Chapter 2 Notes

1. Chapter 2 Notes Measurements and Solving Problems Problem Set: 14-19, 22-25, 29-31, 35-44 Crash Course Chemistry Video

2. Scientific Method 1. Problem state it clearly – usually as a question 2. Gather information do some research on your problem 3. Hypothesis a suggested solution 4. Procedure experiment and examine the situation to check the hypothesis 5. Data Note everything your senses can gather. Record the data and keep careful records. 6. Analysis Put the data in order- charts/tables. Figure out the meaning of the data 7. Conclusion Explain the data. State whether or not it supports the hypothesis.

3. Scientific Method • Theory • A hypothesis that has been rigorously tested, and not found faulty, usually also having been found somewhat useful. • Law • A readily demonstrable fact, that cannot be disproven.

4. 2.1 Units of Measurement • Measurement – comparison of an object to a standard. • The problem is, what do you use as a standard? • Standard should be an object or natural phenomenon of constant value, easy to preserve and reproduce, and practical in size.

5. 2.1 Units of Measurement • The SI System • SI = Standard International • Important base units to know:

6. 2.1 Units of Measurement • Important prefixes(multiples of base units) to know:

7. 2.3 Using Scientific Measurement • Significant Figures (Digits) - “Sig Figs” • Definition: digits in a measurement that are known + 1 estimated digit • 1.15 ml implies 1.15 + 0.01 ml • The more significant digits, the more reproducible the measurement is. • These are the numbers that “count!” Ex1: π= 22/7 = 3.1415927 what do math teachers let you use? Ex2: You collect a paycheck for a 40 hour week – what’s the difference between getting paid pi vs. 3.14 ?

8. Rules for finding the # of sig figs 1. All non-zeros are significant ex. 7 [] 77 []4568 [] 2. Zeros between non-zeros are significant ex. 707 [] 7053 [] 7.053 [] 3. Zeroes to the left of the first nonzero digit serve only to fix the position of the decimal point and are not significant ex: 0.0056 [] 0.0789 [] 0.0000001 [] 4. In a number with digits to the right of a decimal point, zeroes to the right of the last nonzero digit are significant ex: 43 [] 43.00 [] 43.0 [] 0.00200 [] 0.040050 [] 5. In a number that has no decimal point, and that ends in zeroes (ex. 3600), the zeroes at the end may or may not be significant (it is ambiguous). To avoid ambiguity, express in scientific notation and show in the coefficient the number of significant digits. ex. 3600 = 3.6 x 103[]

9. Scientific Notation • A way to express very small or very large numbers • Example: • 12345 = 1.2345 x 104 • 0.00456 = 4.56 x 10-3 Exponent – the # of times the decimal was moved (+) to the left (-) to the right Coefficient – must be between 1 and 9 Base

10. Scientific Notation • 56934 = • 0.0000037 = • 2.347 x 10-3 = • 8.98736 x 105 = Reverse it! (+) right (-) left

11. Counting significant digits 1. Convert to scientific notation 2. Disappearing zeroes just hold the decimal point, they aren’t significant • Ex1: 700 [ ] - means “about 700 people at a football game” 700. [ ] - means “exactly 700 ......” 700.0[ ] - means “teacher weighs exactly 700.0 lbs” • Other examples 0.5 [ ] 0.50 [ ] 0.050 [ ] • Sig. figs apply to scientific notation as well 9.7 x 10 2 = 970 [ ] 1.20 x 10 -4 = .000120 [ ]

12. Calculating with Measurements ( Sig Fig Math ) • Rounding Rules • XY ---------------------> Y • When Y > 5, increase X by 1 • When Y < 5, don’t change X • When Y = 5, • If X is odd, increase X by 1 • If X is even, then don’t change X • Ex1: round to 3 sig figs 35.27 = 87.24 = 95.25 = 95.15 = • Note - the “5” rule only applies to a “dead even” 5 - if any digit other than 0 follows a 5 to be rounded, then the number gets rounded up without regard to the previous digit. • Ex2: round to 3 sig figs 35.250000000000000000000000001 =

13. Calculating rules: • Multiplying or dividing – round results to the smaller # of sig. figs in the original problem.  • Ex1: 3.10 cm Ex2: 7.9312 g 4.102 cm / 0.98 m x 8.13124 cm

14. Calculating rules: 2. Adding or subtracting - round to the last common decimal place on the right.  • Ex1: 21.52 Ex2: 73.01234 g + 3.1 - 73.014 g

15. Partner Share Partner Share: How do you determine the proper sig figs when adding and subtracting? How do you determine the proper sig figs when multiplying or dividing? What is the 5 rule?

16. 2.1 Units of Measurement • Factor Label Method (Dimensional Analysis) • A method of problem solving that treats units like algebraic factors • Rules 1. Put the known quantity over the number 1. 2. On the bottom of the next term, put the unit on top of the previous term. 3. On top of the current term put a unit that you are trying to get to. 4. On the top and bottom of the current term, put in numbers in order to create equality. 5. If the unit on top is the unit of your final answer, multiply/divide and cancel units. If not, return to step # 2. 6. As far as sig figs are concerned, end with what you start with!

17. 2.1 Units of Measurement • Factor Label Method (Dimensional Analysis) • Ex1 - convert 26 inches to feet • Ex2 - convert 1.8 years to seconds • Ex3 - convert 2.50 ft to cm if 1 inch = 2.54 cm

18. 2.1 Units of Measurement • Factor Label Method (Dimensional Analysis) • Ex4 -   convert 150. g to ug • Ex5 -   convert 75 cm to Hm • Ex6 - convert 0.75 L to cm3 (1 cm3 = 1 mL)

19. 2.1 Units of Measurement • Density – ratio of mass to volume • The common density units are: • g/cm3 for solids • g/ml for liquids • g/L for gases • Formula is D = m/v • Density is a) a characteristic b) and intensive property c) temperature dependent • Two ways to find volume in density problems: 1. Water displacement 2. Volume formula • Note: the density is the same no matter what is the size or shape of the sample.

20. 2.1 Units of Measurement • Ex1:Find the density of an object with m= 10g and v=2 cm3 • Ex2:A cube of lead 3.00 cm on a side has a mass of 305.0 g. What is the density of lead?   • First, calculate it’s volume: • Next, calculate the density: • Density = mass/volume =

21. 2.1 Units of Measurement • Ex 3: A graduated cylinder contains 25 mL of water. When a 4.5 g paper clip is dropped into the water, the water level rises to 36 mL. What is the density of the paper clip?

22. 2.3 Using Scientific Measurement • Precision vs. Accuracy

23. 2.3 Using Scientific Measurement • Precision vs. Accuracy

24. 2.3 Using Scientific Measurement • Percent Error - experiments don’t always give true results - error is pretty much a given • Actual (experimental value) - data found in an experiment • True value (theoretical value) - data that is generally accepted as true • Percent (%) error = (actual - theoretical) x 100 theoretical value • +/- shows the direction of the error - values are either too high or too low • Note: some texts teach that percent error should be treated as absolute value - I say you should use +/- in order to show direction of error and better analyze your experiments. • Ex1: 66 Co is the answer in your experiment 65 CO is the theoretical value

25. 2.3 Using Scientific Measurement • Two important points: • Uncertainty in Measurement • making a measurement usually involves comparison with a unit or a scale of units • When making a measurement, include all readable digits and 1 estimated digit • always read between the lines! • the digit read between the lines is always uncertain

26. 2.3 Using Scientific Measurement • Uncertainty in Measurement