The electron gain enthalpy values of halogens become more negative in the order:
`F gt C l gt B rgt I`
Comment on the statement.

Would you expect the second electron gain enthalpy O as positive, more negative or less negative than the first ? Justify your answer.

The amount of energy released when an electron is gained by an isolated gaseous atom, is electron gain enthalpy (E.A). E.A values of some halogens are given below: [349 KJ//mol, 295 KJ//mol, 328 KJ//mol and 325 KJ//mol] Supply the values for corresponding halogen based on the trend of E.A in group.

Assertion : F atom has a less negative election gain enthalpy than Cl atom. Reason : Additional electrons are repelled more effectively by 3p electrons in Cl atom than by 2p electrons in F-atom.

The amount of energy released when an electron is gained by an isolated gaseous atom, is electron gain enthalpy (E.A). E.A values of some halogens are given below: [349 KJ//mol, 295 KJ//mol, 328 KJ//mol and 325 KJ//mol] Draw a graph by taking E.A along y axis and atomic number along X axis.

a) On moving down a group what happens to electron gain enthalpy? b) Why chlorine shows more negative electron gain enthalpy than fluorine?

Chlorine has the most negative electron gain enthalpy'. Justify the statement.

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 ?

The variation in electron gain enthalpies of elements is less systematic than for ionization enthalpies. Out of oxygen and sulphurwhich has greater negative value for electron gain enthalpy? Justify.

"Removal of electron becomes easier on moving down the group". Comment on the statement based on ionisation enthalpy.