Question

From elementary molecular orbital theory, we can. deduce the electronic configuration of the singly positive nitrogen molecular ion $N_2^+$ as

• A. $\sigma 1s^2, \sigma^*1s^2,\sigma2s^2,\sigma^*2s^2, \pi2p^4, \sigma2p^1$
• B. $\sigma 1s^2, \sigma^*1s^2,\sigma2s^2,\sigma^*2s^2, \sigma2p^1, \sigma2p^3$
• C. $\sigma 1s^2, \sigma^*1s^2,\sigma2s^2,\sigma^*2s^2, \sigma2p^2, \sigma2p^4$
• D. $\sigma 1s^2, \sigma^*1s^2,\sigma2s^2,\sigma^*2s^2, \sigma^*2p^2, \sigma2p^1_x, \sigma2p^2_y$
• E. $\sigma 1s^2, \sigma ^*1s^2, \sigma2s^2,\sigma^*2s^2, \sigma^*2p^2, \pi2p^2_x, \pi2p^2_y, \sigma2p^1_z$

Answer 1

Answer: (E)

$N^+_2$ ion is formed by the removal of one electron from $N_2$ molecule. The electronic configuration of $N^+_2$ ion eill be as: $N^+_2 : \sigma 1s^2, \sigma^*1s^2,\sigma2s^2, \sigma^*2s^2, \pi2p^2_x, \approx\pi2p^2_y,\sigma2p^1_z$