Lewis Structures

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

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Lauren Lewis3L
Posts: 57
Joined: Wed Feb 20, 2019 12:16 am

Lewis Structures

Postby Lauren Lewis3L » Sun Nov 17, 2019 9:31 pm

I know this may be a stupid question, but how can you determine the shape by doing the Lewis Structures. I understand you can see all the bonds and the lone pairs but I am just confused because I'm afraid that if I draw it out that I won't be able to determine the shape from that.

SVajragiri_1C
Posts: 115
Joined: Thu Jul 11, 2019 12:16 am

Re: Lewis Structures

Postby SVajragiri_1C » Sun Nov 17, 2019 9:35 pm

To determine shape all you need to know is the number of lone pairs and the number of bonds about the central atom, so if you draw the Lewis structure right then that's all you need to know.

ASetlur_1G
Posts: 101
Joined: Fri Aug 09, 2019 12:17 am

Re: Lewis Structures

Postby ASetlur_1G » Sun Nov 17, 2019 9:35 pm

When you draw the lewis structure, you look at the central atom and count how many atoms it's attached to and how many lone pairs it has. This will give you the AXE notation (A = central atom, X = # of attached atoms, E = # lone pairs). Each AXE notation corresponds to a certain shape that I think we just need to memorize.

Fdonovan 3D
Posts: 101
Joined: Sat Aug 17, 2019 12:16 am

Re: Lewis Structures

Postby Fdonovan 3D » Sun Nov 17, 2019 9:37 pm

I think the point is to show you the lone/bonding pairs so that you can find the VSEPR formula (Ex. CCl4 is AX4 which would tell you that its shape is tetrahedral). I also remember Prof. Lavelle saying that if you put atoms symmetrically around the central atom, that's a pretty safe bet for getting an accurately shaped Lewis structure.

Maika Ngoie 1B
Posts: 97
Joined: Fri Aug 02, 2019 12:16 am

Re: Lewis Structures

Postby Maika Ngoie 1B » Sun Nov 17, 2019 9:39 pm

Once you can make the most stable lewis structure, the regions of electron density, and and the lone pairs, you should be able to correspond these numbers with a specific shape. You'll need to memorize the names and the characteristics for this one. For example, ammonia (NH3) has 3 regions of electron density and 1 LP, which creates the template AX3E (where A=central atom, X=number of bonded atoms, and E=number of LP) which corresponds with the trigonal pyramidal shape.

Haley Pham 4I
Posts: 51
Joined: Fri Aug 09, 2019 12:16 am

Re: Lewis Structures

Postby Haley Pham 4I » Sun Nov 17, 2019 9:40 pm

You can name the shape of the molecule by determining the number of the bound atoms and lone pairs around the central atom, which correlate to a certain shape.

KaitlynBali_4B
Posts: 51
Joined: Fri Aug 02, 2019 12:16 am

Re: Lewis Structures

Postby KaitlynBali_4B » Sun Nov 17, 2019 9:44 pm

To add onto this, the number of atoms bonded to the central atom will almost always be the best indication of the molecular shape. The book even states that when naming the molecular shape, only the positions of the atoms are considered. For example, if there are three atoms bonded to the central atom, you know for sure that the molecule either has a trigonal planar shape or a trigonal pyramidal shape. If there is a lone pair of electrons (in addition to these three atoms) you cannot conclude that it has a tetrahedral shape (because the lone pair is not an atom). The presence of this lone pair would confirm that the shape is a trigonal pyramidal shape because the repulsive effect of the lone pair would cause the three other bonds to move closer to each other.


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