What is the bond order of H₂⁺² based on MO theory?
Answers
Explanation:
For H2, bond order = 1/2 (2-0) = 1, which means H2has only one bond. The antibonding orbital is empty. Thus, H2 is a stable molecule. Again, in the MO, there is no unpaired electron, so H2 is diamagnetic.
Explanation:
Answers:
1-
MO for H2+.jpg
Bond order = 1/2 (1-0) = 1/2
Paramagnetic because it has one unpaired e- in the σ(1s) orbital.
2-
MO for H2-.jpg
Bond order = 1/2 (2-1) = 1/2
Paramagnetic because it has one unpaired e- in the σ*(1s) orbital.
3- H2 is the most stable because it has the highest bond order (1), in comparison with the bond orders (1/2) of H2+ and H2-.
4- Theoretically it would not be possible to form a molecule from two hydrides because the anti-bonding and bonding orbitals would cancel each other out. So, the bond order is zero. Because the antibonding ortibal is filled, it destabilizes the structure, making the "molecule" H22- very non-stable.
MO for H2 2-.jpg
Bond order = 1/2 (2-2) = 0 ---> no bond formation. Thus, this molecule doesn't exist.
