Hybrid orbitals

[paulacamara1E]

On my notes I have the sentence that says regions of electron density equal the number of hybrid orbitals. I copied it from Dr. Lavelle's powerpoint but I am having a hard time understanding this concept. Could someone further explain it in simple terms?

[Gabi Landes 1-H]

# of regions of electron density = # bonds and lone pairs around an atom

- a double bond, triple bond, or a lone pair counts as only one region of electron density

[404975170]

A region of electron density is either a pair of lone pair electrons or a bond (every single, double and triple bonds just counts as one region). The number of regions correspond to a hybrid orbital (s, sp, sp2 etc.)
1 region - s
2 regions- sp
3 regions- sp2
4 regions- sp3
5 regions- sp3d
6 regions-sp3d2

Count the number of regions of electron density around the particular atom you are focusing on and then it’s hybridization is shown above which should be memorized.

[Kalsuda Lapborisuth 1B]

Electrons are more likely going to be found in the bonding region. Logically, the amount of electron density region would be equal to the number of hybrid orbital.

[Haison Nguyen 1I]

Regions of electron density are the amount of bonds (single, double, and triple all count as one) or lone pairs a central atom has. So if there are 5 regions of electron density for example, it would be sp3d.

[Cameron Smith 1I]

What are the energy levels of hybrid orbitals in comparison to other orbitals?

[Raquel Floyd 1K]

The hybridized energy level becomes between the original energy levels. I am not sure if we are excepted to know how to find what the exact energy level value of the hybridized molecule.