Question

Which one of the following is unstable
CCl2
SiCl2
SnCl2
PbCl2​

Answer 1

Pbcl2

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Answer 2

Answer:

d) PbCI2 is the right answer of this question

Explanation:

This can be explained on the basis of stability of lower oxidation states down the groups. When we move down the group, the lower oxidation states become more stable due to the inert pair effect, according to which due to poor shielding of d and f orbitals the valence orbital electrons don't participate in bonding.

In case of PbCl4, Pb is in (+4) oxidation state while in PbCl2 it is in (+2) oxidation state. Due to inert pair effect +2 oxidation state of Pb is more stable than +4 . But in case of Sn it's +4 oxidation state is more stable than +2 oxidation state.

Thus, PbCl4 is less stable than SnCl4, while PbCl2 is more stable than SnCl2.

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