Welcome to AP Chemistry!

Welcome to AP Chemistry! I am really looking forward to next year and hope you feel the same way. Taking AP Chemistry is a privilege. The road to success in this class will not be easy. Students and parents should not be surprised at the amount of work required for this class. Students should spend at least five- seven hours a week outside of class studying for this class. Also, do not be surprised if some students who are accustomed to making all A s, will suddenly begin making B s or C s on tests and start to doubt themselves, their teacher, and their decision to enter this course. You must keep in mind that you are taking a college level course with standards that are higher than usual. Students do not have to make A s on every test to do very well on the AP Exam! It is also a welldocumented fact that students having AP Chemistry in high school do much better even in higherlevel chemistry courses as compared to those who take only the first year equivalent course in college. In addition to these facts, colleges are known to use the first chemistry classes to weed out those students who are least qualified. With these considerations in mind, it is obvious that a good preparation in high school is required and will only benefit those who choose to take this course. Due of the vast amount of time required for this class or any other AP class, your extracurricular activities should be chosen wisely. I have known many AP Chemistry students in the past who have been involved in activities such as band, athletics, or other clubs, and have done well in the class. However, you must truly be able to budget your time and keep yourself organized. Selfdiscipline and self-motivation is a key part of being successful in the AP Chemistry course. I look forward to next year and I hope that this information has been helpful. As you probably already know, AP Chemistry is a very challenging course with an equally challenging AP test (Thursday, May 9, 2019, 8a.m.). The material is detailed and we have several topics to cover. You will need to refresh your memory on information that was taught in your prior Chemistry class so that we can move on to expand on your knowledge base. Your goal should be to complete this summer assignment that covers material from your honors course here at SV. You will turn these in by the end of week 1 for credit. You should email me questions as they arise. I have also posted some review videos and websites in Google Classroom if you need them. (Our class is called AP Chemistry 18-19. You should join this group as soon as possible (Invite code: 2vsxi1t)). I would encourage you to pace yourself so you do not end up trying to cram all the material in right before school begins in September. We will reinforce this review during the beginning of the school year. We will have a test within the first 2 weeks of school to check on your progress of understanding and preparation. The course will move on from the initial review into more advanced studies of first year college chemistry. The topics will build upon your knowledge from prior Chemistry class and cover more application and detail. You will begin to place the pieces together in the jigsaw puzzle called Chemistry. Good Luck! Mrs. Guille aguille@pdsdstudents.org

Mrs. Guille s AP Chemistry Summer Assignments Attached you will find some chemistry problems that you are expected to complete. Most of the problems, as stated in the letter, are review from your honors course. I have posted notes and videos on each of these new topics on the Google Classroom page. On the ABOUT tab, I have also posted a link and a pdf file to our old AP textbook: CHEMISTRY: PRINCIPLES AND REACTIONS by Masterton and Hurley for reference. You are getting new textbooks this year.yeah! My recommendation is that you pace yourself on the attached so that you do not get caught trying to get all the work done in late August. **A written effort is expected for all problems. However, if you truly get stuck on some of these problems, do not hesitate to contact a classmate for help. It is ok to work together to gain an understanding, but you will do yourself no good if you just copy the work. You can also feel free to email me or message me on Google Classroom with questions you have over the summer and I will do my best to help you. I also recommend referencing the videos in Google Classroom. If after that you still cannot come to an answer, star it and list questions you would like me to answer when we return! Recommendations for materials in this course: Obtain a three ring binder with lined paper to do your work in. It will be helpful in the fall once we start class to be able to add pages to your notebook as you will receive a lot of paperwork and do a lot of problem solving for this class. A scientific calculator (doesn t have to be graphing) Notecards for writing down pertinent information to use for review later (common ions as you will not have a charge sheet to use on tests or quizzes; rules (solubility, etc.); strong acids and bases, etc.) Purchase an AP Chemistry study guide. Some suggested resources will be posted in Google Classroom. SOME HELPFUL AP Chemistry TIPS: TIP #1: Memorize the names of the elements and their corresponding symbols You need to know elements 1-56, plus Pt, Au, Hg, Pb, Rn, Fr, Ra, U, Pu Many of these elements you will already know Making flashcards is helpful! It s important to know these elements because the periodic table you are provided has only the symbols and not the names of the elements. TIP #2: Memorize the ionic charges of the basic ions Think about the valance electrons! Think about the common elements/ions in that group o Group 1 ions = +1 o Group 2 ions = +2 o Group 15 (5A) ions (N and P) = -3 o Group 16 (6A) ions (O and S) = -2 o Group 17 (7A)/ halogens = -1 o Zn = +2 o Ag = +1 o Cu = +1 or +2 o Fe = +2 or +3 o Pb = +2 or +4 o Sn = +2 or +4

TIP #3: Memorize the names, symbols, and charges of Polyatomic ions below: Oxyanions polyatomics containing oxygen, names end in ate or ite -ate is used for the most common form -ite is used for the form with the same charge, but one less oxygen o Example: NO3- = nitrate NO2- = nitrite Prefixes are also used o Per- indicates one more oxygen than the ate form (think perfect = overachieving, ie = more) o Hypo- indicates one fewer oxygen than the ite form o Example: ClO4- = perchlorate (b/c it has one more O than the ate form) ClO3- = chlorate (b/c it is the most common) ClO2- = chlorite (b/c it has one less oxygen than ate form) ClO4- = hypochlorite (b/c it has one less oxygen than the ite form) o F, Cl, Br, I all behave the same Therefore, if chlorate is ClO3-, the bromate ion is BrO3-!!!! Simply substitute one halogen for the other If you learn the chlorate series, you also automatically know the bromate, iodate, and fluorate series Hydrogen can be added to -2 or -3 ions to make a new ion i.e. H2PO4 1 is dihydrogen phosphate (note the charge went up 1 for each H+ added)

DIRECTIONS: Solve the problems below, showing your setup, calculations, units and correct Significant Figures (SigFigs). Neatly-written solutions are acceptable. (Points are deducted from AP tests if correct SigFig rules and labels are ignored, so get into the habit of using them all of the time!) 1. Demonstrate that you know the correct use of significant figures (SigFig digits) by completing the following: a. 738.90 m has SigFgs. b. 0.0304 g has SigFigs. c. 1.4 X 10 4 joules has SigFigs. d. 1 dozen donuts has SigFigs. e. 40 ml has SigFigs. f. 800. m has SigFigs. 2. A cylinder rod formed from silicon is 21.3 cm long and has a mass of 5.00 kg. The density of silicon is 2.33 g/cm 3. What is the diameter of the cylinder? (The volume of cylinder is given by V = πr2h, where r is the radius and h is the length.) 3. Calculate the following to the correct number of significant figures. a. 1.27 g / 5.296 cm 3 = b. 12.235 g / 1.01 L = c. 12.2 g + 0.38 g = d. 17.3 g + 2.785 g = e. 2.1m x 3.215m = f. 200.1mi x 120 mi = g. (17.6 + 2.838 + 2.3 + 110.77)g =

4. Conversions (round answers correctly and show work with units) Make the following conversions: a) 16.2 m to km b) 5.44 nl to ml c) 45.7 ml/s to kl/hr 5. Provide names for the following ionic compounds: a. AlF3 b. Fe(OH)2 c. Cu(NO3)2 d. Ba(ClO4)2 e. Li3PO4 f. Hg2S g. Cr2(CO3)3 h. (NH4)2SO4 6. Write the chemical formulas for the following compounds: a. Copper(I) oxide b. Potassium peroxide c. Iron(III) carbonate d. Zinc nitrate e. Sodium hypobromite f. Aluminum hydroxide

7. Give the name or chemical formula for each of the following molecular substances: a. SF6 b. XeO3 c. Dinitrogen tetroxide d. Hydrogen cyanide e. IF5 f. Dihydrogen monoxide g. Tetraphosphorous hexasulfide 8. Give the name or chemical formula for the following compounds: a. Ammonium oxalate b. Manganese(III) dichromate c. Ti(OH)4 d. Ni(ClO2)3 e. Dinitrogen pentoxide f. Aluminum oxide g. Fe2S3 9. Name the following acids a. H2C2O4 b. HBrO3 c. HBr d. HNO2 e. H2SO4 f. HClO 10. Write formulas for the following acids. a. hydrochloric acid b. sulfuric acid c. nitric acid d. phosphoric acid e. carbonic acid f. acetic acid

11. Balance the following and equations and tell what type of reaction it is (synthesis, decomposition, single replacement, double replacement, or combustion) a) KNO3 KNO2 + O2 Type: b) AgNO3 + K2SO4 Ag2SO4 + KNO3 Type: c) CH3NH2 + O2 CO2 + H2O + N2 Type: d) N2O5 + H2O HNO3 Type: e) Na + Zn(NO3)2 Zn + NaNO3 Type: 12. What are diatomic molecules? List the 7. 13. What is the Activity Series of metals, and how does it help us in studying properties of elements? 14. Write balanced chemical equations for the reaction of sodium with the following nonmetals to form ionic solids: a. Nitrogen b. Oxygen c. Sulfur d. Bromine 15. Write a balanced chemical equation for each of the following: a. The reaction of magnesium oxide with iron to form iron(iii) oxide and magnesium. b. The decomposition of dinitrogen oxide gas to its elements. c. The reaction of solid calcium carbide with water to form calcium hydroxide and acetylene (C2H2) gas. d. The reaction of solid calcium cyanamide (CaCN2) with water to form calcium carbonate and ammonia gas.

16. In Nature, strontium consists of four isotopes with masses and percent abundance of 83.9134 amu (0.50%), 85.9094 amu (9.9%), 86.9089 amu (7.0 %), and 87.9056 amu (82.6 %). Calculate the average atomic mass of Sr. 17. Determine number of protons, neutrons and electrons in each of the following. a. 39 K 19 b. 23 11 Na +1 c. 208 Pb 82 d. 33 15 P -3 18. Calculate the molar mass ( g/ mol) of a. Ammonia ( NH 3) d. Calcium bicarbonate ( Ca(HCO 3) 2 ) b. Baking soda ( NaHCO 3) c. Osmium Metal (Os) e. Calcium sulfate, dehydrate ( CaSO 4 2H 2O ) 19. Calculate the percentage by mass of the following compounds: a. SO 3 b. CH 3COOCH 3 c. Ammonium Nitrate

20. The hormone, thyroxine is secreted by the thyroid gland, and has the formula: C15H17NO4I4. How many milligrams of iodine can be extracted from 15.0 grams of thyroxine? 21. Calculate the number of moles of the following: a) 42.8 g of KNO 3 b) 155.7 L of CO 2 at STP c) 9.25 x 10 26 molecules of CaCl 2 22. Determine the number of molecules present in a 4.56 mol sample of methane gas (CH 4) ; then determine the number of hydrogen atoms in the sample. 23. Calculate the mass in grams of each of the following: a. 6.02 x 10 23 atoms of Mg b. 3.01 x 10 23 formula units of CaCl 2 c. 12.4 x 10 15 molecules of formaldehyde (CH 2O)

24. Using the following equation: 2 NaOH + H2SO4 2 H2O + Na2SO4 How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid? 25. Using the following equation: Pb(SO4)2 + 4 LiNO3 Pb(NO3)4 + 2 Li2SO4 How many grams of lithium nitrate will be needed to make 250 grams of lithium sulfate, assuming that you have an adequate amount of lead (IV) sulfate to do the reaction? 26. Using the following equation: Fe2O3 + 3 H2 2 Fe + 3 H2O Calculate how many grams of iron can be made from 16.5 grams of Fe2O3. 27. Determine the grams of sodium chloride produced when 10.0 g of sodium react with 10.0 g of chlorine gas according to the equation: 2 Na + Cl2 2 NaCl 28. Determine the mass of lithium hydroxide produced when 50.0g of lithium are reacted with 45.0g of water according to the equation: 2 Li + 2 H2O 2 LiOH + H2

29. Determine the percent yield of water produced when 68.3 g of hydrogen reacts with 85.4g of oxygen and 86.4g of water are collected. 2 H2 + O2 2 H2O 30. In an experiment, a student gently heated a hydrated copper compound to remove the water of hydration. The following data was recorded: a. Mass of crucible, cover, and contents before heating = 23.4 g. b. Mass of empty crucible and cover = 18.82 g. c. Mass of crucible, cover, and contents after heating to constant mass = 20.94 g. d. Calculate the percent by mass of water in the copper compound. 31. Determine the empirical and molecular formula of each of the following substances: a. Ibufuren, a headache remedy contains 75.6 % C, 8.80 % H, and 15.5% O by mass and a molar mass about 206 g/mol. 32. Epinerphine (adrenaline), a hormone secreted into the bloodstream in times of danger or stress contains 59% C, 7.1% H, 26.2% O, and 7.7% N by mass; its molar mass is about 180 g/mol.

33. Arsenic reacts with chlorine to form a chloride. If 1.587 g of arsenic reacts with 3.755 g of chlorine, what is the empirical formula of the chloride? 34. Vanillin, a flavoring agent, is made up of carbon, hydrogen, and oxygen atoms. When a sample of vanillin weighing 2.500g burns in pure oxygen, 5.79 g of carbon dioxide and 1.18 g of water are obtained. Calculate the empirical formula of vanillin. 35. Define solubility. Prepare a list of solubility rules for ionic compounds in water, and learn them. (Use a textbook or online resources.) (This is IMPORTANT for the AP test since you are expected to make predictions!)

36. Define Oxidation and Reduction. Provide at least three examples of oxidation and reduction, and write the balanced chemical reaction for each. (Example: Rusting of Iron: 4Fe + 3O 2 2Fe 2O 3) (**I know this is newer territory, but it will be discussed in multiple chapters in the AP course. We will cover this together in greater detail!) 37. Define Oxidation number. 38. Determine the Oxidation number of: a. Carbon in CO 2 b. Sulfur in H 2SO 4 c. Phosphorus in PO 4 3- d. Manganese in MnO 4 2-39. Which of the following statements are always true? Never true? Sometimes true? a. A compound with the molecular formula C 6H 6 has the same empirical formula. b. The mass percent of copper in CuO is less than in Cu 2O. c. The limiting reactant is the one present in the smallest number of grams. d. Since C 3H 6O 3 and C 6H 12O 6 reduce to the same formula, they represent the same compound. 40. A bedroom 11.0 ft x 12.4 ft x 8.0 ft contains 35.41 kg of air at 25 C. Express the volume of the room in liters, the amount of air in moles (Use the molar mass of air as 29.0 g/mol.) and the temperature in Kelvin.

41. A sample of carbon dioxide gas, CO 2 (g), occupies a volume of 5.75 L at 0.890 atm. If the temperature and the number of moles remain constant, calculate the volume when the pressure a. increased by a factor of 10.0 b. decreases to 0.445 atm 42. An open flask contains 0.200 mol of air. Atmospheric pressure is 745 mmhg and room temperature is 25 C. How many moles are present in the flask when the pressure is 1.10 atm and the temperature is 33 C? 43. On a warm day, an amusement park balloon is filled with 47.8 g He. The temperature is 33 C and the pressure in the balloon is 2.25 atm. Calculate the volume of the balloon. 44. Distinguish between strong and weak electrolytes, and provide two examples of each. 45. A volatile liquid (one that evaporates) is put into a jar and the jar is then sealed. How does the mass of the sealed jar and its contents change upon the vaporization of the liquid? 46. Distinguish between an Exothermic and an Endothermic reaction. In each case, how does the temperature of the surroundings change during such reactions?

47. How much heat is required to raise the temperature of 100 grams of water from 250 C to 820 C? 48. A piece of unknown metal with mass 14.9 g is heated to 1000 C and dropped into 75.0 g of water at 200 C. The final temperature of the system is 280 C. What is the specific heat capacity of the metal? 49. Calculate the molarity of a solution that contains 20.0grams of sodium hydroxide in 200. ml of solution. 50. How many grams of solute are present in 50.0 ml of 0.360 M sodium chloride? 51. What volume of 12.0 M HCl solution is needed to prepare 5.00 liters of 0.0250 M solution? 52. What volume of 0.100 M HCl solution is needed to neutralize 50.0 ml of 0.350 M KOH? 53. Describe in detail what happens when the following are dissolved in water: Polar solute (CH 3OH) vs. non polar solute (CH 3(CH 2) 4CH 3).

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AP CHEMISTRY EQUATIONS AND CONSTANTS Throughout the exam the following symbols have the definitions specified unless otherwise noted. L, ml = liter(s), milliliter(s) mm Hg = millimeters of mercury g = gram(s) J, kj = joule(s), kilojoule(s) nm = nanometer(s) V = volt(s) atm = atmosphere(s) mol = mole(s) ATOMIC STRUCTURE E = hν c = λν E = energy ν = frequency λ = wavelength Planck s constant, h = 6.626 10 34 Js Speed of light, c = 2.998 10 8 ms 1 Avogadro s number = 6.022 10 23 mol 1 Electron charge, e = 1.602 10 19 coulomb EQUILIBRIUM K c = c [C] [D] a [A] [B] d b ( P K p = C ) ( P D ) a ( P ) ( P ) K a = K b = A c b B [H ][A ] [HA], where a A + b B c C + d D d [OH ][HB ] [B] K w = [H + ][OH ] = 1.0 10 14 at 25 C = K a K b ph = log[h + ], poh = log[oh ] 14 = ph + poh ph = pk a + log [A ] [HA] Equilibrium Constants K c (molar concentrations) K p (gas pressures) K a (weak acid) K b (weak base) K w (water) pk a = logk a, pk b = logk b KINETICS ln[a] t ln[a] 0 = kt 1 1 = kt A A 0 t t ½ = 0.693 k k = rate constant t = time t ½ = half-life -3-

GASES, LIQUIDS, AND SOLUTIONS PV = nrt P A = P total X A, where X A = P total = P A + P B + P C +... n = m M K = C + 273 D = m V KE per molecule = 1 2 mv 2 moles A total moles Molarity, M = moles of solute per liter of solution A = abc THERMODYNAMICS / ELECTROCHEMISTRY q = mc T S = S products S reactants H = DH products DH reactants f G = DG products DG reactants G = H T S = RT ln K = n E I = q t f f f P = pressure V = volume T = temperature n = number of moles m = mass M = molar mass D = density KE = kinetic energy v = velocity A = absorbance a = molar absorptivity b = path length c = concentration Gas constant, R = 8.314 J mol 1 K 1 = 0.08206 L atm mol 1 K 1 = 62.36 L torr mol 1 K 1 1 atm = 760 mm Hg = 760 torr STP = 273.15 K and 1.0 atm Ideal gas at STP = 22.4 L mol 1 q = heat m = mass c = specific heat capacity T = temperature S = standard entropy H = standard enthalpy G = standard Gibbs free energy n = number of moles E = standard reduction potential I = current (amperes) q = charge (coulombs) t = time (seconds) Faraday s constant, = 96,485 coulombs per mole of electrons 1 joule 1 volt = 1 coulomb -4-