Hello I have another hybridization question.
For example in BeF2 ... the electron configuration is 1s2, 2s2, 2p1. It gets hybridized to 1s2, 2s1, 2p2. I know that it will be a sp2 hybridization but I'm not exactly sure why. It's because the last p orbital has 2 electrons right? I'm not totally sure so I want to be positive. Please help thank you!
Be is 1s2 2s2. There are only four electrons.
To determine the hybridization in BeF2, we need to consider the number of electron pairs around the central atom (Be) and the number of atomic orbitals involved in bonding.
In BeF2, the central atom (Be) has two regions of electron density due to the presence of two fluoride (F) atoms. Since regions of electron density include both lone pairs and bonds, we count the number of bonded atoms and lone pairs around the central atom.
In this case, there are two bonded atoms and no lone pairs around Be.
Now, let's consider the atomic orbitals involved. The electronic configuration of Be (1s2, 2s2) indicates that it has two valence electrons in the 2s orbital.
During hybridization, the atomic orbitals mix to form new hybrid orbitals with different geometries and energies. The number of hybrid orbitals formed is equal to the number of involving atomic orbitals.
Since there are two regions of electron density (bonded atoms and no lone pairs), Be undergoes sp hybridization to form two sp hybrid orbitals.
In the process of hybridization, one 2s orbital and one 2p orbital of Be combine to form two new sp hybrid orbitals. These hybrid orbitals have a linear geometry.
Therefore, in BeF2, the central atom Be is sp hybridized.