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:

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 affinities of halogens are: F=332, CI =439, Br=324, I=295 kJ mol^(-1) . The higher value for Cl as compared to that of F is due to

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

The electron affinity of halogens are F=322 Cl=349 Br=324,I=295kJ mol^-1 the higher value for Cl as compared to that of F is due to

Electron gain enthalpy is F is less negative than Cl Why ?

Electron gain enthalphy is the amount of energy involved when an isolated gaseous atom accepts an electron to form a monovalent anion the value of the electron gain enthalpy of halogens are given below: F : -328 KJ mol^(-1) Cl - 349 KJ mol^(-1) Br : -325 KJ mol^(-1) I : -295 KJ mol^(-1) Why the negative electron gain enthalpy decreases from chlorine iodine?

Electron gain enthalphy is the amount of energy involved when an isolated gaseous atom accepts an electron to form a monovalent anion the value of the electron gain enthalpy of halogens are given below: F : -328 KJ mol^(-1) Cl - 349 KJ mol^(-1) Br : -325 KJ mol^(-1) I : -295 KJ mol^(-1)Chlorine has more negative electron gain enthalpy than fluorine. why ?