Select the correct statement for non-bonding and anti-bonding orbitals:
Select the correct statement for non-bonding and anti-bonding orbitals:
The correct options are
A Non - bonding orbitals have same energy as that of the atomic orbitals from which they are formed.
B Anti - bonding orbitals have higher energy than the atomic orbitals from which they are formed
A non-bonding orbital, also known as non-bonding molecular orbital (NBMO), is a molecular orbital whose occupation by electrons neither increases nor decreases the bond order between the involved atoms.
A non-bonding orbital could also be interpreted as a molecular orbital for which the addition or removal of an electron does not change the energy of the molecule.
Molecular orbitals come from the linear combination of atomic orbitals. In a simple diatomic molecule such as HF, F has more electrons than H.
If we construct a molecular orbital diagram, the unpaired valence - say present in the 2pz orbital - can combine with the 1s orbital of teh Hydrogen atom.
This gives two orbitals - a σ bonding orbital and a σ∗ antibonding orbital (unoccupied).
What happens to the 2p2x and the 2p2y orbitals of the fluorine atom? If we were using Lewis structures - they'd be considered lone pairs.
But here, for molecular orbitals, they become non-bonding orbitals (NBOs or NBMOs). Each of these NBOs (there are two - each with a pair of electrons),
will have the same energy as the parent atomic 2px and 2py orbitals. So adding or removing electrons to these doesn't change the energy of the overall molecule. Also,
it doesn't affect the bond-order! The NBMOs (non-bonding molecular orbitals) lie between the σ and the σ∗ orbitals.
A
Non - bonding orbitals have same energy as that of the atomic orbitals from which they are formed.
B
Anti - bonding orbitals have higher energy than the atomic orbitals from which they are formed
A non-bonding orbital, also known as non-bonding molecular orbital (NBMO), is a molecular orbital whose occupation by electrons neither increases nor decreases the bond order between the involved atoms.
A non-bonding orbital could also be interpreted as a molecular orbital for which the addition or removal of an electron does not change the energy of the molecule.
Molecular orbitals come from the linear combination of atomic orbitals. In a simple diatomic molecule such as HF, F has more electrons than H.
If we construct a molecular orbital diagram, the unpaired valence - say present in the 2pz orbital - can combine with the 1s orbital of teh Hydrogen atom.
This gives two orbitals - a σ bonding orbital and a σ∗ antibonding orbital (unoccupied).
What happens to the 2p2x and the 2p2y orbitals of the fluorine atom? If we were using Lewis structures - they'd be considered lone pairs.
But here, for molecular orbitals, they become non-bonding orbitals (NBOs or NBMOs). Each of these NBOs (there are two - each with a pair of electrons),
will have the same energy as the parent atomic 2px and 2py orbitals. So adding or removing electrons to these doesn't change the energy of the overall molecule. Also,
it doesn't affect the bond-order! The NBMOs (non-bonding molecular orbitals) lie between the σ and the σ∗ orbitals.
