lone pairs

(Polar molecules, Non-polar molecules, etc.)

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Alysia Garcia 1B
Posts: 40
Joined: Wed Feb 21, 2018 3:02 am

lone pairs

Postby Alysia Garcia 1B » Sun May 27, 2018 10:11 pm

for there to be a 120 degree rather than a straight line the line pair must be on the middle electron? also how does this make the molecule angled?

Chris Fults 1C
Posts: 27
Joined: Wed Nov 15, 2017 3:01 am

Re: lone pairs

Postby Chris Fults 1C » Sun May 27, 2018 10:19 pm

In bent molecular geometry, there is a middle element with two other elements at the bottom end making a 120-degree angle. The lone pairs are straight ahead of the middle electron. When there are more than one lone pairs the angle between the two elements decrease making it <109 degrees.

Alexandra Wade 1L
Posts: 32
Joined: Fri Apr 06, 2018 11:05 am
Been upvoted: 1 time

Re: lone pairs

Postby Alexandra Wade 1L » Wed May 30, 2018 11:30 am

The reason the molecule is bent is because the repulsion between the two bonding pairs is less than it would be between either bonding pair and the lone pair. This causes the molecule to no longer be linear and take on the bent shape.

Salena Chowdri 1I
Posts: 66
Joined: Fri Apr 06, 2018 11:02 am

Re: lone pairs

Postby Salena Chowdri 1I » Wed May 30, 2018 5:10 pm

Commonly, a linear compound consists of 3 atoms that lie at 180 degrees. The compound takes a bent structure when there is a lone pair found on the central atom (usually on top). This creates a repelling force that pushes both the present bonds downwards into a 120 degree angle.

Melissa_Aguirre1J
Posts: 38
Joined: Tue Nov 14, 2017 3:02 am

Re: lone pairs

Postby Melissa_Aguirre1J » Thu May 31, 2018 12:31 am

How does the addition of lone pairs affect the bond angle? I know that lone pairs are not included in the VSEPR model, but would the lone pairs affect the VESPR model in any way?

Faisal Alshamaa - 1L
Posts: 31
Joined: Fri Apr 06, 2018 11:01 am

Re: lone pairs

Postby Faisal Alshamaa - 1L » Fri Jun 01, 2018 12:12 am

think of the ball and stick module that Dr. Lavelle showed us in class when he asked someone to pull out an atom and make it a lone pair. Since lone pair repulsion is stronger than the repulsion of a bonded pair of electrons, the lone pair pushes the other atoms away from it and causes bond angles to decrease an you get that "bent" shape.


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