The molecular electronic configuration of $H_{2}^{-}$ ion is:

(σ 1 s)^{2}

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(σ 1 s)^{2} (σ^{*} 1 s)^{2}

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(σ 1 s)^{2} (σ^{*} 1 s)^{1}

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(σ 1 s)^{3}

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Solution

The correct option is C $(σ 1 s)^{2} (σ^{} 1 s)^{1}$
Total number of electrons in $H_{2}^{-}$ are 3 so, we can assume that the $H_{2}^{-}$ molecule is formed by the combination of $H$ and $H^{-}$ atoms. Therefore, electronic configuration is $1 s^{2} 1 s^{1}$ .

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The molecular electronic configuration of H−2 ion is:

The correct option is C (σ1s)2(σ∗1s)1Total number of electrons in H−2 are 3 so, we can assume that the H−2 molecule is formed by the combination of H and H− atoms. Therefore, electronic configuration is 1s2∗1s1.

The molecular electronic configuration of $H_{2}^{-}$ ion is:

The correct option is C $(σ 1 s)^{2} (σ^{} 1 s)^{1}$
Total number of electrons in $H_{2}^{-}$ are 3 so, we can assume that the $H_{2}^{-}$ molecule is formed by the combination of $H$ and $H^{-}$ atoms. Therefore, electronic configuration is $1 s^{2} 1 s^{1}$ .