm{NH}}_3\right)}_6{]}^{2+}$ > $[\mathrm{Ni}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6{]}^{2+}$ > $[\mathrm{Ni}{\left({\mathrm{NO}}_2\right)}_6{]}^{4-}$

  $[\mathrm{Ni}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6{]}^{2+}$ > ${\left[\mathrm{Ni}{\left({\mathrm{NO}}_2\right)}_6\right]}^{4-}$ > [Ni(NH₃)₆]²⁺

1, 4, 5

2, 4, 5

0, 3, 4

2, 3, 4

a, b

a, c

b, c

a, b, c 

i=d, ii=c, iii=b, iv=a

 i=c, ii=d, iii=b, iv=a

 i=c, ii=d, iii=a, iv=b

i=a, ii=c, iii=b, iv=d

None of the above.

Diethylenetriamine

Oxalato

Both 1 and 2

None of the above.

Cis- Platin is a coordination compound of Platinum.

Gold is extracted by the addition of zinc metal. 

None of the above.

Chlorophyll is a coordination compound of magnesium. 

 $[\mathrm{Cr}{\left(\mathrm{ox}\right)}_3{]}^{3+}$

 $[{\mathrm{PtCl}}_2{\left(\mathrm{en}\right)}_2{]}^{2+}$

 ${\left[\mathrm{Cr}{\left({\mathrm{NH}}_3\right)}_2{\mathrm{Cl}}_2\mathrm{en}\right]}^{+}$

All of the above.

In a coordination entity, the central atom or ion is surrounded by a suitable number of neutral molecules or negative ions ( called ligands). 

Coordination number is also referred as ligancy.

 Coordination polyhedrons is the spatial arrangement of the ligands that are directly attached to the central metal ion in the coordination sphere.

None of these.

Complexes in which the metal ion is bound to only one kind of a donor group are homoleptic complexes.

 Heteroleptic complexes are those complexes where the central metal ion is bound to only one type of donor group.

 $[\mathrm{Pt}{\left(\mathrm{Cl}\right)}_4{]}^{2-}$ is an example of a homoleptic complex.

Both (1) and (3) 

Bidentate ligand with two "N" donor atoms

Tridentate ligand with three "N" donor

Hexadentate ligand with four "O" and two atoms "N'' donor atoms

Unidentate ligand