![]() ![]() ![]() The most energy to remove is going to be helium! Therefore, as you move down a period (row) the ionization energy increases. Meanwhile, all the noble gasses are completely filled in subshells so they REALLY dont wanna give away an electron, so it takes even more energy to remove. For atoms like flourine, it is SO close to getting that 6th electron that it takes a lot fo energy to remove an electrona nd take it away from its goal. Subshell occupancy also plays a big role. So, then as shell number increases, the less the electron feels attached to the nucleus of the atom, so the easier it will be for it to be removed-so ionization energy decreases down groups (columns) on the periodic table since the n increases as you go "down". Some things that impact how much the electron is 'happy' are: shell number (n) as the further you are from the nucleus the less it is pulled to it (like how you feel the heat of a campfire the closer you are to it and the less people in front of you), subshell occupancy. How much energy it takes to remove the electron is directly tied to how much the electron is 'attached' to staying with its atom. The ionization energy is going to be the amount of energy it takes to remove an electron from the valence shell of an atom. Hi! I have a question - I understand but Im still a bit confused so can someone explain to me how does the trend in ionization energy vary across the periodic table, and what factors contribute to this trend? Thanks! ![]()
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