As we move from left to right in periodic table ionisation enthalpy increases due to increase in number of protons and decrease in size. So the expected order is C < N < O < F.
But the outer most electronic configuration of the elements are as below
C: 1s2 2s2 2p2
N: 1s2 2s2 2p3
O: 1s2 2s2 2p4
F: 1s2 2s2 2p5
As nitrogen have half field orbital so its stability is higher (Hund’s rule), and removal of electron form the outer most shell of nitrogen is more difficult.
Therefore actual order of ionisation enthalpy is C < N > O < F.