Which of the following I a correct statement?

Options

A. The firstand second ionization enthalpies of group elementsare greater than those of group 1 elements
B. the first and second ionization enthalpies of group elementsare smaller than those of group 1 elements
C. the first ionization enthalpy of group 2 element greater but he second ionization enthalpy issmall than those of group 1 elements.
D. The first ionization enthalpy of group 2 elements smaller but the seconds but the seconds ionization enthalpy is greater that those of group 1 elements.

Answer

C

Explanation

As such, group 2 elements (like group 1 elements) possesslow ionization enethalpies on account of relatively smaller nuclear charge andrealtively larger atomic size. The first ionization enthalpies of group 2 elements are greater than those of group 1 elements because of increased effective than those of group 1 elements because of increased effective nuclear charge in addition to decreased atomic size. However, the second ionization enthalpies of group 2 elements are smaller than those of group 1 elements because after the loss of second electron, they acquire stable configuration of the nearest noble gas while alkali metals already possess noble gas configuration after the loss of first electron. The third ionization enthalpies of group 2 elements are very high and greater than those of group 1 elements.