How Does Atomic Hydrogen Transform into Molecular Hydrogen?

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Discussion Overview

The discussion revolves around the transformation of atomic hydrogen into molecular hydrogen, exploring the conditions under which this occurs, particularly in the context of water dissociation and the role of electrodes in such reactions. Participants also delve into the characteristics of atomic versus molecular hydrogen and oxygen.

Discussion Character

  • Exploratory
  • Technical explanation
  • Debate/contested

Main Points Raised

  • One participant questions whether atomic hydrogen can be converted to molecular hydrogen through a chemical reaction, suggesting that the process occurs spontaneously without an energy barrier.
  • Another participant challenges the feasibility of producing atomic hydrogen in water and seeks clarification on the context of using electrodes in such a reaction.
  • A later reply introduces the concept of water dissociation using radio waves, referencing a university professor's claim that this process yields atomic hydrogen and oxygen without producing molecular forms.
  • Participants discuss the stability of atomic species, noting that they tend to recombine into molecular forms quickly, raising questions about the detection of molecular hydrogen in the described experiments.
  • There is a mention of the dissociation of water into H+ and OH- versus H* and OH*, with implications for the energy requirements of such processes.
  • Concerns are raised about the role of electrodes in the dissociation process, with one participant asserting that the dissociation into radical species does not constitute a redox reaction, suggesting that electrodes would not influence the outcome.

Areas of Agreement / Disagreement

Participants express differing views on the definitions and processes involved in the conversion of atomic to molecular hydrogen, with no consensus reached on the feasibility of producing atomic hydrogen in water or the implications of using electrodes in the reaction.

Contextual Notes

The discussion highlights limitations in the definitions of chemical reactions and the conditions under which atomic hydrogen can exist, as well as the potential instability of atomic species and their tendency to recombine.

Butterfly_grl
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As simple as the questions seems, I can't seem to find an answer.

1. Can atomic hydrogen by chemical reaction, be converted to molecular hydrogen?

2. what happens when putting electrodes in a reaction that would give me atomic hydrogen? would it be collected at the cathode like molecular hydrogen? The same question for atomic oxygen.

3. Finally, what are the main characteristics of atomic hydrogen and oxygen, and how are they differentiated from the molecular form.

If you please, could you mention any good books that would aid me with the subject ..

Thank you​
 
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1. Depends on how you define 'chemical reaction'. I wouldn't call it that. Atoms of hydrogen will spontaneously combine to form H2 molecules. There's no energy barrier ('activated complex') in doing so, so I would not characterize it as a 'proper' reaction.

2. What do you mean putting electrodes 'in the reaction'? You can't really produce atomic hydrogen in water.

3. Atomic species, with the exception of noble gases, are unstable. As I said, they form bonds with no barrier to doing so.
 
First of all thanks for the reply,

When I said water reaction to obtain atomic hydrogen, I meant "the dissociation of water with radio waves", I have emailed a university professor who stated in their email that --quote "we believe the radiation is ATOMIC H and O" and they also said that by examination there was no signs for H2 and O2 spectra.

That is why I thought about what would happen if we put electrodes in the reaction?

Any Ideas!
 
Okay, but the dissociation of water into H+ and OH- or into H* and OH*?

I'd need to know the details of what you're talking about. Saying atomic would indeed seem to imply the latter. (But the dissociation energy would require UV rather than radio waves)

You can naturally form atomic H and O in solution for brief periods of time, but since they're unstable they're going to eventually recombine to form water, H2, O2 etc. You'd normally expect at least some hydrogen atoms to find other ones to combine into H2, so that's probably why they were looking for H2 formation.

Anyway dissociation into the radical species isn't a redox reaction, no ions are formed, so electrodes wouldn't really change anything.
 

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