Question

Mark the incorrect statement in the following
(a) The bond order in the species O₂, O₂⁺ and O₂⁻
decreases as O₂⁺ > O₂ > O₂⁻
(b) The bond energy in a diatomic molecule always
increases when an electron is lost
(c) Electrons in antibonding M.O. contribute to repulsion
between two atoms.
(d) With increase in bond order, bond length decreases
and bond strength increases.

Answer 1

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Option [B] is correct

Answer 2

The bond energy in a diatomic molecule always increases when an electron is lost is the incorrect option given here.

Explanation:

• The bond order of the species that are given in the 1st option should be calculated.

• Bond order of O2+ is 2.5, that of O2 is 2 and of O2- is 1.5.

• So bond order is in the  O₂⁺ > O₂ > O₂⁻ format and is correctly given in option.

• Electrons of antibonding orbitals actually have energy to nullify the energy created by electrons of bonding orbitals.

• So they repulse the atoms away from each other and that is why a molecule with more electrons in antibonding orbitals cannot exist.

• With increase in bond order, the bond length of the molecule decrease and hence, they have more bond strength and bond energy.

• But with an electron lost, if the electron is lost from bonding orbital, the bond strength decrease and if it's lost from antibonding orbital, the bond strength increase.

• So the option 2 is incorrect.

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