IB SL Chemistry INTERMOLECULAR FORCES

Front

What are intermolecular forces?

Back

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

Front

What is hydrogen bonding?

Back

Hydrogen bonding is a type of strong dipole-dipole attraction that occurs when hydrogen is bonded to a highly electronegative atom (such as N, O, or F), resulting in a significant partial positive charge on the hydrogen atom.

Front

Does H2O have hydrogen bonding?

Back

Yes, H2O (water) exhibits hydrogen bonding due to the presence of hydrogen atoms bonded to oxygen, which is highly electronegative.

Front

What is the reason for the high boiling point of SiO2?

Back

The high boiling point of SiO2 is due to strong covalent bonds within its giant repeated structure, requiring a significant amount of energy to break.

Front

Does HF have hydrogen bonding?

Back

Yes, HF (hydrogen fluoride) has hydrogen bonding because hydrogen is bonded to fluorine, which is highly electronegative.

Front

Does CH4 have hydrogen bonding?

Back

No, CH4 (methane) does not have hydrogen bonding as it lacks highly electronegative atoms bonded to hydrogen.

Front

Which of the following has hydrogen bonding: CBr4, NO2, H2S, NH3?

Back

NH3 (ammonia) has hydrogen bonding due to the presence of hydrogen bonded to nitrogen, which is electronegative.

Front

What are dipole-dipole interactions?

Back

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

Front

What are London dispersion forces?

Back

London dispersion forces are weak intermolecular forces that arise from temporary dipoles in molecules, occurring in all molecules, whether polar or nonpolar.

Front

How do intermolecular forces affect 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.