Lesson: Hybridization in Molecular Orbital Theory

In this lesson, we will learn how to explain the origin of hybrid orbitals based on electron pair energies and the symmetries of molecular orbitals.

Worksheet • 4 Questions

Q1:

How many bonds can an atom form using sp³ hybrid orbitals?

Q2:

How many bonds can an atom form using sp³d hybrid orbitals?

Q3:

In the valence bond theory description of methane, which of the following statements is not a valid justification for the use of sp³ hybrid orbitals?

AA atom could not form four bonds without hybridization, as the energy for promoting a 2s electron to the 2p subshell is too large.
BA tetrahedral bonding geometry with zero dipole moment is only possible if electron density is distributed equally between the four bonds.
CThe s orbital of each atom must overlap with the s orbital of the atom and at least one p orbital.
DOverlap of the s orbitals with the three p orbitals of the atom would produce bonds at to each other.
EThe bonds are exactly equivalent so must be generated by orbitals of equal energy.

Q4:

How many bonds can an atom form using sp hybrid orbitals?

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