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Question

The stability of dihalides of Si,Ge.Sn, and Pb increases steadily in the sequence :

A
GeX2<SiX2<SnX2<PbX2
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B
SiX2<GeX2<<PbX2<SnX2
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C
SiX2<GeX2<SnX2<PbX2
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D
PbX2<GeX2<SnX2<SiX2
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Solution

The correct option is B SiX2<GeX2<SnX2<PbX2
Due to the inert pair effect, the stability of M2+ ions (of group IV elements) increases as we go down the group. The stability of dihalides increases down the group: SiX2<GeX2<SnX2<PbX2
Hence, correct option is c.

THEORY
Stability of halides:
GeX4 is more stable than GeX2, but PbX2 is more stable than PbX4.
Heavier members Ge to Pb are able to make halides of formula MX2. The stability of dihalides increases down the group.
Except for CCl4 tetra-chlorides are easily hydrolysed by water. The central atom can accommodate the lone pair of electrons from the oxygen atom of water molecules in d orbital.
Hydrolysis of SiCl4:

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