Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. c. OF₂ d. CO₂

Verified step by step guidance

1. Identify the central atom in the molecule. For OF₂, the central atom is oxygen (O).
2. Determine the number of valence electrons for each atom. Oxygen has 6 valence electrons, and each fluorine has 7 valence electrons.
3. Calculate the total number of valence electrons in the molecule: 6 (from O) + 2*7 (from F) = 20 valence electrons.
4. Draw the Lewis structure for OF₂. Oxygen will form single bonds with each fluorine atom, using 4 electrons, and the remaining electrons will be lone pairs on the oxygen and fluorine atoms.
5. Determine the hybridization of the central atom. Oxygen in OF₂ has two lone pairs and two bonding pairs, leading to sp³ hybridization.

Key Concepts

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In the case of OF2, the central oxygen atom undergoes sp3 hybridization, resulting in four equivalent hybrid orbitals that can form sigma bonds with the fluorine atoms and accommodate lone pairs.

Bonding and Molecular Geometry

Bonding refers to the interactions between atoms that lead to the formation of molecules. In OF2, the oxygen atom forms two single bonds with two fluorine atoms, resulting in a bent molecular geometry due to the presence of two lone pairs on the oxygen, which repel the bonding pairs and influence the overall shape of the molecule.

Orbital Overlap Theory

Orbital overlap theory explains how atomic orbitals combine to form bonds. In OF2, the overlap of the sp3 hybrid orbitals of oxygen with the p orbitals of fluorine leads to the formation of sigma bonds. This concept is crucial for visualizing the bonding interactions and understanding the electron distribution in the molecule.