1F.5a

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Jessica Chen 2C
Posts: 103
Joined: Thu Jul 11, 2019 12:17 am

1F.5a

Postby Jessica Chen 2C » Sun Oct 27, 2019 11:11 pm

Can someone explain why Na has a smaller first ionization energy than Al? Their valence electrons are both the first electrons in a subshell (3s1 vs 3p1).

Michelle Song 1I
Posts: 102
Joined: Thu Jul 11, 2019 12:17 am

Re: 1F.5a

Postby Michelle Song 1I » Sun Oct 27, 2019 11:16 pm

Because Na also has a smaller effective nuclear charge than Al, and they have the same number of "shielding electrons".

Jenna Ortiguerra 4G
Posts: 50
Joined: Sat Aug 17, 2019 12:18 am

Re: 1F.5a

Postby Jenna Ortiguerra 4G » Wed Oct 30, 2019 12:24 am

Typically, ionization energy increases the higher the period and as you go from left to right on the periodic table. Na is in the 3s orbital, while Al is on the 3p orbital, which is why Al has a higher ionization energy.

Abigail Sanders 1E
Posts: 112
Joined: Wed Sep 11, 2019 12:16 am

Re: 1F.5a

Postby Abigail Sanders 1E » Wed Oct 30, 2019 12:33 am

Na has a smaller first ionization energy compared to Cl as ionization energy increases across a row on the periodic table. This is because as you move across a row the numbers of protons and electrons increase making the attraction between the two greater as well. This makes it increasingly hard to remove an electron from elements like Cl.

Natalie Nartz 4F
Posts: 50
Joined: Thu Jul 11, 2019 12:17 am

Re: 1F.5a

Postby Natalie Nartz 4F » Wed Oct 30, 2019 1:33 am

The periodic trends show that ionization energy increases when moving left to right. This is because when moving left to right across a period, atomic radius decreases, so electrons are more attracted to the nucleus. With this in mind, since Na is further left, it will have a lower ionization energy than Al.


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