(a) How would you account for the following:
(i) The chemistry of actinoids is more complicated as compared to lanthanoids
(ii) Transition metals form complex compounds
(b) Complete the following equation:
$2 {M n O_{4}}^{-} + 6 H^{+} + S {O_{3}}^{2 -} ⟶$

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Solution

(a) (i) Chemistry of actinoids is more complicated than actinoids because
1) actinoid elements show a variety of oxidation states.
2) they are mostly radioactive (thus, studying their properties) becomes difficult.
3) they are mostly present in small quantities.
4) their half-life is extremely small.
(ii) Transition metals ions form coordination complexes because they have empty valance shell orbitals that can accept pairs of electrons from a Lewis base. Ligands must, therefore, be Lewis bases.

(b) ${2 M n O}_{4}^{-} + 6 H^{+} + 5 O_{3}^{2 -} ⟶ 2 {M n}^{+ 2} + 5 {S O}_{4}^{2 -} + 3 H_{2} O$

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Similar questions

(a) How would you account for the following:

(i) The chemistry of actinoids is more complicated as compared to lanthanoids.

(ii) Transition metals form complex compounds.

(b) Complete the following equation:

$2 {M n O_{4}}^{-} + 6 H^{+} + {S O_{3}}^{2 -} \to$

2 M n O_{4}^{-} + 6 H^{+} + 5 N O_{2}^{-} \to

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M n^{3 +} / M n^{2 +}

C r^{3 +} / C r^{2 +}

(n - 2) f^{1 - 14} (n - 1) d^{0 - 1} n s^{2}

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