What is meant by bonding and antibonding molecular orbitals? Give number of electron which occupy bonding orbital in H_2^ + ,{H_2} and {H_{{e_{2 - }}}}

In molecular chemistry, bonding and antibonding molecular orbitals are the result of the combination of atomic orbitals from two or more atoms to form molecular orbitals. These molecular orbitals are responsible for the formation and stability of molecules. Here's a brief explanation of bonding and antibonding molecular orbitals:

Bonding Molecular Orbitals (σ, π, etc.):

Bonding molecular orbitals are formed when atomic orbitals overlap constructively in-phase with each other.
Electrons in bonding orbitals contribute to the stability of the molecule.
The energy of bonding molecular orbitals is lower than that of the parent atomic orbitals, which indicates a lower energy state and increased stability of the molecule.
Electrons in bonding orbitals help hold the atoms together, forming a chemical bond.
Antibonding Molecular Orbitals (σ, π, etc.)**:

Antibonding molecular orbitals are formed when atomic orbitals overlap destructively out-of-phase with each other.
Electrons in antibonding orbitals contribute to the instability of the molecule.
The energy of antibonding molecular orbitals is higher than that of the parent atomic orbitals, which indicates a higher energy state and decreased stability of the molecule.
Electrons in antibonding orbitals oppose the bonding electrons and can weaken or break the chemical bond.
Now, let's consider your specific examples:

H₂⁺ (Hydrogen Cation):

H₂⁺ has only one electron, as it's a positively charged hydrogen ion.
This electron occupies the lowest-energy molecular orbital available, which is the bonding σ orbital. So, there's 1 electron in the bonding orbital.
H₂ (Hydrogen Molecule):

H₂ has two electrons, each coming from one of the hydrogen atoms.
Both electrons occupy the bonding σ orbital. So, there are 2 electrons in the bonding orbital.
H₂₋ (Hydride Dianion):

H₂₋ has two electrons as well.
Both electrons occupy the antibonding σ* orbital. So, there are 2 electrons in the antibonding orbital.
In summary, bonding molecular orbitals are lower in energy and stabilizing, while antibonding molecular orbitals are higher in energy and destabilizing. The number of electrons occupying these orbitals depends on the specific molecule or ion in question.