Which of the following arrangement of bond dissociation enthalpy of halogens is correct?

F - F > C l - C l > B r - B r

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F - F < C l - C l < B r - B r

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F - F > C l - C l < B r - B r

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F - F < C l - C l > B r - B r

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Solution

The correct option is B $F - F < C l - C l > B r - B r$
Bond energy is inversely dependent on bond length. The order of bond length is $B r_{2} > C l_{2} > F_{2} .$ .

Hence, the order of bond energy should be $B r_{2} < C l_{2} < F_{2} .$ . But, bond dissociation enthalpy of $F_{2}$ is less than $C l_{2}$ because of small size of $F_{2}$ and large inter-electronic repulsions.

Thus, order of bond energy is $C l_{2} > F_{2}$ and $B r_{2} < C l_{2}$ .

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Similar questions

Among halogens, the correct order of amount of energy released in electron gain (electron gain enthalpy ) is
(a) F > Cl > Br > I (b) F < Cl < Br < I (c) F < Cl > Br > I (d) F < Cl < Br < I

Q. The correct order of polarizability is

I^{-}, B r^{-}, C l^{-}, F^{-}

Q. The decreasing order of electron affinity of

F, C l, B r i s F > C l > B r

Q. Which of the following options does not give to the correct trends indicated against it?
(I)

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

: Bond dissociation energy
(II)

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

: Oxidizing nature
(III)

C l > F > B r > I

: Electron gain enthalpy
(IV)

F > C l > B r > I

: Electronegativity

Q. Arrange the following bonds according to their average bond energies in descending order:

C - C l, C - B r, C - F, C - I

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