Which of the following determines the strength of a covalent bond?

• A. The number of lone pairs on the central atom
• B. The amount of overlap between the atomic orbitals of the bonded atoms
• C. The presence of hydrogen atoms in the molecule
• D. The difference in electronegativity between the bonded atoms

Answer: (B)

Verified step by step guidance

1. Understand that the strength of a covalent bond depends on how effectively the atomic orbitals of the bonded atoms overlap to form a stable bond.
2. Recall that greater overlap between atomic orbitals leads to stronger bonding interactions because electrons are held more tightly between the nuclei.
3. Recognize that the number of lone pairs on the central atom does not directly affect the bond strength between two bonded atoms, although lone pairs can influence molecular shape and bond angles.
4. Note that the presence of hydrogen atoms in the molecule does not inherently determine the strength of a covalent bond; bond strength depends on the specific atoms involved and their orbital interactions.
5. Understand that while electronegativity differences affect bond polarity, they do not directly determine the covalent bond strength; the key factor is the extent of orbital overlap.