2. Intermolecular Forces and the States of Matter
Solids: The particles of a solid have fixed positions and exhibit motions of vibration. Liquids: The particles of a liquid are free to move within the confines of the liquid. Gas: The particles of a gas are far apart and move randomly and rapidly.

3. Intermolecular Forces and the States of Matter
Melting point: The temperature at which a solid becomes a liquid.
Vaporization: The process of a liquid becoming a gas.
Boiling point: The temperature at which the particles of a liquid escape and become a gas.

4. Intermolecular Forces and the States of Matter
Condensation: The process by which a gas becomes a liquid.
Freezing: The process by which a liquid becomes a solid. This occurs at the freezing point, which is the same as the melting point.
Sublimation: When a solid changes directly from the solid to the gaseous state.

5. Intermolecular Forces and the States of Matter

6. Intermolecular Forces and the States of Matter
Ionic bonds: Ionic bonds are the strongest of
forces that hold matter in the condensed states.

7. Intermolecular Forces and the States of Matter
Dipole forces: Polar molecules exist as dipoles.
These oppositely charged ends will attract each
other.

8. Intermolecular Forces and the States of Matter
Hydrogen bonds: When a hydrogen atom is covalently bonded to a highly electronegative atom like nitrogen, oxygen, or fluorine (N,O,F), it can exhibit an additional polar attraction. This attraction is called a hydrogen bond.

9. Intermolecular Forces and the States of Matter
Dispersion forces: Nonpolar molecules exhibit a dynamic induced dipole, the strength of which increases with molecular weight. The resulting dipole attractions are called dispersion forces or London dispersion forces.
© 2013 Pearson Education, Inc.

10. Intermolecular Forces and the States of Matter
Solution: A homogeneous mixture of two or more substances.
Solute: A substance that is dispersed in a solution.
Solvent: The substance doing the dissolving, usually present in greatest quantity.

11. Intermolecular Forces and the States of Matter

12. Intermolecular Forces and the States of Matter
“Like dissolves like”: Solutions form most readily
when both the solute and solvent have similar
intermolecular forces.

13. Intermolecular Forces and the States of Matter
Ionic substances dissolve in water through ion-dipole interactions.

14. Kinetic Molecular Theory of a Gas
The Gas Laws
Kinetic Molecular Theory of a Gas
Postulates:
The particles of a gas are in rapid constant motion.
The particles of a gas are tiny compared to the distance between them.
There is little attraction between the particles of a gas.
Collisions between gas molecules are perfectly elastic.
Temperature is a measure of the average kinetic energy of gas molecules.

15. The Gas Laws

16. The Gas Laws
Boyle’s law: At constant temperature, the volume of a gas is inversely proportional to its pressure.
V α 1/P
V = a/P
PV = a
V1P1 = V2P2

17. The Gas Laws Boyle’s law: At constant temperature,
the volume of a gas is
inversely proportional
to its pressure.

18. The Gas Laws Boyle’s law: At constant temperature,
the volume of a gas is
inversely proportional to its pressure.

19. The Gas Laws
Charles’s law: At constant pressure, the volume of a gas is directly proportional to its absolute temperature.
V α T
V = bT
V/T = b
V1/T1 = V2/T2

20. The Gas Laws Charles’s law: At constant pressure, the
volume of a gas is
directly proportional to
its absolute
temperature.

21. The Gas Laws
Charles’s Law

22. The Gas Laws
Avogadro’s law: At fixed temperature and pressure, the volume of a gas is directly proportional to the amount of gas.
V α n
V = cn
V/n = c
V1/n1 = V2/n2

23. The Gas Laws
Standard temperature and pressure: Standard temperature = 0 oC Standard pressure = 1 atm A mole of any gas at STP occupies 22.4 L

24. The Gas Laws
Combined gas law:
P1V1 = P2V2
T T2

25. The Gas Laws
Ideal gas law:
PV = nRT
R =