Answer: Option (b) is the correct answer.
Step-by-step explanation:
The energy required to remove the most loosely bound electron from a neutral gaseous atom is known as ionization energy.
So, when there is increase in atomic size of the atom there is less force of attraction between the nucleus and the valence electrons of the atom.
Hence, it is easy to remove the most loosely bound electron. Therefore, with increase in size there will occur a decrease in ionization energy of atom.
And, when we move across a period then there occurs a decrease in size of atom. Hence, ionization energy across a period increases.
Out of the given options neon is smaller is size that fluorine atom. So, ionization energy of neon is more than the ionization energy of fluorine atom.
Thus, we can conclude that Ne > F shows a correct relationship between first ionization energies of the given atoms.