1. Liquids Liquids Chapter 10

2. Review: Gases Indefinite shape Indefinite shape Indefinite volume Indefinite volume Take the shape and volume of container Take the shape and volume of container Particles are far apart Particles are far apart Particles move fast Particles move fast Low Density Low Density Easy to expand and compress Easy to expand and compress

3. Review: Solids Review: Solids Definite shape Definite shape Definite volume Definite volume Particles close together, fixed Particles close together, fixed Particles move very slowly Particles move very slowly High density High density Hard to expand/compress Hard to expand/compress

4. Liquids: in between Closer to properties of solids Closer to properties of solids Slow diffusion Slow diffusion High attraction between particles High attraction between particles Medium amount of energy Medium amount of energy

5. Forces of Attraction Intramolecular forces: Hold atoms together within a molecule Intramolecular forces: Hold atoms together within a molecule covalent and ionic bonds covalent and ionic bonds Intermolecular forces: Hold molecules to each other Intermolecular forces: Hold molecules to each other 3 types 3 types

6. Dipole-Dipole Attraction Dipole: molecule with a separation of charge (polar covalent) Dipole: molecule with a separation of charge (polar covalent) Due to differences in electronegativity Due to differences in electronegativity ~1% as strong as a covalent bond ~1% as strong as a covalent bond

7. Hydrogen Bond Hydrogen Bond Very strong dipole-dipole attraction (10% of a covalent bond’s strength) Very strong dipole-dipole attraction (10% of a covalent bond’s strength) Occurs when H is bonded to O, N, F in a very polar bond Occurs when H is bonded to O, N, F in a very polar bond O H O H 3.5 2.1 3.5 2.1 Gives water its unusual properties Gives water its unusual properties

8. H-Bonding Affects Boiling Points Strong attraction requires much energy to overcome, so water is a liquid at normal temperatures Strong attraction requires much energy to overcome, so water is a liquid at normal temperatures

9. London Dispersion Forces Occur in all substances-polar and nonpolar Occur in all substances-polar and nonpolar Due to formation of instantaneous dipoles as electrons moving around nucleus concentrate on 1 side of molecule or atom Due to formation of instantaneous dipoles as electrons moving around nucleus concentrate on 1 side of molecule or atom

10. This induces a dipole in neighboring atoms or molecules This induces a dipole in neighboring atoms or molecules These are the weakest intermolecular forces These are the weakest intermolecular forces These are the only forces of attraction in nonpolar substances These are the only forces of attraction in nonpolar substances

11. Importance of Water Covers 70% earth’s surface Covers 70% earth’s surface Necessary for reactions in living cells Necessary for reactions in living cells Moderates earth’s temperature Moderates earth’s temperature Coolant for engines & nuclear power plants Coolant for engines & nuclear power plants Transportation Transportation Growth medium for many organisms Growth medium for many organisms

12. Properties of Water Colorless Colorless Tasteless Tasteless At 1 atm, water freezes at 0°C and vaporizes completely at 100°C At 1 atm, water freezes at 0°C and vaporizes completely at 100°C  Liquid phase occurs from 0-100°C  Liquid phase occurs from 0-100°C

13. Special Properties of Water Surface Tension Surface Tension Liquids tend to form a “skin” making the surface less penetrable by solids Liquids tend to form a “skin” making the surface less penetrable by solids

14. Unequal attraction at surface, mainly down Unequal attraction at surface, mainly down Equal attraction in all directions

15. Surface Tension Detergents can interfere with the attractions and will cause the paperclip to fall Detergents can interfere with the attractions and will cause the paperclip to fall

16. Adhesion Attraction of the surface of a liquid to the surface of a solid Attraction of the surface of a liquid to the surface of a solid Depends on the material Depends on the material Water is attracted to glass Water is attracted to glass Mercury is not Mercury is not No adhesion

17. Cohesion Molecular attractions within a material Molecular attractions within a material (water molecules to water molecules, for example) (water molecules to water molecules, for example) Here, cohesion Here, cohesion causes water to form beads; ad- hesion causes it to stick to the web

18. Capillary Action A liquid rises in a narrow tube when it breaks the surface tension A liquid rises in a narrow tube when it breaks the surface tension Movement of water through paper Movement of water through paper

19. Ice Floats! Molecules in a liquid have more movement than a solid and more energy (particles move apart Molecules in a liquid have more movement than a solid and more energy (particles move apart Generally, solids are more dense than theirir liquids Generally, solids are more dense than theirir liquids Liquid water Liquid water

20. Ice When water becomes fixed points in a solid, hydrogen bonds hold molecules in place When water becomes fixed points in a solid, hydrogen bonds hold molecules in place Gives ice an open hexagonal structure Gives ice an open hexagonal structure Greater volume means lower density than a liquid Greater volume means lower density than a liquid

21. Lower K.E. causes distance between molecules to be less Higher K.E. causes distance between molecules to be more Max. density at 4  C

22. Phase Changes of Water At 1 atm, water freezes at 0°C and vaporizes completely at 100°C At 1 atm, water freezes at 0°C and vaporizes completely at 100°C  Liquid phase occurs from 0-100°C  Liquid phase occurs from 0-100°C Changes from one phase to another will either require energy or release energy Changes from one phase to another will either require energy or release energy Solid Liquid Solid Liquid Liquid Gas Liquid Gas Solid Gas Solid Gas Melting/Freezing Vaporization/Condensation Sublimation/Deposition

23. From Solid to Liquid As energy is added, K.E. increases As energy is added, K.E. increases Solid warms up Solid warms up At 0°C, solid begins to melt and temperature remains at 0 until all solid is turned to liquid At 0°C, solid begins to melt and temperature remains at 0 until all solid is turned to liquid When all is liquid, temperature begins to rise When all is liquid, temperature begins to rise

24. From Liquid to Gas As heat is added, K.E. increases (increase in temperature) As heat is added, K.E. increases (increase in temperature) At 100  C, bubbles form in liquid At 100  C, bubbles form in liquid Temperature remains the same until all liquid is converted to a gas. Temperature remains the same until all liquid is converted to a gas. Once all is a gas, added energy causes temperature to increase Once all is a gas, added energy causes temperature to increase

25. Ice melting/water vaporizing When a substance is in phase, increasing the energy increases the temperature When a substance is in phase, increasing the energy increases the temperature When a substance is changing phase, increasing the energy does not increase the temperature but is used to break forces of attraction between molecules When a substance is changing phase, increasing the energy does not increase the temperature but is used to break forces of attraction between molecules

26. Phase diagram Temperature vs. Energy Temperature vs. Energy

27. Heating a Solid

28. Melting a Solid

29. Heating a Liquid

30. Vaporizing a Liquid

31. Heating a Gas

32. Calculating Energies Energy is measured in calories or Joules Energy is measured in calories or Joules 1.00 cal = 4.184 J 1.00 cal = 4.184 J The amount of energy needed to change states depends on: The amount of energy needed to change states depends on: 1. Type of matter 2. Quantity of matter

33. Type of matter Molar heat of fusion (  H fusion )= energy needed to melt 1 mole of a substance Molar heat of fusion (  H fusion )= energy needed to melt 1 mole of a substance Molar heat of vaporization (  H vap )= energy needed to vaporize 1 mole of a substance Molar heat of vaporization (  H vap )= energy needed to vaporize 1 mole of a substance

34. For Water (  H fusion ) = 80.0 cal/g =.334 kJ/g (  H fusion ) = 80.0 cal/g =.334 kJ/g (  H vap ) = 540. cal/g = 2.26 kJ/g (  H vap ) = 540. cal/g = 2.26 kJ/g

35. Finding Energy in a Phase Change Change from a solid liquid Change from a solid liquid q = m  H fusion q = m  H fusion Change from a liquid gas Change from a liquid gas q = m  H vap q = m  H vap q = energy (cal or J) m = mass (g)  H fusion =heat of fusion (cal/g) q = energy (cal or J) m = mass (g)  H vap =heat of vaporization

36. Example How much heat in calories is needed to melt 15.0 g of water? q = m  H fusion q = m  H fusion 15.0 g water x 80.0 cal = 1.20 x 10 3 cal 1 g water 1 g water

37. Energy and Being In Phase When all of a substance is in one phase, (e.g. all liquid), the amount of energy required to cause a temperature change depends on: When all of a substance is in one phase, (e.g. all liquid), the amount of energy required to cause a temperature change depends on: 1. type of substance 2. amount of substance 3. range of temperature change

38. Type of Matter Specific Heat (c): Energy required to change the temperature of 1 gram of a substance by 1 Celsius degree Specific Heat (c): Energy required to change the temperature of 1 gram of a substance by 1 Celsius degree c g = specific heat of a gas c g = specific heat of a gas c l = specific heat of a liquid c l = specific heat of a liquid c s = specific heat of a solid c s = specific heat of a solid

39. For Water c g =.480 cal/g  C or 2.01 J/g  C c g =.480 cal/g  C or 2.01 J/g  C c l = 1.00 cal/g  C or 4.18 J/g  C c l = 1.00 cal/g  C or 4.18 J/g  C c s =.500 cal/g  C or 2.09 J/g  C c s =.500 cal/g  C or 2.09 J/g  C

40. Finding Energy When In Phase q = mc  T q = mc  T  T = T final – T initial  T = T final – T initial q = energy (cal or J) m = mass (g) c = specific heat (cal/g  C)  T =change in temperature (  C)

41. Example How much energy is required to heat 50.0 g of water from 20.0  C to 85.0  C? How much energy is required to heat 50.0 g of water from 20.0  C to 85.0  C? q = mc l  T q = mc l  T  T = 85.0 – 20.0 = 65.0  C  T = 85.0 – 20.0 = 65.0  C q = (50.0g)(1.00 cal/g  C)(65.0  C) q = (50.0g)(1.00 cal/g  C)(65.0  C) q = 3,250 cal q = 3,250 cal

42. Phase changes

43. In Phase

44. Phase diagram Temperature vs. Energy Temperature vs. Energy

45. Phase Change Problems 1. Draw graph. 2. Mark start and stop points. 3. Every corner means a new equation is needed. 4. Flat sections will use q = m  H ( no  T means no slope). 5. Find each energy (q 1, q 2, q 3..). 6. Add all energies to get the total energy.

46. Phase Changes Vaporization (evaporation): molecules of a liquid escape the liquid’s surface Vaporization (evaporation): molecules of a liquid escape the liquid’s surface Requires energy to overcome intermolecular forces Requires energy to overcome intermolecular forces Molecules with enough energy to evaporate Maxwell Boltzman distribution

47. To evaporate, a particle must: To evaporate, a particle must: Be at the surface Be at the surface Have sufficient energy Have sufficient energy Be moving in the right direction Be moving in the right direction Not at surface Moving in the wrong direction Not enough energy I’m free!!

48. Evaporation produces Vapor Pressure 1. A closed container with a vacuum has a liquid added to it. 2. Molecules begin to evaporate 3. Some particles are recaptured by the liquid 4. Eventually rate of particles leaving = rate of being recaptured

49. Equilibrium Vapor Pressure When rate of evaporation = rate of condensation the pressure becomes constant (Equilibrium vapor pressure) When rate of evaporation = rate of condensation the pressure becomes constant (Equilibrium vapor pressure)

50. Vapor pressure and temperature As temperature increases, more particles evaporate As temperature increases, more particles evaporate

51. Vapor Pressure The vapor pressure of substances varies greatly, depending on the strength of the forces of attraction between particles. The vapor pressure of substances varies greatly, depending on the strength of the forces of attraction between particles.

52. Volatile liquids evaporate easily Volatile liquids evaporate easily Small particle size Small particle size Only London dispersion forces of attraction Only London dispersion forces of attraction

53. Boiling Occurs when the equilibrium vapor pressure reaches atmospheric pressure Occurs when the equilibrium vapor pressure reaches atmospheric pressure Only then can a bubble maintain itself anywhere in the liquid Only then can a bubble maintain itself anywhere in the liquid Particle of gas exerts pressure on surrounding molecules, pushing them out of the way, and therefore up against air pressure

54. This is the difference between evaporation and boiling This is the difference between evaporation and boiling

55. As atmospheric pressure changes, so does the equilibrium vapor pressure necessary for boiling to occur As atmospheric pressure changes, so does the equilibrium vapor pressure necessary for boiling to occur Therefore, the boiling point depends on the pressure Therefore, the boiling point depends on the pressure

56. Vapor Pressure vs. Temperature can give us the boiling point of a substance at any pressure Vapor Pressure vs. Temperature can give us the boiling point of a substance at any pressure The b.p. at 1 atm is called the normal boiling point. The b.p. at 1 atm is called the normal boiling point.

57. P vs. T Phase Diagram We can expand our graph to see the effect of pressure on melting/freezing and sublimation/deposition We can expand our graph to see the effect of pressure on melting/freezing and sublimation/deposition For a “normal” substance: For a “normal” substance: Increasing pressure raises the melting point (AD) Increasing pressure raises the melting point (AD)

58. Important Points on Diagram A: Triple point: temperature & pressure at which solid, liquid and gas coexist at equilibrium A: Triple point: temperature & pressure at which solid, liquid and gas coexist at equilibrium B: Critical Point: indicates critical temp and pressure B: Critical Point: indicates critical temp and pressure Critical Temp: temp above which substance cannot exist in a liquid state Critical Temp: temp above which substance cannot exist in a liquid state Critical Pressure: lowest pressure required for substance to exist as a liquid at the critical temperature Critical Pressure: lowest pressure required for substance to exist as a liquid at the critical temperature

59. Phase Diagram for Water Line AB slants backwards. Line AB slants backwards. Increasing the pressure lowers the melting point. Increasing the pressure lowers the melting point.

60. 1 atm 0°C 100°C