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Answer: 4. \([SiCl_6]^{2-}\)

Key idea: silicon (period 3) can expand its octahedral coordination, but only with small ligands.

\(\mathrm{[SiF_6]^{2-}}\) is known because the small F atoms fit around Si. \(\mathrm{[GeCl_6]^{2-}}\) and \(\mathrm{[Sn(OH)_6]^{2-}}\) are known because Ge and Sn are larger central atoms that can hold six ligands.

In \(\mathrm{[SiCl_6]^{2-}}\), six large Cl atoms cannot be packed around the small Si atom, and the interaction of Si with the Cl lone pairs is too weak to stabilise the ion. So it is not stable. Option (4).

Doubtly AI · 30 Oct 2026 AI-generated · not yet verified Report
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