1. Anything that has mass and takes up space.

3. Substances Versus Mixtures Substances- cannot be separated by physical means. Mixtures- can be separated by physical means

4. Pure Substance uniform composition All samples have identical properties like boiling point, melting pt., color, and density which can be used to identify the substance **Review: Are these intensive or extensive properties?

5. Element Building block for everything else Cannot be broken down or separated by ordinary chemical or physical means Represented by chemical symbol Ex. Iron, copper, silver, hydrogen Remember the diatomic elements/molecules

6. Compounds 2 or more different elements chemically combined Have different properties than components Separated into elements ONLY by chemical means (chemical reactions) Definite composition (constant element proportion) Represented by a chemical formula Ex. H 2 O (water), NaCl (sodium chloride)

7. Mixture A physical blend of 2 or more substances Can be separated by physical means like filtration, distillation, etc. Individual components keep their identifying properties

8. Homogeneous mixture Components are uniformly distributed, there are parts but you cannot see them. Also called solutions. Ex. Salt water, air, brass Heterogeneous mixture Not uniform, you can see the parts Can settle upon standing Ex. Oil and vinegar, salt and pepper, soil, trail mix

10. Classify 1. Which represent substances? 2. Which represent mixtures? 3. Which is an element? 4. Which is a heterogeneous mixture?

11. CFU

12. Separation Techniques

13. MAGNETISM Use when: one of the substances in the mixture is magnetic.

14. FILTRATION Use when: one of the substances in the liquid mixture is an insoluble solid Other information: the insoluble substance is removed from the liquid mixture using a porous barrier (filter paper).

15. EVAPORATION Use when: the mixture is an aqueous solution containing a soluble solid Other information: the water will boil off and the soluble solid will remain in the evaporating dish

16. DISTILLATION http://www.youtube.com/watch?v=3VRi0KPGb3o http://www.youtube.com/watch?v=3VRi0KPGb3o Use when: the mixture is composed of two or more liquids Other information: based on differences in boiling points; liquid with lowest BP will boil (and then condense) first

17. CHROMOTOGRAPHY Use when: separating a mixture such as ink, chlorophyll Other information: based on the distance the components of a mixture travel (mobile phase) on the surface of, or within, another material (usually cellulose paper, called stationary phase) https://www.youtube.com/watch?v=ZCzgQXGz9Tg

18. A Homogeneous Mixture that can be separated by physical means.

19. Solution Vocabulary Solution – a homogeneous mixture that consists of: Solute – substance that dissolves, present in lesser amount Solvent – thing that does the dissolving, present in greatest amount.

20. heating curves solutions are NOT pure substances the amount of solute varies in solutions, and so does the BP and FP ↑amount of solute, ↑BP, ↓FP heating curves for solutions will not be consistent

21. Dissociate – to separate into ions Electrolyte-any substance that dissociates and produces ions that conduct electricity. Ex. Salt (solute) dissociates in water and the solution conducts electricity Non-electrolyte – any substance that does not dissociate and therefore does not contain ions that conduct electricity. Ex. Sugar (solute) does not dissociate in water so the solution does not conduct electricity

22. Dissolving a solvent surrounds a solute Your body relies on water to dissolve the molecules in your body. Watch this:

23. Soluble substance dissolves in solvent Ex. Sugar (solute) is soluble in water (solvent) Insoluble substance does not dissolve in solvent Ex. Sand is insoluble in water

24. Miscible- describes two liquids that do mix Immiscible – describes two liquids that do not mix

25. Solution Types Solvent is Gas – ex. Air (nitrogen gas is the solvent) Solvent is Liquid –ex. Sugar water (water is the solvent) WATER IS THE MOST COMMON SOLVENT AND IS CALLED THE UNIVERSAL SOLVENT Solvent is Solid – ex. Nitrinol (titanium dissolved in nickel, nickel is solvent, used to make braces)

26. Solubility Maximum amount of solute that will dissolve in a given amount of solvent at a given temp & pressure Usually expressed as “grams of solute per 100 g of solvent”. Affected by changes in the temperature or pressure

27. To Increase Solubility for a solid solute in a liquid solvent 1. Increase temperature of solvent 2. Increase surface area of solute (crush) 3. Agitate (stir or shake) Not affected by changes in pressure

28. To Increase Solubility for a gas solute in a liquid solvent 1. Decrease temperature of solvent 2. Increase pressure Not affected by surface area of solute

29. Gas solubility High Temp Low Temp You want more gas particles in the liquid

30. Saturated Solution contains the maximum amount of dissolved solute for a given amount of solvent at a specific temp and pressure.

31. Unsaturated Solution contains less dissolved solute for a given temp and pressure than a saturated solution

32. Supersaturated Solution contains more dissolved solute than a saturated solution at the same temp Must heat a saturated solution, then slowly cool

33. Determining the solubility of a solution Add more solute “seed crystal”. If… 1) It dissolves, the original solution was unsaturated (still more available space). 2) It does not dissolve and falls to the bottom of the container, the original solution was saturated (no more available space). 3) It crystallizes, the original solution was supersaturated (over full, past capacity).

35. Concentration is the amount of solute dissolved in a given amount of solvent. Concentrated Dilute

36. Molarity A unit of concentration The number of moles of solute dissolved in 1.00 L of solution. Molarity (M) = Moles of solute Liter of solution

37. Practice Problem What is the molarity if 2.0 moles of glucose are added to 5.0 L of solution?

38. http://wiki.chemeddl.org/mediawiki/index.php/3.5.1_Concen tration Preparing Molar Solutions From the number of moles you need, calculate the mass. Measure solute mass. Place solute in volumetric flask Add exact volume up to calibration mark. Close lid, and swirl solution

39. Changing the concentration Add more solvent (yellow)  decreases concentration The amount of solute is the same, but now the solution volume has increased How would you increae the concentration? http://wps.prenhall.com/wps/media/objects/1053/1078985/ist/ch03_11.html

40. Solution Dilution When you need to make a concentrated solution more dilute, use this formula: M 1 V 1 = M 2 V 2 M 1 = concentrated solution V 1 = amount of concentrated solution need to make dilute solution M 2 = dilute solution V 2 – amount of diluted solution wanted

41. Practice How many liters of 16.8M HCl is need to make 2.5L of 3.5M HCl?

42. Practice problem Mrs. Imamazing needs to make 12 liters of a 0.10 M HCl solution for her chemistry students to use in a lab. She finds a large bottle of 12.00 M HCl solution in the acid cabinet. Describe how she would make the solution?

43. Dalton’s Law of Partial Pressures at constant volume & temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures Total pressure = P gas1 + P gas2 + Pgas3…. P total = P 1 + P 2 + P 3 ….

44. Dalton’s Law What is the pressure of hydrogen, in atm, if it is mixed with oxygen, which exerts a pressure of 2.1 atm, and the total pressure is 3.6 atm?

45. Dalton’s Law Standard Deviants