Which of the following is not correct regarding bond energies

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The F₂ molecule it self has a notoriously weak bond 159KJ mole^–1 compared with chlorine 243 KJ mole^–1

The extent of overlap of the atomic orbitals decreases as the size of the atoms increase

According to Mulliken pπ – π bonding is not possible in fluorine

Among the halogens the bond energy of F₂ is abnormally high (159 KJ mole^–1)

answer is B.

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Detailed Solution

Bond dissociation energy of halogen family decreases down the group as the size of atom increases.
The decreasing order for the bond dissociation enthalpy of halogen molecules is Cl₂57 kcal/mol > Br₂ 45.5 kcal/mol >F₂38 kcal/mol >I₂ 35.6 kcal/mol.
A halogen molecule having larger atoms should have low dissociation energy and vice versa.
Fluorine is an exception because of interelectronic repulsion is present in small atom fluorine.

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