NCERT Solutions for Class 12 Chemistry Chapter 9 Coordination Compounds

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NCERT Solutions for Class 12 Chemistry Chapter 9 Coordination Compounds presented here help students learn about “coordination compounds” and understand the concepts related to it. However, this chapter which is included in Class 12 chemistry syllabus is an important concept as we talk about atoms and chemical reactions. As such, coordination compounds include detailed solutions for all the questions of the NCERT textbooks. Students need to understand the topics clearly in order to score good marks and to avoid any difficulty in the future.

NCERT solutions for class 12 Chemistry chapter 9 have detailed step by step solutions along with complete explanations. The students can also freely download NCERT solutions for class 12 Chemistry chapter 9 pdf to study in offline mode as well.

The chapter covers the following exercises:

  • § Exercise 9.1 – Werner’s Theory of Coordination Compounds
  • § Exercise 6.2 – Definitions of Some Important Terms Pertaining to Coordination Compounds
  • § Exercise 6.3 – Nomenclature of Coordination Compounds
  • § Exercise 6.4 – Isomerism in Coordination Compounds
  • § Exercise 6.5 – Bonding in Coordination Compounds
  • § Exercise 6.6 – Bonding in Metal Carbonyls
  • § Exercise 6.7 – Stability of Coordination Compounds
  • § Exercise 6.8 – Importance and Applications of Coordination Compounds

NCERT Solutions Chemistry 12 Chapter 9 Coordination Compounds

NCERT Solutions Class 12 Chemistry
Chapter 9 Coordination Compounds

Q1. Explain the bonding in coordination compounds in terms of Werner’s postulates.

Q2. 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.

Q3. Explain with two examples each of the following: coordination entity, ligand, coordination number, coordination polyhedron, homoleptic and heteroleptic.

Q4. What is meant by unidentate, bidentate and ambidentate ligands? Give two examples for each.

Q5. Specify the oxidation numbers of the metals in the following coordination entities:
(i) [Co(H2O)(CN)(en)2]2+

(ii) [CoBr2(en)2]+

(iii) [PtCl4]2–

(iv) K3[Fe(CN)6]

(v) [Cr(NH3)3Cl3]  

Q6. Using IUPAC norms write the formulas for the following:
(i) Tetrahydroxidozincate(II)
(ii) Potassium tetrachloridopalladate(II)
(iii) Diamminedichloridoplatinum(II)
(iv) Potassium tetracyanidonickelate(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)

Q7. Using IUPAC norms write the systematic names of the following:

(i) [Co(NH3)6]Cl3

(ii) [Pt(NH3)2Cl(NH2CH3)]Cl

(iii) [Ti(H2O)6]3+

(iv) [Co(NH3)4Cl(NO2)]Cl

(v) [Mn(H2O)6]2+

(vi) [NiCl4]2–

(vii) [Ni(NH3)6]Cl2

(viii) [Co(en)3]3+

(ix) [Ni(CO)4]

Q8.  List various types of isomerism possible for coordination compounds, giving an example of each.

Q9. How many geometrical isomers are possible in the following coordination entities?
(i) [Cr(C2O4)3]3–

(ii) [Co(NH3)3Cl3]

Q10. Draw the structures of optical isomers of:
(i) [Cr(C2O4)3]3–

(ii) [PtCl2(en)2]2+

(iii) [Cr(NH3)2Cl2(en)]+

Q11. Draw all the isomers (geometrical and optical) of:
(i) [CoCl2(en)2]+

(ii) [Co(NH3)Cl(en)2]2+

(iii) [Co(NH3)2Cl2(en)]+

Q12. Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of these will exhibit optical isomers?

Q13. 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

Q14. 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?

Q15. Discuss the nature of bonding in the following coordination entities on the
basis of valence bond theory:
(i) [Fe(CN)6]4–

(ii) [FeF6]3–

(iii) [Co(C2O4)3]3–

(iv) [CoF6]3-

Q16. Draw figure to show the splitting of d orbitals in an octahedral crystal field.

Q17. What is the spectrochemical series? Explain the difference between a weak
field ligand and a strong field ligand.

Q18. What is crystal field splitting energy? How does the magnitude of ∆o decide the actual configuration of d orbitals in a coordination entity?

Q19. [Cr(NH3)6]3+ is paramagnetic while [Ni(CN)4]2– is diamagnetic. Explain why.




Q30. What is the oxidation number of cobalt in K[Co(CO)4]?

Q31. Amongst the following, the most stable complex is
(i) [Fe(H2O)6]3+

(ii) [Fe(NH3)6]3+

(iii) [Fe(C2O4)3]3–

(iv) [FeCl6]3–

Q32. 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+?

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