Bond Enthalpies for Diatomic Molecule
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Bond Enthalpies for Diatomic Molecule
In the lecture where we solved for the enthalpy of a reaction using bond enthalpies, it was mentioned that using bond enthalpies is not the most accurate way because while bond enthalpies for diatomic molecules are accurate as they are measured, the bond enthalpies for all others are averages from many different molecules. In chem 14A we learned that the diatomic molecules were H2, N2, F2, O2, I2, Cl2, and Br2, however in the lecture it was also mentioned that HCl would be considered a diatomic molecule, and I was wondering why would we be considering HCl a diatomic molecule even though it does not have two of the same atoms?
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Re: Bond Enthalpies for Diatomic Molecule
I think diatomic just means that the molecule has two atoms and it doesn't matter if they're of the same element. The diatomic molecules we learned are just the ones that occur as naturally diatomic, i.e. you would not find just H in nature.
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Re: Bond Enthalpies for Diatomic Molecule
The term "diatomic molecule" doesn't exclusively refer to a molecule consisting of two of the same atoms, but can include molecules with any two atoms.
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Re: Bond Enthalpies for Diatomic Molecule
When we talk about diatomic molecules, I believe that we are referring to the idea that the molecule has two atoms, but they do not have to be of the same element. Thus, HCl would be considered a diatomic molecule in the same sense that the naturally occurring diatomic molecules would be, such as H2, O2, etc. However, the bond enthalpies of the naturally diatomic molecules (H2, O2, N2, F2, Br2, I2) are accurate as they are measured for those molecules. All others are averages from many different molecules, so using bond enthalpies is the least accurate method. Hope that helps!
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