Hybridization in Lewis Structures

[806021969]

When you have a Lewis Structure, how do you determine the hybridization of an atom in the molecule. Is there a rule or chart that makes it easier to determine this, I know that certain number of lone pairs contribute to the hybridization of an atom in a molecule, but I would like a more simplified explanation if possible.

[Shaniya Kerns 4D]

In order to determine the hybridization of a molecule you would look at the amounts of bonds/ electron groups the element is connected to. You would count the lone pairs as 1, single bond as 1, and the double bonds as 1. So if there were 3 single bonds(sigma) and 1 lone pair it would have 4 electron groups therefore it would have a hybridization of sp^3. sp^3 simply just means 1 s orbital, and 3 p orbitals. Each orbital has 2 electrons.

[Valeria Perez 3J]

In order to determine hybridization, you want to observe the electron domains in a similar way that we do when we are determining shape. This means that all bond to outer atoms, regardless of whether they are single, double, or triple bonds, count as one domain, and lone pairs also count as a single domain. Then, once you have your number of domains, you add up orbitals until you reach your domain number. I.e. if you have a domain number of 4, you take the single s orbital and it to 3 p orbitals to get 4 hybrid orbitals. if you have 5, you would use the single s and the 3 p orbitals, and also add in a single d orbital to get sp3d. Hope that makes sense!

[Isabelle Huerta 2I]

Count Electron Groups: Each bond (single, double, or triple) and each lone pair around the atom counts as one electron group.

Determine Hybridization:
Two Electron Groups: Hybridization: sp
Three Electron Groups: Hybridization: sp2
Four Electron Groups: Hybridization: sp3
Five Electron Groups: Hybridization: sp3d
Six Electron Groups: Hybridization: sp3d2