In which one of the following pairs does the two species have identical shape but differ in hybridization?

I_{3}^{-}, B e {C l}_{2}

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N H_{3}, B F_{3}

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X e F_{2}, I_{3}^{-}

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N H_{4}^{+}, S F_{4}

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Solution

The correct option is A $I_{3}^{-}, B e {C l}_{2}$
Both $I {_{3}}^{-}$ and $B e C l_{2}$ are linear in shape.
The ion is linear and symmetrical. According to VSEPR theory, the central iodine atom has three equatorial lone pairs and the terminal iodines are bonded axially in a linear fashion due to the three lone pairs bonding to the central iodine atom.

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N H_{3}, H_{2} S, C O_{2}, I_{3}^{-}, X e F_{2}, B e C l_{2}, I C l_{2}^{+}, X e F_{4}, X e O_{4}, C_{3} O_{2}

T e F_{5}^{-},

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In which of the following pairs of molecules,the species have identical shape but differ in hybridisation

N I_{3}

I_{3}^{-}

S O_{3}^{2 -}

N O_{3}^{-}

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