Which one of the following has lowest bond dissociation energy?

C l - C l

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F - F

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B r - B r

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I - I

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Solution

The correct option is B $I - I$
$∴$ Lowest bond energy is of $I_{2}$
( $F_{2}$ has unexpectedly low bond dissociation energy due to its small size and high electron-electron repulsion).

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Similar questions

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. 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

Q. The correct order of polarizability is

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

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

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Which one of the following has lowest bond dissociation energy?

The correct option is B I−I∴ Lowest bond energy is of I2(F2 has unexpectedly low bond dissociation energy due to its small size and high electron-electron repulsion).

The correct option is B $I - I$
$∴$ Lowest bond energy is of $I_{2}$
( $F_{2}$ has unexpectedly low bond dissociation energy due to its small size and high electron-electron repulsion).