The decreasing order of electron affinity of halogens is :

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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C l > F > B r > I

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Solution

The correct option is D $C l > F > B r > I$
Electron affinity increases in a period and decreases in a group. But, fluorine atom, due to its small size cannot release high amount of energy. Hence, among halogens, chlorine atom has high value of electron affinity and the order is $C l > F > B r > I$ .

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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 decreasing order of electron affinity is:

F > C l > B r > I

Q. The correct order of polarizability is

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

Q. The electron affinity of halogens are

F - 322, C l - 347, B r - 324, I = 295 k J {m o l}^{- 1}

. The higher value of

C l

as compared to that of

F

is due to:

Q. The decreasing order of electron affinity of

F, C l,

and

B r

is:

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The decreasing order of electron affinity of halogens is :

The correct option is D Cl>F>Br>IElectron affinity increases in a period and decreases in a group. But, fluorine atom, due to its small size cannot release high amount of energy. Hence, among halogens, chlorine atom has high value of electron affinity and the order is Cl>F>Br>I.