Advanced Placement Chemistry Summer Assignment Ms. Morrissey ([email protected])

DUE THE FIRST DAY OF SCHOOL! (Tuesday Sept. 8, 2020)

A.P. Chemistry is a highly rigorous course that covers most of the material that would be covered in a first year college chemistry course. It is intended for students who are highly motivated to accept the challenge of a college course at the high school level and have demonstrated a willingness to commit considerable time to studying and completing assignments outside of class.

The topics to be covered extensively over the summer are provided as test review questions and are usually included in the first 3 chapters of most textbooks used for Honors or AP Chemistry. These chapters are Chapter 1 (Matter and Measurement), Chapter 2 (Atoms, Molecules, and Ions), and Chapter 3 (Stoichiometry). If you have an Honors Chemistry textbook then you may reference that. If you do not then I have posted a pdf version of another textbook used in other AP Chemistry classes on Google Classroom. You must email Ms. Morrissey for the class code to join the Google Classroom. You may also use notes from your previous chemistry class or any reputable online resources. The list of test review questions have been provided to help you focus your review this summer. I highly suggest you utilize this list as your first assessment will be on these topics/calculations. I will also provide additional resources on Google Classroom for you to fully prepare/practice topics that normally require it such as applying sig figs, nomenclature, and all calculations. Depending on your comfort level you may want to complete these extra practice resources before or after completing the 50 multiple choice questions.

The summer assignment is being proficient with the list of topics/calculations provided and completing the packet of 50 multiple choice questions. It is your choice whether or not to print the packet of 50 MC questions. The packet will not be collected but your answers will be submitted via a google form that will be provided on the first day of class. Your goal is to be prepared to take a test on the material shortly after the beginning of school.

AP Chemistry is designed to expand on previously covered material from Honors Chemistry. Due to the fast paced nature of the course you will have to get accustom to reading and comprehending the material in the text book, using other resources, completing additional/suggested problems outside of class, and forming study groups. If you get help with your summer assignment make sure you understand how to get the answers yourself as you will be the one taking the tests. Email me with any questions or concerns.

The following topics will be covered this year:  Ch. 4 Aqueous Reactions and Solution Stoichiometry  Ch. 5 Thermochemistry  Ch. 6 Electronic Structure of Atoms  Ch. 7 Periodic Properties of the Elements  Ch. 8 & 9 Chemical Bonding and Molecular Geometry  Ch. 10 Gases (This entire chapter will most likely be assigned during winter break)  Ch. 11 Intermolecular Forces, Liquids, and Solids  Ch. 13 Properties of Solutions  Ch. 14 Chemical Kinetics  Ch. 15 Chemical Equilibrium  Ch. 16 & 17 Acid-Base Equilibria and Additional Aspects of Aqueous Equilibria  Ch. 19 Chemical Thermodynamics  Ch. 20 Electrochemistry AP Chemistry Ch.1-3 Test Review Questions

1. Be familiar with the following separation techniques for mixtures: filtration, distillation, chromatography. 2. What role does each subatomic particle play? How is the number of protons, neutrons, and electrons determined? 3. How is the average atomic mass of an element calculated? How is the mass of one isotope or the percent abundances determined if all other information is given? 4. How does a mass spectrometer work? What type of information does it provide? Suggested videos to watch: https://www.youtube.com/watch?v=EzvQzImBuq8 Optional but more detailed videos: https://www.youtube.com/watch?v=tOGM2gOHKPc https://www.youtube.com/watch?v=KF9_f7uRMoY 5. Which are the diatomic elements? 6. Which elements are metalloids and what are some uses for them? 7. What are the different groups found on the periodic table and distinctive properties about each one? 8. How do you name and write formulas for ionic compounds, molecules, and acids? 9. How do you write balanced chemical equations? 10. How do you determine how many decimal places to include in your data when recording measurements in lab? 11. What are the rules for sig figs when calculating data? 12. What is Avogadro’s number? When and how is it used? 13. What are the SI prefixes and their values? How do you convert between the SI prefixes and units that are squared and cubed? 14. How do you convert between Celsius and Kelvin? 15. Being that percent composition is an intensive property, how does that help you in determining information about elements in a specific compound? 16. Compare and contrast empirical and molecular formulas. 17. How is the empirical formula of a compound determined given the masses or percentages of each element? How is empirical formula determined through combustion analysis? 18. How is the molecular formula determined? 19. When do you have to determine if there is limiting reactant? How is the limiting reactant identified? 20. How do you determine how much excess reactant is left over? 21. How is percent yield calculated? 22. How is percent error calculated?

AP Chemistry Summer Assignment

1. Express 7,500 nm as picometers. A) 7.50 pm B) 75.0 pm C) 750 pm D) 7.5 × 106 pm E) 7.5 × 1012 pm

2. The diameter of Earth is 12.7 Mm. Express this diameter in centimeters. A) 1.27 × 105 cm D) 1.27 × 108 cm B) 1.27 × 106 cm E) 1.27 × 109 cm C) 1.27 × 107 cm

3. Which of the following represents the largest mass? A) 2.0 × 102 mg B) 0.0010 kg C) 1.0 × 105 ng D) 2.0 × 102 cg E) 10.0 dg

4. After carrying out the following operations, how many significant figures are appropriate to show in the result? (13.7 + 0.027) ÷ 8.221 A) 1 B) 2 C) 3 D) 4 E) 5

5. How many significant figures does the difference 218.7201 – 218.63 contain? A) 1 B) 2 C) 3 D) 5 E) 7

6. How many significant figures does the result of the following operation contain? 8.52010 × 7.90 A) 2 B) 3 C) 4 D) 5 E) 6

7. Give the correct number of significant figures to the problem below. 5.80 x 10-1 – 3.4 x 10-2 = A) 5.5 x 10-1 B) 5.46 x 10-1 C) 2.4 x 10-3 D) 2.4 x 102 E) 5.5 x 10-2

8. How many square kilometers are equivalent to 28.5 cm2? A) 2.85 × 10–9 km2 D) 2.85 × 10–4 km2 B) 2.85 × 10–6 km2 E) none of these C) 285 km2

9. A block of iron has a mass of 826 g. What is the mass of a block of magnesium that has the same volume as the block of iron? The following densities at 25°C are provided: magnesium, 1.7 g/cm3 ; graphite, 1.8 g/cm3 ; iron, 7.9 g/cm3. A) 1,400 g B) 3,800 g C) 830 g D) 180 g E) none of them are within 10 g of the right answer.

10. The "escape velocity" from Earth (the speed required to escape Earth's gravity) is 2.5 × 104 miles per hour. What is this speed in m/s? (1 mile = 1609 m) A) 4.2 × 10–3 m/s B) 6.9 m/s C) 4.2 × 102 m/s D) 1.1 × 104 m/s E) 4.0 × 107 m/s

11. Convert 4.5 m3 to L A) 4.5 x 10-1 L B) 4.5 x 101 L C) 4.5 x 10-3 L D) 4.5x103 L E) 4.5 x 102L

12. Iron has a density of 7.87 g/cm3. What mass of iron would be required to cover a football playing surface of 120 yds × 60 yds to a depth of 1.0 mm? (1 inch = 2.54 cm; 1 lb = 453.6 g) A) 6.4 × 103 lb B) 6.4 × 104 lb C) 1.0 × 105 lb D) 4.7 × 107 lb E) 4.7 × 108 lb

13. Which of the following elements is most likely to be a good conductor of electricity? A) N B) S C) He D) Cl E) Fe

14. Which of the following elements is chemically similar to oxygen? A) sulfur B) calcium C) iron D) nickel E) sodium

15. Complete the following chart, in order from left to right Ion Mass Number Protons Neutrons Electrons 40Ca2+

A) 40, 20, 20, 20 D) 40, 20, 20, 22 B) 40, 20, 20, 18 E) 20, 40, 20, 22 C) 20, 20, 40, 20

16. Complete the following chart, in order from left to right Ion Mass Number Protons Neutrons Electrons 4 2 0

A) 4He, 2 B) 4Be, 4 C) 4Be, 2 D) 4He, 4 E) 2H, 2

17. What are the ions present in the compound CH4? A) C4+, H+ B) C4-, H+ C) C-, H+ D) C4- H4+ E) no ions present

18. What are the two different ions present in the compound Li3N? + 3- + - 3+ 3- + - 3+ 3- A) Li , N B) Li3 , N C) Li3 , N D) Li , N E) Li , N

19. Which of the following is the formula for hydroiodic acid? A) HIO4 B) HIO3 C) HIO2 D) HIO E) HI

20. The formula for calcium phosphate is A) CaPO4. B) Ca3(PO4)2. C) Ca2(PO4)3. D) Ca3P2. E) Ca3(PO3)2.

21. The formula for sodium sulfide is A) NaS. B) K2S. C) NaS2. D) Na2S. E) SeS.

22. The name for NH4NO3 is A) ammonium nitrate. D) hydrogen nitrogen . B) ammonium nitrogen trioxide. E) hydrogen nitrate. C) ammonia nitrogen oxide.

23. The name for KHCO3 is A) calcium bicarbonate. D) calcium hydrogen . B) calcium carbonate. E) potassium hydrogen carbonate. C) potassium carbonate.

24. Which is the formula for lead(IV) chloride? A) Pb4Cl B) PbCl2 C) PbCl3 D) PbCl4 E) Pb2Cl4

25. What type of compound is HBrO2? A) Ionic B) Binary C) Acid D) Base E) Hydrate

26. Name the acid H2SO3 (dissolved in water). A) Sulfuric acid D) Persulfuric acid B) Sulfurous acid E) Hyposulfurous acid C) Hydrosulfuric acid

27. The chemical formula for iron(II) nitrate is A) Fe2(NO3)3 B) Ir(NO2)2 C) Fe2N3 D) Fe(NO3)2 E) Fe(NO2)2

28. Name the compound Cl2O5 A) chlorine pentoxide D) chloride oxide B) dichlorine pentoxygen E) dichloride pentoxide C) dichlorine pentoxide

29. Name the compound CrO3. A) chromium oxide D) chromium(III) oxide B) chromium(II) oxide E) chromium(VI) oxide C) chromium(III) trioxide

30. There are two stable isotopes of chlorine: chlorine-35, with a mass of 34.968853 amu; and chlorine-37, with a mass of 36.965903. Given that the average atomic mass of a chlorine atom is 35.45 amu, which of the following statements is true? A) 35 37 Chlorine contains almost exclusively 17 Cl with very little 17 Cl. B) 35 37 Chlorine contains more 17 Cl than 17 Cl. C) 35 37 Chlorine contains roughly equal amounts of 17 Cl and 17 Cl. D) 37 35 Chlorine contains more 17 Cl than 17 Cl. E) 37 35 Chlorine contains almost exclusively of 17 Cl, with very little 17 Cl.

31. Calculate the average atomic mass of lithium using the following data: Isotope Abundance Mass 6Li 7.5 % 6.0151 amu 7Li 92.5% 7.0160 aum

A) 6.51 amu B) 6.02 amu C) 6.94 amu D) 7.02 amu E) 6.50 amu

32. A mass spectrometer works by ionizing atoms or molecules, and then accelerating them through oppositely charged plates. The mass is obtained by A) measuring the force of impact on a detecting screen, and then calculating the mass using force = mass × acceleration. B) suspending the ions in an applied electric field, and then calculating mass by the setting the downward gravitational force equal to the upward electrostatic force. C) measuring the magnitude of deflection as the ions pass through a magnetic field to obtain the charge-to-mass ratio, and then calculating the mass from that ratio. D) measuring the time it takes for the ions to hit the detector at a known distance to calculate the acceleration, and then calculating mass from force = mass × acceleration.

33. How many molecules are there in 8.0 g of ozone, O3? A) 3.0 molecules D) 3.0 × 1023 molecules B) 3.6 × 1024 molecules E) 6.0 × 1023 molecules C) 1.0 × 1023 molecules

34. How many fluorine atoms are there in 65 g of CF4? A) 0.74 atoms D) 1.8 × 1024 atoms B) 3.0 atoms E) 2.4 × 1023 atoms C) 4.5 × 1023 atoms

35. The mineral pyrolusite is a compound of 55Mn and 16O. If 63% of the mass of pyrolusite is due to manganese, what is the empirical formula of pyrolusite? A) MnO B) Mn2O C) Mn2O2 D) MnO2 E) none of these

90 36. Zircon is a mineral with the empirical formula ZrSiO4. If all the zirconium is Zr, all the silicon is 28Si, and all the oxygen is 16O, what mass of oxygen is present in 10. g of zircon? A) 0.88 g B) 1.2 g C) 1.8 g D) 3.5 g E) 5.4 g

37. An unknown compound with a molar mass of 155.06 g/mol consists of 46.47% C, 7.80% H, and 45.72% Cl. Find the molecular formula for the compound. A) CHCl B) C9H18Cl3 C) C6H12Cl D) C6H12Cl2 E) C3H6Cl

38. What is the coefficient of H2O when the following equation is properly balanced? ___ Al4C3 + ___ H2O  ___ Al(OH)3 + ___ CH4 A) 3 B) 4 C) 6 D) 12 E) 24

39. When balanced the coefficient of O2 in the following equation is __ C2H4 + __ O2  __ CO2 + __ H2O A) 1. B) 2. C) 3. D) 4. E) 6.

40. Lithium metal reacts with nitrogen gas to form lithium nitride. Identify the balanced reaction that describes this process. A) Li + N  LiN D) 6Li + N2  2Li3N B) Li + N2  LiN2 E) 2Li + N2  2LiN C) 2Li + N2  Li2N2

41. Iron metal reacts with hydrochloric acid to produce iron (II) chloride and hydrogen gas. Identify the balanced reaction that describes this process. A) Fe + 2 HCl  FeCl2 + H2 D) 2Fe + 2HCl  2FeCl2 + H2 B) Fe + HCl  FeCl2 + H2 E) Fe + 3HCl  FeCl3 + H2 C) Fe + HCl  FeCl + H

42. Aluminum metal reacts with nitric acid to produce aluminum nitrate and hydrogen gas. Identify the balanced reaction that describes this process. A) Al + HNO3  AlNO3 + H2 D) Al + 3HNO3  Al(NO3)3 + H2 B) Al + HNO3  AlNO3 + H E) 2Al + 6HNO3  2Al(NO3)3 + 3H2 C) Al + 2HNO3  Al(NO3)2 + H2

43. Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid. How many total moles of acid are formed when starting with 4.5 g of PCl5 and excess H2O? PCl5 + 4H2O  5HCl + H3PO4 A) 0.022 moles B) 0.12 moles C) 0.13 moles D) 27 moles E) 23 moles

44. Chlorine gas reacts with phosphorus to produce phosphorus pentachloride. How many grams of PCl5 are produced from 3.5 g of Cl2 and excess P? 5Cl2(g) + 2P(s)  2PCl5(s) A) 1.4 g B) 4.1 g C) 8.2 g D) 0.020 g E) 730 g

45. Liquid heptane, C7H16, burns in oxygen gas to yield and water. What is the minimum mass of oxygen required for the complete reaction of 25.5 mL of heptane? (density of heptane = 0.6838 g/mL) C7H16 + 11O2  7CO2 + 8H2O A) 5.57 g B) 8.14 g C) 30.6 g D) 61.3 g E) 89.6 g

46. A sample of aluminum metal is placed in a graduated cylinder. It is noted that 5.50 mL of water is displaced by the aluminum. The aluminum is then reacted with excess nitric acid to produce aluminum nitrate and hydrogen gas. Given the density for aluminum is 2.702 g/mL, how many grams of aluminum nitrate are produced in the reaction? 2Al(s) + 6HNO3(aq)  2Al(NO3)3(aq) + 3H2(g) A) 161 g B) 11.0 g C) 14.9 g D) 117 g E) 235 g

47. Ammonia reacts with oxygen to form and water vapor: 4NH3 + 5O2  4NO + 6H2O When 20.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent? A) NH3 B) O2 C) NO D) H2O E) No reagent is limiting.

48. Vanadium(V) oxide reacts with calcium according to the chemical equation below. When 10.0 moles of V2O5 are mixed with 10.0 moles of Ca, which is the limiting reagent? How much of the excess reactant is left? V2O5(s) + 5Ca(l)  2V(l) + 5CaO(s) A) V2O5 , 5.0 moles D) CaO , 10.0 moles B) Ca , 5.0 moles E) No reagent is limiting. C) V , 10.0 moles

49. What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the chemical equation below? 2Al + Cr2O3  Al2O3 + 2Cr A) 7.7 g B) 15.4 g C) 27.3 g D) 30.8 g E) 49.9 g

50. The first step in the Ostwald process for producing nitric acid is 4NH3(g) + 5O2(g)  4NO(g) + 6H2O(g). If the reaction of 150. g of ammonia with 150. g of oxygen gas yields 87. g of nitric oxide (NO), what is the percent yield of this reaction? A) 33% B) 49% C) 62% D) 77% E) 100%