Which characteristic of a molecule is most important for intermolecular forces, such as hydrogen bonding, to be effective in bonding?

• A. Polarity of the molecule
• B. Presence of metallic bonds
• C. Molecular mass
• D. Number of atoms in the molecule

Answer: (A)

Verified step by step guidance

1. Understand that intermolecular forces are attractions between molecules, not within them, and their strength depends on certain molecular characteristics.
2. Recognize that hydrogen bonding is a specific type of dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine, creating a strong dipole.
3. Identify that for hydrogen bonding to be effective, the molecule must have a significant polarity, meaning there is an uneven distribution of electron density creating partial positive and negative charges.
4. Note that metallic bonds are not related to intermolecular forces but are a type of bonding within metals, so they do not influence hydrogen bonding.
5. Understand that molecular mass and the number of atoms can affect physical properties like boiling point but are less directly related to the effectiveness of hydrogen bonding compared to molecular polarity.