Which has higher bond energy and stronger bond?

F_{2}

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C l_{2}

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B r_{2}

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I_{2}

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Solution

The correct option is B $C l_{2}$
Bond dissociation energy
${C l}_{2} > {B r}_{2} > F_{2} \geq I_{2}$
The general trend of bond strength is that it decreases down the group. But, $F_{2}$ shows exceptionally low bond enthalpy.
This is due to the more interelectronic repulsion of the electron on $F_{2}$ (small size) there is a weak bond between $F - F$ , So it is easy to break.

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Similar questions

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

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

{C l}_{2}, {B r}_{2}

I_{2}

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

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

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

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

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

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

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

H O C l > H C l O_{2} > H C l O_{3} > H C l O_{4} :

H O C l > H C l O_{2} > H C l O_{3} > H C l O_{4} :

(x^{2} + y^{2})

x

y

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