Chemical Bonding and Molecular Structure - Result Question 95

####97. Which of the following options represents the correct bond order?

[2015]

(a) O2<O2<O2+

(b) O2>O2<O2+

(c) O2<O2>O2+

(d) O2>O2>O2+

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Solution:

  1. (a) Oxygen molecule (O2) - Total number of electrons =16 and electronic configuration is

$\sigma 1 s^{2}<\sigma^{} 1 s^{2}<\sigma 2 s^{2}<\sigma^{} 2 s^{2}<\sigma 2 p_x^{2}$

$ <\pi 2 p_y^{2}=\pi 2 p_z^{2}<\pi^{} 2 p_y^{1}=\pi^{} 2 p_z^{1} $

Bond order =NbNa2=1062=42=2

O2+ion - Total number of electrons (161)=15.

Electronic configuration

$ \begin{aligned} \sigma 1 s^{2}<\sigma^{} 1 s^{2}<\sigma 2 s^{2} & <\sigma^{} 2 s^{2}<\sigma 2 p_x^{2} \ <\pi 2 p_y^{2} & =\pi 2 p_z^{2}<\pi^{*} 2 p_y^{1} \end{aligned} $

Bond order =NbNa2=1052=52=212

O2(Super oxide ion) Total number of electrons (16+1)=17. Electronic configuration

$ \begin{aligned} \sigma 1 s^{2}<\sigma^{} 1 s^{2} & <\sigma 2 s^{2}<\sigma^{} 2 s^{2}<\sigma 2 p_x^{2} \ & <\pi 2 p_y^{2}=\pi 2 p_z^{2}<\pi^{} 2 p_y^{2}=\pi^{} 2 p_z^{1} \end{aligned} $

Bond order =(NbNa)2=1072=32=112



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