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Question

(a) Complete the following equations:
(i) Cr2O27+2OH (ii) MnO4+4H++3e
(b) Account for the following:
(i) Zn is not considered as a transition element.
(ii) Transition metals form a larger number of complexes.
(iii) The E0 value for the Mn3+/Mn2+ couple is much more positive than that for Cr3+/Cr2+ couple.

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Solution

(a) The balanced chemical equation :
(i) Cr2O72+2OH2CrO42+H2O
(ii) MnO4+4H++3eMnO2+2H2O

(b)(i) Zinc has the stable filled valence shell d10 electronic configuration in its ground state as well as in its most common oxidation state of +2. Hence, it is not considered as a transition element.

(ii) Ions formed by transition metals have small sizes and high ionic charges. They possess vacant d-orbitals to accommodate lone pairs of electrons for bond formation. As a result transition metals forms a large number of complexes.

(iii) The Eo value for the Mn+3/Mn2+ couple is more positive than that for Cr3+/Cr2+ couple. This is because Mn2+ ion is particularly stable due to extra stability of its half filled valence electronic configuration(d5). Thus Mn+3 ion has a very high tendency to gain an electron and form the much more stable Mn+2 ion.

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