Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules?

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Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules?

A $Cl_{2} > Br_{2} > F_{2} > I_{2}$
B $Br_{2} > I_{2} > F_{2} > Cl_{2}$
C $F_{2} > Cl_{2} > Br_{2} > I_{2}$
D $I_{2} > Br_{2} > Cl_{2} > F_{2}$

Solution & Step-by-step Explanation

Generally, bond enthalpy decreases down the group. However, F_{2} has an unexpectedly low bond dissociation enthalpy due to the large inter-electronic repulsion between lone pairs on the very small fluorine atoms. The correct order is: Cl_{2} > Br_{2} > F_{2} > I_{2}

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Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules?

Cl_{2} > Br_{2} > F_{2} > I_{2}

Br_{2} > I_{2} > F_{2} > Cl_{2}

F_{2} > Cl_{2} > Br_{2} > I_{2}

I_{2} > Br_{2} > Cl_{2} > F_{2}

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P-Block Elements Halogens

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