Chemical Bonding and Hybridization Concepts

What is formed when atomic orbitals hybridize?

• Ionic bonds

• Molecular orbitals

• Metallic bonds

• Van der Waals forces

Why does a hydrogen molecule (H2) have lower energy than two separate hydrogen atoms?

• Due to increased kinetic energy of electrons.

• Because of additional electrostatic interaction between electrons and opposite nuclei.

• Due to the repulsion between the two hydrogen nuclei.

• Because the electrons are in a higher energy state.

How does carbon achieve sp3 hybridization to form four bonds, as seen in methane (CH4)?

• It combines one 2s orbital with two 2p orbitals.

• It promotes one 2s electron to a vacant 2p orbital, then hybridizes one 2s and three 2p orbitals.

• It only uses its 2p orbitals for bonding.

• It forms ionic bonds with hydrogen atoms.

What type of bond is formed by the overlap of unhybridized p-orbitals in an sp2 hybridized carbon atom?

• Sigma bond

• Ionic bond

• Pi bond

• Hydrogen bond

What is the bond order for a molecule with 8 electrons in bonding orbitals and 4 electrons in antibonding orbitals?

• 1

• 2

• 3

• 4