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Postby KNguyen_1I » Wed Nov 13, 2019 3:50 pm

So due to things in nature wanting to be at a lower state of energy, when we calculate the net interaction potential energy, the greater the magnitude of the negative value the more favorable the interaction is right?
For example, LDF has a Ep of -2 kJ/mole but for hydrogen bonding it's like around -20 kJ/mole, which indicates that hydrogen bonding in not too large sized molecules generally holds stronger precedence in terms of strength over LDF forces right? Because it has a greater negative value and is therefore stronger because a lower state of energy is more favorable.

ishaa Diwakar 4E
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Re: Energy

Postby ishaa Diwakar 4E » Wed Nov 13, 2019 9:45 pm

I think you are right, but also the main reason that the Hydrogen bonds are stronger is due to electronegativity (EN). Since Hydrogen bonds are formed between H (with the lowest EN) and N,O, or F (with the three highest ENs), the EN difference is the greatest and therefore the dipole is strongest. The stronger dipole causes the intermolecular forces to also be stronger. The Ep is probably also lower for these bonds because of their strength, as you said.

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Re: Energy

Postby Micah3J » Wed Nov 13, 2019 10:02 pm

What are the units of the formula for Interaction Potential Energy?

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