Professor Dave explains molecular orbitals, starting with atomic orbitals and their hybridization into molecular orbitals. He discusses the formation of covalent bonds through orbital overlap, using H2 as an example. The video covers hybridization, including sp3, sp2, and sp hybridization, and their roles in forming sigma and pi bonds. Orbital diagrams are used to calculate bond order, with examples like O2 and N2. The video concludes with a comprehension check and a call to subscribe.

What is the primary reason hydrogen atoms form diatomic molecules?

• To increase their atomic mass

• Due to electrostatic interactions between electrons and nuclei

• To decrease their atomic number

• Because they have more protons than electrons

What is the result of hybridizing carbon's 2s and 2p orbitals?

• Formation of sp hybridized orbitals

• Formation of sp3 hybridized orbitals

• Formation of d orbitals

• Formation of sp2 hybridized orbitals

In sp2 hybridization, how many p orbitals remain unhybridized?

• Two

• Three

• None

• One

What type of bond is formed by the overlap of unhybridized p orbitals in sp2 hybridization?

• Ionic bond

• Pi bond

• Metallic bond

• Sigma bond

How many pi bonds are formed in a molecule with sp hybridized carbon atoms?

• Three

• Two

• Four

• One

What is the orientation of unhybridized p orbitals in a molecule with sp hybridization?

• In the same plane as the sigma bond

• Parallel to the sigma bond

• Perpendicular to the sigma bond

• At a 45-degree angle to the sigma bond

What is the bond order of an H2 molecule?

• Three

• Two

• One

• Zero

How many electrons are in the antibonding orbitals of an O2 molecule?

• Eight

• Six

• Four

• Two

What is the bond order of an O2 molecule?

• Four

• Three

• Two

• One

What is the bond order of a nitrogen molecule (N2)?

• Four

• Three

• Two

• One