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d-and F-Block Elements & Coordination Compounds
Study Material
d-and F-Block Elements & Coordination Compounds
Very Short Answer Questions
Q1. What are transition elements? Give examples.
Q2. Which elements of 3d. 4d, and 5d series are not regarded as transition elements and why?
Q3. Why are d-block elements called transition elements?
Q4. Write the general electronic configuration of transition elements.
Q5. In what way is the electronic configuration of transition elements different from non transition elements?
Q6. Write the electronic configuration of chromium $\ce{(Cr)}$ and copper $\ce{(Cu)}$.
Q7. Why do transition elements exhibits characteristic properties?
Q8. Scandium is a transition element. But zinc is not. Why?
Q9. Even though silver has d configuration, it is regarded as transition element. Why?
Q10. Write the electronic configuration of $\ce{Co^{2+}}$ and $\ce{Mn^{2+}}$.
Q11. Why are $\ce{Mn^{2+}}$ compounds more stable than $\ce{Fe^{2+}}$ towards oxidation to their +3 state?
Q12. Which metal in the first series of transition metals exhibits +1 oxidation state most frequently and why?
Q13. Why do transition elements exhibit more than one oxidation state (variable oxidation states)?
Q14. Though Sc is a transition element, it does not exhibit variable oxidation state. Why?
Q15. Why is it difficult to obtain $\ce{M^{3+}}$ oxidation state in Ni, Cu and Zn?
Q16. Why is $\ce{Cr^{2+}}$ reducing and $\ce{Mn^{2+}}$ oxidizing even though both have the same d' electronic configuration.
Q17. Although $\ce{Cr , Mo }$ and $\ce{W}$ belong to the same group (group 6) $\ce{Cr (VI)}$ is a strong oxidizing agent while $\ce{Mo (VI)}$ and $\ce{W (VI)}$ are not. Why?
Q18. What do you infer from the fact that $\ce{M^{3+}/M^{+2}}$ standard electrode potential of Mn is comparatively higher and that of $\ce{Fe}$ is comparatively lower?
Q19. Transition elements have high melting points. Why?
Q20. Among the first transition series (3d series) Chromium has highest melting point. Why?
Q21. Compared to s-block elements, the transition elements exhibit higher enthalpy of atomization. Why?
Q22. Among the first transition series (3d series) zinc has lowest enthalpy of atomization. Why?
Q23. How do you expect the density of transition elements to vary in a given series and why?
Q24. How do the atomic and ionic sizes vary among transition metals in a given series?
Q25. Why do Mn, Ni and Zn exhibit more negative $\ce{E^{\circleddash }}$ values than expected?
Q26. Among the first transition series (3d series) only copper has positive $\ce{E^{\circleddash } M^{2+}/M }$ value. Why?
Q27. $\ce{Cu^{II}}$ forms halides like $\ce{CuF2 , CuCl2}$ and $\ce{CuBr2}$ but not $\ce{Cul2}$. Why?
Q28. The highest Mn fluoride is $\ce{MnF4}$ where as the highest oxide is $\ce{Mn2O7}$. Why?
Q29. In its fluoride or Oxide, in which a transition metal exhibits highest oxidation state and why?
Q30. Why $\ce{Zn^{2+}}$ is diamagnetic whereas $\ce{Mn^{2+}}$ is paramagnetic?
Q31. Write 'spin only' formula to calculate the magnetic moment of transition metal ions.
Q32. Calculate the 'spin only' magnetic moment of Felon.
Q33. What is meant by 'disproportionation? Give an example of disproportionation reaction in aqueous solution.
Q34. Aqueous Cut lons are blue in colour, where as Aqueous $\ce{Zn^{2+}}$ ions are colourless. Why?
Q35. What are complex compounds? Give examples
Q36. Why do the transition metals form a large number of complex compounds?
Q37. How do transition metals exhibit catalytic activity?
Q38. Give two reactions in which transition metals or their compounds acts as catalysts.
Q39. What is an alloy? Give example.
Q40. Why do the transition metals readily form alloys?
Q41. How do the ionic character and acidic nature vary among the oxides of first transition series?
Q42. What is the effect of increasing $\ce{p^{H}}$ on a solution of potassium dichromate?
Q43. Name the oxometal anions of the first series of transition metals in which the metal exhibits the oxidation state equal to its group number.
Q44. Permanganate titrations are carried out in the presence of sulphuric acid but not in presence of hydrochloric acid. Why?
Q45. What is lanthanoid contraction?
Q46. What are the different oxidation states exhibited by the lanthonoids?
Q47. What is mischmetal? Give its composition and uses.
Q48. What is actinoid contraction?
Q49. What are coordination compounds? Give two examples.
Q50. What is a coordination polyhedron?
Q51. What is a double salt? Give example.
Q52. What is the difference between a double salt and a complex compound?
Q54. Give one example each for ionic and neutral ligands.
Q55. How many moles of $\ce{AgCl}$ is precipitated when I mole of $\ce{CoCl3}$ is treated with $\ce{AgNO3}$ solution?
Q56. What is a chelate ligand? Give example.
Q57. What is an ambidentate ligand? Give example.
Q58. $\ce{CuSO4.5H2O}$ is blue in colour where as anhydrous $\ce{CuSO4}$ is colourless. Why?
Q59. $\ce{FeSO4}$ solution mixed with $\ce{(NH4)2SO4}$ solution in $\ce{1:1}$ molar ratio gives the test for $\ce{Fe^{2+}} $ lon but $\ce{CuSO4}$ mixed with aqueous ammonia in $\ce{1:4}$ molar ratio does not give the test of $\ce{Cu^{2+}} $ ion. why?
Q60. How many geometrical isomers are possible in the following coordination entities? (i) $\ce{ [Cr(C2O4)3]^{3-}}$ (ii) $\ce{[Co(NH3)3Cl3]}$
Q61. What is the coordination entity formed when excess of aqueous $\ce{KCN}$ is added to an aqueous solution copper sulphate? Why?
Q62. $\ce{ [Cr(NH3)6]^{3+}}$ is paramagnetic while $\ce{[Ni(CN)4]^{2-}}$, is diamagnetic. Why?
Q63. A solution of $\ce{[Ni(H2O6)]^{2+}}$ is green but a solution of $\ce{[Ni(CN)4]^{2-}}$ is colourless. Why?
Q64. $\ce{[Fe(CN)4]^{2-}}$ and $\ce{[Fe(H2O6)]^{2+}}$ are of different colours in dilute solutions. Why?
Q65. What is the oxidation state of cobalt in (i) $\ce{K[Co(CO)4]}$ and (ii) $\ce{ [Co(NH3)6]^{3+}}$ ?
Q1. Compared to 3d series the corresponding transition metals of 4d and 5d transition series show high enthalpy of atomization. Explain
Q2. Compared to the changes in atomic and lonic sizes of elements of 3d and 4d series, the change in radil of elements of 4d and 5d series is virtually the same. Comment.
Q3. Account for the zero oxidation state of $\ce{Ni}$ and $\ce{Fe}$ in $\ce{[Ni (CO)4]}$ and $\ce{[Fe(CO)5]}$ respectively.
Q4. Why do the transition metal tons exhibit characteristic colours in aqueous solution. Explain giving examples.
Q5. Explain the catalytic action of Iron(III) in the reaction between I' and $\ce{S2O8^{2-}$, lons.
Q6. What are interstitial compounds? How are they formed? Give two examples.
Q7. Write the characteristics of interstitial compounds.
Q8. Write the characteristics properties of transition elements.
Q9. Write down the electronic configuration of $\ce{(i) Cr^{3+} (ii) Cu^{+} (iii) Co^{2+} (iv) Mn^{2+}}$
Q10. What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of their atoms: $\ce{3d^3 3d^5 3d^8 \, \, and\, \, 3d^4}$?
Q11. What is lanthanoid contraction? What are the consequences of lanthanoid contraction?
Q12. How is the variability in oxidation states of transition metals different from that of the non transition metals? Illustrate with examples.
Q13. Describe the preparation of potassium dichromate from iron chromite ore.
Q14. Describe the oxidising action of potassium dichromate and write the ionic equations for its With (i) iodide (ii) iron(II) solution (iii) $\ce{H2S}$ and (iv)Sn(II)
Q15. Describe the preparation of potassium permanganate.
Q16. How does the acidified permanganate solution react with (i) iron (ii) ions (iii) $\ce{SO2}$ and (iv) oxalic acid.Write the ionic equations for the reactions.
Q17. Predict which of the ions, $\ce{Cu^+ , Sc^{3+} , Mn^{2+}, Fe^{2+}}$ are coloured in aqueous solution? Give reasons.
Q18. Compare the stability of +2 oxidation state of the elements of the first transition series.
Q19. Use Hund's rule to derive the electronic configuration of $\ce{Ce^{3+}}$ ton, and calculate Its magnetic moment on the basis of 'spin-only' formula.
Q20. Write down the number of 3d electrons in each of the following ions: $\ce{Ti^{3+}, V^{2+}, Cr^{3+} \,and\,\, Mn^{3+} }$. Indicate how would you expect the five 3d orbitals to be occupied for these hydrated fons (octahedral).
Q21. Explain Werner's theory of coordination compounds with suitable examples.
Q22. Give the geometrical shapes of the following complex entities (i) $\ce{[Co(NH3)6]^{3+}}$ (ii) $\ce{[NI(CO)4]}$ (iii) $\ce{[Pt Cl4] ^{4-}}$ and (iv)$\ce{ [Fe(CN)6]^{4-}}$
Q23. Explain the terms (i) Ligand (ii) Coordination number (iii) Coordination entity(iv) Central metal atom/ion
Q24. Explain the terms (i) Unidentate ligand (ii) bidentate ligand (iii) polydentate ligand and (iv)ambidentate ligand giving one example for each.
Q25. What is meant by chelate effect? Give example.
Q26. Give the oxidation numbers of the central metal atoms in the following complex entities (i) $\ce{[NI(CO)4]}$ (ii) $\ce{[Co(NH3)6]^{3+}}$ (iii) $\ce{ [Fe(CN)6]^{4-}}$ and (iv) $\ce{[Fe(H2O6)]^{2+}}$
Q27. Using IUPAC norms write the formulas for the following: (i) Tetrahydroxozincate(II) (ii) Hexaamminecobalt(III) sulphate (iii) Potassium tetrachloropalladate(II) and (iv) Potassium tri(oxalato) chromate(III)
Q28. Using IUPAC norms write the systematic names of the following: (i) $\ce{[Co(NH3)6] Cl3}$(ii) $\ce{[Pt(NH3)2CI(NH2 CH3)] Cl}$ (iii) $\ce{[Ti(H2O6)]^{3+}}$ and (iv) $\ce{[NiCl4]^{2-}}$
Q29. Explain geometrical isomerism in coordination compounds giving suitable examples.
Q30. What are homoleptic and heteroleptic complexes? Give one example for each.
Q1. Explain giving reasons: (i) Transition metals and many of their compounds show paramagnetic behaviour. (ii) The enthalpies of atomisation of the transition metals are high. (iii) The transition metals generally form coloured compounds. (iv) Transition metals and their many compounds act as good catalysts.
Q2. Describe the preparation of potassium permanganate. How does the acidified permanganate solution react with (1) tron(II) tons (ii) $\ce{SO2}$ and (iii) oxalic acid? Write the ionic equations.
Q3. Compare the chemistry of actinoids with that of the lanthanoids with special reference to: (i) electronic configuration (ii) oxidation state (iii) atomic and ionic sizes and (iv) chemical reactivity
Q4. How would you account for the following: (i) Of the $\ce{d4}$ species, $\ce{Cr^{2+}}$ is strongly reducing while oxidising.manganese(III) is strongly (ii) Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised. (iii) The $\ce{d1}$ configuration is very unstable in ions.
Q5. Give examples and suggest reasons for the following features of the transition metals (i) The lowest oxide of transition metal is basic, the highest is amphoteric/ acidic. (ii) A transition metal exhibits highest oxidation state in oxides and fluorides. (iii) The highest oxidation state is exhibited in oxoanions of a metal
Q6. Compare the chemistry of the actinoids with that of lanthanoids with reference to: (i) electronic configuration (ii) oxidation states and (iii) chemical reactivity
Q7. Explain IUPAC nomenclature of coordination compounds with suitable examples.
Q8. Explain different types of isomerism exhibited by coordination compounds, giving suitable examples.
Q9. Discuss the nature of bonding and magnetic behaviour in the following coordination entities on the basis of valence bond theory (i) $\ce{ [Fe(CN)6]^{4-}}$ (ii) $\ce{ [FeF6]^{3-}}$ (iii) $\ce{ [Co(C2O4)3]^{3-}}$ and (iv) $\ce{ [ CoF6]^{3-}}$
Q10. Sketch the splitting of d orbitals in an octahedral crystal field.
Q11. What is spectrochemical series? Explain the difference between a weak field ligand and a strong field ligand.
Q12. Discuss the nature of bonding in metal carbonyls.
Q13. Explain the applications of coordination compounds in different fields.