With respect to halogens, four statements are given below. Which of them is correct?

The bond dissociation energies for halogens is in the order :

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

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The only oxidation state is -1

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The amount of energy required for the excitation of electrons to first excited state decreases progressively as we move from F to 1

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They form

H X_{2}^{-}

species in their aqueous solutions (X=halogen)

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Solution

The correct option is A The bond dissociation energies for halogens is in the order : $I_{2} < F_{2} < B r_{2} < C l_{2}$
The bond dissociation energy of halogens is given in order: $I_{2} < F_{2} < B r_{2} < C l_{2}$ .
The bond dissociation energy decreases down the group, but fluorine shows remarkably small dissociation energy.
In halogens, there are two bonding pair and 3 nonbonding pairs. Because of the small size of fluorine, these non-bonding pairs come closer to each other and repel each other to a maximum extent which causes a decrease in bond strength.

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Similar questions

F_{2}

C l_{2}

F_{2}

C l_{2}

B r_{2}

I_{2}

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

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

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

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