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Electron gain enthalphy is the amount of...

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 ?

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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?

Ionisation energy of F^Ɵ is 320 kJ mol^(-1) . The electron gain enthalpy of fluorine would be

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

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.

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.

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.

Generally electron gain enthalpy increases along a period and decreases down the group. But electron gain enthalpy of oxygen is -141 kJ//mol while that of sulphur is -200 kJ//mol . Explain.

The electron gain ethalpy of chlorine is - 349kJ mol^(-1) . Calculate the energy released when 5.5g of chlorine is converted into Cl^(-) ions in the gaseous state.

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