Are the chlorine atoms hybridized in BeCl2?
Hybridization occurs when atomic orbitals blend to form new atomic orbitals. Covalent bonds form when the atomic orbitals of two atoms overlap.
According to VSEPR theory, `BeCl_2` has a linear molecular geometry. This molecular geometry cannot be obtained by using `s, p` and `d` orbitals. Hybridization of the `2s` with one of the unoccupied `2p` orbitals in Be is the solution. The two `sp` hybrids of `Be` overlap with 3p orbitals of two ` Cl` atoms and form two bonds with bond angle of` 180^o`.
Beryllium needs two hybrid orbitals for the two sigma bonds. The two unhybridized `2p` orbitals of ` Be` remain unoccupied.
The number of the atomic orbitals mixed equals the number of hybrid orbitals. The types of atomic orbitals fused influence the types of hybrid orbitals.