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The electron affinities of halogens are ...

The electron affinities of halogens are `F=322, Cl=349,Be=324,I=295kJ mol^(-1)`. The higher value for `Cl` as compared to that of `F` is due to

A

Weaker electron-electron repulsion in Cl

B

Higher atomic radius of F

C

Higher atomic radius of F

D

More vacant p-subshell in Cl

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The correct Answer is:
A
Due to high electronegativity value and small size of F , its not easy to add the electron as compared to the Cl . Cl is less electronegative and large in size as compare to the F hence addition of `e^(-)` takes place easily. Therefore high electron affinity value.
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The amount of energy released when an electron is added to an isolated gaseous atom to produce a monovalent anion is called electron affinity of first electron affinity or electron gain enthalpy. The first electron affinity is given a negative sign as the addition of an electron to a neutral atom is an exoergic process. The addition of electron to A^(-) requires energy to overcome the force of repulsion. Thus, the second electron affinity is an endoergic process. The magnitude of electron affinity depends on a number of factors such as (i) atomic size (ii) effective nuclear charge (iii) screening effects (iv) half and fully filled orbitals and (v) shape of orbital. In general, electron affinity increase as the atomic radii decrease in a period. However, there are exceptions when the atoms have stable configuration. In a group, electron affinity decreases as the size increases. However, the members of 3rd period have somewhat higher values than the members in the 2nd period of the same subgroups. The electron affinities of halogens are: F =- 332, CI =- 349, Br =- 324,I =- 295 kJ mol^(-1) The higher value of CI as compared to that of F^(-) is due to:

The electron gain enthalpies of halogens are as given below: F =- 332, CI =- 349, Br =- 324, I =- 295 kJ mol^(-1) . The less negative value for F as compared to that of CI is due to:

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The electron affinity values of element A, C and D are respectively -135,-60,-200 and -348 kJ mol^(-1) . The outer electronic configuration of element B is

The bond dissociation energy of -F in BF_(3) is 646 kJ mol^(-1) whereas that of C-F in CF_(4) is 515kJ mol^(-1) . The correct reason for higher B-F bond dissociation energy as compared to that of C-F is

ERRORLESS-CLASSFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES -NCERT BASED QUESTIONS (Electron Affinity)
  1. Which one of the following statements is false

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  2. The electron affinity for the inert gases is

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  3. The electronic configuration of the element with maximum electron affi...

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  4. Which of the following has the least electron affinity in kJ mol^(-1)?

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  5. Fluorine has lower electron affinity than chlorine because of

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  6. Which of the following species has the highest electron affinit...

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  7. Which of the following species has the highest electron affinit...

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  8. Which one of the elements has the maximum electron affinity?

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  9. Order of electron affinity of F,Cl,Br and I is

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  10. Which one of the following ionic species has the greatest proton affin...

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  11. The electron affinity of Be is almost similar to that of

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  12. The element with positive electron gain enthalpy is

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  13. Arrange S,O and Se in ascending order of electron affinity?

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  14. The energy evolved is highest for which of the following reactions

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  15. Increasing order of electron affinity is

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  16. The correct order of electron affinity of B, C, N, O is

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  17. The electron affinities of halogens are F=322, Cl=349,Be=324,I=295kJ m...

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  18. The electron gain enthalpy values (in kJ mol^(-1) ) of three halogens,...

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  19. Which of the following pairs show reverse properties on moving along a...

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  20. the amount of energy released when 10^(6) atoms of iodine in vapour st...

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