On the basis of molecular orbital theory, pick out a molecule from the following that does not exist:

He₂⁺

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He₂

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O₂

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H₂⁺

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Solution

The correct option is B
He₂

The electronic configuration of He₂ molecule is (σ1s)² (σ*1s)²

So its bond order = 1/2 (2 - 2) = 0

Since the bond order is zero it indicates that He₂ molecule does not exist.

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Similar questions

Use molecular orbital theory to explain why the Be₂ molecule does not exist.

H e_{2}

Question 19

Which of the following statement is not correct from the view point molecular orbital theory?

(a) $B e_{2}$ is not a stable molecule

(b) $H e_{2}$ is not stable but $H e_{2}^{+}$ is expected to exist.

(d) The order of energies of molecular orbitals in $N_{2}$ molecule is

$σ 2 s < σ^{*} 2 s < σ 2 p_{z} < (π^{*} 2 p_{x} ≃ π^{*} 2 p_{y}) < σ^{*} 2 p_{z}$

H e

H e_{2}

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