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(C) The successive ionization enthalpy values are given as: $\Delta_i H_1 = 899 \ kJ/mol$,$\Delta_i H_2 = 1757 \ kJ/mol$,$\Delta_i H_3 = 14847 \ kJ/mo

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Alkaline earth metal group

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(C) The successive ionization enthalpy values are given as: $\Delta_i H_1 = 899 \ kJ/mol$,$\Delta_i H_2 = 1757 \ kJ/mol$,$\Delta_i H_3 = 14847 \ kJ/mol$,and $\Delta_i H_4 = 17948 \ kJ/mol$. We observe a very large jump in energy between the second and third ionization enthalpies ($\Delta_i H_2$ to $\Delta_i H_3$). This indicates that the element has $2$ valence electrons in its outermost shell,as removing the third electron requires breaking a stable noble gas configuration. Elements with $2$ valence electrons belong to Group $2$,which is the alkaline earth metal group.

The successive ionization enthalpy values for an unknown element are $\Delta_i H_1 = 899 \ kJ/mol$,$\Delta_i H_2 = 1757 \ kJ/mol$,$\Delta_i H_3 = 14847 \ kJ/mol$,and $\Delta_i H_4 = 17948 \ kJ/mol$. To which group of the periodic table does this element belong?

Similar Questions

The ionization energy of hydrogen is:

Which of the following represents the correct order of first ionization enthalpy?
$(i) \ Li < B < Be < C$ $(ii) \ O < N < F$ $(iii) \ Be < N < Ne$

Which of the following elements has the lowest ionization energy?

Which of the following has the least ionization potential?

The order of first ionization potentials of elements $Li, Be, B, Na$ is:

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