Which of the following has an incorrect order of listed properties?

F_{2} > C l_{2} > B r_{2} > I_{2}

: Bond dissociation energy

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F_{2} > C l_{2} > B r_{2} > I_{2}

: Oxidising power

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F > C l > B r > I

: Electron gain enthalpy

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F > C l > B r > I

: Electronegativity

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Solution

The correct option is C $F > C l > B r > I$ : Electron gain enthalpy
The correct order of bond dissociation energy is $C l_{2} > B r_{2} > F_{2} > I_{2}$ because in $F_{2}$ there is more inter-electronic repulsion because of which its bond becomes weak.

Oxidising power $\propto$ electronegativity
Thus the order of oxidising power is $F_{2} > C l_{2} > B r_{2} > I_{2}$

Electron gain enthalpy: The amount of heat released when an extra electron is added.

$electron gain enthaly \propto size \propto inter electronic repulsion$

The electron gain enthalpy of chlorine is greater because of less inter electronic repulsion than florine.
The correct order of electron gain enthalpy is $C l > F > B r > I$

Down the group electronegativity decrease.

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