Lone pairs
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 53
- Joined: Sat Aug 17, 2019 12:18 am
Lone pairs
Why are lone pairs more likely to be found in certain locations around a central atom? And which locations are these?
-
- Posts: 99
- Joined: Sat Aug 17, 2019 12:17 am
Re: Lone pairs
Lone pairs occupy more space around the central atom than bonding pairs and lone pairs are also more impacted by electrostatic repulsion between like charges
-
- Posts: 103
- Joined: Sat Aug 17, 2019 12:18 am
Re: Lone pairs
The lone pairs can either be axial or equatorial. The axial lone pairs lie on the axis of the molecule and the equatorial lone pairs lie on the equator of the molecule, the plane perpendicular to the axis.
-
- Posts: 59
- Joined: Thu Jul 11, 2019 12:17 am
-
- Posts: 102
- Joined: Fri Aug 09, 2019 12:15 am
Re: Lone pairs
You determine whether a lone pair is axial or equatorial by looking at the bond angles and making sure the lone pair has enough room to evenly repel the other bonded electrons.
Re: Lone pairs
Lone pairs are usually located in a place where they form fewer bond angles with other atoms. So in the See Saw shape they are located on the equatorial plane where they only interact with 2 bonds.
-
- Posts: 131
- Joined: Fri Aug 02, 2019 12:15 am
Re: Lone pairs
If a lone pair is a radical would it have a weaker repulsion than a complete lone pair?
Re: Lone pairs
Nathan Rothschild_3D wrote:If a lone pair is a radical would it have a weaker repulsion than a complete lone pair?
I'm assuming so because a radical would occupy less space than a complete lone pair. Please correct me if I'm wrong though!
Return to “Bond Lengths & Energies”
Who is online
Users browsing this forum: No registered users and 7 guests