1. Chapter 10 2015 *

2. Kinetic Molecular Theory Particles of matter are in constant motion

3. The state of a substance at room temperature depends on the strength of the intermolecular forces between the particles.

4. 5 assumptions of Kinetic Theory 1. gases are tiny particles 2. particles have elastic collisions with each other 3. particles in constant motion 4.no forces between particles 5. speed of particles determined by temperature

5. Bonding (Intramolecular) ionic bond- transfer of electrons between cation (+) and anion(-) Subtract electronegativities to predict bond type Covalent bond- sharing of electrons – Nonpolar- equal sharing of electrons – Polar –unequal sharing of electrons

6. Polar molecule (covalent) has a slightly + and – side due to the difference in electronegativities of the elements involved.

7. Intermolecular forces Occur between 2 molecules (polar covalent) 3 major types: 1.dispersion 2. dipole to dipole 3. hydrogen bond

8. Dispersion force- temporary and weak strong polar molecule causes a nonpolar molecule to become slightly polar Dipole to Dipole slightly + end of one molecule is attracted to the slightly – end of another molecule Shape can cancel out polarity Hydrogen bond- attraction between molecules – Uses H,F, O, N. (generally the strongest attraction)

9. Properties of Gases Fluidity, expansion, diffusion occur due to the weak or none attraction between molecules Ideal gases have NO attraction between molecules Real gases have some attraction between molecules Ideal Gases are gases that follow the Kinetic Molecular theory Real Gases (all gases) deviate from the KMtheory

10. Which diffuses faster? High molar mass or low molar mass? Polar or nonpolar molecules? High IMF or low IMF?

11. A change of state occurs when IMF are formed or broken Increase in heat  ? Decrease in heat  ?

12. Changing gases into liquids – Increase pressure – Decrease temperature – This causes increase in IMF

13. How is a liquid changed to a gas? What happens to the IMF when this occurs?

14. Nonpolar gases nonpolar bonding– equal sharing of electrons Example– diatomics – List these? – Do these gases form IMF with other molecules? – Why?

15. Polar Gases Polar bonding- unequal sharing of electrons Form IMF with other molecules Examples- ammonia (NH 3 ) Water vapor

16. Liquids Liquids have strong enough IMF to prevent the substance from being a gas at room temp Physical properties are determined by the strength and type of IMF

17. Properties of Liquids Higher density than gases Slightly compressible Fluidity Viscosity Surface tension Capillary action Expansion Slow diffusion

18. Why is density higher than gases Why can a liquid pour

19. Viscosity- resistance to flow Effect of heat? Effect of heat on IMF? Surface tension- film that forms on the top of a liquid- due to the imbalance of forces

20. Why does water have a high viscosity? Why does water have a high surface tension?

21. Capillary Action- the movement of a liquid(water) in a small tube. This occurs because the attraction between the sides of the tube (adhesion) is greater than the attraction between the molecules (cohesion). The difference in the strength causes the water to rise (also explains the meniscus)

22. Evaporation- liquid to gas- depends on strength of IMF Slow rate of evaporation  IMF Strength? Fast rate of evaporation  IMF strength? Does water evaporate fast or slow? Why? Volatile and nonvolatile liquids—difference?

23. Low expansion  strength of IMF? Fast diffusion  strength of IMF

24. Properties of Solids High density Incompressibilty Definite shape Definite volume IMF strength?

25. Change of state/endo or exo Melting Freezing Sublimation Deposition Condensation Vaporization ** endothermic- heat is absorbed **exothermic- heat is released

28. Equilibrium vapor pressure is the pressure exerted by a liquid at equilibrium Boiling occurs when the equilibrium vapor pressure equals the atmospheric pressure.

29. Increase in Temperature increase or decrease IMF? Increase or decrease molecules going into a gas phase? Increase or decrease the equilibrium vapor pressure?

30. Decrease the Atmospheric pressure  decrease in the boiling point Increase in Atmospheric pressure  increases the boiling point