IMFs

Front

What are intermolecular forces (IMFs)?

Back

Intermolecular forces (IMFs) are the forces of attraction or repulsion between neighboring particles (molecules, atoms, or ions). They are weaker than intramolecular forces, which hold atoms together within a molecule.

Front

How do intermolecular forces compare to intramolecular forces?

Back

Intramolecular forces are chemical bonds that hold atoms together within a molecule, while intermolecular forces are the attractions between molecules.

Front

What type of intermolecular force is present in water (H2O)?

Back

Water exhibits hydrogen bonding, which is a strong type of dipole-dipole interaction.

Front

What are London dispersion forces (LDF)?

Back

London dispersion forces (LDF) are weak intermolecular forces that arise from temporary dipoles in molecules, occurring in all atoms and molecules, but are the only type of IMF present in nonpolar substances.

Front

What is dipole-dipole interaction?

Back

Dipole-dipole interactions are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.

Front

Which substance has stronger intermolecular forces: H2O or CH4?

Back

H2O has stronger intermolecular forces due to hydrogen bonding, while CH4 has weaker London dispersion forces.

Front

What factors affect the strength of intermolecular forces?

Back

The strength of intermolecular forces is affected by molecular size, shape, polarity, and the presence of functional groups.

Front

What is the relationship between intermolecular forces and boiling point?

Back

Substances with stronger intermolecular forces generally have higher boiling points because more energy is required to overcome these forces.

Front

What type of intermolecular forces are present in PH3?

Back

PH3 exhibits dipole-dipole interactions due to its polar nature.

Front

How do intermolecular forces influence evaporation rates?

Back

Stronger intermolecular forces result in lower evaporation rates, as more energy is needed to break these forces for molecules to escape into the vapor phase.