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Ionization Enthalpy

The values of...

Question

The values of $I P_{1}, I P_{2}, I P_{3}$ and $I P_{4}$ of an atom are $7.5 e V, 25.6 e V, 48.6 e V$ and $170.6 e V$ respectively. The electronic configuration of the atom will be:

A

1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{1}

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B

1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{1}

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C

1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{3}

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D

1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}

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Solution

The correct option is B $1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{1}$
Whenever there is a sudden increase in the ionisation potential, it indicates that the species had a stable configuration.
It is given that $I p_{4} >>> I p_{3}$ , which indicate that the species attained stability by loosing 3 electrons.
So, option (b) represents this high energy change due to the removal of the fourth electron from a fully filled $2 p^{6}$ orbital.

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Similar questions

Q. The values of

I P_{1}, I P_{2}, I P_{3}

I P_{4}

7.5 e V, 25.6 e V, 48.6 e V

170.6 e V

respectively. The electronic configuration of the atom will be:

Q. Successive ionisation energies of an element

X

are given(in K. Cal)

$I P_{1}$	$I P_{2}$	$I P_{3}$	$I P_{4}$
$165$	$195$	$556$	$595$

Electronic configuration of the element

X

{I P}_{1}, {I P}_{2}, {I P}_{3}, {I P}_{4}

{I P}_{5}

of an element are

7.1, 14.3, 34.5, 46.8, 162.2 e V

The element is likely to be:

I P_{1^{'}} I P_{2^{'}} I P_{3^{'}} I P_{4^{'}}

I P_{5}

of an element are

7.1, 14.3, 34.5, 46.8, 162.2

eV respectively. The element is likely to be:

Q. Sucessive ionisation energies of an element 'X' are given below (in K. Cal)

$I P_{1}$	$I P_{2}$	$I P_{3}$	$I P_{4}$
165	195	556	595

Electronic configuration of the element 'X' is:

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Ionization Enthalpy

Standard XII Chemistry

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