Which of the following is the increasing order of electron affinity of halogens ?

I < B r < C l < F

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I < B r < F < C l

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F < C l < B r < I

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B r < F < I < C l

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Solution

The correct option is D $I < B r < F < C l$
Electron affinity is the energy released when 1 mole of gaseous atoms each acquire an electron to form an ion. The trend for electron affinity is to decrease but for fluorine it increases. It is the measure of attraction between incoming electron and the nucleus. As the atom gets bigger going down the group the incoming electron feels less attraction and the electron affinity falls. Fluorine atom is small and the existing electron density is high. The repulsion is great and lessens the attraction from the nucleus to lower the electron affinity than chlorine.

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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 is:

F > C l > B r > I

Q. Arrange the following as per the instructions given in the brackets:

C l, F, B r, I

(increasing order of electron affinity)

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:

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