2.67 Ed 6, electron afinity

Moderators: Chem_Mod, Chem_Admin

Meghanhe1l
Posts: 60
Joined: Fri Sep 28, 2018 12:17 am

2.67 Ed 6, electron afinity

Postby Meghanhe1l » Mon Oct 29, 2018 11:06 pm

In question 2.67 for the 6th edition textbook, it states that C has a higher electron affinity than N even though N is further right on the periodic table. Why is that?

Elisa Bass 4L
Posts: 61
Joined: Fri Sep 28, 2018 12:23 am

Re: 2.67 Ed 6, electron afinity

Postby Elisa Bass 4L » Mon Oct 29, 2018 11:13 pm

This has to do with the orbitals. All three of N’s p orbitals already have one e- each in them. C has one open p orbital, so it has a higher electron affinity because it has space to put another e-. N does not have the space unless it pairs electrons, which would cause it to have higher energy due to electron-electron repulsion than if it didn’t have that extra e-. Therefore, it has a lower affinity.

Matthew Choi 2H
Posts: 59
Joined: Fri Sep 28, 2018 12:18 am

Re: 2.67 Ed 6, electron afinity

Postby Matthew Choi 2H » Thu Nov 01, 2018 2:38 pm

Electron affinity is described as the propensity for an atom or ion to gain an electron. The way that you can tell that C has a higher electron affinity than N is by looking at the 2p sublevels of a C and N atom. C has one electron in two of its three orbitals. N has one electron in each of its orbitals. If N were to gain another electron, the electron would have to be added to an already occupied orbital. If O were to gain another electron, the electron would be added to the empty third orbital. The energy required to add an electron to N is higher than the energy required to add an electron to O because there are more interelectronic repulsions for N. Therefore, it's harder to add an electron to N than C. Therefore, C has a higher electron affinity than N.


Return to “Trends in The Periodic Table”

Who is online

Users browsing this forum: No registered users and 1 guest