Hydrogen Bonding

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

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905085650
Posts: 62
Joined: Fri Sep 28, 2018 12:19 am

Hydrogen Bonding

Postby 905085650 » Sun Nov 11, 2018 3:55 pm

What is the typical attractive energy for hydrogen bonds?

Thank you!!

AustinGrove3B
Posts: 53
Joined: Fri Sep 28, 2018 12:23 am

Re: Hydrogen Bonding

Postby AustinGrove3B » Sun Nov 11, 2018 3:59 pm

It is -20 kJ / mol. This is stronger than the dipole-dipole interactions, but not as strong as a full covelent/ionic bond.

Michelle Fu 1H
Posts: 35
Joined: Fri Sep 28, 2018 12:19 am

Re: Hydrogen Bonding

Postby Michelle Fu 1H » Sun Nov 11, 2018 4:01 pm

The typical attractive energy is around 20 kJ per mol. Note that this attractive energy quite high compared to other Van Der Waals forces such as dipole dipole and dispersion but still less than covalent bonding.

Cienna Henry 1J
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Re: Hydrogen Bonding

Postby Cienna Henry 1J » Sun Nov 11, 2018 4:15 pm

What does the attractive energy measure?

Michael_Navarro_1H
Posts: 29
Joined: Fri Sep 28, 2018 12:17 am

Re: Hydrogen Bonding

Postby Michael_Navarro_1H » Sun Nov 11, 2018 4:20 pm

Attractive energy is just a determinant of the relative strength of a bond in relation to the energy required to break it. The higher the dissociation energy of a bond, the stronger its attractive energy is.

RoopshaChatterjee 1G
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Re: Hydrogen Bonding

Postby RoopshaChatterjee 1G » Sun Nov 11, 2018 6:24 pm

How do we use the attractive energy to determine the structure of the molecule?

Cienna Henry 1J
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Re: Hydrogen Bonding

Postby Cienna Henry 1J » Sun Nov 18, 2018 10:13 am

RoopshaChatterjee 1G wrote:How do we use the attractive energy to determine the structure of the molecule?

Are you sure attractive energy matters when determining the structure of a molecule?

Hannah Padilla 1H
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Joined: Fri Sep 28, 2018 12:19 am

Re: Hydrogen Bonding

Postby Hannah Padilla 1H » Sun Nov 18, 2018 10:27 am

I don't think that attractive energy determines the structure of the entire molecule. Attractive energy refers to the strength of the bond. Hydrogen bonds are stronger than Van der Waals but weaker than covalent.


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