1. Chapter 9: liquids, solids, and solutions

3. The Rock Cycle

7. Igneous metamorphic Sedimentary The Rock Cycle

8. Igneous The Rock Cycle Igneous means “born of fire”

9. Magma Bedrock

11. But then the EARTH Won’t leave The poor rock alone!

12. Ice Wind Water ice water wind

15. Compression of sediments is One way Sedimentary Rock can be formed

16. Igneous metamorphic Sedimentary The Rock Cycle ?

18. Igneous metamorphic Sedimentary The Rock Cycle squished kinda melted

19. HOT!

20. Bands (can) form Metamorphic means “changed”

25. igneous metamorphic Sedimentary The Rock Cycle

28. liquids  Made up of particles in constant motion  Particles closer together than gases  Less KE than gases

29.  Definite volume  Fluidity  Relatively high density  Relatively incompressible  Dissolving ability  Ability to diffuse  Tendency to evaporate and boil  Tendency to solidify

30. Solids (2 types)  Crystalline (crystal): particles in orderly geometric pattern  Amorphous: random arrangement

31.  Definite shape  Definite volume  Nonfludity  Definite melting point  High density  Incompressibility  Slow rate of diffusion

32. Changes of state  Solid  liquid (melting)  Solid  gas (sublimation)

33.  Liquid  solid (freezing)  Liquid  gas: (vaporization)

34.  Gas  liquid: (condensation)

35.  Gas  solid: (deposition)

37. Phase diagram

39.  Triple point: solid, liquid, gas coexist at equilibrium for water = 273.16 kelvins (0.01 °C) and a pressure of 611.73 pascals (ca. 6.1173 millibars, 0.0060373057 atm). for water = 273.16 kelvins (0.01 °C) and a pressure of 611.73 pascals (ca. 6.1173 millibars, 0.0060373057 atm).kelvinspascalsmillibars atmkelvinspascalsmillibars atm  Critical temperature: gas can not be converted to a liquid no matter how much pressure is exerted beyond the critical temp. for water =374°C (647.096 K) for water =374°C (647.096 K)

40. Water cycle

41. Solutions  Homogeneous mixtures

42. Electrolyte  Substance that dissolves in water and gives a solution that conducts electric current, e.g. NaCl

43. Nonelectrolyte  Does not conduct electricity, e.g.sugar  WHY??

44. Solvent  Dissolving medium

45. Solute  Substance dissolved

46. Types of Solutions  1. Gaseous, e.g. air

47.  2. Liquid, e.g. vinegar

48.  3. Solid, e.g. brass (solution of copper (solution of copper and zinc) and zinc) + = + =

49. Alloy  Mixtures in which 2 or more elements (usually metals) are uniformly mixed

50. Solubility  The amt. of a substance required to form a saturated soln. with a specific amt. of solvent at a given temp.

51. Effect of temperature  Increase in temp. usually decreases solubility of a gas in a liquid  Increase in temp. usually increases solubility of a solid in a liquid

52. Solubility of a gas in water

54. Factors affecting solubility  Types of solvents, solutes  Pressure  temperature

55. Heat vs. temperature  Temperature is a number that is related to the average kinetic energy of the molecules of a substance. kinetic energykinetic energy  Heat is a measurement of the total energy in a substance

56. Saturated solution  Max. amt. of dissolved solute

57. Unsaturated soln.  Less solute than sat. soln

58. Supersaturated soln  More solute than sat. soln

59. Suspensions  Heterogeneous mixture, particles settle out, e.g. muddy water

60. Colloids  Particles intermediate in size between solutions and suspensions, e.g. a cloud

61. Factors affecting rate of dissolving  Increased surface area  Agitating soln  Heating

62. Freezing point depression  the difference between the freezing points of a pure solvent and a solution mixed with a solute. It is directly proportional to the concentration of the solution freezing pointssolventsolutionsolutefreezing pointssolventsolutionsolute

64. Boiling point elevation  a solution will have a higher boiling point than that of a pure solvent after the addition of a dissolved solute solutionboiling pointsolventsolutionboiling pointsolvent

66. Concentration  Measurement of the amt. of solute in a given amt of solvent

67. Molarity (M)  The number of moles of solute in one liter of solution molarity = # moles of solute molarity = # moles of solute # L of solution # L of solution

68. 0.500 mol of NaOH is dissolved in enough water to yield 1.00 L of solution 0.500 mol of NaOH is dissolved in enough water to yield 1.00 L of solution 0.500 mol NaOH 0.500 mol NaOH Molarity = 1.00 L soln. = 0.500 M NaOH

69. What is the molarity of 2.5 L of soln that contains 80.0 g of NaCl? 80.0 g NaCl x 1 mol NaCl x 1 58.4 g NaCl 2.5 L soln 58.4 g NaCl 2.5 L soln = 0.55 M NaCl (M = mol/ L) (M = mol/ L)

70. How many g of NaCl are needed to make 2,0 L of a 0.40 M soln? 0.40 mol NaCl x 58.4 g NaCl 1 mol NaCl 1 mol NaCl = 23.36 g/L 23.36 g x 2.0 L = 47 g NaCl in 2 L soln

71. Diluting Solutions  (M i ) (V i ) = (M f ) (V f )

72. You are given a solution of commercially available aqueous ammonia (14.8 M NH 3 ). How many mL of this soln is required to prepare 100.0 mL of 1.00 M NH 3 when diluted? M i V i = M f V f V i = M f V f M i M i =(1.00M) (100.0 mL) 14.8 M = 6.76 mL

73. Standard Deviation  Most common measure of statistical dispersion (how widely spread the values in a data set are) statistical dispersiondata setstatistical dispersiondata set  If the data points are close to the mean, then the standard deviation is small  If many data points are far from the mean, then the standard deviation is large

74.  Standard deviation calculated as follows:  For each value x i calculate the difference between x i and the average value.  Calculate the squares of these differences.  Find the average of the squared differences. This quantity is the variance σ2. variance  Take the square root of the variance.

75. Water  Most abundant liquid on Earth  70-90% of living mass  Covalent bonds between atoms within molecule  Hydrogen bonds between molecules  Highest density at 4 deg. C  biological/ ecological implications

76. Structure of water

77. Crystal structure of ice

78. Water cycle

79. JEOPARDY SOLIDSLIQUIDSSOLNSWATER 400400400400 300300300300 200200200200 100100100100

80. SCORES  TEAM 1  TEAM 2  TEAM 3  TEAM 4