Favorable Bonds

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Brandon Valafar
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Joined: Sat Aug 17, 2019 12:16 am
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Favorable Bonds

Postby Brandon Valafar » Tue Nov 05, 2019 4:05 pm

How many bonds would Nitrogen and Oxygen like to have?

karinaseth_1A
Posts: 57
Joined: Sat Jul 20, 2019 12:15 am

Re: Favorable Bonds

Postby karinaseth_1A » Tue Nov 05, 2019 4:07 pm

Nitrogen would want 3 and oxygen would want 2. However, depending on the molecule and formal charge distribution this can change. Neither of these elements can accommodate anything less or more than an octet, however.

Rohit Ghosh 4F
Posts: 99
Joined: Thu Jul 25, 2019 12:17 am

Re: Favorable Bonds

Postby Rohit Ghosh 4F » Thu Nov 07, 2019 4:09 pm

The number of bonds these atoms actually have is also dependent on what other atom it's bonding with.

Vicki Liu 2L
Posts: 101
Joined: Sat Aug 24, 2019 12:15 am

Re: Favorable Bonds

Postby Vicki Liu 2L » Thu Nov 07, 2019 4:38 pm

To expand on the first response, the reasoning behind why nitrogen atoms would want 3 bonds and oxygen atoms would want 2 is because this gets them to a formal charge of zero.

If N has 3 bonds, it would need 1 lone pair to have a completed octet. So, formal charge = 5 - (2 + 6/2) = 0
If O has 2 bonds, it would need 2 lone pairs to have a completed octet. So, formal charge = 6 - (4 + 4/2) = 0

Having a formal charge of 0 means the atoms are at their lowest energy and stable, which is favorable.

Manav Govil 1B
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Re: Favorable Bonds

Postby Manav Govil 1B » Fri Nov 08, 2019 1:37 pm

Although N and O have favorable bonds, certain structures require them to have more or fewer bonds - causing them to have a charge. For example, NO+ shows a triple bond between the N and the O. The N is pleased with a formal charge of 0, but the O has a formal charge of +1, which causes the positive nature of the molecule.

Giselle Littleton 1F
Posts: 78
Joined: Wed Sep 18, 2019 12:20 am

Re: Favorable Bonds

Postby Giselle Littleton 1F » Fri Nov 08, 2019 2:56 pm

To form an octet, oxygen needs 2 electrons while nitrogen needs 3. But unless the atom(s) they're bonded to is specified, the more bonds the harder it is to break the molecule.


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