Arrange the following in the order of leaving group ability.
$F^{-}, C l^{-}, B r^{-}, I^{-}$

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

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

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F^{-} < C l^{-} < B r^{-} > I^{-}

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F^{-} < C l^{-} > B r^{-} < I^{-}

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Solution

The correct option is C $F^{-} < C l^{-} < B r^{-} > I^{-}$
The increasing order of the leaving group ability in a $S N_{2}$ reaction is $F^{-} < C l^{-} < B r^{-} < I^{-}$ .
Large-sized iodide ion can easily accommodate negative charge. Hence it is a good leaving group.
On the other hand, small-sized fluoride ion cannot easily accommodate negative charge due to greater interelectronic repulsions. Hence, fluoride ion is a poor leaving group.

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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

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. 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. For the species

(I^{-}, C l^{-}, B r^{-})

, the increasing order of nucleophilicity in water would be:

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Arrange the following in the order of leaving group ability.F−, Cl−, Br−, I−

Arrange the following in the order of leaving group ability.
$F^{-}, C l^{-}, B r^{-}, I^{-}$