Chapter 1 Reading Guide Introduction: Matter and Measurement Name Section 1.1 The Study of Chemistry 1. Chemistry is the study of matter and the it undergoes. 2. Matter is characterized as anything that has and. Section 1.2 Classifications of Matter 3. Solid shape and volume. 4. Liquid shape and volume. 5. Gas shape and volume. 6. Pure substances can be or. 7. The properties of a compound are different than the elements that make it up. Give an example showing the difference. 8. Hydrogen, oxygen and water are all composed of molecules. What is it about a molecule of water that makes it a compound, whereas hydrogen and oxygen are elements? 9. In a mixture, the parts that make up the mixture their own unique properties. Section 1.3 Properties of Matter 10. Which of these changes are physical and which are chemical? Explain. a. Plants make sugar from carbon dioxide. b. Water vapor in the air forms frost. c. A goldsmith melts a nugget of gold and pulls it into a wire.
Section 1.3 cont. 11. List at least 4 ways to separate a mixture. Section 1.4 Units of Measurement 12. Quantitative properties or measurements involve. (Qualitative do not.) 13. Which quantity is the smallest? (Circle it) 1 mg 1 pg 1 dg 14. Mass and weight are usually interchanged, but there is a difference between the two. What is it? 15. Which way does heat flow? 16. The high temperature for today is predicted to be 75 F. What is that in C and K? 17. Which of the following quantities represents a (plain) volume measurement: 15 m 2 2.5 x 10 2 m 3 5.77 L/s How do you know?
AP Chemistry Section 1.5 Notes/Guided Problems Name Hours Section 1.5 Uncertainty in Measurements 1. Two types of numbers: A. Exact B. Inexact 2. Precision vs. accuracy: Precision Accuracy 3. Why do scientists usually do several trials of an experiment? 4. There is always some in the last digit reported for any measured quantity. 5. The more significant figures, the greater the of the measurement. Guided Problems Counting Sig Figs 1. 30,040 g sig figs 2. 0.0663 kg sig figs 3. 20.05 ml sig figs 4. 1500 mg sig figs 5. 0.000008 sig figs
Adding and Subtracting with Sig Figs 6. 164 ml + 39.7 ml + 18.16 ml = 7. 170.11 cm 2 + 3.5 cm 2 28.031 cm 2 = Multiplying and Dividing with Sig Figs 8. In an experiment, it is found that 1.82 L of a gas has a mass of 5.430g. What is the density of the gas in g/l? Round your answer to the correct number of sig figs. 9. 651 cm x 75 cm = Scientific Notation Recap Correct format: 6.02 x 10 23 Only ONE non-zero number in front of the decimal and exponent is a whole number (can be negative or positive) Positive exponent original (non-scientific notation) number is BIGGER THAN 1 Negative exponent original number is LESS THAN 1 Conversions To scientific notation: Out of scientific notation: 10. 310,000 14. 9.003 x 10-3 11. 0.000874 15. 8.8 x 10 6 12. 33.8 16. 1.2 x 10 4 13. 0.2105 17. 7.5 x 10-1
AP Chemistry 1.6 Dimensional Analysis Practice Name Examples 1. How long is the Indy-500 (which is exactly 500.0 miles) in kilometers? 2. Convert 8.0 meters to inches. 3. Convert 515 m/s to miles/hr. 4. The density of benzene is 0.879 g/ml. What is the mass (in grams) of 1.00 quart of benzene?
AP Chemistry Chapter 1 Homework (from the book) These are found at the end of the chapter. Problems are listed as 1.1, 1.2, 1.17, 1.19, etc. Sections 1.1-1.3 Problems 1.1, 2, 17, 19 and 22 Section 1.4 1.24, 25, 28 and 30 Section 1.5 1.33, 36, 37 and 39-42 Section 1.6 1.45-47, 49-50 and 53-54
AP Chemistry Chapter 1 Review Questions Name 1. How many significant figures are there in each of the following values? a. 1406.20 c. 1600.0 e. 1.250 x 10-3 b. 0.0007 d. 0.0261140 2. Which value has more significant figures, 7.63 x 10-11 or 0.00076? 3. Use scientific notation to express the number 37,100,000 with: a. one sig fig b. two sig figs c. three sig figs d. six sig figs 4. Perform the indicated calculations on the following measured values, giving the final answer with the correct number of significant figures. (Show your un-rounded answer as well.) a. 2.85 + 3.4621 + 1.3 b. 7.442 7.429 c. 1.65 x 14 d. 27 / 4.148 e. [(3.901 3.887)/3.901] x 100.0 f. 6.404 x 2.91 x (18.7 17.29) 5. How many Liters is 3.5 quarts equal to? How many cm 3? (2 answers)
6. Convert 4.2 yards to centimeters. 7. If you put 8 gallons of gas in your car and it cost you a total of $30, what is the cost of gas per liter? 8. A student made the 27.0 kilometer drive to school in 16 minutes. a. How many miles did the student drive? b. If the speed limit is 55 miles per hour, was the student speeding? How fast was the student driving? 9. Which is the higher temperature, 42 C or 92 F? 10. Convert 300 K to F. 11. What is -100 C in Kelvin? 12. Convert 1555 K to C. 13. A sample of motor oil with a mass of 440 g occupies 500 ml. What is the density of the motor oil in g/ml? 14. The density of an object is 1.63 g/ml. Its volume is 0.27 L. What is the mass of the object? (Be careful!)