(a) Write the electronic configuration of Ce3+ ion, and calculate the magnetic moment on the basis of ‘spin-only’ formula. [Atomic No. of Ce = 58] (b) Account for the following: (i) Thf enthalpies of atomisation of the transition metals are high. (ii) The lowest oxide of a transition metal is basic, the highest is amphoteric/ acidic. (iii) Cobalt (II) is stable in aqueous solution but in the presence of complexing agents, it is easily oxidised.

(a) Write the electronic configuration of Ce3+ ion, and calculate the magnetic moment on the basis of ‘spin-only’ formula. [Atomic No. of Ce = 58] (b) Account for the following: (i) Thf enthalpies of atomisation of the transition metals are high. (ii) The lowest oxide of a transition metal is basic, the highest is amphoteric/ acidic. (iii) Cobalt (II) is stable in aqueous solution but in the presence of complexing agents, it is easily oxidised.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter8: Bonding In Transition Metal Compounds And Coordination Complexes

Section: Chapter Questions

Problem 73AP

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(a) Calculate the number of unpaired electrons in the following gaseous state ions: Mn2+, Cr3+, V3+ and Fe2+ which one of these in the most stable in aqueous solutions? (At. nos. V = 23, Cr = 24, Mn = 25, Fe = 26) (b) Explain the following observations: (i) The transition metal ions are usually coloured in aqueous solutions. (ii) Cu(I) is not stable in an aqueous solution. (iii) The highest oxidation state of a transition metal is exhibited in its oxide or fluoride.
State reasons for the following observations: (i) The enthalpies of atomisation of transition elements are quite high. (ii) There is a greater horizontal similarity in the properties of the transition elements than of the main group elements.
Account for the following: (a) (i) Transition elements form interstitial compounds. (ii) Mns+(3d4) is strongly oxidising, whereas Cr2+(3d4) is strongly reducing. (iii) Transition metals have high melting points. (b) What is misch metal? Write its one use.
How would you account for the following :(i) Among lanthanoids, Ln (III) compounds are predominant. However, occasionally in solutions or in solid compounds, + 2 and + 4 ions are also obtained.(ii) The E°M2+/M for copper is positive (0.34 V).Copper is the only metal in the first series of transition elements showing this behaviour.(iii) The metallic radii of the third (5d) series of transition metals are nearly the same as those of the corresponding members of the second series.
How would you account for the following: (i) Among lanthanoids, Ln(III) compounds are predominant. However, occasionally in solutions or in solid compounds, +2 and +4 ions are also obtained. (ii) The E°M2+/M for copper is positive (0.34V). Copper is the only metal in the first series of transition elements showing this behaviour. (iii) The metallic radii of the third (5d) series of transition metals are nearly the same as those of the corresponding members of the second series.
Explain the ways in which the elements act: (a) How do you explain that fluoride, a small anion, is responsible for a weak field while water, a neutral molecule, gives rise to a much stronger binding field? (b) Explain why, for the same metallic cation and the same ligands, the energy of the binding field is lower in tetrahedral compounds than in octahedral compounds.
Explain the following observations giving appropriate reasons: (i) The stability of +5 oxidation state decreases down the group in group 15 of the periodic table. (ii) Solid phosphorus pentachloride behaves as an ionic compound. (iii) Halogens are strong oxidizing agents.
Write the general electron configuration of a transition ele-ment (a) in Period 5; (b) in Period 6.
Explain the following observations: (i) Many of the transition elements are known to form interstitial compounds. (ii) There is a general increase in density from titanium (Z = 22) to copper (Z = 29). (iii) The members of the actinoid series exhibit a larger number of oxidation states than the corresponding members of the lanthanoid series.
Explain the following observations :(i) Copper atom has completely filled d orbitals (3d10) in its ground state, yet it is regarded as a transition element.(ii) Cr2+ is a stronger reducing agent than Fe2+ in aqueous solutions.
(a) What is the range in electronegativity across the first (3d)transition series? (b) What is the range across Period 4 of main-group elements? (c) Explain the difference.
Assign a reason for each of the following observations:(i) The transition metals (with the exception of Zn, Cd and Hg) are hard and have high melting and boiling points.(ii) The ionization enthalpies (first and second) in the first series of the transition elements are found to vary irregularly.