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

Define electronegativity. How does it differ from electron gain enthalpy ?

The ionization enthalpy of Na^+ formation from Nad is 495.8 kJ mol^(-1) , while the electron gain enthalpy of Bris -325.0 kJ mol^(-1) .Given the lattice enthalpy of NaBr is -728.4 kJ mol^(-1) The energy for the formation of NaBr ionic solid is (-)"______" xx 10^(-1)kJ "mol"^(-1)

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) .

Explain the terms ionization enthalpy and electron gain enthalpy.