Question

How does a hybrid orbital differ from a pure atomic orbital? Can two \(2 p\) orbitals of an atom hybridize to give two hybridized orbitals?

Short answer

A hybrid orbital differs from a pure atomic orbital in that it is a combination of two or more atomic orbitals, resulting in an orbital with a different characteristic shape and energy level. Yes, two \(2p\) orbitals can hybridize to give two hybridized orbitals.

Step-by-step solution

Defining Pure Atomic Orbital

A pure atomic orbital is the region in an atom where an electron with a given energy is likely to be found. They have characteristic shapes, denoted as \(s\), \(p\), \(d\), and \(f\) orbitals, each corresponding to a different shape and energy level.

Defining Hybrid Orbital

A hybrid orbital is a kind of atomic orbital that results from the mixing or 'hybridization' of two or more different pure atomic orbitals, resulting in a new, different orbital. They have characteristic shapes different from the pure atomic orbitals, and are often involved in covalent bonding.

Explaining the Difference

The key difference therefore between a pure atomic orbital and a hybrid orbital is that while the former exists alone and defines the space in which an electron is likely to be found, the latter is a combination of two or more atomic orbitals that results in an orbital with a different characteristic shape and energy level.

Hybridization of \(2p\) Orbitals

Indeed, two \(2p\) orbitals can hybridize to give two hybridized orbitals. In the process known as 'hybridization', different atomic orbitals mix to form new, equivalent hybrid orbitals. Therefore, two \(2p\) orbitals can mix to create two hybrid orbitals.