According to molecular orbital theory, which of the following will not be a viable molecule ?

Question

According to molecular orbital theory, which of the following will not be a viable molecule ? (A) H2+2 (B) H+2 (C) H-2 (D) H2-2

Tardigrade Admin · Accepted Answer

Electronic configuration of H 2 2-=(σ s 2)(σ* s 2) Bond order of H 22 ominus=( N b - N a /2)=(2-2/2)=0. If a bond order of zero is obtained, that means that the molecule is too unstable and so it will not exist. Hence, H 22 ominus does not exit, due to zero bond order.

Q. According to molecular orbital theory, which of the following will not be a viable molecule ?

$H_{2}^{2 +}$

$H_{2}^{+}$

$H_{2}^{-}$

$H_{2}^{2 -}$

Q. According to molecular orbital theory, which of the following will not be a viable molecule ?

H22+​

H2+​

H2−​

H22−​

Electronic configuration of H2​2−=(σs2)(σ∗s2) Bond order of H22⊖​=2Nb​−Na​​=22−2​=0. If a bond order of zero is obtained, that means that the molecule is too unstable and so it will not exist. Hence, H22⊖​ does not exit, due to zero bond order.

$H_{2}^{2 +}$

$H_{2}^{+}$

$H_{2}^{-}$

$H_{2}^{2 -}$