Which one of the following is expected to have maximum bond length?

Which one of the following is expected to have maximum bond length?
  1. $\mathrm{NO}^{+}$
  2. $\mathrm{NO}^{2+}$
  3. NO
  4. $\mathrm{NO}^{-}$

Solution

Electronic configuration follows the order $(\sigma 2 \mathrm{~s})(\sigma * 2 \mathrm{~s})\left(\pi 2 \mathrm{p}_{x}ight)\left(\pi 2 \mathrm{p}_{y}ight)\left(\sigma 2 \mathrm{p}_{z}ight)\left(\pi^{*} 2 \mathrm{p}_{x}ight)$
$\mathrm{NO}^{+}$ (Valence electrons=10); Bond order $=(8-2) / 2=3$
$\mathrm{NO}^{2+}$ (Valence electrons=9); Bond order $=(7-2) / 2=2.5$
$\mathrm{NO}$ (Valence electrons=11); Bond order $=(8-3) / 2=2.5$
$\mathrm{NO}^{-}$ (Valence electrons=12); Bond order $=(8-4) / 2=2.0$
Smaller the bond order, larger the bond length. Hence, $\mathrm{NO}^{-}$will having maximum bond length.

Asked in: JEE-TOPICTESTS-CHEMISTRY

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