[" 39lonization of energy "F^(-)" is "320kJ/mol" .The electron "],[" gain enthalpy of fluorine is "]

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

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

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

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

Ionisation energy of F is 320 kJ mol^(-1) . The electron affinity of fluorine would be:

Why fluorine has lesser electron gain enthalpy than chlorine?

Calculate the lattice enthalpy of KCl from the following data by Born- Haber's Cycle. Enthalpy of sublimation of K = 89 kJ mol^(–1) Enthalpy of dissociation of Cl = 244 kJ mol^(–1) Ionization enthalpy of potassium = 425 kJ mol^(–1) Electron gain enthalpy of chlorine = –355 kJ mol^(–1) Enthalpy of formation of KCl = –438 kJ mol^(-1)