9.4. Hybridization of Atomic Orbitals http://www.ck12.org
- The hybridization of nonequivalent atomic orbitals is necessary to correctly predict the bonding and molecular
geometries of many molecules. Hybrid orbitals form on the central atom and can either besp,sp^2 ,sp^3 ,sp^3 d,
orsp^3 d^2. The type of hybrid orbitals that are used is dictated by the electron domain geometry. - Sigma bonds are formed by the end-to-end overlap of bonding orbitals. Pi bonds are formed by the side-to-
side overlap ofporbitals. Single bonds are normally sigma bonds. A double or triple bond consists of one
sigma bond and either one or two pi bonds.
Lesson Review Questions
Reviewing Concepts
- How does valence bond theory describe covalent bonding?
- What is meant by hybridization of atomic orbitals?
- Indicate the hybridizations associated with each of the following electron domain geometries:
a. linear
b. tetrahedral
c. octahedral
d. trigonal planar
e. trigonal bipyramidal - Can two 2porbitals of an atom hybridize to give two hybridized orbitals? Explain.
- What are the bond angles between two orbitals of each hybrid?
a.sp^2
b.sp^3 d^2
c.sp
d.sp^3 - What is the difference between a sigma bond and a pi bond?
Problems
- Describe the bonding that occurs in each of the following diatomic molecules according to valence bond
theory, including which atomic orbitals overlap.
a. Br 2
b. H 2 S
c. N 2 - Given the following structure:
a. Indicate the hybridization of each of the five carbon atoms.
b. How many total sigma bonds and pi bonds are there in the molecule?- State the electron domain geometry and hybridization of the central atom in each of the following molecules.
Then, give the molecular geometry of each.