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NCERT solutions Chemistry Class 12 Part 1 chapter 9 Coordinate Compounds

Chapters

NCERT Solutions for Chemistry Class 12 Part 2

NCERT Chemistry Class 12 Part 1

Chemistry Textbook for Class 12 Part 1

Chapter 9 - Coordinate Compounds

Pages 244 - 256

Write the formulas for the given coordination compounds:

Tetraamminediaquacobalt(III) chloride

Q 1.1 | Page 244

Write the formulas for the given coordination compounds : Potassium tetracyanonickelate(II)

 

Q 1.2 | Page 244

Write the formulas for the given coordination compounds:

Tris(ethane−1,2−diamine) chromium(III) chloride

Q 1.3 | Page 244

Write the formulas for the given coordination compounds: Amminebromidochloridonitrito-N-platinate(II)

Q 1.4 | Page 244

Write the formulas for the given coordination compounds:-

Dichloridobis(ethane−1,2−diamine)platinum(IV) nitrate

 

Q 1.5 | Page 244

Write the formulas for the following coordination compounds:

Iron(III) hexacyanoferrate(II)

Q 1.6 | Page 244

Write the IUPAC names of the following coordination compounds

[Co(NH3)6]Cl3

 

Q 2.1 | Page 244

Write the IUPAC names of the following coordination compounds [Co(NH3)5Cl]Cl2

Q 2.2 | Page 244

Write the IUPAC names of the following coordination compounds : K3[Fe(CN)6]

Q 2.3 | Page 244

Write the IUPAC names of the following coordination compounds: K2[PdCl4]

Q 2.5 | Page 244

Write the IUPAC names of the following coordination compounds

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

Q 2.6 | Page 244

Indicate the types of isomerism exhibited by the following complexes and draw the structures for these isomers: K[Cr(H2O)2(C2O4)2

Q 3.1 | Page 247

Indicate the types of isomerism exhibited by the following complexes and draw the structures for these isomers:

[Co(en)3]Cl3

Q 3.2 | Page 247

Indicate the types of isomerism exhibited by the following complexes and draw the structures for these isomers:

[Co(NH3)5(NO2)](NO3)2

Q 3.3 | Page 247

Indicate the types of isomerism exhibited by the following complexes and draw the structures for these isomers:[Pt(NH3)(H2O)Cl2]

Q 3.4 | Page 247

Give evidence that [Co(NH3)5Cl]SO4 and [Co(NH3)5SO4]Cl are ionization isomers.

Q 4 | Page 247

Explain on the basis of valence bond theory that [Ni(CN)4]2− ion with square planar structure is diamagnetic and the [NiCl4]2− ion with tetrahedral geometry is paramagnetic.

Q 5 | Page 254

[NiCl4]2− is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Why?

Q 6 | Page 254

[Fe(H2O)6]3+ is strongly paramagnetic whereas [Fe(CN)6]3− is weakly paramagnetic. Explain.

Q 7 | Page 254

Explain [Co(NH3)6]3+ is an inner orbital complex whereas [Ni(NH3)6]2+ is an outer orbital complex.

Q 8 | Page 254

Predict the number of unpaired electrons in the square planar [Pt(CN)4]2− ion.

Q 9 | Page 254

The hexaquo manganese(II) ion contains five unpaired electrons, while the hexacyanoion contains only one unpaired electron. Explain using Crystal Field Theory.

Q 10 | Page 254

Calculate the overall complex dissociation equilibrium constant for the Cu(NH3)42+ ion, given that β4 for this complex is 2.1 × 1013.

Q 11 | Page 256

Pages 258 - 260

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

Q 1 | Page 258

FeSO4 solution mixed with (NH4)2SO4 solution in 1:1 molar ratio gives the test of Fe2+ ion but CuSO4solution mixed with aqueous ammonia in 1:4 molar ratio does not give the test of Cu2+ ion. Explain why?

Q 2 | Page 258

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

Q 3 | Page 258

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

Q 4 | Page 258

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

 

Q 5.1 | Page 258

Specify the oxidation numbers of the metals in the following coordination entities: [CoBr2(en)2]+

 

Q 5.2 | Page 258

Specify the oxidation numbers of the metals in the following coordination entities: [PtCl4]2−

Q 5.3 | Page 258

Specify the oxidation numbers of the metals in the following coordination entities: K3[Fe(CN)6]

 

Q 5.4 | Page 258

Specify the oxidation numbers of the metals in the following coordination entities: [Cr(NH3)3Cl3]

Q 5.5 | Page 258

Using IUPAC norms write the formulas for following: Tetrahydroxozincate(II)

Q 6.1 | Page 258

Using IUPAC norms write the formulas for the following: Potassium tetrachloridopalladate(II)

Q 6.2 | Page 258

Using IUPAC norms write the formulas for the following: Diamminedichloridoplatinum(II)

Q 6.3 | Page 258

Write the formula for the following complex:

Pentaamminenitrito-o-Cobalt (III).

Q 6.5 | Page 258

Using IUPAC norms write the formulas for the following: Hexaamaminecobalt(III) sulphate

Q 6.6 | Page 258

Using IUPAC norms write the formulas for the following: Potassium tri(oxalato)chromate(III)

Q 6.7 | Page 258

Using IUPAC norms write the formulas for the following: Tetrabromidocuprate(II)

Q 6.9 | Page 258

Using IUPAC norms write the systematic names of the following: [Co(NH3)6]Cl3

Q 7.1 | Page 258

Using IUPAC norms write the systematic names of the following: [Pt(NH3)2Cl(NH2CH3)]Cl

Q 7.2 | Page 258

Using IUPAC norms write the systematic names of the following: [Ti(H2O)6]3+

Q 7.3 | Page 258

Using IUPAC norms write the systematic names of the following [Co(NH3)4Cl(NO2)]Cl

Q 7.4 | Page 258

Using IUPAC norms write the systematic names of the following - [Mn(H2O)6]2+

Q 7.5 | Page 258

Using IUPAC norms write the systematic names of the following - [NiCl4]2−

Q 7.6 | Page 258

Using IUPAC norms write the systematic names of the following: [Ni(NH3)6]Cl2

Q 7.7 | Page 258

Using IUPAC norms write the systematic names of the following [Co(en)3]3+

Q 7.8 | Page 258

Using IUPAC norms write the systematic names of the following: [Ni(CO)4]

Q 7.9 | Page 258

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

Q 8 | Page 258

How many geometrical isomers are possible in the following coordination entities? 

[Cr(C2O4)3]3−

Q 9.1 | Page 258

How many geometrical isomers are possible in the following coordination entities

[Co(NH3)3Cl3]

Q 9.2 | Page 258

Draw the structures of optical isomers of: [Cr(C2O4)3]3−

Q 10.1 | Page 258

Draw the structures of optical isomers of: [PtCl2(en)2]2+

Q 10.2 | Page 258

Draw the structures of optical isomers of [Cr(NH3)2Cl2(en)]+

Q 10.3 | Page 258

Draw all the isomers (geometrical and optical) of [CoCl2(en)2]

Q 11.1 | Page 259

Draw all the isomers (geometrical and optical) of: [Co(NH3)Cl(en)2]2+

Q 11.2 | Page 259

Draw all the isomers (geometrical and optical) of: [Co(NH3)2Cl2(en)]+

Q 11.3 | Page 259

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

Q 12 | Page 259

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.

Q 13 | Page 259

What is the coordination entity formed when 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?

Q 14 | Page 259

Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:

[Fe(CN)6]4−

Q 15.1 | Page 259

Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:

[FeF6]3−

Q 15.2 | Page 259

Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:

[Co(C2O4)3]3−

Q 15.3 | Page 259

Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:

 [CoF6]3−

Q 15.4 | Page 259

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

Q 16 | Page 259

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

Q 17 | Page 259

What is crystal field splitting energy? How does the magnitude of Δo decide the actual configuration of d-orbitals in a coordination entity?

Q 18 | Page 259

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

Q 19 | Page 259

A solution of [Ni(H2O)6]2+ is green but a solution of [Ni(CN)4]2− is colourless. Explain.

Q 20 | Page 259

[Fe(CN)6]4− and [Fe(H2O)6]2+ are of different colours in dilute solutions. Why?

Q 21 | Page 259

Discuss the nature of bonding in metal carbonyls.

Q 22 | Page 259

Give the oxidation state, d-orbital occupation and coordination number of the central metal ion in the following complexes

K3[Co(C2O4)3]

Q 23.1 | Page 259

Give the oxidation state, d-orbital occupation and coordination number of the central metal ion in the following complexes:

cis-[Cr(en)2Cl2]Cl

Q 23.2 | Page 259

Give the oxidation state, d-orbital occupation and coordination number of the central metal ion in the following complexes:

(NH4)2[CoF4]

Q 23.3 | Page 259

Give the oxidation state, d-orbital occupation and coordination number of the central metal ion in the following complexes:

[Mn(H2O)6]SO4

Q 23.4 | Page 259

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:

K[Cr(H2O)2(C2O4)2].3H2O

Q 24.1 | Page 259

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:

 [Co(NH3)5Cl]Cl2

Q 24.2 | Page 259

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:

CrCl3(py)3

Q 24.3 | Page 259

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

Cs[FeCl4]

Q 24.4 | Page 259

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:

K4[Mn(CN)6]

Q 24.5 | Page 259

What is meant by stability of a coordination compound in solution? State the factors which govern stability of complexes.

Q 25 | Page 259

What is meant by the chelate effect? Give an example.

Q 26 | Page 259

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

Q 27 | Page 259

How many ions are produced from the complex Co(NH3)6Cl2 in solution?

(i) 6

(ii) 4

(iii) 3

(iv) 2

Q 28 | Page 259

Amongst the following ions which one has the highest magnetic moment value?

(i) [Cr(H2O)6]3+

(ii) [Fe(H2O)6]2+

(iii) [Zn(H2O)6]2+

Q 29 | Page 259

The oxidation number of cobalt in K[Co(CO)4] is

(i) +1

(ii) +3

(iii) −1

(iv) −3

Q 30 | Page 259

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−

Q 31 | Page 260

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+

Q 32 | Page 260

NCERT Chemistry Class 12 Part 1

Chemistry Textbook for Class 12 Part 1
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