Question

Question #fbdfe

Answer 1

The difference in ionization energy between `B` and `Be` can be explained by detailing their respective electron configurations:

`Be`: `1s^(2)2s^2`
`B`: `1s^(2)2s^(2)2p^(1)`

Notice that `Be` has a stable electron configuration, which means that more energy is required to remove an electron from it. On the other hand, `B`'s ionization energy is smaller because of the electron present in its p-orbital.

Since p-orbitals are higher in energy than s-orbital, therefore less stable, it is easier for an electron to be removed from a p-orbital. Electrons located in p-orbitals are further away from the nucleus, which means that they can withstand its effective nuclear charge better `<=>` more easy to remove from the atom.

Losing an electron from its outermost shell will make `B` more stable, since it will be lower in energy.