Ncert Exercises & Solutions

Amongst the following elements whose electronic configuration are given below, the one having the highest ionisation enthalpy is:

1.	$[Ne] 3 s^{2} 3 p^{1}$	2.	$[Ne] 3 s^{2} 3 p^{3}$
3.	$[Ne] 3 s^{2} 3 p^{2}$	4.	$[Ar] 3 d^{10} 4 s^{2} 4 p^{3}$

Hint: Left to right across the period ionization energy increases and down the group ionization energy increases.

Step 1:

The electronic configuration represents

[Ne] 3 s^{2} 3 p^{1}

represents aluminium

[Ne] 3 s^{2} 3 p^{3}

represents phosphorus

[Ne] 3 s^{2} 3 p^{2}

represents silicon

[Ar] 3 d^{10} 4 s^{2} 4 p^{3}

represents arsenic

Step 2:

Aluminium, silicon and phosphorus same period and left to right across the period ionization energy increases. Arsenic belongs to phosphorus group and position of arsenic just belong phosphorus. Down the group ionization energy decreases. Hence,

[Ne] 3 s^{2} 3 p^{3}

has the maximum ionization enthalpy.

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