Question on 1F.5 b

Moderators: Chem_Mod, Chem_Admin

Alvaro Chumpitaz 4D
Posts: 56
Joined: Wed Sep 11, 2019 12:17 am

Question on 1F.5 b

Postby Alvaro Chumpitaz 4D » Sat Oct 26, 2019 9:35 pm

Which member of each pair is likely to have the smaller first ionization energy?
b) Mg or Na
The answer is Na but I do not necessarily understand why

ckilkeary 2G
Posts: 58
Joined: Fri Aug 09, 2019 12:16 am

Re: Question on 1F.5 b

Postby ckilkeary 2G » Sat Oct 26, 2019 10:29 pm

The ionization energy is the energy it takes to remove an electron from an atom. Ionization energies are paired with atomic radius. Since atomic radius increases from left to right on the periodic table so does ionization energy. Na is to the left of Mg so this would mean that Na has the smaller atomic radius as well as the smaller first ionization energy.

Joowon Seo 3A
Posts: 80
Joined: Sat Aug 24, 2019 12:17 am

Re: Question on 1F.5 b

Postby Joowon Seo 3A » Sun Oct 27, 2019 11:39 am

A good way to remember is that the farther away an electron is, the easier it is to remove. Since Na has a greater size than Mg, it is easier to remove an electron; therefore, Na has a lower ionization energy.

Gabriella Bates 2L
Posts: 95
Joined: Thu Jul 11, 2019 12:15 am

Re: Question on 1F.5 b

Postby Gabriella Bates 2L » Sun Oct 27, 2019 11:50 am

ckilkeary 1H wrote:The ionization energy is the energy it takes to remove an electron from an atom. Ionization energies are paired with atomic radius. Since atomic radius increases from left to right on the periodic table so does ionization energy. Na is to the left of Mg so this would mean that Na has the smaller atomic radius as well as the smaller first ionization energy.


Actually, the atomic radius decreases from left to right, since the effective nuclear charge increases and the electrons are pulled more tightly towards the nucleus. This is why ionization energy increases across a group: electrons are pulled more strongly towards the nucleus, and are therefore more difficult to remove.


Return to “Trends in The Periodic Table”

Who is online

Users browsing this forum: No registered users and 2 guests