O vs N  [ENDORSED]

Moderators: Chem_Mod, Chem_Admin

Noh_Jasmine_1J
Posts: 71
Joined: Fri Sep 28, 2018 12:15 am

O vs N

Postby Noh_Jasmine_1J » Tue Nov 06, 2018 2:31 pm

why does Oxygen have lower ionization energy than Nitrogen ?

Mayaal_Khan_4H
Posts: 41
Joined: Fri Sep 28, 2018 12:28 am

Re: O vs N

Postby Mayaal_Khan_4H » Tue Nov 06, 2018 3:08 pm

Ionization energy increases across a table because the valence shell of the elements as you go towards the right is nearly filled whereas as, as you go towards the left, the electrons have a low ionization energy from their willingness to lose electrons and become cations which is why Oxygen has a lower ionization energy than Nitrogen.

rosemarywang4i
Posts: 34
Joined: Fri Sep 28, 2018 12:28 am

Re: O vs N  [ENDORSED]

Postby rosemarywang4i » Tue Nov 06, 2018 3:24 pm

It's because nitrogen's p orbital is half filled, so it's more stable than oxygen and thus requires more energy to remove an electron.

jonathanjchang2E
Posts: 61
Joined: Fri Sep 28, 2018 12:26 am

Re: O vs N

Postby jonathanjchang2E » Tue Nov 06, 2018 5:04 pm

The fourth valence electron in oxygen's p orbitals has a lower ionization energy because of the electron electron repulsion formed by the lower three valence electrons. This ionization energy is lower than nitrogen because of the three parallel electrons in nitrogen's p orbitals.

Katie Frei 1L
Posts: 64
Joined: Fri Sep 28, 2018 12:27 am

Re: O vs N

Postby Katie Frei 1L » Tue Nov 06, 2018 9:28 pm

Oxygen has a lower ionization energy because, even though it is technically further down the period than Nitrogen, its p orbital is half-filled, making it more stable and so harder to remove an electron.


Return to “Ionic & Covalent Bonds”

Who is online

Users browsing this forum: No registered users and 2 guests