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Ionization Energy: Na vs. Al

Posted: Wed Oct 09, 2019 5:54 pm
by madawy
Will someone please explain to me how Aluminum has a higher ionization energy than Sodium? Thanks.

Re: Ionization Energy: Na vs. Al

Posted: Wed Oct 09, 2019 6:02 pm
by Shivam Rana 1D
Sodium has one unpaired electron in the 3s subshell, thus it is more inclined to lose that electron. If it loses that electron to an electronegative atom like chlorine the subshells are "satisfied" because the valence electrons are balanced in a "full" subshell. Aluminum requires more energy because it has an unpaired electron in the 3p subshell and it is less likely to lose that electron.

Re: Ionization Energy: Na vs. Al

Posted: Fri Oct 11, 2019 9:40 am
by Kelvin Chung 1C
The atomic radius of Aluminum is smaller than that of Sodium. Therefore, the outer electrons of an Aluminum atom are closer to the nucleus, and thus are more strongly attracted to the nucleus than are Sodium's electrons.

Re: Ionization Energy: Na vs. Al

Posted: Fri Oct 11, 2019 3:52 pm
by chrischyu4a
Simply put, aluminum has 3 valence electrons while sodium only has 1. It takes more energy for aluminum to lose 3 electrons to complete its octet shell than it does for sodium to lose one electron.