AP Chemistry 1: Summer 2015 Assignment

Transcription

1 AP Chemistry 1: Summer 2015 Assignment TEXTBOOK: Chemistry, 2 nd Edition CK-12 Foundation (Berwick & Parsons); customized as AP Chemistry 1 Summer Reading Assignment The textbook & content outline can be accessed through: **If you cannot access the textbook, please contact Dr. Best at bests@tesd.net** This is the textbook for the summer assignment. You will be given an additional hardcopy textbook on the first day of school that we will use for the duration of the AP Chemistry 1 course. The textbook seems long at first glance (98 pages), but it is a relatively easy read. Each page in the Chemistry e-textbook are shorter than most pages in a traditional textbook and cover less material (~2 pages in the e-book to 1 page in a normal Chemistry text). There are also lots of YouTube videos that you can access as well as practice problems included for each of the sections to enhance your understanding of the material. CONTENT OUTLINE: Read the textbook and fill out the notes outline by HAND as you go along. NO typewritten notes outlines will be accepted! Sometimes you will just need to fill in a blank, while other times you may need to glean the most important concepts from the textbook. In general, the notes outline follows the textbook with a few noted exceptions. If you cannot find something, feel free to access the additional resources noted in the textbook and/or the internet. SUMMER ASSIGNMENT QUIZ: There will be a quiz on the material covered in the summer assignment that will occur on the Friday before Labor Day, September 4 th, You may use your packet to take this quiz. In addition, you will also turn in your packet at the end of the quiz. These packets will be graded for completeness, not accuracy, and will count as a homework grade. NO typewritten notes outlines may be used for the quiz or turned in for homework points! REVIEW PROBLEMS: There are review problems at the end of each section in the textbook. Please complete these problems in your notes packet. Remember that you will be able to use your packet for the quiz, so if you think it would be helpful to write out the questions/statements, you may do so. Also feel free to include additional handwritten pages if you need additional space to complete the problems. REMINDER: **Packet Due Date & Quiz: Friday, September 4, 2015** Pg.1

2 CHAPTER 1: INTRODUCTION TO CHEMISTRY 1.1 What is Chemistry? A. Chemistry is. B. The man who would greatly advance the development of modern chemistry was. Considered the father of modern chemistry, (seen in Figure 1.2) discovered that although matter may change its shape or form, its always remains the. As a result, he would state the first version of the. C. Chemists apply information about and the to improve our lives in many different ways. D. Using complete sentences, answer the review questions on the bottom of p. 4 in the space below: The Process of Science A. Describe why Aristotle s methods were unsuitable for describing the nature of the physical world. B. The is a method of investigation involving experimentation and observation to. Scientists frequently list the as a. Some scientists oppose this listing of because not all occur in every case, nor do they always. The is listed here as a series of, but you should remember that you are not required to rigidly follow this list. Instead, the is a valuable tool that provides a basic and adaptable. C. List the steps in the scientific method: Pg.2

3 D. Define the following: 1. Hypothesis 2. Theory 3. Scientific Law 4. Experiment 5. Controlled experiment 6. Control sample 7. Model E. List two examples of scientific laws as described in the reading: F. From your previous science courses or general knowledge, list one example of a scientific theory: Pg.3

4 D. Answer the review questions on p. 12 to p. 16. Place the answer to each multiple choice question in the numbered space below: CHAPTER 2: Measurement in Chemistry 2.1 Making Observations A. Define the following: 1. Observation 2. Quantitative observations 3. Qualitative observations D. Answer the review questions on p. 20 to 21. Label each of the following observations as qualitative or quantitative. Label each observation as qualitative or quantitative. 1. The temperature of this room is 25_C. 2. It is comfortably warm in this room. 3. Most people have removed their coats. 4. The building is 25 stories high. 5. It is a very tall building. 6. The building is taller than any nearby trees. 7. The bottle is green. 8. The bottle contains 250 milliliters of liquid. 9. Robert bought his son a small car. 10. The car is smaller than his hand. 11. The car is about three inches long. 12. The race is about 27 miles long. Pg.4

5 2.2 Measurement Systems A. The is an international -based system of measurement. Because the metric system is a system, making conversions between different units of the metric system are always done with. B. Explain why the metric system is more useful and easier to manipulate than the US customary system: C. Fill in the missing blanks in Table 2.4 below: Prefix Meaning Symbol piconanomicromillicentidecikilo- D. Fill in the missing blanks below: Length: millimeters = 1 meter centimeters = 1 meter millimeters = 1 centimeter Mass: milligrams = 1 gram grams = 1 kilogram Volume: 1 liter = milliliters 2.3 The SI System of Measurement A. The International System of Units, abbreviated from the French Le Système International d Unites, is the main system of measurement units used in science. Since the 1960s, the International System of Units has been agreed upon internationally as the. The SI are based on standards. The definitions of the SI base units have been and continue to be modified, and new base units are added as advancements in science are made. Each SI, except the, is described by stable properties of the universe. B. Mass Pg.5

6 Define Mass: Define weight: Explain how mass and weight differ: The basic unit of mass in the SI system is the. C. Length Define Length: The basic unit of length in the SI system is the. D. Volume Define Volume: Volume is a, meaning that. The is the SI unit of length and is based on the. More common units of volume used in chemistry are the: Liter; 1 liter = meter = quart Milliliter; 1 milliliter = liter = cm 3 E. Temperature Define Temperature: Define heat: Explain how temperature and heat differ: F. Temperature Scales Pg.6

7 1. Comparison of Fahrenheit, Celsius, and Kelvin scales 2. Describe what the Fahrenheit temperature scale is based on: 3. Describe what the Celsius temperature scale is based on: 4. Describe what the Kelvin temperature scale is based on: 5. List the formula used to convert between degrees C and Kelvin: 6. Define absolute zero: 7. It should be noted that many mathematical calculations in chemistry involve the between two temperatures, symbolized by (pronounced delta T). Since the is the same in and in, the will be the for either scale. For example, 20 o C = K and 50 o C = K; the difference between the Celsius temperatures is, and the difference between the Kelvin temperatures is. When the calculations involve, it is not necessary to convert Celsius to Kelvin, but when the in an equation, it is necessary to convert Celsius to Kelvin. G. Time The SI unit for time is the. Pg.7

8 H. Using complete sentences, answer the review questions on p. 30 in the space below: Significant Figures A. Measurements do not produce numbers; the only numbers in science are such as. Since measurements are fundamental to science, science does not. It is very important to recognize and report the of a measurement along with the and of the measurement.. B. Significant figures, also known as, are C. In the first ruler illustration shown on p. 31, the measurement is (estimated to the place). D. In the second ruler illustration shown on the top of p. 32, the measurement is (estimated to the place). E. In the third ruler illustration shown on p. 32, the measurement is (estimated to the place). Pg.8

9 F. In the fourth ruler illustration shown on p. 32, the measurement is (estimated to the place). G. List the rules for determining the Number of Significant Figures: H. Equipment Determines Significant Figures: 1. Examine the two graduated cylinders found on the bottom of p. 33. The one on the left can be estimated to place, while the one on the right can be estimated to place. 2. Examine the two balances found on p. 34. The one on the left can measure to, while the one on the right can measure to. I. Significant Figures in Calculations 1. List the rule for determining the number of significant figures in an addition or subtraction problem: 2. List the rule for determining the number of significant figures in a multiplication or division problem: J. Using the significant figures rules, answer the review questions on pp in the space below: 1. How many significant figures are in the following numbers? (a) (b) (c) (d) Pg.9

10 (e) (f) (g) 2. Perform the following calculations and give your answer with the correct number of significant figures: (a) (b) (c) 3. Perform the following calculations and give your answer with the correct number of significant figures: (a) (b) (c) (d) 2.5 Using Algebra in Chemistry A. The formula for density is D (density) = B. Examine the examples given on the bottom of p. 37 and the top of p. 38. Solve the following problems: Problem #1 What is the density of Hg (mercury) if g occupy a volume of 12.1cm 3? Problem #2 Using the density you solved for in Problem #1, what is the mass of 2.15 cm 3 of Hg? Problem #3 Using the density you solved for in Problem #3, what is the volume of 94.2 g of Hg? Pg.10

11 C. A conversion factor is. D. Dimensional analysis is. E. Review the dimensional analysis problems shown on p. 39, and answer the following review questions from p. 40. Show all of your work, and use significant figures in your final answers. 1. For the equation PV = nrt, re-write it so that it is in the form of T =. 2. The equation for density is D = mv. If D is 12:8 g/cm3 and m is 46:1 g, solve for V, keeping significant figures in mind. 3. The equation P 1 xv 1 = P 2 x V 2, known as Boyle s law, shows that gas pressure is inversely proportional to its volume. Re-write Boyle s law so it is in the form of V 1 =. 4. The density of a certain solid is measured and found to be 12:68 g/ml. Convert this measurement into kg/l. 5. In a nuclear chemistry experiment, an alpha particle is found to have a velocity of 14, 285 m/s. Convert this measurement into miles/hour (mi/h). 2.6 Scientific Notation A. In, very large and very small numbers are expressed as the of a number between multiplied by some power of. Pg.11

12 B. As you can see from the examples in Table 2.7, to convert a number from decimal form into scientific notation, you needed to move the decimal, and that number becomes the. If you are moving the decimal to the, the exponent is, and if you are moving the decimal to the, the exponent is. You should note that are maintained in scientific notation. C. Scientific Notation in Calculations 1. Addition and Subtraction: When numbers in exponential form are added or subtracted, the exponents must be the. If the exponents are the, the coefficients are and the exponent remains the. 2. Multiplication and Division: When multiplying or dividing numbers in exponential form, the numbers. To exponential numbers, the coefficients and the exponents. To exponential numbers, the coefficients and the exponents. D. Review the scientific notation examples shown on pp , and answer the following review questions from p a) b) c) d) Evaluating Measurements A. Precision vs. Accuracy Pg.12

13 Definitions: Accuracy how close measurement is to. Precision how close values in a set of measurements are to. B. Percent Error: Note that % error is always positive, so take the absolute value of any answer you obtain! Equation: C. Answer the review questions on pp in the space below: Graphing A. Define the following: Pg.13

14 1. Graph 2. Interpolation 3. Extrapolation 4. Slope D. Review the data tables and graphs shown on pp , and answer the following review questions from p. 54.For questions #2 and #3, either use the graph paper grids provided, or graph the data using Excel and paste copies of the graph onto the page a) b) c) Pg.14

15 3. Relationship: Slope: Meaning of slope: CHAPTER 3: Matter and Energy 3.1 What is Matter? A. Define the following: 1. matter Pg.15

16 2. atom 3. pure substance 4. mixture 5. homogeneous mixture 6. heterogeneous mixture 7. element 8. compound 9. molecule 10. periodic table 11. chemical symbol 12. chemical formula B. Answer the review questions on p. 61 to 62. Place the answer to each multiple choice question in the numbered space below: Pg.16

17 3.2 Properties and Changes of Matter A. Define the following: 1. physical properties 2. chemical properties 3. physical changes 4. chemical changes B. Answer the review questions on p. 65 to 66. Place the answer to each multiple choice question in the numbered space below: Energy A. Define the following: 1. kinetic energy 2. potential energy 3. chemical potential energy 4. Law of Conservation of Energy Pg.17

18 B. Answer the review questions on p. 69. Place the answer to each multiple choice question in the numbered space below: CHAPTER 4: ATOMIC THEORY 4.1 THE ATOMIC THEORY 1. ~ BC, Democritus atomos 2. Middle Ages, Alchemists (see Chapter 1.1) John Dalton 4. Law of Definite Proportions (define and give an example) 5. Law of Multiple Proportions (define and give an example) 6. Dalton s Atomic Theory & Model of the Atom Pg.18

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20 Chapter 4.1 Review Questions on Pages : Pg.20

21 4.2 FURTHER UNDERSTANDING OF THE ATOM JJ Thomson a. Cathode ray tubes (Crooke s tubes) b. mass to charge ratio (how did mass & charge relate to Thompson s study) c. Plum Pudding Model of the Atom Robert Millikan Oil Drop Experiment Ernest Rutherford a. Gold Foil Experiment: what it was and how it was done b. Main Conclusions of Gold Foil Experiment c. Planetary Model of the Atom (Solar System Model of the Atom) Pg.21

22 Chapter 4.2 Review Questions on Pages : Pg.22

23 4.3 ATOMIC STRUCTURES Antoine Lavoisier -Chemist, Biologist, Economist, & Royal Tax Collector -Made quantitative observations (to.0001 g) -Articulated the Law of Conservation of Matter a. Law of Conservation of Matter (Chapter 3.3) b. Law of Constant Composition (Law of Definite Composition) - All samples of a compound have the same composition and have the same proportions by mass of the elements present Ex. All H2O molecules are exactly the same! Henri Becquerel, and 1898 Marie Curie Radioactivity -Observed elements that could darken photographic plates even though they were covered = Radioactivity! -3 Types: Alpha ( ), Beta ( ), Gamma ( ) -Contradicted Dalton s idea that atoms are indivisible since they determined that there must be particles smaller than atoms (sub-atomic) 3. Composition of the Nucleus a. Electrons (e - ) b. Protons (p + ) c. Neutrons (n o ): 1932, Chadwick Pg.23

24 d. Properties of subatomic particles: symbol, mass, charge, location Particle Symbol Mass Charge Location Protons Neutrons Electrons 4. Atomic Number (Z) 5. Mass Number (A) 6. Atomic Symbol -Unique combination of one, two, or three letters that represents each element *Capital letter is always written first -Names usually indicate properties or discoverers Ex. Fe = Iron (Ferrous) 7. Isotopes -Ex. Hydrogen Protium Deuterium Tritium 1p + 1p + and 1n o 1p + and 2n o 8. Mass Spectrometer and Percent Abundance -Uses mass-charge ratio to break apart and separate fragments of compounds -Shows isotopic abundance for elements % Abundance = (# atoms-isotope)/(total # atoms-all isotopes)*100 Chapter 4.3 Review Questions on Pages : 1. Pg.24

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