1. Chemistry 103 Lecture 3

2. Outline I. Mathematics of Chemistry –Dimensional Analysis –Density –Temperature Scales II. Matter Classified

3. Math Operations Calculate each to the correct number of sig figs. 32.145 cm x 17.8 cm x 25 cm = 1450.0 kg + 250 kg + 1.235 kg =

4. Dimensional Analysis Review

5. Dimensional Analysis A problem solving method in which the units (associated with numbers) are used as a guide in setting up the calculations. Conversion Factor

6. Dimensional Analysis How many seconds are in 2 minutes? 2 minutes x 60 seconds = 1 minute 120 seconds (exactly)

7. Learning Check If a bucket contains 4.65L of water. How many gallons of water is this? (1 gallon = 4qts, 1L = 1.057qt) A.1.23 gallons B.4.92 gallons C.17.6 gallons

8. Dimensional Analysis If Jules Vern expressed the title of his famous book, “Twenty Thousand Leagues Under the Sea” in feet, what would the title be? (1mile = 5280ft, 1 League = 3.450miles)

9. Practice Problem During surgery, a patient received 5.0 pints of plasma. How many mL of plasma is this? (1L = 1.057qts, 2 pints = 1qt) A.2400mL B.2.4mL C.4700mL D.4.7mL

10. Dimensional Analysis If a particular fad diet claims a weight loss of 3.0 pounds per week, how many grams per day would this be? (1lb = 453.6g) A.1400 g/day B.0.046g/day C.190 g/day

11. Converting from squared units to squared units or cubed units to cubed units Warning: This type of conversion gives many students difficulties!!!!! The one thing you have to remember: –What does it mean to say that a unit is squared or cubed? –m 2 = m x m; s 3 = s x s x s When there are squared or cubed units, you have multiple units to cancel out!

12. Examples Convert 127.4 cm 3 to m 3. (100cm = 1m) Convert.572 miles 2 to km 2. (1km =.621miles)

13. Percent Factor in a Problem If the thickness of the skin fold at the waist indicates an 11% body fat, how much fat is in a person with a mass of 86 kg? percent factor 86 kg mass x 11 kg fat 100 kg mass = 9.5 kg fat Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

14. Even MORE Practice with Conversion Factors A lean hamburger is 22% fat by weight. How many grams of fat are in 0.25 lb of the hamburger?

15. Density A ratio of the mass of an object divided by its volume Density = Mass/Volume Typical units = g/mL (NOTE: 1mL=1cm 3 )

16. Measuring Density in Lab

17. 68.60g = 68.60g (45.0mL - 35.5mL) 9.5mL

18. Measuring Density in Lab 68.60g = 68.60g = 7.2g/mL (45.0mL - 35.5mL) 9.5mL

19. Densities of Common Substances

20. Sink or Float Ice floats in water because the density of ice is less than the density of water. Aluminum sinks because its density is greater than the density of water. Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

21. Sink or Float Ice floats in water because the density of ice is less than the density of water. Aluminum sinks because its density is greater than the density of water. Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

22. Which diagram correctly represents the liquid layers in the cylinder? Karo (K) syrup (1.4 g/mL), vegetable (V) oil (0.91 g/mL,) water (W) (1.0 g/mL) A B C K K W W W V V V K Learning Check

23. A) Vegetable oil 0.91 g/mL Water 1.0 g/mL Karo syrup 1.4 g/mL K W V Solution

24. Osmium is a very dense metal. What is its density in g/cm 3 if 50.0 g of osmium has a volume of 2.22 cm 3 ? a) 2.25 g/cm 3 b) 22.5 g/cm 3 c) 111 g/cm 3 Learning Check

25. Osmium is a very dense metal. What is its density in g/cm 3 if 50.0 g of osmium has a volume of 2.22 cm 3 ? a) 2.25 g/cm 3 b) 22.5 g/cm 3 c) 111 g/cm 3 50.0g = 22.5g/cm 3 2.22cm 3 Learning Check

26. Density can be written as an equality. For a substance with a density of 3.8 g/mL, the equality is: 3.8 g = 1 mL From this equality, two conversion factors can be written for density. Conversion 3.8 g and 1 mL factors1 mL 3.8 g Density as a Conversion Factor

27. DENSITY PRACTICE

28. The density of octane, a component of gasoline, is 0.702 g/mL. What is the mass, in kg, of 875 mL of octane? A) 0.614 kg B) 614 kg C) 1.25 kg Learning Check

29. Density Example You have been given 150g of ethyl alcohol which has a density of 0.785g/mL. Will this quantity fit into a 150mL beaker? A. YESB. NO

30. A group of students collected 125 empty aluminum cans to take to the recycling center. If 21 cans make 1.0 lb aluminum, how many liters of aluminum (D=2.70 g/cm 3 ) are obtained from the cans? A) 1.0 LB) 2.0 LC) 4.0 L Learning Check

31. 31 Temperature Is a measure of how hot or cold an object is compared to another object Indicates that heat flows from the object with a higher temperature to the object with a lower temperature Is measured using a thermometer Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

32. Temperature Scales

33. Solving a Temperature Problem A person with hypothermia has a body temperature of 34.8°C. What is that temperature in °F? T F = 1.8 T C + 32  T F = 1.8 (34.8°C) + 32° exact tenths exact = 62.6 + 32° = 94.6°F tenths Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

34. Converting between Temperature Scales ***Conversions between Celsius and Kelvin –(Temperature in K) = (temperature in o C) + 273 –(temperature in o C) = (temperature in K) – 273 Conversions between Celsius and Fahrenheit – o F = 9/5 ( o C) + 32 – o C = 5/9( o F – 32)

35. Chemistry is the study of Matter Matter is anything that has mass and takes up space.

36. Matter has both physical and chemical properties

37. Physical Properties Physical properties are: Characteristics observed or measured without changing the identify of a substance. Shape, physical state, odor, boiling and freezing points, density, and color of that substance. (Changes of state)

38. Chemical Properties Chemical properties describe the ability of a substance To interact with other substances To change into a new substance Example: Oxygen reacts with methane Gas to form carbon dioxide & water

39. Matter Classified Matter Pure Substance Mixture

40. Matter Classified Matter Pure Substance Mixture

41. Classification of Matter Pure Substances: A form of matter that always has a definite and constant composition. Properties always the same under a given set of conditions (temperature & pressure)

42. Matter Pure SubstanceMixture Element Compound

43. Pure Substances: Elements Element –Pure substance that can not be broken down into simpler substances by chemical means. Copper (Cu) Lead (Pb) Aluminum (Al) –The most basic form of matter. –Each element can be found on the periodic table.

44. Periodic Table of Elements

45. Names and Symbols of the Elements Each element has a unique name and is represented by a unique symbol –Chemical symbol: a one- or two-letter designation for an element derived from the element’s name –First letter of the symbol is always capitalized

46. Several symbols are derived from Latin names as shown below: Cu, copper (cuprum) Au, gold (aurum) Fe, iron (ferrum) Ag, silver (argentum) Symbols from Latin Names Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

47. Select the correct symbol for each: 1. Calcium A) CB) CaC) CA 2. Sulfur A) SB) SlC) Su 3. Iron A) IrB) FEC) Fe Learning Check

48. Select the correct symbol for each: 1. Calcium B) Ca 2. Sulfur A) S 3. IronC) Fe Learning Check

49. Select the correct name for each symbol: 1. N A) neon B) nitrogen C) nickel 2. P A) potassium B) phlogistonC) phosphorus 3. Ag A) silver B) ageanC) gold Learning Check

50. Select the correct name for each symbol: 1. N A) neon B) nitrogen C) nickel 2. P A) potassium B) phlogistonC) phosphorus 3. Ag A) silver B) ageanC) gold Learning Check