CBSE Class 12 Chemistry Chapter 9 Important Questions – Free PDF Download
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Important Questions Class 12 Chemistry Chapter 9 – Coordination Compounds
CBSE Class 12 Chemistry Important Questions Chapter 9 – Coordination Compounds
5 Marks Questions
1. What are ligands? Explain different types of ligands.
Ans. The ions or molecules bound to central atom or ion in the coordination entity are ligands e.g 
has six 
ligands.
Types:-
(1) On the basis of charges on them ligands can be negative, positive (e.g.
, 
etc.) or neutral (e.g. CO, 
,
).
(2) On the basis of their donor atoms ligands can be monodentate or unidentate (one donor atom) e.g-, , 
etc, or didentate (two donor atoms) 
or 
etc. or polydentate (several donor atoms) e.g 
is a hexadentate ligand.
(3) Ligands which can ligate through two different atoms are called ambidentate ligands eg. 
and 
ions. Whereas when a di– or polydentate ligand uses its two or more donor atoms to bind a single metal ion, it is called chelate ligand.
2. Write the formulas for the following coordination compounds:
(i) Tetraamminediaquacobalt (III) chloride
(ii) Potassium tetracyanonickelate (II)
(iii) Tris(ethane-1,2-diamine) chromium(III) chloride
(iv) Amminebromidochloridonitrito-N-platinate (II)
(v) Dichloridobis(ethane-1,2-diamine)platinum(IV) nitrate
(vi) Iron(III) hexacyanoferrate (II)
Ans. (i) 
(ii) 
(iii) 
(vi) 
(v) 
(vi) 
3. Write the IUPAC names of the following coordination compounds:
(i) 
(ii) 
(iii) 
(iv) 
(v) 
(vi) 
Ans. (i) Hexaamminecobalt(III) chloride
(ii) Pentaamminechloridocobalt(III) chloride
(iii) Potassium hexacyanoferrate(III)
(iv) Potassium trioxalatoferrate(III)
(v) Potassium tetrachloridopalladate(II)
(vi) Diamminechlorido(methylamine)platinum(II) chloride
4. Indicate the types of isomerism exhibited by the following complexes and draw the structures for these isomers:
(i) 
(ii) 
(iii) 
(iv) 
Ans. Both geometrical (cis-, trans-) isomers for can exist. Also, optical isomers for cis-isomer exist.
Trans-isomer is optically inactive. On the other hand, cis-isomer is optically active.
(ii) Two optical isomers for 
exist.
Two optical isomers are possible for this structure.
(iii) 
A pair of optical isomers:
It can also show linkage isomerism.
and
It can also show ionization isomerism.
(iv) Geometrical (cis-, trans-) isomers of can exist.
5. Explain on the basis of valence bond theory that 
ion with square planar structure is diamagnetic and the 
ion with tetrahedral geometry is paramagnetic.
Ans. Ni is in the +2 oxidation state i.e., in 
configuration.
There are 4 
ions. Thus, it can either have a tetrahedral geometry or square planar geometry. Since ion is a strong field ligand, it causes the pairing of unpaired 3d electrons.
It now undergoes 
hybridization. Since all electrons are paired, it is diamagnetic.
In case of , ion is a weak field ligand. Therefore, it does not lead to the pairing of unpaired 3d electrons. Therefore, it undergoes 
hybridization.
Since there are 2 unpaired electrons in this case, it is paramagnetic in nature.
6. is paramagnetic while 
is diamagnetic though both are tetrahedral. Why?
Ans. Though both and are tetrahedral, their magnetic characters are different. This is due to a difference in the nature of ligands. is a weak field ligand and it does not cause the pairing of unpaired 3d electrons. Hence, is paramagnetic.
In 
, Ni is in the zero oxidation state i.e., it has a configuration of 
.
But CO is a strong field ligand. Therefore, it causes the pairing of unpaired 3d electrons. Also, it causes the 4s electrons to shift to the 3d orbital, thereby giving rise to hybridization. Since no unpaired electrons are present in this case, is diamagnetic.
7. 
is strongly paramagnetic whereas 
is weakly paramagnetic. Explain.
Ans. In both and 
, Fe exists in the +3 oxidation state i.e., in 
configuration.
Since is a strong field ligand, it causes the pairing of unpaired electrons. Therefore, there is only one unpaired electron left in the d-orbital.
Therefore,
=1.732 BM
On the other hand, 
is a weak field ligand. Therefore, it cannot cause the pairing of electrons. This means that the number of unpaired electrons is 5.
Therefore,
= 6 BM
Thus, it is evident that is strongly paramagnetic, while 
is weakly paramagnetic.
8. Explain 
is an inner orbital complex whereas 
is an outer orbital complex.
Ans.
| |
| Oxidation state of cobalt = +3 | Oxidation state of Ni = +2 |
Electronic configuration of cobalt =  | Electronic configuration of nickel = |
  being a strong field ligand causes the pairing. Therefore, Cobalt can undergo  hybridization. Hence, it is an inner orbital complex. |  If causes the pairing, then only one 3d orbital is empty. Thus, it cannot undergo hybridization. Therefore, it undergoes  hybridization. Hence, it forms an outer orbital complex. |
9. 
solution mixed with 
solution in 1:1 molar ratio gives the test of 
ion but 
solution mixed with aqueous ammonia in 1:4 molar ratio does not give the test of 
ion. Explain why?
Ans. 
Both the compounds i.e., 
and 
fall under the category of addition compounds with only one major difference i.e., the former is an example of a double salt, while the latter is a coordination compound.
A double salt is an addition compound that is stable in the solid state but that which breaks up into its constituent ions in the dissolved state. These compounds exhibit individual properties of their constituents. For e.g. breaks into 
and 
ions. Hence, it gives a positive test for ions.
A coordination compound is an addition compound which retains its identity in the solid as well as in the dissolved state. However, the individual properties of the constituents are lost. This happens because does not show the test for . The ions present in the solution of are 
and.
10. Explain with two examples each of the following: coordination entity, ligand, coordination number, coordination polyhedron, homoleptic and heteroleptic.
Ans. (i) Coordination entity:
A coordination entity is an electrically charged radical or species carrying a positive or negative charge. In a coordination entity, the central atom or ion is surrounded by a suitable number of neutral molecules or negative ions (called ligands). For example:
= cationic complex
= anionic complex
= neutral complex
(ii) Ligands
The neutral molecules or negatively charged ions that surround the metal atom in a coordination entity or a coordinal complex are known as ligands. For example,
, Cl – , – OH. Ligands are usually polar in nature and possess at least one unshared pair of valence electrons.
(iii) Coordination number:
The total number of ligands (either neutral molecules or negative ions) that get attached to the central metal atom in the coordination sphere is called the coordination number of the central metal atom. It is also referred to as its ligancy.
For example:
(a) In the complex, 
, there as six chloride ions attached to Pt in the coordinate sphere. Therefore, the coordination number of Pt is 6.
(b) Similarly, in the complex 
, the coordination number of the central atom (Ni) is 4.
(vi) Coordination polyhedron:
Coordination polyhedrons about the central atom can be defined as the spatial arrangement of the ligands that are directly attached to the central metal ion in the coordination sphere. For example:
(a)
(b) Tetrahedral
(v) Homoleptic complexes:
These are those complexes in which the metal ion is bound to only one kind of a donor group. For eg: 
etc.
(vi) Heteroleptic complexes:
Heteroleptic complexes are those complexes where the central metal ion is bound to more than one type of a donor group.
For e.g.: 
11. What is meant by unidentate, didentate and ambidentate ligands? Give two examples for each.
Ans. A ligand may contain one or more unshared pairs of electrons which are called the donor sites of ligands. Now, depending on the number of these donor sites, ligands can be classified as follows:
(a) Unidentate ligands: Ligands with only one donor sites are called unidentate ligands. For e.g., 
, Cl – etc.
(b) Didentate ligands: Ligands that have two donor sites are called didentate ligands. For e.g.,
(a) Ethane-1, 2-diamine
(b) Oxalate ion
(c)Ambidentate ligands:
Ligands that can attach themselves to the central metal atom through two different atoms are called ambidentate ligands. For example:
(a)
(The donor atom is N)
(The donor atom is oxygen)
(b)
(The donor atom is S)
(The donor atom is N)
12. Specify the oxidation numbers of the metals in the following coordination entities:
(i) 
(ii) 
(iii) 
(iv) 
(v) 
Ans. (i) 
Let the oxidation number of Co be x.
The charge on the complex is +2.
(ii) 
Let the oxidation number of Pt be x.
The charge on the complex is –2.
(iv)
13. Using IUPAC norms write the formulas for the following:
(i) Tetrahydroxozincate(II)
(ii) Potassium tetrachloridopalladate(II)
(iii) Diamminedichloridoplatinum(II)
(iv) Potassium tetracyanonickelate(II)
(v) Pentaamminenitrito-O-cobalt(III)
(vi) Hexaamminecobalt(III) sulphate
(vii) Potassium tri(oxalato)chromate(III)
(viii) Hexaammineplatinum(IV)
(ix) Tetrabromidocuprate(II)
(x) Pentaamminenitrito-N-cobalt(III)
Ans. (i) 
(ii) 
(iii) 
(iv)
(v) 
(vi) 
(vii) 
(viii) 
(ix) 
(x) 
14. Using IUPAC norms write the systematic names of the following:
(i) 
(ii)
(iii) 
(iv) 
(v) 
(vi)
(vii) 
(viii) 
(ix)
Ans. (i) Hexaamminecobalt(III) chloride
(ii) Diamminechlorido(methylamine) platinum(II) chloride
(iii) Hexaquatitanium(III) ion
(iv) Tetraamminichloridonitrito-N-Cobalt(III) chloride
(v) Hexaquamanganese(II) ion
(vi) Tetrachloridonickelate(II) ion
(vii) Hexaamminenickel(II) chloride
(viii) Tris (ethane-1, 2-diammine) cobalt(III) ion
(ix) Tetracarbonylnickel (0)
15. List various types of isomerism possible for coordination compounds, giving an example of each.
Ans.
(a) Geometric isomerism:
This type of isomerism is common in heteroleptic complexes. It arises due to the different possible geometric arrangements of the ligands. For example:
(b) Optical isomerism:
This type of isomerism arises in chiral molecules. Isomers are mirror images of each other and are non-superimposable.
(c) Linkage isomerism: This type of isomerism is found in complexes that contain ambidentate ligands. For example:
and 
Yellow form Red form
(d) Coordination isomerism:
This type of isomerism arises when the ligands are interchanged between cationic and anionic entities of differnet metal ions present in the complex.
and 
(e) Ionization isomerism:
This type of isomerism arises when a counter ion replaces a ligand within the coordination sphere. Thus, complexes that have the same composition, but furnish different ions when dissolved in water are called ionization isomers. For e.g., 
and 
.
(f) Solvate isomerism:
Solvate isomers differ by whether or not the solvent molecule is directly bonded to the metal ion or merely present as a free solvent molecule in the crystal lattice.
Violet Blue-green Dark green
16. Draw the structures of optical isomers of:
(i) 
(ii) 
(iii) 
Ans. (i)
(ii)
(iii)
17. Draw all the isomers (geometrical and optical) of:
(i) 
(ii) 
(iii) 
Ans. (i)
In total, three isomers are possible.
(ii)
Trans-isomers are optically inactive.
Cis-isomers are optically active.
(iii)
18. Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:
(i) 
(ii) 
(iii) 
(iv) 
Ans. (i) In the above coordination complex, iron exists in the +II oxidation state.
: Electronic configuration is
Orbitals of ion:
As 
is a strong field ligand, it causes the pairing of the unpaired 3d electrons.
Since there are six ligands around the central metal ion, the most feasible hybridization is 
.
hybridized orbitals of are:
6 electron pairs from ions occupy the six hybrid orbitals.
Then,
Hence, the geometry of the complex is octahedral and the complex is diamagnetic (as there are no unpaired electrons).
(ii)
In this complex, the oxidation state of Fe is +3.
Orbitals of 
ion:
There are 6 F- ions. Thus, it will undergo or 
hybridization. As 
is a weak field ligand, it does not cause the pairing of the electrons in the 3d orbital. Hence, the most feasible hybridization is .
hybridized orbitals of Fe are:
Hence, the geometry of the complex is found to be octahedral.
(iii)
Cobalt exists in the +3 oxidation state in the given complex.
Orbitals of 
ion:
Oxalate is a weak field ligand. Therefore, it cannot cause the pairing of the 3d orbital electrons. As there are 6 ligands, hybridization has to be either or hybridization.
hybridization of :
The 6 electron pairs from the 3 oxalate ions (oxalate anion is a bidentate ligand) occupy these orbitals.
Hence, the geometry of the complex is found to be octahedral.
(iv)
Cobalt exists in the +3 oxidation state.
Orbitals of ion:
Again, fluoride ion is a weak field ligand. It cannot cause the pairing of the 3d electrons. As a result, the ion will undergo hybridization.
hybridized orbitals of ion are:
19. What is crystal field splitting energy? How does the magnitude of 
decide the actual configuration of d-orbitals in a coordination entity?
Ans. The degenerate d-orbitals (in a spherical field environment) split into two levels i.e., 
and 
in the presence of ligands. The splitting of the degenerate levels due to the presence of ligands is called the crystal-field splitting while the energy difference between the two levels (and ) is called the crystal-field splitting energy. It is denoted by .
After the orbitals have split, the filling of the electrons takes place. After 1 electron (each) has been filled in the three orbitals, the filling of the fourth electron takes place in two ways. It can enter the orbital (giving rise to 
like electronic configuration) or the pairing of the electrons can take place in the orbitals (giving rise to 
like electronic configuration). If the value of a ligand is less than the pairing energy (P), then the electrons enter the orbital. On the other hand, if the value of a ligand is more than the pairing energy (P), then the electrons enter the orbital.
20. 
is paramagnetic while 
is diamagnetic. Explain why?
Ans. Cr is in the +3 oxidation state i.e., 
configuration. Also, 
is a weak field ligand that does not cause the pairing of the electrons in the 3d orbital.
Therefore, it undergoes 
hybridization and the electrons in the 3d orbitals remain unpaired. Hence, it is paramagnetic in nature.
In , Ni exists in the +2 oxidation state i.e., 
configuration.
:
is a strong field ligand. It causes the pairing of the 3d orbital electrons. Then, undergoes 
hybridization.
As there are no unpaired electrons, it is diamagnetic.
21. Give the oxidation state, d-orbital occupation and coordination number of the central metal ion in the following complexes:
(i) 
(ii) cis-
(iii) 
(iv) 
Ans. (i)
The central metal ion is Co.
Its coordination number is 6.
The oxidation state can be given as:
x – 6 = –3
x = + 3
The d orbital occupation for 
is 
.
(ii) cis-
The central metal ion is Cr.
The coordination number is 6.
The oxidation state can be given as:
x + 2(0) + 2(–1) = +1
x – 2 = +1
x = +3
The d orbital occupation for is
.
(iii)
The central metal ion is Co.
The coordination number is 4.
The oxidation state can be given as:
x – 4 = –2
x = + 2
The d orbital occupation for 
is 
.
(iv)
The central metal ion is Mn.
The coordination number is 6.
The oxidation state can be given as:
x + 0 = +2
x = +2
The d orbital occupation for Mn is 
.
22. Write down the IUPAC name for each of the following complexes and indicate the oxidation state, electronic configuration and coordination number. Also give stereochemistry and magnetic moment of the complex:
(i) 
(ii) 
(iii) 
(iv) 
(v) 
Ans. (i) Potassium diaquadioxalatochromate (III) trihydrate.
Oxidation state of chromium = 3
Electronic configuration: 
Coordination number = 6
Shape: octahedral
Stereochemistry:
Magnetic moment, 
(ii)
IUPAC name: Pentaamminechloridocobalt(III) chloride
Oxidation state of Co = +3
Coordination number = 6
Shape: octahedral.
Electronic configuration: 
.
Stereochemistry:
Magnetic Moment = 0
(iii) 
IUPAC name: Trichloridotripyridinechromium (III)
Oxidation state of chromium = +3
Electronic configuration for 
Coordination number = 6
Shape: octahedral.
Stereochemistry:
Both isomers are optically active. Therefore, a total of 4 isomers exist.
Magnetic moment,
(iv)
IUPAC name: Caesium tetrachloroferrate (III)
Oxidation state of Fe = +3
Electronic configuration of 
Coordination number = 4
Shape: tetrahedral
Stereochemistry: optically inactive
Magnetic moment:
(v)
Potassium hexacyanomanganate(II)
Oxidation state of manganese = +2
Electronic configuration: 
Coordination number = 6
Shape: octahedral.
Streochemistry: optically inactive
Magnetic moment,
= 1.732
23. What is meant by stability of a coordination compound in solution? State the factors which govern stability of complexes.
Ans. The stability of a complex in a solution refers to the degree of association between the two species involved in a state of equilibrium. Stability can be expressed quantitatively in terms of stability constant or formation constant.
Stability constant, 
For this reaction, the greater the value of the stability constant, the greater is the proportion of 
in the solution.
Stability can be of two types:
(a)Thermodynamic stability:
The extent to which the complex will be formed or will be transformed into another species at the point of equilibrium is determined by thermodynamic stability.
(b)Kinetic stability:
This helps in determining the speed with which the transformation will occur to attain the state of equilibrium.
Factors that affect the stability of a complex are:
(a) Charge on the central metal ion: Thegreater the charge on the central metal ion, the greater is the stability of the complex.
(b) Basic nature of the ligand: A more basic ligand will form a more stable complex.
(c) Presence of chelate rings: Chelation increases the stability of complexes.
24: Discuss briefly giving an example in each case the role of coordination compounds in:
(i) biological system
(ii) medicinal chemistry
(iii) analytical chemistry
(iv) extraction/metallurgy of metals
Ans. (i) Role of coordination compounds in biological systems:
We know that photosynthesis is made possible by the presence of the chlorophyll pigment. This pigment is a coordination compound of magnesium. In the human biological system, several coordination compounds play important roles. For example, the oxygen-carrier of blood, i.e., haemoglobin, is a coordination compound of iron.
(ii) Role of coordination compounds in medicinal chemistry:
Certain coordination compounds of platinum (for example, cis-platin) are used for inhibiting the growth of tumours.
(iii) Role of coordination compounds in analytical chemistry:
During salt analysis, a number of basic radicals are detected with the help of the colour changes they exhibit with different reagents. These colour changes are a result of the coordination compounds or complexes that the basic radicals form with different ligands.
(iii) Role of coordination compounds in extraction or metallurgy of metals:
The process of extraction of some of the metals from their ores involves the formation of complexes. For example, in aqueous solution, gold combines with cyanide ions to form 
. From this solution, gold is later extracted by the addition of zinc metal.