Molecular orbitals of H2 and H2+

Q.
Use a molecular-orbital analysis to predict which species in each of the following pairs has the stronger bonding between atoms.
A.

The s-orbitals of the two H atoms merge to form one bonding orbital, sigma-1 and one antibonding orbital, sigma-1*. The strongest bonding between the two hydrogen atoms exists when we have 2 electrons in the sigma-1 bonding orbital and no electrons in the sigma-1* orbital.
The H ₂ molecule has 2 electrons in the sigma-1s bonding orbital which fills before the sigma-1s* orbital which has higher energy. That is equivalent ot 1 whole covalent bond.
The H ₂⁺ molecule has only 1 electron which goes into the sigma-1s bonding orbital and no electrons in sigma-1s*. That is equivalent to half a covalent bond. That should explain why the H ₂ molecule is more stable than the H ₂⁺ ion.
For more on molecular orbitals of diatomic molecules and ions, go to:

http://www.sparknotes.com/chemistry/bonding/molecularorbital/section1.html

http://www.ch.ic.ac.uk/vchemlib/course/mo_theory/main.html
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