The ionization enthalpy of sulphur is `1014 kJ mol^(-1)`. If its electronegativity is 2.4, what is its electron gain enthalpy?

The ionisation enthalpy of sulphur is "1014kJmol"^(-1) . If its electronegativity is 2.4, what is its electron gain enthalpy?

If the electron gain enthalpy of S and Se are -200 KJ " mol"^(-1) and -195 KJ " mol"^(-1) respectively. Wha is the electron gain enthalpy of O atom?

Use the following data to calculate Delta_("lattice") H^(@) for NaBr. Delta_("sub")H^(@) for sodium metal =108.4 kJ mol^(-1) , ionization enthalpy of sodium =496 kJ mol^(-1) ., electron gain enthalpy of bromine =-325 kJ mol^(-1) bond dissociation enthalpy of bromine =192 kJ mol^(-1) , Delta _f H^(@) for NaBr(s) - 360 kJ mol^(-1) .

The formation of O^(2-)(g) startng from O(g) is endothermic by 603 kJ mol^(-1) . If electron gain enthalpy of O(g) is -141 kJ mol^(-1) , the second electron gain enthalpy of oxygen would be :

Explain the terms ionization enthalpy and electron gain enthalpy.