Amongst the following, the total number of species which do not exist are:
$S F_{6}, B F_{6}^{3 -}, S F_{4}, O F_{4}, A l F_{6}^{3 -}, P H_{5}, P C l_{5}, N C l_{5}, S C l_{6}$

5

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Solution

The correct option is A $5$
(A) Amongst hexahalides of sulphur, only $S F_{6}$ is exceptionally stable for steric reason. In $S C l_{6}$ , smaller $S$ cannot accommodate six larger $C l^{-}$ ions. $S F_{4}$ also exists.
(B) $P H_{5}$ does not exist as there is a large difference in the energies of $s, p$ and $d$ orbitals of $P$ , and hence, it does not undergo $s p^{3} d$ hybridisation.
(C) $N C l_{5}$ does not exist as there is no empty $d -$ orbital in $N$ . So, it can't expand its octet.
(D) $B F_{6}^{3 -}$ does not exist as there is no vacant $d -$ orbital in $B$ , and hence, it cannot exceed its covalency beyond four.
(E) Oxygen cannot exceed its covalency, as it does not have a d-orbital. Therefore, $O F_{4}$ does not exist.

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Similar questions

S F_{6}

{B F_{6}}^{3 -}

S F_{4}

{A l F_{6}}^{3 -}

P H_{5}

N C l_{5}

S C l_{6}

N C l_{3}, P C l_{3}, P C l_{5}, N C l_{5}, P F_{2}, O F_{4}, O F_{6}

P C I_{5}

N C I_{5}

O F_{4}

O F_{2}

S F_{4}

S F_{6}

P H_{5}

X e H_{4}

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I F_{7}

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P {B r}_{6}^{-}

C l F_{3}

P C l_{6}, N C l_{5}, X e F_{4}, O F_{4}, S H_{2}, T e F_{7}

S F_{4}, B F_{4}^{-}, C l F_{3}, A s F_{3}, P C l_{5}, B r F_{5}, X e F_{4}, S F_{6}

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