What is the significance of the terms - isolated gaseous atom and ground state while defining the ionization enthalpy and electron gain enthalpy?

Second electron gain enthalpy Is ͟ ͟ ͟͟͟

Which of the following has largest negative electron gain enthalpy?

The formation of chemical compounds takes place as a result of combination of atoms of various elements. Explain how ionization enthalpy (I.E) and electron gain enthalpy (E.G.E) determine whether atoms of elements will combine to form ionic compounds.

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 ?

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?

Justify the following: 'Ne' has positive value for electron gain enthalpy.

The energy released during the addition of an electron to an isolated neutral atom is called electron gain enthalpy. a) Explain how electron gain enthalpy differ from electronegativity. b) The second ionisation enthalpy of an element is always greater than the first ionisation enthalpy. Give reason.