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Because the ns² electrons of the valence shell do not readily take part in bonding, which statement is correct?

1. Sn2+ is oxidising, whereas Pb4+ is reducing
2. Both Sn2+ and Pb2+ can act as oxidising as well as reducing agents
3. Sn4+ is reducing, whereas Pb4+ is oxidising
4. Sn2+ is reducing, whereas Pb4+ is oxidising

Correct answer: Sn2+ is reducing, whereas Pb4+ is oxidising

Solution

Because the inert pair effect stabilises the lower oxidation state down the group, Sn2+ tends to be oxidised (a reducing agent) while Pb4+ tends to be reduced (an oxidising agent). So option 3 is correct.

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