Front

What are intermolecular forces?

Back

Intermolecular forces are the forces of attraction or repulsion between neighboring particles (molecules, atoms, or ions). They play a crucial role in determining the physical properties of substances.

Front

What is the strongest type of intermolecular force?

Back

Hydrogen bonding is the strongest type of intermolecular force, occurring between molecules that have hydrogen bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine.

Front

What is dipole-dipole attraction?

Back

Dipole-dipole attraction is an intermolecular force that occurs between polar molecules, where the positive end of one molecule is attracted to the negative end of another.

Front

What are London dispersion forces?

Back

London dispersion forces are weak intermolecular forces that arise from temporary dipoles in molecules, present in all molecules but are the only forces in nonpolar molecules.

Front

Which molecules exhibit hydrogen bonding?

Back

Molecules that have hydrogen bonded to nitrogen (N), oxygen (O), or fluorine (F) exhibit hydrogen bonding.

Front

What is the relationship between molecular size and London forces?

Back

As molecular size increases, London dispersion forces also increase due to a larger electron cloud, leading to greater polarizability.

Front

What is the significance of intermolecular forces in determining boiling points?

Back

Stronger intermolecular forces result in higher boiling points, as more energy is required to overcome these forces during the phase change from liquid to gas.

Front

What type of intermolecular force is present in I2?

Back

I2 exhibits only London dispersion forces, as it is a nonpolar molecule.

Front

How do dipole-dipole forces compare to London forces?

Back

Dipole-dipole forces are generally stronger than London dispersion forces because they involve permanent dipoles rather than temporary ones.

Front

What is a metallic bond?

Back

A metallic bond is the attraction between positive metal ions and a 'sea' of delocalized electrons, allowing for conductivity and malleability.