Represents the correct order of first ionisation enthalpy?

Along a period, ionisation enthalpy rises with nuclear charge, but two anomalies occur. Boron ($2s^22p^1$) is lower than beryllium ($2s^2$) because the $2p$ electron is removed more easily than a $2s$ electron of a full subshell. Oxygen ($2p^4$) is lower than nitrogen ($2p^3$) because pairing repulsion in oxygen makes removal easier than from the half-filled $2p^3$ set. Values in $\mathrm{kJ\,mol^{-1}}$: Li 520, B 801, Be 899, C 1086, O 1314, N 1402. Hence $\mathrm{Li}<\mathrm{B}<\mathrm{Be}<\mathrm{C}<\mathrm{O}<\mathrm{N}$.