Ionization Energy

[Shaniya Kerns 4D]

How does ionization energy work and what is the trend on the periodic table? How do I come to the conclusion that Cl- has less ionization energy than Cl, and F has a greater ionization energy than Cl, while Cl- has a higher ionization energy than F?

[805909756]

Ionization energy is the energy required to remove an electron from a neutral atom or a positive ion. It is an indicator of the atom's ability to lose an electron and form a positive ion. Ionization energy increases from left to right across a period and increases up a group (from bottom to top).

Chlorine (Cl) has a higher ionization energy than chloride (Cl-) because Cl has one more electron than Cl-. The extra electron in Cl increases the repulsion between electrons, making it easier to remove an electron from Cl-. Fluorine (F) has a greater ionization energy than chlorine (Cl) because fluorine is to the right of chlorine in the same period. Again, the chloride ion (Cl-) has higher ionization energy than fluorine (F) because Cl- has gained an extra electron compared to F.