An element has successive ionization enthalpy as 940, 2080, 3090, 4140, 7030, 7870, 16000 and 19,500 KJ/mole. To which group of the periodic table does the element belong to?

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Solution

The correct option is C
16

There is an abnormal jump in the $7^{t h}$ I.E. So the element must be attaining inert gas configuration after losing 6e^-. It should belong to $16^{t h}$ group

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An element has successive ionization enthalpy as 940, 2080, 3090, 4140, 7030, 7870, 16000 and 19,500 KJ/mole. To which group of the periodic table does the element belong to?

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An element has successive ionization enthalpy as 940, 2080, 3090, 4140, 7030, 7870, 16000 and 19,500 KJ/mole. To which group of the periodic table does the element belong to?

The correct option is C 16 There is an abnormal jump in the 7th I.E. So the element must be attaining inert gas configuration after losing 6e-. It should belong to 16th group

The correct option is C
16

There is an abnormal jump in the $7^{t h}$ I.E. So the element must be attaining inert gas configuration after losing 6e^-. It should belong to $16^{t h}$ group