Which one of the following order is correct for the first ionization energies of the elements

First ionization energy increases in a period. Thus, the first IE of the elements of the second period should be as follows $Be<B<N<O$

But in practice, the elements do not follow the above order. The first IE of these elements is$B<Be<O<N$

The lower IE of B than that of Be is because in B $\left(1s^2,2s^{2}2p^1\right),$ electron is to be removed from 2p which is easy while in Be$\left(1s^2,2s^2\right),$ electron is to be removed from 2s than that of N is because of the half-filled 2p orbitals in $N\left(1s^2,2s^{2}2p^3\right).$