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(C) The successive ionization energies are $IE_1 = 191 \ kcal$,$IE_2 = 578 \ kcal$,$IE_3 = 872 \ kcal$,and $IE_4 = 5962 \ kcal$. There is a very large

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$3$

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(C) The successive ionization energies are $IE_1 = 191 \ kcal$,$IE_2 = 578 \ kcal$,$IE_3 = 872 \ kcal$,and $IE_4 = 5962 \ kcal$. There is a very large jump in energy between the third and fourth ionization energy $(IE_4 - IE_3 = 5962 - 872 = 5090 \ kcal)$. This indicates that after removing $3$ electrons,the fourth electron is being removed from a stable,noble gas-like inner shell configuration. Therefore,the element has $3$ valence electrons.

The first four ionization energy values of an element are $191$,$578$,$872$ and $5962 \ kcal$. The number of valence electrons in the element is

Similar Questions

Which ionisation potential $(IP)$ in the following equations involves the greatest amount of energy?

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Which one of the following statements is incorrect in relation to ionisation enthalpy?

The second ionization potential of elements is invariably higher than the first ionization potential because:

The first ionization potential $(IP)$ of $Be$ $(Z=4)$ is higher than which of the following elements?
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$(e) K (Z=19)$

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