Valence Bond Theory, Hybrid Orbitals, and Molecular Orbital Theory

The video explains molecular orbitals, starting with atomic orbitals and their hybridization into molecular orbitals. It covers the formation of covalent bonds, using hydrogen as an example, and discusses the conservation of orbitals. The concept of hybridization is explored with carbon, detailing sp3, sp2, and sp hybridized orbitals. The video also demonstrates how to use orbital diagrams to calculate bond order, using examples like H2, O2, and N2.

What is the primary reason hydrogen atoms form diatomic molecules?

• Because they have no electrons

• To increase their atomic mass

• Due to additional electrostatic interaction

• To decrease their atomic number

How many hybridized molecular orbitals does carbon form when it is sp3 hybridized?

• Two

• Three

• Five

• Four

In an sp2 hybridized carbon, how many p orbitals remain unhybridized?

• Three

• None

• One

• Two

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

• Sigma bond

• Ionic bond

• Hydrogen bond

• Pi bond

How many pi bonds are present in a molecule of C2H2?

• Two

• Four

• Three

• One

What is the bond order of an oxygen molecule (O2)?

• 1

• 2

• 4

• 3

Why do nitrogen molecules have a triple bond between them?

• Because of their high atomic mass

• Due to a bond order of 1

• Due to a bond order of 3

• Because they are inert gases