2. solid to liquid Melting

3. What phase of matter is “B”? A B C Temperature  Pressure  Liquid

4. ________is the gas phase of a substance normally solid or liquid at room temperature Vapor

5. Freezing occurs by the release of _____ energy

6. Describe a volatile liquid in terms of its rate of evaporation. Evaporates quickly

7. ______ is the resistance of a liquid to flow Viscosity

8. What phase of matter is “A”? A B C Temperature  Pressure  Solid

9. What is the normal boiling point of water? 100  C

10. Melting occurs by energy being ______. absorbed

11. ____________ is the temperature and pressure at which all 3 states of matter are at equilibrium Triple point

12. _______shows how states of matter are affected by changes in temperature/pressure Phase diagram

13. solid to gas Sublimation

14. The triple point of this substance occurs at: 5.2 atm & 216.6 K

15. __________ is a dynamic condition in which two opposing physical or chemical changes occur at equal rates in a given closed system Equilibrium

16. ________ is the temperature at which equilibrium vapor pressure equals atmospheric pressure Boiling point

17. _______ is the pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature. Equilibrium vapor pressure

18. ____________ is the spontaneous mixing of two or more substances. Diffusion

19. When energy is added to a substance, the particles would move ___________ Faster

20. When does a liquid boil? Equilibrium vapor pressure EQUALS atmospheric pressure

21. When energy is taken away from a substance, the particles would move __________ Slower

22. What is the most abundant liquid? Water

23. _____________ is a force common to all liquids that tends to pull adjacent parts of a liquid’s surface together. Surface tension

24. List 2 examples of surface tension. Meniscus Droplets can form Objects float Capillary rise

25. List a volatile substance Rubbing alcohol Nail polish remover Gasoline hairspray

26. When a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress. This is known as ___________ Le Chatelier’s Principle

27. liquid to solid Freezing

28. C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of H 2 O was increased, the system would shift to the ________ C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of H 2 O was increased, the system would shift to the ________ Right

29. How does a substance evaporate, if equilibrium vapor pressure is LOW? WHY? SLOWLY! B/c there are STRONG IM forces and requires MORE kinetic energy to become a vapor

30. Describe a liquid in terms of particle spacing. Particles are packed relatively closely together

31. Describe a liquid in terms of particle motion. Particles vibrate around MOVING points

32. gas to liquid Condensation

33. Describe the general volume of a liquid and use KMT to explain. Definite VOLUME- b/c particles are close together

34. Describe the general shape of a liquid and use KMT to explain. NO Definite SHAPE- b/c particles vibrate around moving points

35. Describe a liquid-vapor system at equilibrium. The number of particles leaving the liquid (vaporization) EQUAL the number of particles re- entering the liquid (condensation)

36. gas to solid Deposition

37. What happens to the boiling point of liquids on top of Mt. Everest? WHY? Boiling point is lower B/c atmospheric pressure is lower

38. liquid to gas Vaporization

39. What phase of matter is “C”? A B C Temperature  Pressure  Gas

40. What is the difference between the IM forces during melting and freezing? Melting = Less IM forces b/c more particle collisions Freezing = MORE IM forces b/c particles are moving slower