Question:
Identify the species, which does not exist
Identify the species, which does not exist
Show Hint
Small central atoms like silicon can form stable hexacoordinate complexes with small ligands such as \(F^-\), but not with larger ligands such as \(Cl^-\).
Updated On: Jun 22, 2026
- \([SiF_6]^{2-}\)
- \([SiCl_6]^{2-}\)
- \([GeCl_6]^{2-}\)
- \([Sn(OH)_6]^{2-}\)
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The Correct Option is B
Solution and Explanation
Step 1: Understand the stability of hexacoordinate silicon complexes.
Silicon can form hexacoordinate complexes with small and highly electronegative ligands like fluoride.
Therefore, \[ [SiF_6]^{2-} \] exists as hexafluorosilicate ion.
Step 2: Analyze \([SiCl_6]^{2-}\).
Chloride ion is much larger than fluoride ion.
Due to the large size of \(Cl^-\), six chloride ions cannot be accommodated comfortably around small silicon atom.
Thus, \[ [SiCl_6]^{2-} \] does not exist.
Step 3: Analyze the remaining species.
Germanium is larger than silicon, so it can form \[ [GeCl_6]^{2-} \] Tin is still larger and forms stable hydroxo complexes such as \[ [Sn(OH)_6]^{2-} \] Hence, these species can exist.
Step 4: Final conclusion.
Therefore, the species which does not exist is \[ \boxed{[SiCl_6]^{2-}} \]
Silicon can form hexacoordinate complexes with small and highly electronegative ligands like fluoride.
Therefore, \[ [SiF_6]^{2-} \] exists as hexafluorosilicate ion.
Step 2: Analyze \([SiCl_6]^{2-}\).
Chloride ion is much larger than fluoride ion.
Due to the large size of \(Cl^-\), six chloride ions cannot be accommodated comfortably around small silicon atom.
Thus, \[ [SiCl_6]^{2-} \] does not exist.
Step 3: Analyze the remaining species.
Germanium is larger than silicon, so it can form \[ [GeCl_6]^{2-} \] Tin is still larger and forms stable hydroxo complexes such as \[ [Sn(OH)_6]^{2-} \] Hence, these species can exist.
Step 4: Final conclusion.
Therefore, the species which does not exist is \[ \boxed{[SiCl_6]^{2-}} \]
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