Short Answer TypeThe (IE1) and IE2 are as follows:
Na (IE1) = 496 kJ mol-1
Na (IE2) = 4562 kJ mol-1
Mg (IE1 = 737 kJ mol-1
Mg (IE2) = 1450 kJ mol-1
In the case of sodium, the second electron is to be removed from Na+ ion which has a stable electronic configuration.
Na+ (Z = 11) = 1s22s22p6 (all occupied orbitals are fully filled, noble gas configuration).
In the case of magnesium, the second electron is to be removed from Mg+ ion which is yet to achieve a noble gas configuration.
Mg+ (Z = 12) = 1s22s2 2p63s1
Therefore, the removal of the second electron from sodium ion is more difficult than from magnesium atom. As a result, the difference is more in sodium than in magnesium atom.
Energy of an electron in the ground state of the hydrogen atom is -2.18 X 10-18J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol-1.
Long Answer TypeShort Answer TypeDiscuss in brief the factors which influence the magnitude of electron gain enthalpy.
The electron gain enthalpy of fluorine has less negative value than that of chlorine while it is expected to be more. Explain.
Explain which of the following will have the most negative electron gain enthalpy and which the least negative: P, S, CI, F.
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