Question

The correct statement with regard to H₂⁺ and H₂⁻ is
(a) Both H₂⁺ and H₂⁻ do not exist
(b) H₂⁻ is more stable than H₂⁺
(c) H₂⁺ is more stable than H₂⁻
(d) Both H₂⁺ and H₂⁻ are equally stable

Answer 1

Answer:

(d) Both H₂⁺ and H₂⁻ are equally stable

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Answer 2

The correct statement with regard to H₂⁺ and H₂⁻ is :

• Bond order = Nb - Na / 2

where, Nb = electrons present in bonding molecular orbital

Na = electrons present in anti-bonding molecular orbital

• For H₂⁺,

Electronic configuration = σ(1s^1)

Bond order = 1 - 0 / 2 = 0.5

One unpaired electron is present making H₂⁺ paramagnetic.

• For H₂⁻,

Electronic configuration = σ(1s²)σ*(1s^1)

Bond order = 2 - 1 / 2 = 0.5

One unpaired electron is present making H₂⁻ also paramagnetic.

• H₂⁺ is more stable than H₂⁻ because in H₂⁺ last electron is present in bonding molecular orbital while in H₂⁻ last electron is present in anti-bonding molecular orbital.