Match each compound with its major type of intermolecular force. H2CO dipole-dipole C3H8 london dispersion K2CO3 electrostatic H2O hydrogen-bonding Xe atoms dipole-dipole
The Correct Answer and Explanation is:
Here is the correct matching of each compound with its major type of intermolecular force:
- H2CO (formaldehyde): Dipole-dipole
- C3H8 (propane): London dispersion
- K2CO3 (potassium carbonate): Electrostatic
- H2O (water): Hydrogen bonding
- Xe (xenon atoms): London dispersion
Intermolecular forces are the attractions that occur between molecules or atoms, influencing properties such as boiling point, melting point, and solubility. They can be categorized into dipole-dipole interactions, london dispersion forces, hydrogen bonding, and electrostatic forces.
Formaldehyde (H2CO) has a polar molecular structure due to the presence of oxygen, which creates a significant electronegativity difference. This results in dipole-dipole interactions, where polar molecules attract each other due to partial charges.
Propane (C3H8) is a nonpolar molecule because of its symmetric distribution of charge between carbon and hydrogen atoms. Nonpolar molecules primarily experience london dispersion forces, which arise from temporary dipoles induced in electron clouds.
Potassium carbonate (K2CO3) is an ionic compound composed of potassium cations (K+) and carbonate anions (CO3^2-). Ionic compounds exhibit electrostatic forces, which are strong attractions between positively and negatively charged ions.
Water (H2O) is a highly polar molecule with a bent structure, leading to partial positive charges on hydrogen atoms and a partial negative charge on oxygen. This allows water molecules to form hydrogen bonds, which are exceptionally strong intermolecular forces and contribute to its unique properties.
Xenon (Xe) atoms, although noble gases, exhibit london dispersion forces because their electron clouds can become temporarily polarized, creating transient attractions.
Understanding intermolecular forces helps explain why substances behave differently in various physical states and interactions.
