$$ \begin{array}{|c|c|} \hline & \text{Ionization Energy} \\ & \text{(kJ/mol)} \\ \hline \text{First} & 801 \\ \hline \text{Second} & 2{,}430 \\ \hline \text{Third} & 3{,}660 \\ \hline \text{Fourth} & 25{,}000 \\ \hline \text{Fifth} & 32{,}820 \\ \hline \end{array} $$

The table above shows the first five ionization energies for a second-period element. Which identifies the element and provides the best explanation?

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Notice the large jump in ionization energy from the third to the fourth. This corresponds to the third and fourth electron removed.

Once the outer three valence electrons are removed, a large amount of energy is required to remove the next electron since it is a core electron.

We are looking for a group 13 electron. Of the options, boron matches the described characteristics.