1. The scientific method is a logical approach to solving problems by observing and collecting data, formulating hypotheses, testing hypotheses, and formulating theories that are supported by data. CHEMISTRY CHAPTER 2. MEASUREMENTS AND CALCULATIONS SECTION 1. SCIENTIFIC METHOD

2. Observing and Collecting Data Observing is the use of the senses to obtain information. Includes the aid of scientific instruments. Data may be qualitative (descriptive, without numbers) quantitative (numerical)

3. A system is a specific portion of matter in a given region of space that has been selected for study during an experiment or observation. Example – the contents of a flask.

4. Formulating Hypotheses Scientists use generalizations about the data to formulate a hypothesis, or testable statement. Hypotheses are often “if-then” statements. A hypothesis is not just a guess – it has scientific reasoning behind it.

5. What hypothesis was being tested?

6. Testing a hypothesis requires experimentation (or other types of observation) that provides data to support or refute a hypothesis or theory. Controls are the experimental conditions that remain constant. Variables are any experimental conditions that change. Testing Hypotheses

7. Independent variable: what the researcher changes (or is changed by nature, such as time). Usually plotted on the x- axis. Dependent variable – this changes as a result of changes in the independent variable. Usually plotted on the y-axis.

8. What are the independent variables? What is the dependent variable? What do you think was controlled?

10. Depending on the results of testing, a hypothesis may be: confirmed (supported) revised rejected

11. Theorizing One or more hypotheses that are confirmed may lead to a theory: a broad generalization that explains a body of facts or phenomena. example: atomic theory Theories are not proved, but may become more and more established. Successful theories predict results of new investigations.

12. A theory may contain a model, a representation that helps us understand a complex set of information (but is simplified). Example – Bohr model of atom www.umich.edu/~radinfo/images/atom.gif Models

13. A law describes a pattern in nature but does not explain it. Ex. – law of gravitation: force = G m 1 m 2 / r 2 law of multiple proportions (p. 168) Laws

14. Scientific Method

15. Note on commas in numbers SECTION 2. UNITS OF MEASUREMENT Notice that the text does not use commas in writing numbers: 7 000 000 instead of 7,000,000 This is because in other countries commas are used instead of the decimal point: 2,14 instead of 2.14

16. SI Measurement We need to have standard measures that everyone agrees on. Scientists all over the world have agreed on a single measurement system called Le Système International d’Unités, abbreviated SI. SI has seven base units. Most other units are derived from these seven.

17. SI (Le Systé me International d´Unit é s) Base units in bold

18. SI Base Units * * * not used in this course

19. Metric Prefixes (p. 35) Learn these! teraT10 12 gigaG10 9 megaM10 6 kilok10 3 decid10 -1 centic10 -2

20. Metric Prefixes (p. 35) Learn these! millim10 -3 microμ10 -6 nanon10 -9 picop10 -12 femtof10 -15 attoa10 -18

21. American Scientist, Sept.-Oct. 2010

22. Changing metric units by moving the decimal point If the unit gets smaller, the number gets larger. Move the decimal point to the right according to the power of ten. Example 1: change 50 MW (megawatts) to W mega means 10 6 move the decimal point six places to the right: 50 MW = 50 000 000 W

23. Example 2: change 3.25 kg (kilograms) to g kilo means 10 3 move the decimal point 3 places to the right: 3.25 kg = 3 250 g

24. If the unit gets larger, the number gets smaller. Move the decimal point to the left according to the power of ten. Example 1: change 3 000 mm (millimeters) to m milli means 10 -3 move the decimal point 3 places to the left: 3 000 mm = 3 m

25. Example 2: change 68 μmol (micromoles) to mol micro means 10 -6 move the decimal point 6 places to the left: 68 μmol = 0.000 068 mol

26. SI Base Units Mass Mass is a measure of the quantity of matter. The SI standard unit for mass is the kilogram. However, we will normally be using g or mg.

27. Scientists prefer to define base units using fundamental constants of nature. However, the kilogram is still defined by the mass of a solid piece of platinum and iridium in a vault in France.

28. http://www.npr.org/templates/story/story.php?storyId=112003322

29. Some scientists wish to replace the standard kilogram with a new standard (for example, based on the mass of a particular number of atoms in a crystal of silicon).

30. Weight is a measure of the gravitational pull on matter. Mass does not depend on gravity. Your weight will be smaller on the Moon, but your mass will be the same as on Earth. Conversion factors 1 kg = 2.2 lb (learn this) 1 lb = 454 g 16 oz = 1 lb1 oz = 28 g

31. Length Length is a measure of distance. The SI standard for length is the meter. The meter is defined as the distance that light travels in 1/299 792 485 s in a vacuum.

32. Conversion factors 1 m = 3.281 ft = 39.37 in (so a meter is about a yard) 2.54 cm = 1 in (learn) 0.62 miles = 1 km A non-SI unit used by chemists is the Angstrom (Å). 1 Å = 10 -10 m = ____ nm

33. Conversion factors 1 m = 3.281 ft = 39.37 in (so a meter is about a yard) 2.54 cm = 1 in (learn) 0.62 miles = 1 km A non-SI unit used by chemists is the Angstrom (Å). 1 Å = 10 -10 m = 0.1 nm

35. Derived SI Units Combinations of SI base units form derived units (see Table 3, p. 36). Ex.: pressure is measured in kg/(ms 2 ), or pascals

36. Derived SI Units 1 joule = 1 kgm 2 /s 2

37. Area is the amount of surface. The derived SI unit is square meters, m 2 Area of a rectangle = length x width (A = l w) Area of a circle: A = π r 2 (r = radius) Volume is the amount of space occupied by an object. The derived SI unit is cubic meters, m 3 The cubic centimeter, cm 3, is often used

38. The liter, L, is a non-SI unit of volume. 1 mL = 1 cm 3 How many cm 3 in 1 L? 1 gal = 3.785 L 1 dm 3 = ? L

39. 1000 cm 3 = 1 L 1 dm 3 = (10 cm) 3 = 1000 cm 3 = 1 L

40. Density Density is the ratio of mass to volume, or mass divided by volume.

41. The derived SI unit is kilograms per cubic meter, kg/m 3 g/cm 3 or g/mL are also used Density is a characteristic physical property of a substance. (Extensive or intensive?)

42. Density can be used as one property to help identify a substance

43. The density of water at 20° C is almost exactly 1 g/cm 3 If the density of something is less than this it will float in water; if greater, it will sink.

44. Problem solving – general guidelines 1.Write the equation 2.Substitute what you know (including units) 3.Do the calculation 4.Check that the number and units make sense

45. Sample Problem A A sample of aluminum metal has a mass of 8.4 g. The volume of the sample is 3.1 cm 3. Calculate the density of aluminum. Given: mass (m) = 8.4 g volume (V) = 3.1 cm 3 Unknown: density (D) Solution:

46. When solving for mass or volume, you can use two different approaches: 1.Substitute what you know in the equation for density, and use algebra to calculate the unknown. 2.Rearrange the equation to solve for m or V, then substitute. Sample Problem B – solve for mass What is the mass of a sample having a volume of 2 cm 3 and a density of 6 g/mL?

47. Using the approach of substituting in the density equation: D = m/V Substitute: 6 g/ml = m / 2 mL (note that V = 2 cm 3 = 2 mL) Solve: m = (6 g/mL) (2 mL) = 12 g

48. Sample Problem C – solve for volume What is the volume of a sample with a density of 18 g/cm 3 and a mass of 9 g? Using the approach of rearranging the density equation before substituting: D = m/V DV = (m/V)V = m V = m/D Substitute: V = 9 g / (18 g/cm 3 ) Solve: V = 0.5 cm 3

49. Conversion Factors A conversion factor is a ratio (or fraction), equal to 1, derived from the equality between two different units that can be used to convert from one unit to the other. Examples: 60 s / 1 min = 1 1 m / 100 cm = 1 4 quarters / 1 dollar = 1

50. Dimensional analysis (or the factor-label method) is a mathematical technique that allows you to use units to solve problems involving measurements. In dimensional analysis, quantities in one unit are changed to the desired unit by multiplying by one or more conversion factors.

51. You will write the conversion factor so that the unit you want to remove will cancel out when you multiply. For example, to change a unit in the numerator, put it in the denominator of the conversion factor.

52. Example: find the number of quarters in 12 dollars number of quarters = 12 dollars × conversion factor

54. Deriving Conversion Factors You can derive conversion factors if you know the relationship between the unit you have and the unit you want. example: conversion factors for meters and decimeters

55. Sample Problem Express a mass of 5.712 grams in kilograms. 1 000 g = 1 kg Possible conversion factors : Which one should be used?

56. Use the one that cancels out the unit you want to change (g):