How do molecular orbitals differ from atomic orbitals?

Molecular orbitals are combinations of atomic orbitals that spread over two or more atoms and can be bonding, nonbonding, or antibonding.

Think of an atomic orbital like a single lamp shining light around one atom, and a molecular orbital like several lamps whose lights overlap between atoms to make brighter or darker areas. When the overlapping lights add together you get a bonding molecular orbital that holds atoms together, and when they cancel out you get an antibonding molecular orbital that can push atoms apart. Some overlaps do not change the brightness between atoms and those are nonbonding orbitals that mostly act like the original atomic lights. Electrons prefer to sit in the lowest energy orbitals, so they fill bonding orbitals first which helps form stable molecules.

Students often think molecular orbitals belong to only one atom, but they actually extend across the whole molecule, so always imagine them as shared spaces; remember to draw them across the atoms involved. Another common mistake is assuming all overlaps are the same, when in fact the shape and phase of atomic orbitals determine whether the molecular orbital is bonding or antibonding, so check how the lobes align. A last confusion is treating energy and shape separately, but the shape of an orbital affects its energy, so use both ideas together when predicting stability.

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Molecular vs Atomic Orbitals: Key Differences

1. Atomic orbital is like one lamp
2. Molecular orbital is overlapping lamps
3. Overlap adds to form bonding
4. Cancellation creates antibonding orbitals
5. Nonbonding orbitals act like originals
6. Electrons fill lowest energy first

Common Mistakes with Molecular Orbitals

1. Assuming orbitals belong to one atom
2. Treating all overlaps as identical
3. Separating orbital shape from energy

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