The core difference lies in where these orbitals exist: an atomic orbital describes an electron's behavior within a single atom, while a hybrid orbital describes the mixing of atomic orbitals to form new orbitals for bonding in a molecule.
Here's a breakdown:
| Feature | Atomic Orbital | Hybrid Orbital |
|---|---|---|
| Definition | Describes the region of space around a single atom's nucleus where an electron is likely to be found. | Describes the region of space formed by the mixing of two or more atomic orbitals on the same atom. |
| Location | Exists within a single, isolated atom. | Exists between atoms when they form a chemical bond to create a molecule. |
| Formation | Exists naturally around an atom. | Formed through a mathematical process called hybridization, which occurs when atoms bond. |
| Example | s, p, d, and f orbitals of an isolated atom. | sp, sp2, sp3 hybrid orbitals of a carbon atom in methane (CH4). |
| Reference | An atomic orbital is just referring to an atom's orbital in general. | Hybrid orbital refers to overlaps in orbitals between different atoms when they form a bond to form a molecule (i.e. sp3 is a hybridized orbital for a carbon atom in a CH4 molecule). |
In simpler terms, think of atomic orbitals as the "original" electron homes within an atom. When atoms get together to form molecules, their atomic orbitals can "mix" to create new, hybrid orbitals that are better suited for bonding. For example, carbon utilizes sp3 hybridized orbitals in methane (CH4), where one s orbital and three p orbitals mix to form four equivalent hybrid orbitals pointing towards the hydrogen atoms.
