10
$\begingroup$

In the article Discuss. Faraday Soc. 1962, 33, 205, the authors say that in order to form molecular hydrogen from collision to atom we need a third body to remove the excess energy. That is we have the reaction $\ce{H + H + M -> H2 + M}$.

I suppose the reason is because if we have the excess this energy will break the bond. If it this the case why the energy can not be transferred to the electron and so would have $\ce{H + H -> H2^*}$, where $\ce{H2^*}$ denotes an excited state of $\ce{H2}$?

$\endgroup$
12
  • 2
    $\begingroup$ You can use the \ce{...} macro to typeset chemical equations; it's easier and also provides the correct output (chemical symbols should be upright, not in italics). Check out my edit for some examples. $\endgroup$
    – orthocresol
    Dec 1 '20 at 19:18
  • 1
    $\begingroup$ An excited state of H2 would still have the excess energy. $\endgroup$ Dec 1 '20 at 19:22
  • 5
    $\begingroup$ Temperature is irrelevant. Or I'd better put it this way: the rest of the gas might be as cold as you like, but this one molecule that has just formed from two atoms is very, very hot. $\endgroup$ Dec 1 '20 at 19:32
  • 2
    $\begingroup$ All right, speaking of the heat of one molecule is an abuse of language. Would it be better if I said that it has very high energy? $\endgroup$ Dec 1 '20 at 19:37
  • 1
    $\begingroup$ @amiltonmoreira - what is the binding energy of H2? $\endgroup$
    – Jon Custer
    Dec 1 '20 at 20:02
13
$\begingroup$

Yes there is validity to the finding that two atoms of hydrogen form molecular hydrogen at very slow rates. Review Gould, R.J., and Salpeter, Edwin E., Astrophysical Journal, Vol 138, pg. 393. It is publicly available at: http://articles.adsabs.harvard.edu/pdf/1963ApJ...138..393G

The exact answer to your question is found on page 138 of that work, under the heading “II. Mechanisms for the Formation of Molecular Hydrogen.”

In space, molecular hydrogen is destroyed (by cosmic radiation) at rates that exceed its formation without some type of surface catalyst. This conundrum motivated significant research to find the actual mechanisms of molecular hydrogen formation in natural settings. More recent work can be found by Gianfranco Vidali, et.al., Journal of Physics: Conference Series:6, 2005:
https://iopscience.iop.org/article/10.1088/1742-6596/6/1/003/pdf
This more recent work cites the Gould and Salpeter work. It appears to be still accepted as the explanation for the slow rate of formation of molecular hydrogen from atomic hydrogen.

According to this explanation, after ground state hydrogen atoms collide, the new hydrogen molecule will be in a triplet state, and it cannot decay into a singlet state because this is a forbidden transition. A cursory search on the PES's of triplet states of diatomic hydrogen show that indeed these are shallow curves which would lead to rapid dissociation.

$\endgroup$
2
  • 5
    $\begingroup$ Indeed, without a way to release energy the two atoms are perfectly happy to go back to being separate hydrogen atoms, since that is what they were. They have to get rid of energy to be in a bound state. $\endgroup$
    – Jon Custer
    Dec 2 '20 at 2:41
  • 4
    $\begingroup$ The important point is that this triplet state, while being perfectly bound, has a positive formation enthalpy. That means it has a finite lifetime. It just breaks apart after a millisecond or a day, and the two atoms take the energy (+impulse) with them again. $\endgroup$
    – Karl
    Dec 2 '20 at 9:30

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.