# Why does Calcium have a higher ionization energy than Aluminium?

Given their places on the periodic table I'd assume Aluminium has a higher ionization energy, because it has fewer energy levels, and is on a "righter" row on the periodic table, but in reality it is the opposite. Does anyone here know why?

The atomic number of Calcium is 20. So it's orbital configuration is $$\mathrm{1s^2 2s^2 2p^6 3s^2 3p^6 4s^2}$$. This is the arrangement of electrons in the shells. All orbitals are completely filled. So, for removal of an electron from the outermost shell, higher amount of energy is required.
In case of Aluminium, the atomic number is 13. Its orbital configuration is $$\mathrm{1s^2 2s^2 2p^6 3s^2 3p^1}$$. One single electron is present in outermost p-orbital, so it can be easily removed as compared to Calcium.