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Question

The correct order of increasing bond angles in
the following triatomic species is :

A
$NO_{2}^{+}< NO_{2}
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B
$NO_{2}^{+}< NO_{2}^{-}
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C
$NO_{2}^{-}
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D
$NO_{2}^{-}< NO_{2}
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Solution

The correct option is D $NO_{2}^{-}< NO_{2}
NO+2 has no unpaired electrons. Hence, it will be linear i.e. bond angle is 1800
NO2 has one unpaired electron pair which causes repulsion due to which bond angle decreases to 1320.
NO+2 has one unpaired electron pair which causes repulsion due to which bond pairs becomes more close and thus decreases the bond angle of 1150
Hence, order of bond angles is
NO2<NO2<N+2

972841_70286_ans_ed4efa9039144528adbe9dc15c189c84.jpg

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