Consider the elements Nitrogen (N), Oxygen (O), and Fluorine (F). Which of the following options correctly represents the increasing order of their electronegativity and their first ionization enthalpy?

Step-by-step solution

Electronegativity generally increases across a period from left to right due to an increase in effective nuclear charge. Therefore, the correct increasing order of electronegativity for these Period 2 elements is N O F . First ionization enthalpy also generally increases across a period, but there is an exception between Group 15 and Group 16. Nitrogen (Group 15) has a stable half-filled 2p subshell ( 2s² 2p³ ), whereas Oxygen (Group 16) has a 2s² 2p⁴ configuration. Removing an electron from the stable half-filled