An element has successive ionization enthalpies as $1^{s t}$ (940), 2080, 3090, 4140, 7030, 7870, 16000 and 19500 kJ $m o l^{- 1}$ ^. To which group of the periodic table does this element belong?

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Solution

The correct option is C 16
Notice that there is an abnormal jump in the $7^{t h}$ ionization enthalpy.

Therefore, the element has 6 valence electrons and hence it belongs to group 16.

The electronic configuration would be 1s²2s²2p⁶3s²3p⁴

Nevertheless, there is a big jump in the $5^{t h}$ ionization enthalpy. It is due to removal of four electrons from the p-subshell, the $5^{t h}$ electron has to be removed from 3s-orbital.

In general, we can say that when there is a change in the sub-shell or change in the shell, there will be a significant leap in the ionization enthalpy. There are some exceptions though.

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An element has successive ionization enthalpies as 1st (940), 2080, 3090, 4140, 7030, 7870, 16000 and 19500 kJ mol−1. To which group of the periodic table does this element belong?

An element has successive ionization enthalpies as $1^{s t}$ (940), 2080, 3090, 4140, 7030, 7870, 16000 and 19500 kJ $m o l^{- 1}$ ^. To which group of the periodic table does this element belong?