Ionization Energy: Na vs. Al

Moderators: Chem_Mod, Chem_Admin

madawy
Posts: 81
Joined: Fri Aug 09, 2019 12:17 am

Ionization Energy: Na vs. Al

Postby madawy » Wed Oct 09, 2019 5:54 pm

Will someone please explain to me how Aluminum has a higher ionization energy than Sodium? Thanks.

Shivam Rana 1D
Posts: 106
Joined: Fri Aug 09, 2019 12:16 am

Re: Ionization Energy: Na vs. Al

Postby Shivam Rana 1D » Wed Oct 09, 2019 6:02 pm

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.

Kelvin Chung 1C
Posts: 50
Joined: Sat Aug 24, 2019 12:15 am

Re: Ionization Energy: Na vs. Al

Postby Kelvin Chung 1C » Fri Oct 11, 2019 9:40 am

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.

chrischyu4a
Posts: 52
Joined: Thu Jul 25, 2019 12:16 am

Re: Ionization Energy: Na vs. Al

Postby chrischyu4a » Fri Oct 11, 2019 3:52 pm

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.


Return to “Trends in The Periodic Table”

Who is online

Users browsing this forum: No registered users and 1 guest