dissociation energy

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dissociation energy

Postby bellaha4F » Thu Nov 07, 2019 7:59 pm

how do we calculate the dissociation energy? Is there a formula?

Daniel Honeychurch1C
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Re: dissociation energy

Postby Daniel Honeychurch1C » Thu Nov 07, 2019 8:33 pm

The dissociation energy of bonds will always be given because its based on experimental data.

Abhi Vempati 2H
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Re: dissociation energy

Postby Abhi Vempati 2H » Thu Nov 07, 2019 10:21 pm

Like @Daniel Honeychurch 1B mentioned, for Chem 14A, we'll be given the experimental values of the dissociation energies. Professor Lavelle mentioned that we will be calculating dissociation energies in Chem 14B, though.

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Re: dissociation energy

Postby romina_4C » Thu Nov 07, 2019 10:39 pm

I believe the only thing we need to know about bond dissociation energy for now is that stronger bonds have a larger dissociation energy (requires more energy to break them) and weaker bonds have a smaller dissociation energy (requires less energy to break them).

Chetas Holagunda 3H
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Re: dissociation energy

Postby Chetas Holagunda 3H » Fri Nov 08, 2019 1:15 pm

As the number of bonds increases too, like from a single, to double, to triple, the dissociation energy increases as the strength of the bond is more.

Megan Jung 3A
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Re: dissociation energy

Postby Megan Jung 3A » Fri Nov 08, 2019 2:02 pm

Dissociation energies are measured values that have been experimentally calculated. Therefore, they will usually be given if you need to use the values and there isn't any formulas that we need to know for this class in terms of calculating the actual value.

Jordan Ziegler 2J
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Re: dissociation energy

Postby Jordan Ziegler 2J » Fri Nov 08, 2019 3:19 pm

I think our material only covers the definition and patterns surrounding dissociation energy. We will calculate the dissociation energy of bonds next quarter in Chem 14B. However, I remember in high school chemistry that bond dissociation energy is measured by the change in enthalpy (
) as you break a bond.

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