[pikkaso]

Hi,
This is the question ---

The bond dissociation energy of H2 is 435 kj/mol; that is, it takes this amount of energy to dissociate H2 into its atoms. Estimate the bond dissociation of H2+ and explain your answer.

If someone can help, please. Thank you.

[Borek]

How many electrons create bond in the H₂ particle?

And how many in H₂⁺?

[Blueshawk]

How can it be estimated by that???

i used heat of formation

but H2+  doesnt seem stable, so it can be predicted that it will have a - NRG, thus the dissociation is spontaneous, but that is all I could guess without other numbers.

How do you do it Borek?

[Borek]

but H2+  doesnt seem stable

H₂⁺ is quite stable. It is well known particle, the simplest existing (thus researched by quantum chemistry ad nauseatum).

First approximation in the quantum calculations for atoms/particles with more than one electron is that electrons are independent (they don't interact with each other). If so, each electron should be responsible for the same "amount" of bond strength.

In this particular case error caused by the electron interaction neglection is in the 15% range.

[Blueshawk]

hmmm maybe I had a few numbers off,

so what is the bond dissociation NRG, shouldnt it be slightly less with only the interaction of 1 electron with the nuclei, instead of 2 as in H2???

therefore there is slightly less holding them together??, I know..bad wording


EDIT: spellcheck

[Jiro]

So if it has a half filled sigma boding molecular orbital it can still exist but not stable? does He2+ exist? I guess it does 1 anti bond however.?