SUMMARY
The intermolecular bonding in gaseous CH4 (methane) is classified as van der Waals forces, specifically due to its non-polar nature. The discussion clarifies that covalent bonds are intramolecular, holding the carbon and hydrogen atoms within a single molecule together, while intermolecular forces, such as van der Waals, act between separate CH4 molecules. The distinction between intermolecular and intramolecular forces is critical, as covalent and ionic bonds do not apply in this context. The correct answer to the homework question is D, van der Waals, as CH4 does not exhibit hydrogen bonding due to its non-polar characteristics.
PREREQUISITES
- Understanding of intermolecular vs. intramolecular forces
- Knowledge of covalent bonding in organic compounds
- Familiarity with non-polar molecules
- Basic principles of van der Waals forces
NEXT STEPS
- Research the different types of van der Waals forces: London dispersion, Debye, and Keesom forces
- Study the properties of non-polar molecules and their implications in chemistry
- Explore the differences between polar and non-polar molecules in terms of bonding
- Learn about the role of intermolecular forces in physical properties of substances
USEFUL FOR
Chemistry students, educators, and anyone interested in understanding molecular interactions and bonding types, particularly in organic chemistry contexts.