Advanced Placement Chemistry Summer Assignment Ms
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Advanced Placement Chemistry Summer Assignment Ms. Morrissey (morrissey@cranfordschools.org) 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 4 4 4 4 2 A) He, 2 B) Be, 4 C) Be, 2 D) He, 4 E) H, 2 17. What are the ions present in the compound CH4? 4+ + 4- + - + 4- 4+ A) C , H B) C , H C) C , H D) C H 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.