AP Chemistry Summer Assignment Welcome to Advanced Placement Chemistry! The AP chemistry class is an excellent opportunity for students considering careers in chemistry, chemical engineering, or medicine. This college level course includes the study of atomic structure, periodicity, bonding, chemical reactions, oxidationreduction, solutions, acids and bases, thermodynamics, kinetics, equilibrium, nuclear chemistry and electrochemistry. Quantitative and qualitative laboratory investigations will involve critical thinking skills and use of lab equipment and instrumentation. Success in an academically rigorous course requires personal discipline and well-developed study skills. Extensive outside practice and study (3 – 5 hours per week) is expected for mastery of the contents of AP chemistry. Students are expected to acquire a firm grasp of course content. Success in Advanced Placement classes is a steppingstone to becoming an independent learner – a characteristic requisite for achievement in college. Please commit now to give the course the effort and time necessary to gain full benefit. In order to start the year off strong in this course, you will need to review a few basic concepts and methods. Study this material then answer the questions and do the provided problems. Solving a problem does not mean just writing down an answer. You must show your work! The problems will be collected the first week of class. If you have trouble remembering past material, you can search the web for reviews or use the websites provided. The first AP Chemistry test is scheduled for the second week of school and will include the topics addressed in this summer packet. The Elements: You must memorize the names and symbols for these elements. We will have a quiz over them the first week of class. Spelling does count. 1. carbon, C 2. oxygen, O 3. hydrogen, H 4. nitrogen, N 5. calcium, Ca 6. iron, Fe 7. iodine, I 8. silver, Ag 9. aluminum, Al 10. chlorine, Cl 11. sulfur, S 12. sodium, Na 13. helium, He 14. nickel, Ni 15. silicon, Si 16. mercury, Hg 17. zinc, Zn

18. manganese , Mn 19. uranium, U 20. argon, Ar 21. lead, Pb 22. tin, Sn 23. bromine, Br 24. gold, Au 25. copper, Cu 26. potassium, K 27. fluorine, F 28. barium, Ba 29. neon, Ne 30. strontium, Sr 31. tungsten, W 32. platinum, Pt 33. radium, Ra 34. cesium, Cs

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35. magnesium, Mg 36. lithium, Li 37. cobalt, Co 38. chromium, Cr 39. tin, Sn 40. xenon, Xe 41. germanium, Ge 42. selenium, Se 43. gallium, Ga 44. bismuth, Bi 45. boron, B 46. arsenic, As 47. beryllium, Be 48. radon, Rn 49. phosphorus, P 50. antimony, Sb

SI Units of Measure: In 1960 the International System of Units was proposed as a replacement for the Metric System. The SI Base Units are given below. Physical Quantity Name of Unit Symbol length meter m mass Kilogram kg time second s temperature kelvin K electric current ampere A amount of substance mole mol luminous intensity candela cd Temperature Scales and Conversions There are 3 temperature scales you need to be aware of, the Celsius temperature scale, the Fahrenheit temperature scale and the Kelvin temperature scale. In chemistry we use either the Celsius scale or the Kelvin scale. Memorize these 3 conversion formulas. To convert from Celsius temperature scale to Fahrenheit temperature scale use: TºF = 9/5 T ºC + 32 To convert from Fahrenheit temperature scale to Celsius temperature scale use: TºC = 5/9( T ºF - 32) To convert from Celsius temperature scale to Kelvin temperature scale use: TK = T ºC + 273.15 Questions and Problems: Reminder - always show your work. Example: Convert 0.005 kg to cg. 0.005 kg x 1000 g x 100 cg = 500 cg 1 1 kg 1g 1. Convert room temperature (25 ºC) to the Kelvin scale. 2. Convert room temperature to the Fahrenheit scale. 3. What does the term normal boiling point mean? 4. What does melting point mean? 5. What is the freezing point of water in each of the 3 temperature scales? 6. What is the boiling point of water in each of the 3 temperature scales? 7. Determine at what temperature TºF = TºC 8. Gold melts at 1064 ºC. What is this temperature in K and ºF ? 9. The Kelvin scale is an absolute temperature scale. What is meant by absolute temperature? 10. The normal boiling point Liquid nitrogen is 77 K. What is the temperature in ºC? in ºF? Scientific Notation 2

Scientific notation is a method of handling very large or very small numbers easily. In normal notation a number might be 875,000. The same number in scientific notation this number is 8.75 x 10 5. A small number like 0.000324 in normal notation would be 3.24 x 10 -4 in scientific notation. You can study this topic more at http://www.chem.tamu.edu/class/fyp/mathrev/mr-scnot.html . Questions and Problems 11. Convert the following numbers into scientific notation. 1,067,000 cg

245 hm

0.00000209 kg

602000000000000000000000 nm

2500 L

0.0000000011 kL

12. Convert the following numbers into normal notation. 8.361 x 10 7 cg

6.2 x 10 -4 km

3.0 x 10 8 mL

6.626 x 10 –34 Mg

Significant Figures Significant figures are the digits in a number that contribute to the accuracy of the number. (In this course we will often abbreviate with sig. figs. or s.f.) Numbers will normally include some digits that are known accurately plus one digit that has uncertainty. Take the measurement 23.6 cm. The 2 is known in the ten’s place and the 3 is known, but the 6 has uncertainty as described. This number therefore has 3 significant figures. Study the following website to review significant figures. http://www.chem.tamu.edu/class/fyp/mathrev/mr-sigfg.html Questions and Problems 13. When considering significant figures, does 2.00 cm = 2 cm ? 14. What is an exact number versus an inexact number? 15. What do the terms accuracy and precision mean? 16. Indicate the number of significant figures in each of these numbers 0.00345 hm

0.3045 kg

0.03100 daL

7500 mm

9.006 x 105 m

17. Perform the following operations keeping the correct number of sig. figs. in the answer. 1.5 m x 7.6 m =

1.50 g x 7.6 g =

1.50 L x 7.60 L =

1.5 m + 7.6 m =

1.50 g + 7.6 g =

1.0 cm x .01 cm =

1.50 L + 7.60 L = Prefixes for Units

1.0 cm + .01 cm = 3

Memorize these prefixes and be able to use them in problems. Prefix megakilocentimillimicronano-

Abbreviation M k c m μ n

Meaning 106 103 10-2 10-3 10-6 10-9

Example 1 megameter (Mm) = 1 x 106 m 1 kilogram (kg) = 1 x 103 g 1 centimeter (cm) = 1 x 10-2 m 1 milligram (mg) = 1 x 10-3 g 1 micrometer (μg) = 1 x 10-6 μg 1 nanogram (ng) = 1 x 10-9 g

Dimensional Analysis In chemistry we use the method of dimensional analysis to convert between units and help solve problems. The technique requires use of conversion factors which are used to convert from 1 unit to another. For example, how many inches are in 3.0 ft? Since there are 12 inches in 1 ft, the conversion factor is 12 in/1ft. So, 36.0 in x 1 ft = 3.00 ft 1 12 in Study the following website to review dimensional analysis. http://www.chem.tamu.edu/class/fyp/mathrev/mr-da.html Questions and Problems: 18. A kg is how many times larger than a mg? 19. A μm is how many times smaller than a Mg? Solve the following problems using Dimensional Analysis: 20. How many mm are in 2.3 m? 21. How many km are in 3500 m? 22. How many cm are in .25 m? 23. How many nanometers are in .50 meter? 24. How many μg are in 87 mg? 25. Use dimensional analysis to determine how many seconds are in 2.00 years. 26. How many yards are in 126 inches? Solve the following problems using Dimensional Analysis: 4

27. The molecular mass of water is 18.015 g/mole. What is the mass of 3.5 mole of water? 28. How many moles are present in 75.0 g of water? 29. Calculate the number of hydrogen atoms present in100.0 g of water. Remember the formula for water is H2O and that there 6.02 x 10 23 atoms /mol.

Units for Volume In chemistry we use the liter (L) as the base unit for measuring volume. We also use the mL and cm 3 as well. 1 mL = 1 cm 3 Questions and Problems 30. Using the fact that 1 mL = 1 cm 3, use dimensional analysis to show how many Liters are in 655 cm3. 31. Determine the conversion factor between dm3 and liters. 32. Use dimensional analysis and find how many mL are in 12.5 gallons? (1 L = 1.057 quarts, 4 quart = 1 gal.)

Density Density is an intensive physical property defined as D= m/V, where m is the mass of the object and V is the volume. Questions and Problems 33. What is the density of a solution with mass 755.85 g and volume of 600.0 ml? 34. You weigh out 125.0 grams of the solution from problem 35. What is its volume? 35. A certain metal alloy has density of 8.85 g/cm3. How many grams are in 3.0 cm3 of the alloy? 36. What is the density of a solution with mass of 23.6 grams and volume of 18 ml? Common Polyatomic Ions and Acids and Bases 5

You will need to memorize the list of common polyatomic ions as well as the list of acids and bases. You will be tested on these within the first 3 weeks of school. Common Polyatomic Ions ammonium

NH4 +

hydroxide

OH –

hydronium

H3O +

peroxide

O2 2-

mercury (I)

Hg2 2+

oxalate

C2O4 2-

acetate

C2H3O2 - (or CH3COO -)

permanganate MnO4-

carbonate

CO3 2 –

cyanide

CN -

thiocyanate

SCN –

hydrogen carbonate HCO3 – (or bicarbonate) chromate

CrO42-

phosphate

PO43-

dichromate

Cr2O7 2-

phosphite

PO33-

perchlorate

ClO4

-

hydrogen phosphate HPO42-

chlorate

ClO3

-

hydrogen sulfate HSO4 - (or bisulfate)

chlorite

ClO2

-

sulfate

SO4 2-

nitrate

NO3

-

sulfite

SO3 2-

nitrite

NO2

-

Common Acids and Bases 4 Strong Acids hydrochloric acid sulfuric acid nitric acid perchloric

HCl H2SO4 HNO3 HClO4

Weak Acids acetic acid HC2H3O2 (or CH3COOH) phosphoric acid H3PO4 chloric acid HClO3 carbonic acid H2CO3 hydroiodic acid HI hydrofluoric acid HF hydrobromic acid HBr

Strong Bases The hydroxides of IA and IIA metals: KOH, NaOH, LiOH, CsOH, RbOH Sr(OH)2, Ba(OH)2, Ca(OH) 2, Mg(OH)2 Weak Bases ammonia sodium bicarbonate

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NH3 NaHCO3