1. Ch. 2.1 Scientific Method

2. 2.1 Goals 1. Describe the purpose of the scientific method. 2. Distinguish between qualitative and quantitative observations. 3. Describe the differences between hypotheses, theories, and models.

3. The Scientific Method The scientific method is a logical approach to solving problems

4. How can you work like a scientist? Copyright Pearson Prentice Hall 1. 2. 3. 4. 5.

5. Formulating Hypotheses – What could you hypothesize about this?

6. How a Theory Develops As evidence from numerous investigations builds up, a hypothesis may become so well supported that scientists consider it a theory. In science, the word theory applies to a well-tested explanation that unifies a broad range of observations.  Germ Theory  Evolutionary Theory  Cell Theory  Gene Theory

7. Ch. 2.2 1. Name the SI units for length, mass, time, volume, and density. 2. Distinguish between mass and weight. 3. Perform density calculations.

8. Units of Measurement 2.2 Quantity – Something that has magnitude, size, or amount. – A tablespoon is a unit of measurement. – What type of quantity is being measured?

9. Copyright Pearson Prentice Hall What measurement system do most scientists use?

10. Copyright Pearson Prentice Hall The metric system (SI) – measurement system based standards and are scaled on multiples of 10

11. 1. Why doesn’t America use the metric system? 2. How would completely changing to the metric system a/effect your life? 3. Would you be opposed to a full change? Why or why not?

12. Breaking Up

13. The Base Units Mass – quantity of matter - Standard Unit – Kilogram -Measured with balances Weight – gravitational pull on matter -Measured with spring scales

14. Length Meter – Standard Unit

15. The Metric System

16. The Standards

17. Combinations of SI base units Derived SI Units

18. Volume The amount of space occupied by an object. – Cubic meter, m 3 – Cubic centimeter, cm 3 Liter (not metric) mL = cm 3

19. Density Ratio of mass to volume Practice problem A: – A sample of aluminum metal has a mass of 8.4g. The volume of the sample is 3.1 cm 3. Calculate the density of aluminum

20. Conversion Factors – example: How quarters and dollars are related a ratio derived from the equality between two different units that can be used to convert from one unit to the other.

21. Dimensional analysis a mathematical technique that allows you to use units to solve problems involving measurements. quantity sought = quantity given  conversion factor example: the number of quarters in 12 dollars number of quarters = 12 dollars  conversion factor

22. Complete Vocab and 2.2 Questions

23. Go over Questions

24. Section 3 Goals 1.Distinguish between accuracy and precision.

25. Accuracy The closeness of measurements to the accepted value Precision The closeness of a set of measurements of the same quantity made in the same way.

26. Distinguish between accuracy and precision Two technicians independently measure the density of a new substance. – Technician A records values of 2.000, 1.999. and 2.001 g/mL – Technician B records values of 2.5, 2.9, and 2.7 g/mL The correct value is 2.701 g/mL

27. Percentage Error Helps find the accuracy

28. A. A student measures the mass and volume of a substance and calculates its density as 1.4 g/mL. The correct, or accepted, value of the density is 1.3 g/mL. B. What is the percentage error for a mass measurement of 17.7 g, given that the correct value is 21.2 g? C. A volume is measured experimentally as 4.26 mL. What is the percentage error, given that the correct value is 4.15 mL. Percentage Error

29. Schedule Mon – Section 2.3 Tues – Study Guide Wed – Study Guide Check and Review Thur - Test

30. Significant Figures Significant figures in a measurement consist of all the digits known with certainty plus one final digit, which is somewhat uncertain or is estimated. The term significant does not mean certain.

31. Significant Figures Sample Problem D How many significant figures are in each of the following measurements? a. 28.6 g b. 3440. cm c. 910 m d. 0.046 04 L e. 0.006 700 0 kg

32. When adding and subtracting sig figs you will have to round. Rounding

33. Sig. Figs. Math Addition – When adding or subtracting decimals, the answer must have the same number of digits to the right of the decimal point as there are in the measurement having the fewest digits to the right of the decimal point. – Example – a. 5.44 m - 2.6103 m Multiplication and Division – For multiplication or division, the answer can have no more significant figures than are in the measurement with the fewest number of significant figures. – b. 2.4 g/mL  15.82 mL

34. Scientific Notation In scientific notation, numbers are written in the form M  10 n, where the factor M is a number greater than or equal to 1 but less than 10 and n is a whole number. *move decimal so that there is only 1 nonzero number to the left of the decimal point. *Move to the left n is positive, move to the right n is negative. example: 0.000 12 mm = 1.2  10  4 mm

35. Mathematical Operations Using Scientific Notation 1. Addition and subtraction —These operations can be performed only if the values have the same exponent (n factor). example: 4.2  10 4 kg + 7.9  10 3 kg or

36. 2. Multiplication —The M factors are multiplied, and the exponents are added algebraically. Mathematical Operations Using Scientific Notation = 3.7  10 5 µm 2 = 37.133  10 4 µm 2 = (5.23  7.1)(10 6  10  2 ) example: (5.23  10 6 µm)(7.1  10  2 µm)

37. 3. Division — The M factors are divided, and the exponent of the denominator is subtracted from that of the numerator. Mathematical Operations Using Scientific Notation = 0.6716049383  10 3 = 6.7  10 2 g/mol example:

38. Mathematical Operations Using Scientific Notation 1. Addition and subtraction —These operations can be performed only if the values have the same exponent (n factor). 2. Multiplication —The M factors are multiplied, and the exponents are added algebraically. 3. Division — The M factors are divided, and the exponent of the denominator is subtracted from that of the numerator.

39. Direct Proportions Two quantities are directly proportional to each other if dividing one by the other gives a constant value. y = kx

40. Inverse Proportions Two quantities are inversely proportional to each other if their product is constant. xy = k