Question

1. Explain the following phenomena on the basis of electron configurations. Be detailed and specific. a)...

1. Explain the following phenomena on the basis of electron configurations. Be detailed and specific.

a) Tin and lead both form stable +2 and +4 ions.

b) Iron and ruthenium both form stable +3 ions.

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Answer #1

a) Tin and lead belongs to 14th group and have the general valence electronic configuration of [Noble gas]ns2 np2. Due to presence of 4 valence electrons they shows +4 oxidation state by loosing all ns and np electrons. In +4 state they are stable due to noble gas configuration. They also show +2 oxidation state by loosing only np2 electrons. The formation of stable +2 electronic configuration is due to inert pair effect of ns2 electrons

b) Iron and Ruthenium belongs to 8th group and general valence shell configuration of [Noble gas] 3d6 4s2. These two elements can show stable +3 oxidation state by loosing 2 electrons form 4s2 orbital and one electron from 3d orbital and form a stable half filled stable electronic configuration of 3d5

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