Ionization Energy Periodic Trend

[Madison Yee 2B]

Can someone please explain the reasoning behind the ionization energy periodic trend to me?

[Tyler_Kim_2G]

Ionization energy is basically the energy needed to remove an electron. Ionization energy increases when moving towards the right end of the periodic table because there are more protons and thus a greater attraction to the nucleus. Ionization energy decreases when moving down the periodic table because there are more energy levels and hence less attraction to the nucleus.

[Joseph Lee]

ionization energy is simply how much energy it will take to remove an electron from an atom. Most of the time, in the cases of non-metals, it will be harder to take away an electron, mostly because they will try to gain one to fill their valence shells. This is all except for oxygen, between Nitrogen and Flourine, because the electron-electorn repulsion from the four electrons will make it so that the ion would be more appeased if there were one taken out. This isn't too indicative of most other atoms though.

[Anthony Tam]

The ionization energy is the energy needed to remove an electron from an atom. The further away an electron is from the nucleus, the easier it is to remove. Thus, ionization energies decrease going down a period and increases across a period. The ionization energy increases across a period because of the increase in effective nuclear charge.

[Triston Dinh 1D]

Ionization energy increases as you go from left to right across the periodic table because it becomes harder to remove an electron from elements that almost have their octet filled versus elements in the s orbitals that have only a few electrons towards their octet. Ionization energy depends on valence shell stability and how close the element is towards filling its octet.

[Hudson2J]

Ionization energy is the energy required to remove the outermost valence electron. Ionization energy increases across a period because the electrons experience a greater attraction to the nucleus, as it has a greater charge. Going down a group, ionization energy decreases because the outermost electrons are in higher and higher energy levels, meaning they need a lower amount of energy to be removed from the attraction of the nucleus.

[Mia Orr 3B]

Ionization energy increases across the period because as there are more protons in the nucleus, there is a stronger attraction between the electrons and the nucleus, which makes it harder for the electrons to be removed (high ionization energy).

Ionization energy decreases down a group because as there are more electrons in higher energy levels, there will be electrons that are further away from the nucleus, so the attraction between them and the protons in the nucleus isn't as strong, which makes the electrons easier to remove (low ionization energy).