Lone pair location

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Milena Aragon 2B
Posts: 60
Joined: Fri Sep 28, 2018 12:19 am

Lone pair location

Postby Milena Aragon 2B » Sun Dec 02, 2018 11:24 am

Can someone explain what it is that we have to know in order to be able to:
Explain why lone pairs are more likely to found in certain locations around a central atom and
how and why they affect the bond angles in a molecule, cation, or anion.

Chase Yonamine 1J
Posts: 62
Joined: Fri Sep 28, 2018 12:17 am

Re: Lone pair location

Postby Chase Yonamine 1J » Sun Dec 02, 2018 12:38 pm

Lone pairs have a great repulsion strength. This means that lone pairs will repel the bonded pairs. For example, in H2O is not a linear shape because the 2 lone pairs repel the bonded pairs making the shape bent with 104.5 bond angles. In all, lone pairs repel bonded pairs. This makes the shapes "distorted".

sophiebillings1E
Posts: 60
Joined: Fri Sep 28, 2018 12:27 am

Re: Lone pair location

Postby sophiebillings1E » Sun Dec 02, 2018 12:50 pm

If there is more than one lone pair they are located so that they are farthest away from other areas of electron density since they have the greatest repulsion.

Connie Chen 3D
Posts: 31
Joined: Mon Jan 08, 2018 8:12 am

Re: Lone pair location

Postby Connie Chen 3D » Mon Dec 03, 2018 11:29 pm

Lone pairs tend to hog up a lot of space. They end up pushing down on the bonded molecules due to their repulsion. This results in differing shapes for molecules that have lone pairs as compared to having none.


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