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Karnataka 2nd PUC Chemistry Question Bank Chapter 9 Coordination Compounds
2nd PUC Chemistry Coordination Compounds NCERT Textbook Questions and Answers
Explain the bonding in coordination compounds in terms of Werner’s postulates.
The valencies of the elements in cobalt (III) chloride and in ammonia seem to be completely satisfied. However, the two substances react to form a stable compound with the formula COCl3·6NH3. The compound is known as a coordination compound.
- In co-ordination compounds, metal atoms exhibit two types of valencies. These are primary and secondary valencies.
- The ligands attached to the primary valencies are ionizable and represent the oxidation state of the metal. The ligands attached to the secondary valencies are non-ionizable and these correspond to its co-ordination number.
- Every metal has a fixed number of secondary valencies because its co-ordination number is fixed.
- Metal tends to satisfy both these valencies. The primary valencies are satisfied by negative ions (anions) whereas secondary valencies are satisfied by either negative ions or neutral molecules.
FeSO4 solution mixed with (NH4)2SO4 solution in 1:1 molar ratio gives the test of Fe2+ ion but CuSO4 solution mixed with aqueous ammonia in 1 : 4 molar ratio does not give the test of Cu2+ ion. Explain why?
Both compounds i.e. FeSO4 (NH4)2SO4.6H2O and [Cu(NH3)4]SO4.5H2O 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 bnK that which breaks up into its constituent ions in the dissolved state. These compounds exhibit individual properties of their constituents for e.g. FeSO4 (NH4)2SO4.6H2O breaks into Fe2+ NH4+, and SO42- ions.
Hence, it gives a positive test for Fe2+ ions. A coordination compound is an addition compound that retains its identity In the solid as well as in the dissolved state. However, the individual properties of the constituents cost. This happens because [Cu(NH3)]4]SO4.5H2O does not show the test for Cu2+ The ions present in the solution of [Cu(NH3)4]SO4.5H2O are [Cu(NH3)4]2+ and SO42-
Explain with two examples each of the following: coordination entity, ligand, coordination number, coordination polyhedron, homoleptic and heteroleptic complexes;
(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).
[Ni(NH3)6]2+, [Fe(CN)6]4+ = cationic complex
[PtCl4]2-, [Ag(CN)2]– – anionic complex
[Ni (CO)4], [CO (NH3)4Cl2] = neutral complex
The neutral molecules or negatively charged ions that surround the metal atom in a coordination entity or a coordinate complex are known as ligands.
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 legacy.
(a) In the complex K2[PtCl6], there are six chloride ions attached to Pt in the coordinate sphere. Therefore, the coordination number of Pt is 6.
(b) similarly, in the complex [Ni (NH3)4 Cl2], the coordination number of the central atom (Ni) is 6.
(iv) 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.
(a) Square planar
(b) Square planar
(v) Homoleptic complexes:
These are those complexes in which the metal ion is bound to only one kind of a donor group For e.g.:
(vi) Heteroleptic complexes:
Heteroleptic complexes are those complexes where the central metal is bound to more than one type of donor group.
What is meant by unidentate, didentate and ambidentate ligands? Give two examples for each.
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.
(b) Didentate ligands: Ligands that have two donor sites are called didentate ligands.
(a) Ethane – 1, 2 – diamine.
(b) enolic acid
c) Ambidentate ligand:
Ligands that can attach themselves to the central metal atom through two different atoms are called ambidentate ligands.
For Example :
Specify the oxidation numbers of the metals in the following coordination entities:
(i) [CO(H2O) (CN) (en)2]2+
Let the oxidation number of CO be x.
The charge on the complex is + 2
x + 4 (-1) = -2 x = +2
(iii) [COBr2 (en)2]+
x + 2 (-1) + 2.(0) = + 1
x = + 3
x + 6 (-1) = -3
x = + 3
(v) [Cr (NH3)3 Cl3]
x + 3 (0) +3 (-1) = 0
x – 3 = 0
x = 3
Using IUPAC norms write the formula for the following:
- Tetrahydroxozincate (II)
- Potassium tetrachloridopalladate(II)
- Potassium tetracyanonickelate(II)
- Hexaamminecobalt(III) sulphate
- Potassium tri(oxalato)chromate(III)
- [Zn (O4)]2-
- K2 [Pd Cl4]
- [Pt (NH3)2 Cl2]
- [CO (NH3)5 (ONO)]2+
- [CO (NH3)6]2(SO4)3
- K3 [Cr (C2O4)3]
- [Pt (NH3)6]4+
- [Cu (Br4)2-
- [CO (NO2) (NH3)5]2+
Using IUPAC norms write the systematic names of the following:
- Hexaamminecobalt (III) chloride.
- Diamine chlorido (methylamine) platinum (II) chloride.
- Hexaaquatitanium (III) ion.
- Tetraamminichloridonitrite – N – cobalt (HI) chloride.
- Flexaquamanganese (II) ion.
- Tetrachloridononickeiate (II) ion.
- Hexaammmenickei (11) chloride,.
- Tris (ethane -1, 2 – diammine) cobalt (III) ion.
- Tetracarbonylnickel (O)
List various types of isomerism possible for coordination compounds, giving an example of each.
(a) Geometric isomerism:
This type of isomerism is common in heteroleptic complexes It arises dire to the different possible geometric arrangements of the li sands.
(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.
[CO (NH3)5 (NO2)]Cl2 and [CO (NH3)5 (ONO)] Cl2
(d) Coordination isomerism:
This type of isomerism arises when the ligands are inter-changed between cationic and anionic entities of different metal ions present in the complex.
[CO (NH3)6] [Cr (CN)6] and [CO (CN)6][Cr (CN)6]
(e) Ionisation 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 ionisation isomers.
How many geometrical isomers are possible in the following coordination entities?
(i) For [Cr(C2O4)3]3- No geometric isomer is possible as it is a bidentate ligand.
Two geometrical isomers are possible.
Draw the structures of optical isomers of:
Draw all the isomers (geometrical and optical) of:
Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of these will exhibit optical isomers?
[Pt (NH3) (Br) (eC) (Pg)]
From the above isomers, none will exhibit optical isomers. Tetrahedral complexes rarely show optical isomerisation. They do so only in presence of unsymmetric chelating agents.
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 CuSO4 exists as [Cu(H2O)4]SO4. It is blue in colour due to the presence of [CU(H2O)4]2+ ions.
(i) When KF is added
(ii) When KCl is added.
[Cu (H2O)4]2+ 4Cl– → [CuCl4]2- + 4H2O
In both cases, the weak field ligand water is replaced by the F– and Cl– ions.
What is the coordination entity formed when an 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 H2S(g) is passed through this solution?
On mixing the aqueous solutions of KCN and CuSO4, the complex formed is potassium tetracyanocuprate(II). Since CN” ions are strong ligands, the complex is quite stable. It is evident from the stability constant value (K = 2·0 x 1027). It is not cleaved by H2S gas when passed through the aqueous solution and no precipitate of CuS is formed.
[CU(H2O)4]2+ + 4CN– → [CU(CN)4]2- + 4H2O.
Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:
In the above coordination complex. Iron exists in +2 oxidation state.
Fe2+: electronic configuration is 3d6
As CN– is a strong field ligand, it causes pairing of the unpaired 3d electrons.
Since there are six ligands aound the central metal ion, the most feasible hybridisation is d2sp3 6 electrons pairs from CN– ions occupy the six hybrid d2sp3 orbitais .
Hence, the geometry of the complex is octahedral and the complex is diamagnetic (as there are no unpaired electrons).
Oxidation state of Fe is + 3
Orbitais of Fe+3 ion.
There are 6F– ions. Thus, it will undergo d2Sp3 or sp3d2 hybridisation. As F– is a weak ligand, it does not cause pairing of electrons in the 3d orbitals. Hence the most feasible hybridisation is Sp3d2.
Hence the geometry of the complex is found to be octahedral.
Cobalt exists + 3 oxidation state in the complex.
Oxalate is a weak field ligand. Therefore, it cannot cause pairing of the 3d orbital electrons.
As there are 6 ligands, hybridisation has to be either Sp3d2 or d2Sp3 hybridization.
As there are no pairing of electrons Sp3d2 is the most stable hybridisation.
Oxalate being a bidentate ligand donates 2 pairs of electrons each.
Hence, the geometry of the complex is found to be octahedral.
cobalt exists in the +3 oxidation state.
Again, fluoride ion is a weak ligand. It cannot cause the pairing of the 3d electrons. Sp3d2 hybridised orbitals of CO3+ ion are
Hence, the geometry of the complex is octahedral and paramagnetic.
Draw a figure to show the splitting of d orbitals in an octahedral crystal field.
The splitting of d orbitals in an octahedral field takes place in such a way that dx2-y2, dz2 experience a rise in energy and form the e.g. level, dry, dyz, dzx experience a fall in energy and form t2g level.
What is spectrochemical series? Explain the difference between a weak field ligand and a strong field ligand.
The arrangement of ligands in order of their increasing field strengths, i.e., increasing crystal field splitting energy (CFSE) values is called the spectrochemical series.
The ligands with a small value of CFSE (Δ0) are called weak field ligands whereas those with a large value of CFSE (Δ0) are called strong field ligands.
What is crystal field splitting energy? How does the magnitude of ∆o decide the actual configuration of d orbitals in a coordination entity?
When ligands approach a particular metal ion, the d-orbitals split into two sets, one with lower energy while the other with higher energy. The difference of energy between the two sets of orbitals is known as crystal field stabilising energy (CFSE).
- If ∆0 < P, the configuration will be t32ge1g and it is there in case of weak field ligands and high spin complex will be formed.
- If ∆0 > P, the configuration will be t42ge0g and it is there in case of strong-field ligands and low spin complex will be formed.
[Cr(NH3)6]3+ is paramagnetic while [Ni(CN)4]2- is diamagnetic. Explain why?
Cr is in the +3 oxidation state i.e. d3 configuration. Also, NH3 is a weak field ligand that does not cause the pairing of the electrons in the 3d orbitals.
Therefore, it undergoes d2sp3 hybridisation and the electrons in the 3d orbitals remain unpaired. Hence, ibis paramagnetic in nature.
In [Ni CCN)4]2-, Ni exists in the +2 oxidation state.
i.e, d8 Configuration.
CN– is a strong field ligand. It causes the pairing of 3d orbital electrons. Then Ni2+ undergoes dsp2 hybridisation.
As there are no unpaired electrons, it is diamagnetic.
A solution of [Ni(H2O)6]2+ is green but a solution of [Ni(CN)4]2- is colourless. Explain.
In [Ni(H2O)6]2+ is a weak field ligand. Therefore there are unpaired electrons in Ni2+. In this complex, the cl electrons from the lower energy level can be excited to the higher energy level if the possibility of d- d transition is present. Hence [Ni(H2O)6]2+ is colored.
In [Ni(CN)4]2- CN is a strong field ligand. Therefore, d- d transition is not possible due to the absence of unpaired electrons (CN initiates pairing of d electrons). Hence it is colourless.
[Fe(CN)6]4- and [Fe(H2O)6]2- are of different colours in dilute solutions. Why?
In both the complexes, Fe is in +2 oxidation state with cf configuration. This means that it has four unpaired electrons: Both CN– ion and H20 molecules act as ligands occupy different relative positions in the spectrochemical series. They differ in crystal field splitting energy (Δ0). Quite obviously, they absorb radiations corresponding to different wavelengths and frequencies from the -visible region of light, (VIBGYOR) and the transmitted colours are also different. This means that the complexes have different colours in solutions.
Discuss the nature of bonding in, metal carbonyls.
The metal-carbon bonds in’ metal carbonyls have both σ and π characteristics. A σ bond is formed when the carbonyl carbon donates a lone pair of electrons to the vacant orbital of metal. A π bond is formed by the donation of a pair of vacant anti-bonding π orbital (also known as back bonding of the carbonyl group). The σ bond strengthens the π bond and vice-versa. This synergic effect is created due to this metal-ligand bonding. This synergic effect strengthens the bond between CO and metal.
Give the oxidation state, d orbital occupation, and coordination number of the central metal ion in the following complexes:
The central metal ion is CO
coordination number: 6
oxidation state: +3
d orbital occupation : t62g eg0
central metal: Cr
coordination number: 6
oxidation state:+3 .
d orbital occupation : t32g eg0
central metal: Co oxidation state: +2 coordination number: 4
d orbital occupation : eg4 t32g
Central metal: Mn
coordination number: 6
oxidation state : + 2
d orbital occupancy : t32g eg2
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) Potassium diaquadioxatatochromate (III) trihydrate oxidation state of chromium = +3
Electronic configuration: 3d3: t32g
coordination number: 6
(ii) [Co (NH3)5Cl]Cl2
Pentaamminechloridocobalt (III) chloride
oxidation state =+3
coordination number = 6
electronic configuration : d6: t62g
Magnetic moment = 0 (∵ n = 0)
oxidation state = +3
electronic configuration : d3: t32g
coordihation number = 6
shape = octahedral
Both isomers are optically active. Therefore, a total of 4 isomers exist.
(iv) Cs [Fe Cl4]
IVPAC name: Caesium tetrachloroferrate(III)
oxidation state = +3
coordination number = 4
stereochemistry: optically inactive
Potassium hexacyanomanganate (II)
oxidation state =+2
electronic configuration = d5 : t52g
coordination number = 6
stereochemistry: optically inactive
What is meant by the stability of a coordination compound in solution? State the factor which governs the stability of complexes.
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 pr formation constant.
For this reaction, the greater the value of the stability constant, the greater is the proportion of ML3 in the solution.
stability can be 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:
- charge on the central metal ion: The greater the charge on the central metal ion, the greater the stability of the complex.
- Basic nature of ligand: A more basic ligand will form a more stable complex.
(c) Presence of chelate rings: Chelation increases the stability of complexes
What is meant by the chelate effect? Give an example.
When a di-or polydentate ligand uses its two or more donor atoms to bind a single metal ion, it is said to be a chelate ligand. The number of such ligating groups is called the denticity of the ligand. Such complexes, called chelate complexes tend to be more stable than similar complexes containing unidentate ligands.
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.
Application of coordination compounds.
(a) Used in qualitative and quantitative analysis.
(b) Determination of hardness of water
(c) Extraction of Au and Ag through complex formation
(d) Refining of Ni through complex formation
(e) Use of Rhodium complex in hydrogenation ofalkene.
(f) Use of EDTA in lead poisoning etc.
How many ions are produced from the complex CO(NH3)6Cl2 in solution?
The given complex can be written as [CO(NH3)6]Cl2 Thus, [CO (NH3)6]+ along with two Cl– ions are produced.
Amongst the following ions which one has the highest magnetic moment value?
(i) n = 3
(ii) n = 4
(iii) n = 0
μ = 0
Hence [FeCH2O)6]2+ has the highest magnetic moment value.
The oxidation number of cobalt in K[CO(CO)4] is
(i) +1 (ii) +3 (iii) -1 (iv) -3
We know that CG is a neutral ligand and K carries a charge of + 1. Therefore, the complex is written as K+ [Co (CO)4]–. Therefore, the oxidation number of Co in the given complex is -1.
Hence (III) is correct.
Amongst the following, the most stable complex is
We know that the stability of a complex substance increases by chelation. Therefore, the most stable complex is [Fe (C2O4)3]3-
What will be the correct order for the wavelengths of absorption in the visible region for the following:
[Ni(NO2)6]4-, [Ni(NH3)6]2+, [Ni(H2O)6]2+?
The central metal ion in all three complexes is the same. Therefore, absorption in the visible region depends on the ligands. The order in which the CFSE values of the ligands increase in the spectrochemical series as follows.
H2 O < NH3 < NO2–
Thus, the amount of crystal field splitting observed will be in the following order.
Hence, the wavelengths of absorption in the visible region will be in the order
[Ni(H2O)6]2+ > [Ni(NH3)6]2+ > [Ni (NO2)6]4-