Which one of the following species will have maximum bond dissociation energy?

A
$C_{2}$
B
$C_{2}^{+}$
C
$C_{2}^{-}$
D
$C_{2}^{2^{-}}$

Solution:

$C_{2}$ (8 electrons); $KK (σ 2 s)^{2} (σ * 2 s)^{2} {(π * 2 p_{x})}^{2} {(π 2 p_{y})}^{2}$ Bond order $= (6 - 2) / 2 = 2$

$C_{2}^{+}$ (7 electrons); Bond order $= (5 - 2) / 2 = 11 / 2$

$C_{2}^{-}$ (9 electrons); $KK (σ 2 s)^{2} (σ * 2 s)^{2} {(π 2 p_{x})}^{2} {(π 2 p_{y})}^{2} {(σ 2 p_{y})}^{1}$ Bond order $= (7 - 2) / 2 = 2 \frac{1}{2}$

$C_{2}^{2 -}$ -(10 electrons); Bond order $= (8 - 2) / 2 = 3$

Larger the bond order, larger the dissociation energy.

Solution:

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