Lone Pairs

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Abigail Carter 4G
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Joined: Sat Sep 07, 2019 12:19 am

Lone Pairs

Postby Abigail Carter 4G » Sun Oct 27, 2019 8:03 pm

How do you figure out how many lone pairs each molecule has when you are drawing a lewis structure?

FDeCastro_1B
Posts: 54
Joined: Thu Jul 25, 2019 12:16 am

Re: Lone Pairs

Postby FDeCastro_1B » Sun Oct 27, 2019 8:04 pm

Lone pairs are the two dots next to the atom

RasikaObla_1I
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Joined: Thu Jul 25, 2019 12:15 am

Re: Lone Pairs

Postby RasikaObla_1I » Sun Oct 27, 2019 8:06 pm

You count the number of electrons that aren't shared in a bond between another molecule. For example in a C-O (single) bond, the oxygen has 3 lone pairs and Carbon has 3 lone pairs.

Tracy Tolentino_1C
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Joined: Sat Sep 07, 2019 12:17 am

Re: Lone Pairs

Postby Tracy Tolentino_1C » Sun Oct 27, 2019 8:07 pm

Well, generally most atoms wants to follow the octet rule. It depends on the total number of valence electrons, because you got to make sure the central atom has its' octet, then you add the lone pairs to the outside atoms. If you realize that there isn't enough for the outside, then you create the shared bonds.

J Medina 4A
Posts: 51
Joined: Wed Sep 25, 2019 12:17 am

Re: Lone Pairs

Postby J Medina 4A » Sun Oct 27, 2019 8:11 pm

In a Lewis structure they're the two dots on the sides.

Callum Guo 1A
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Re: Lone Pairs

Postby Callum Guo 1A » Sun Oct 27, 2019 8:26 pm

a lone pair is 2 dots next to an atom

Harry Zhang 1D
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Joined: Sat Sep 14, 2019 12:16 am

Re: Lone Pairs

Postby Harry Zhang 1D » Sun Oct 27, 2019 8:32 pm

Lone pair electrons are just electrons that are not shared with another atom therefore just count the electrons that are not in between two atoms but instead only on the side of ONE atom.

Sreyes_1G
Posts: 44
Joined: Fri Sep 28, 2018 12:19 am

Re: Lone Pairs

Postby Sreyes_1G » Sun Oct 27, 2019 8:48 pm

lone pairs are going to be two single dots next to each other that are not bonded to anything, thus making them lone pairs.

MeeraBhagat
Posts: 44
Joined: Sat Aug 24, 2019 12:15 am

Re: Lone Pairs

Postby MeeraBhagat » Sun Oct 27, 2019 10:49 pm

As long as each atom in a molecule has an octet, including lone pairs, that is how you figure it out. When trying to determine whether to draw a lone pair or to add another bond, calculate formal charge to see what is optimal (always aim for formal charge of 0 on each atom).

Alison Trinh 1A
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Re: Lone Pairs

Postby Alison Trinh 1A » Sun Oct 27, 2019 11:43 pm

Can lone pairs become bonds?

Jacob Villar 3K
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Joined: Sat Aug 17, 2019 12:18 am

Re: Lone Pairs

Postby Jacob Villar 3K » Sun Oct 27, 2019 11:45 pm

Lone pairs are the dots on a lewis structure that do not form bonds, for example, on an atom, they would be the two dots on the side.

J Medina 4A
Posts: 51
Joined: Wed Sep 25, 2019 12:17 am

Re: Lone Pairs

Postby J Medina 4A » Sun Nov 03, 2019 10:34 pm

It's easy to think of it as any valence electrons that aren't touching (being shared by) any other atoms in the lewis structure

305376058
Posts: 35
Joined: Thu Jul 11, 2019 12:17 am

Re: Lone Pairs

Postby 305376058 » Sun Nov 03, 2019 10:56 pm

You figure out the number of pairs not included in one of the bonds.


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