"Removal of electron becomes easier on moving down the group".
Comment on the statement based on ionisation enthalpy.

Removal of electron becomes easier on moving down the group. a) Comment the above statement based on ionization enthalpy. b) How electronic configuration influences the ionization enthalpy value?

"Removal of electron becomes easier on moving down the group". What is the relevance of half-filled and fully filled sub-levels in I.E determination?

Ions having same number of electrons are called isoelectronic ions. Out of Na^+ and Ne which has higher ionisation enthalpy. Explain why?

Analyse the following statements and correct them if there is a mistake. Down the group in .a periodic table ionisation energy decreases electronegativity increases.

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.

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.

Eventhough the first element in the periodic table is Hydrogen, it does not have a fixed position in the periodic table. Comment on this statement. Outline the similarities of hydrogen with the first group element as well as the Halogen family.

Discuss the general characteristics of Group 15 elements with reference to their electronic configuration, oxidation state, atomic size, Ionisation, enthalpy, and electronegativity.