Hi everyone!
For this problem, I understand that none of the compounds given are considered radicals because they do not have an unpaired electron. I was a little confused by the answer that the solution manual gave for part (b) of this problem, which states that "all of these species are expected to be diamagnetic, so therefore none are radicals." I was wondering what diamagnetic meant?
2.27: (a) Draw a Lewis structure for each of the following species: CH3+; CH4; CH3–; CH2; CH2^2+; CH^2−
(b) Identify each as a radical or not.
(c) Rank them in order of increasing HCH bond angles. Explain your choices.
Thank you so much!
Focus Exercise 2.27
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 177
- Joined: Wed Sep 30, 2020 9:46 pm
- Been upvoted: 1 time
-
- Posts: 108
- Joined: Wed Sep 30, 2020 9:48 pm
- Been upvoted: 3 times
Re: Focus Exercise 2.27
Diamagnetic means that the substance does not have any unpaired electrons. In the case of this problem, that means that all of the electrons in each compound are either in a bonding pair or a lone pair, but there are no single, lone electrons
-
- Posts: 107
- Joined: Wed Sep 30, 2020 9:53 pm
- Been upvoted: 1 time
Re: Focus Exercise 2.27
I think it just means that there are no unpaired electrons, and like you mentioned none of them have those!
-
- Posts: 86
- Joined: Wed Sep 30, 2020 10:04 pm
Re: Focus Exercise 2.27
I had question about the radical part. So they are not radicals because they at least have paired electrons? So they're only radicals if the central atom has 1 unpaired electron?
Return to “*Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)”
Who is online
Users browsing this forum: No registered users and 2 guests