AP Chemistry Summer Packet

Transcription

1 AP Chemistry Summer Packet Get excited (and ready) for AP Chemistry! Name: Included in this packet is information about the exam and information you should KNOW (memorize or be able to derive from the wonderful periodic table) or know how to CALCULATE. FYI the PT on the AP exam has NO NAMES given, only symbols. If you need help SEE me. We will start class in August with the expectation that you are competent with ALL of this material. There will be several assessments that cover this material in the first two weeks of school. Don t freak out about this packet. You probably know more than you think. The answer key will be available in my classroom for you to check your work as you go. If you need more practice in a certain area, let me know. The first two pages are informational (should be kept in reference section of your notebook and the rest are things you should already know how to do! Your first test and the due date for this packet will be Friday, August 19, Need help? Drop by room F123 or me: chiltonc@fultonschools.org The 2017 AP Chemistry Exam will be Monday, May 1 st! Registration information for the exam will be given to you as soon as it is available. FYI: The AP Chemistry exam is the FIRST exam given, and it is given at the same time as AP Environmental Science. Yes, you can take both classes & both exams. You will just have to contact the AP coordinator at our school to take an alternate exam (different than the one given on May 1) on a different date set by College Board. Stuff to KNOW 1. SI base units and prefixes 2. Rules for significant figures 3. Element Names & Symbols (Element symbols 1 to 38 and Ag, Cd, I, Xe, Cs, Ba, W, Hg, Pb, Sn, Rn, Fr, U, Th, Pu, and Am written correctly careful with capital letters Co, not CO! 4. Monatomic Ions a. Ions with (usually) one oxidation state: Li +, Na +, K +, Mg 2+, Ca 2+, Sr 2+, Ba 2+, Ag +, Zn 2+, Cd 2+, Al 3+ N 3-, O 2-, S 2-, F -, Cl -, Br -, I - b. Ions with more than one oxidation state: Cu + Copper (I) ion Mn 2+ Manganese (II) ion Cu 2+ Copper (II) ion Mn 3+ Manganese (III) ion Hg2 2+ Mercury (I) ion Co 2+ Cobalt (II) ion Hg 2+ Mercury (II) ion Co 3+ Cobalt (III) ion Fe 2+ Iron (II) ion Sn 2+ Tin (II) ion Fe 3+ Iron (III) ion Sn 4+ Tin (IV) ion Cr 2+ Chromium (II) ion Pb 2+ Lead (II) ion Cr 3+ Chromium (III) ion Pb 4+ Lead (IV) ion 5. Strong Acids (for all practical purposes, all others are weak acids): HCl, HBr, HI, H2SO4, HNO3, HClO4 6. Strong Bases (for all practical purposes all others are weak): Group I hydroxides and Group II hydroxides (except Be(OH)2 and Mg(OH)2) 7. Colors of common ions in aqueous solution most common ions are colorless in solution, however, some have distinctive colors. These colors have appeared on past AP Chemistry exams: Fe 2+ and Fe 3+ - various colors Co 2+ - pink Cu blue to green MnO 4 - dark purple Mn faint pink CrO 4 - yellow Ni 2+ - green Cr 2O orange

2 8. Polyatomic Ions (most you learned in Honors Chemistry) C2H3O2 - acetate SO4 2- sulfate PO4 3- phosphate NO3 - nitrate SO3 2- sulfite AsO4 3- arsenate NO2 - nitrite CO3 2- carbonate AsO3 3- arsenite CN - cyanide C2O4 2- oxalate OCN - cyanate CrO4 2- chromate SCN - thiocyanate Cr2O7 2- dichromate MnO4 - permanganate S2O3 2- thiosulfate OH - hydroxide O2 2- peroxide HSO4 - bisulfate SeO4 2- selenate HCO3 - bicarbonate HPO4 2- hydrogen phosphate +1 O2 - superoxide NH4 + ammonium H2PO4 - dihydrogen phosphate ClO4 - perchlorate * ClO3 - chlorate * ClO2 - chlorite * ClO - hypochlorite * * Br, I and F may be substituted 9. Solubility Rules Soluble Ionic Compounds Exceptions Group IA and ammonium (NH4 + ) salts none nitrates (NO3 - ) and acetates (C2H3O2 - ) none 10. Patterns of Reactions a. Metallic carbonates when heated decompose into metallic oxides and CO2 (g) Ex: CaCO3(s) CaO(s) + CO2(g) b. Most metallic hydroxides, when heated, decompose into metallic oxides and water. Ex: Ca(OH)2(s) CaO(s) + H2O(g) c. Metallic chlorates, when heated, decompose into metallic chlorides and oxygen. Ex: 2KClO3(s) 2KCl(s) + 3O2(g) d. Metal + oxygen metal oxide Ex: 2Mg(s) + O2(g) 2MgO(s) e. Nonmetal + oxygen nonmetallic oxide Ex: C(s) + O2(g) CO2(g) f. Metal oxide + water metallic hydroxide Ex: MgO(s) + H2O(l) Mg(OH)2(s) g. Nonmetallic oxide + water acid Ex: CO2(g) + H2O(l) ; H2CO3(aq) h. Metal + nonmetal salt Ex: 2 Na(s) + Cl2(g) 2NaCl(s)

3 AP Chemistry Summer Assignment Name: Period: Stuff to know how to CALCULATE (show ALL work and use proper significant figures!!) 1. Use dimensional analysis method to convert the following: a. 3 meters into centimeters b. 15,050 milligrams into grams c. 3,264 milliliters into liters d. 9,674,444 grams into kilograms 2. Classify each of the following as units of mass, volume, length, density, energy, or pressure a. mg e. kg/m 3 b. ml f. kj c. cm 3 d. mm g. atm h. cal 3. How many significant figures are in each of the following? a mm b kj c x10 23 atoms d L 4. Record the following in correct scientific notation: a. 350,000,000 cal b mol e. 100 f g Calculate the following to the correct number of significant figures. a g / cm 3 b g / 1.01 L c. 2.1 x 3.21 c Ǻ d. 765,400,000,000 atoms d x 120 e Calculate the mass of a sample of copper that occupies 4.2x10 3 cm 3 if the density of copper is 8.94g/cm Fill in the following table: Element or ion Complete Name # protons # neutrons # electrons Fe-55 K + O 2- Pb Find the average atomic mass of an element if, out of 100 atoms, 5 have a mass of 176amu, 19 have a mass of 177amu, 27 have a mass of 178amu, 14 have a mass of 179amu and 35 have a mass of 180amu. 9. Strontium consists of four isotopes with masses and percent abundances as follows: amu (0.5%), amu (9.9%), amu (7.0%), and amu (82.6%). Calculate the atomic mass of strontium.

4 10. Write the complete & Noble gas (abbreviated) ground state electron configurations: a. strontium b. iron c. sulfur 11. Write formulas for the following substances: a. Barium sulfate b. Ammonium chloride c. Chlorine monoxide d. Silicone tetrachloride e. Magnesium fluoride f. Sodium oxide g. Sodium peroxide h. Copper (I) iodide i. Zinc sulfide j. Hydrobromic acid k. Lead (II) acetate l. Sodium permanganate m. Lithium oxalate n. Potassium cyanide o. Iron (III) hydroxide p. Silicon dioxide q. Nitrogen trifluoride r. Chromium (III) oxide s. Cobalt (III) nitrate t. Nitrous acid 12. Name each of the following compounds (Give acid names where appropriate) a. CuSO 4 b. PCl 3 c. N 2 F 4 d. KClO 4 e. (NH 4 ) 2 Cr 2 O 7 f. HNO 2 g. Sr 3 P 2 h. Mg(OH) 2 i. Al 2 S 3 j. AgBr k. P 4 O 10 l. HC 2 H 3 O 2 m. FeI 3 n. Cu 3 PO 4 o. Cs 3 N p. HF 13. Find the mass percent (percent composition) of nitrogen in each of the following compounds: a. NO b. NO 2 c. N 2O 4

5 14. Complete the Following Table: Name of Acid Formula of Acid Name of Anion hydrochloric chloride H 2SO 4 sulfate HC 2H 3O 2 or CH 3COOH 15. Predict the products of the following reactions, write balanced chemical equations, include states of matter and identify the reaction type. a. sodium carbonate (heated) b. decomposition of aluminum oxide c. magnesium burned in oxygen d. Ammonium sulfate reacts with barium nitrate. e. Zinc metal is added to a solution of copper (II) chloride. f. Propane gas (C 3 H 8 ) is burned in excess oxygen. g. Solid calcium chlorate is heated strongly. h. Solutions of lead (II) nitrate and calcium iodide are combined. i. Sulfuric acid is combined with sodium hydroxide. j. Iron metal shavings are added to hydrochloric acid. k. Sodium metal is added to distilled water. 16. What is an Activity series of metal? How is it useful in studying chemical reactions? 17. Benzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol. Analysis shows the compound to be 7.74 % hydrogen by mass. Find the empirical and molecular formulas of benzene.

6 18. Hydrogen gas and bromine gas react to form hydrogen bromide gas. a. Write a balanced equation for this reaction. b. 3.2 grams of hydrogen react with 9.5 grams of bromine. Which is the limiting reactant? c. How many grams of hydrogen bromide gas can be produced using the amounts in (b)? d. How many grams of excess reactant are left unreacted? e. What volume of HBr, measured at STP is produced in (b)? 19. When ammonia gas, oxygen gas and methane gas (CH4) are combined, the products are hydrogen cyanide gas and water. a. Write a balanced chemical equation for this reaction. b. Calculate the mass of each product produced when 225 grams of oxygen gas is reacted with an excess of the other two reactants. c. If the actual yield of the experiment in (b) is 105 grams of HCN, calculate the percent yield.

7 20. When solutions of potassium iodide and lead (II) nitrate are combined, the products are potassium nitrate and lead (II) iodide. d. Write a balanced equation for this reaction, including (aq) and (s). e. Calculate the mass of precipitate produced when 50.0mL of 0.45M potassium iodide solution and 75mL of 0.55M lead (II) nitrate solution are mixed. f. Calculate the volume of 0.50M potassium iodide required to react completely with 50.0mL of 0.50M lead (II) nitrate 21. Determine number of protons and neutrons in each of the following a. 19K b. 11Na c. 82Pb d. P White gold is an alloy that typically contains 45.0% by mass gold and the remainder is platinum. If 154 g of gold are available, how many grams of platinum are required to combine with the gold to form this alloy? 23. What is the empirical formula of a compound that contains 53.73% Fe and 46.27% of S? 24. Determine the number of molecules present in 4.56 mol of nitrogen (N2). 25. List the following as diatomic molecule, molecular compound, ionic compound, Atomic element. a. F2 b. Cl2 c. C d. NaCl e. KF f. CO2 g. H2 h. Ag i. Rust (Fe2O3) j. MgO k. O2 l. I2 m.co n. K2CO3 26. What is the difference between: a. Chlorine and Chloride? b. Sodium atom and sodium ion? 27. How many grams of methane (CH4) are present in 5.6 moles of methane gas?

8 28. Calculate the mass in grams of each of the following: a x atoms of Mg b x Formula units of CaCl2 c x atoms of neon 29. In an experiment, a student gently heated a hydrated copper compound to remove the water of hydration. The following data was recorded: 1. Mass of crucible, cover, and contents before heating 23.4 g. 2. mass of empty crucible and cover g. 3. mass of crucible, cover, and contents after heating to constant mass g. Calculate the experimental percent of water in the compound. 30. 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? 31. A sample of methane gas is at 50 0 C and 20 atm. Would you expect it to behave more or less ideally if: a) The pressure was reduced to 1 atm. b) The temperature were reduced to C? 32. A sample of carbon dioxide gas, CO2 (g), occupies a volume of 5.75 L at atm. If the temperature and the number of moles remain constant, calculate the volume when the pressure is increased to 1.25 atm. 33. A nitrogen sample at 30 C has a volume of 1.75L. If the pressure and the amount of gas remain unchanged, determine the volume when the Celsius temperature is doubled. 34. An open flask contains mol of air. Atmospheric pressure is 745 mmhg and room temperature is 68 F. How many moles are present in the flask when the pressure is 1.10 atm and the temperature is 33 C?

9 35. 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. 36. Calculate the densities of the following gases at 27 C and 763 mmhg: a) Carbon monoxide, b) Chlorine 37. Define strong electrolyte, weak electrolyte, precipitation reactions and solubility. 38. A volatile liquid (one that evaporates) is put into a jar and the jar is then sealed. Does the mass of the sealed jar and its contents change upon the vaporization of the liquid? 39. Define the terms exothermic and endothermic reactions. How much heat is required to raise the temperature of 100 grams of water from 25 0 C to 82 0 C? 40. A piece of unknown metal with mass 14.9 g is heated to C and dropped into 75.0 g of water at 20 0 C. The final temperature of the system is 28 degree Celsius. What is the specific heat of the metal? 41. What is a solute and solvent? Define Molarity, Molality, Mole-fraction and Mass percent of a solution. 42. Calculate the molarity of a solution that contains mol NH4Cl in exactly 400. ml of solution.

10 43. Calculate the molarity of a solution that contains 20.0 grams of sodium hydroxide in 200. ml. 44. How many grams of solute are present in 50.0 ml of M sodium chloride? 45. List 4 factors that affect the rate of reaction. How do each of these factors specifically affect the rate of reaction? 46. Write the equilibrium expression for the following equation: HNO3(aq) + NH3(g) NH4NO3(aq) 47. Write the equilibrium expression for the following equation: SiO2(s) + 4HF(g) SiF4(g) + 2H2O(g) 48. Define Acid, Base and Salt. Give three examples of each. Label each Acid and Base or strong or weak. Label each Salt as acidic, basic or neutral. 49. Fill in the following table: Substance Conjugate Acid Substance Conjugate Base NH3 H 3 O + Br CH 3 COOH 50. What volume of M HCl solution is needed to neutralize 50.0 ml of M KOH? What chemistry course(s) have you taken, including level (Honors, on-level, IB) When did you take the above listed chemistry course? What was your approximate grade in your chemistry class? What math are you enrolled in this year? Recommended AP Chemistry Review books: (get them early!!) 5 Steps to a 5, AP Chemistry, 2016 edition, by John Moore and Richard Langley, McGraw-Hill (Best resource for the school year) Cracking the AP Chemistry Exam, 2016 edition, by Paul Foglino, The Princeton Review (Best resource for AP Exam Prep) AP Chemistry Crash Course, 2 nd Edition, by Adrian Dingle, Research & Education Association