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The successive ionization energies (in kJ/mol) for an element are shown below.
$\begin{matrix} E_{1} & E_{2} & E_{3} & E_{4} & E_{5} \\ 577 & 1820 & 2740 & 11600 & 14800 \end{matrix}$
What is the electron configuration of this element?

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$\begin{array}{r} 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{3} \end{array}$

$\begin{aligned} 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1} \end{aligned}$

$\begin{array}{r} 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3} \end{array}$

$\begin{aligned} 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1} \end{aligned}$

answer is B.

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Detailed Solution

The successive ionization energies given (in kJ/mol) are of alaumminium.Hence the given element is Allumium.
Therefore the electronic configuration of alluminium is $\begin{aligned} 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1} \end{aligned}$

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