![]() ![]() Reason: The decrease in ionization enthalpy down the group from C to Sn is due to increase in atomic size and screening effect of the inner electrons which outweigh the effect of increased nuclear charge. The decrease is very sharp from carbon to silicon while there is a slight increase in the first ionization enthalpy of lead as compared to that of tin. The first ionisation enthalpy decreases steadily on moving down the group from carbon to tin. Reason: Because of greater nuclear charge and smaller size of the atoms of group 14 elements. The first ionisation enthalpies of group 14 elements are higher than those of elements of group 13. ![]() The increase in covalent radius from Silicon onwards is however small due to ineffective shielding of the valence electrons by the intervening d and f orbitals. Reason: It is due to addition of a new energy shells in each succeeding element. Reasons: When we move from group 13 to group 14 within the same period ,the effective nuclear charge increases and hence the covalent radius decreases due to stronger attractive influence of the nucleus on the outer electrons.Ĭovalent radii of group 14 elements regularly increases as we move down the group. The covalent radii of group 14 elements are smaller than those of the elements of group 13. The general valence shell electronic configuration of elements of group 14 is ns 2 np 2 where n is the number of the outermost principal shell. ![]()
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