Which of the following species have only one type of bond length?

A s F_{3}

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A s F_{4}^{-}

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A s F_{4}^{+}

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A s F_{6}^{-}

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Solution

The correct options are
A $A s F_{3}$
C $A s F_{4}^{+}$
D $A s F_{6}^{-}$
A) $A s F_{3}$ is trigonal pyramidal, where all $F$ atoms are present in axial position. So, all bond lengths are equal.
B) The shape of $A s F_{4}^{-}$ is See-saw. So, two axial bonds are longer than the two equitorial bonds.
C) $A s F_{4}^{+}$ is tetrahedral in shape. All bond lengths are equal.
d) $A s F_{6}^{-}$ is octahedral in shape. All bond lengths are equal to each other in a octahedral.

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Similar questions

{C l F}_{3}

C I F_{3} + A s F_{3} ⟶ [C l F_{2}]^{+} [A s F_{4}]^{-}

C l F_{3} + N O F . . . \to [N O]^{+} [C l F_{4}]^{-}

What is the hybridisation in $A s F_{4}^{-}$ ion :

O_{2} [A s F_{4}]

N - O

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