Valence Bond Theory: A Journey into Chemical Bonding

The video tutorial explains the valence bond theory proposed by Hitler and London, focusing on the concept of atomic orbital overlap in bond formation. It describes how half-filled atomic orbitals overlap to form covalent bonds, using hydrogen atoms as an example. The tutorial highlights the importance of orbital overlap in reducing energy and forming stable molecules. It also explains the formation of a sigma bond in a hydrogen molecule through axial overlap of atomic orbitals, emphasizing the role of electron cloud concentration in molecular stability.

What is the primary condition for atomic orbitals to overlap and form a covalent bond?

• They must have opposite spins.

• They must be empty.

• They must be half-filled.

• They must be fully filled.

How does the overlap of atomic orbitals affect the energy of the system?

• It increases the energy.

• It doubles the energy.

• It decreases the energy.

• It has no effect on the energy.

What determines the strength of a covalent bond according to valence bond theory?

• The extent of orbital overlap.

• The temperature of the environment.

• The number of electrons involved.

• The type of atoms involved.

In the formation of a hydrogen molecule, what type of overlap occurs between the 1 S orbitals?

• Pi overlap

• Delta overlap

• Theta overlap

• Sigma overlap

What is the significance of the electron cloud being concentrated between the nuclei in a hydrogen molecule?

• It causes the molecule to ionize.

• It decreases the bond length.

• It stabilizes the molecule.

• It increases repulsive forces.