Question

compare the ionisation energy for fluorine and neon​

Answer 1

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Explanation:

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Answer 2

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Simple explanation : neon has a greater ionization energy than fluorine.

As you move from left to right across the periodic table, staying in a single period, the elements gain protons one-by-one. For example, oxygen has one more proton than nitrogen, and fluorine has one more proton than oxygen. They also gain electrons one-by-one. But the number of energy levels stays the same. So as you move from carbon to nitrogen to oxygen to fluorine to neon, you’re loading up more and more protons and electrons, but you’re not increasing the number of energy levels in which the electrons can live.

Consequently, the attractive force between the nucleus and the valence electrons increases, but the shielding effect of inner electrons doesn’t. The atoms get smaller as you move from left to right across a period, owing to this increased attraction between the nucleus and outermost electrons.

Because the atoms get smaller from left to right, the outermost electrons are closer to the nucleus and even more strongly attracted to the protons; ergo, it becomes increasingly hard to remove electrons as you move from left to right. There are some small deviations from this trend, but as a general rule, the first ionization energy of elements increases as you move from left to right across the periodic table.

That’s why neon has a greater ionization energy than fluorine. It has one more proton and one more electron, resulting in a greater attraction between the nucleus and valence electrons, resulting in the valence electrons being more tightly bound to the nucleus, resulting in a larger energy requirement to separate one of the valence electrons from the atom.

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