AP Chemistry

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1 Welcome to AP Chemistry! I am so glad that you have decided to take this journey with me. I hope that you are looking forward to an exciting and challenging year. Hard work does pay off, and I hope you will find AP Chemistry to be a very rewarding experience. The AP Chemistry course is designed to be the equivalent of a full year college level chemistry course. Students may earn up to 8 hours of college credit for successful completion of the course and a strong score on the AP Chemistry exam. It is a challenging course that moves at a brisk pace. Classroom attendance is a must along with out of class time spent on practice, preparation, and review. I will do my very best to provide you with a college level course experience which not only prepares you for the AP Chemistry exam but provides a fundamental foundation in chemistry. I also intend for it to be fun! The 2019 AP Chemistry Exam will be Thursday, May 9. To be successful on the AP exam, students will need to spend on average five to ten additional hours per week outside of class working on AP Chemistry. This statement is not meant to discourage, but to state the truth to avoid any misconceptions about the high expectations for the course. The AP Chemistry Summer Assignment reviews many of the basic chemistry concepts covered during your first-year chemistry course and will help ensure that you are on track to a smooth start in the fall. This is a required assignment and your first few assessments will be based on the content contained in this review. You may find it useful to read sections of your text before you complete the problems on the review. The summer assignment is divided into three sections. Section A: Basic information that that should be memorized before the first day of school. Section B: Reference Material o You might find it useful to review these sections of your text as you complete the problems in part C of the summer assignment. o Also included are questions that remind you about some of the concepts that were developed during Honors Chemistry. These do no need to be answered formally but make sure that you can discuss them as we review the summer assignment the first week of school. Section C: Practice Problems o This should be printed and completed ready to turn in on the first day of school. o o Questions #1-11 should completed directly on the worksheet. Questions #12-50 should be completed on a separate sheet of paper. You should clearly show your work and box your final answers for computational questions. I look forward to working with you next year. During the summer, do not hesitate to reach out with questions or comments. My address is blineberger@cannonschoool.org and I check my frequently during the summer. If you have questions about a specific problem, help me to understand what you are thinking so that I can provide a few hints to guide your work. If you find that you are having a great deal of difficulty with the summer assignment, let s have a conversation about how much more challenging you will find the entire AP Chemistry course. Have a fun and safe summer and arrive in the fall ready to learn! 1

2 Summer Assignment Section A The following information should be memorized before the first day of school. 1) SI base units and prefixes 2) Rules for correct use of significant figures 3) Element names and symbols Elements # 1-38 Additional: Ag, Cd, Sn, I, Xe, Cs, Ba, W, Au, Hg, Pb, Bi, Rn, Fr, Ra, U 4) Name and symbol/formula with charge for Common Ions* that are listed on the following page. Tips for learning the ions and their charges can be found at: 5) Strong Acids: HCl, HBr, HI, H2SO4, HNO3, HClO3; HClO4 6) Strong Bases: Group I and Group II hydroxides except Be(OH)2 and Mg(OH)2. 7) Solubility Rules: See the table below. Given a name or formula, you are expected to be able to identify a salt as soluble or insoluble in water. Solubility Rules* Soluble Ionic Compounds Exception in salts with: Group 1 and Ammonium (NH4 + ) NONE Nitrates (NO3 ) and acetates (C2H3O2 ) NONE Chlorides (Cl ), bromides (Br ), and iodides (I ) Ag +, Hg2 2+, and Pb 2+ Sulfates (SO4 2 ) Ca 2+, Ba 2+, Sr 2+, and Pb 2+ Insoluble Ionic Compounds Exception in salts with: Sulfides (S 2 ) NH4 +, Group 1 ions, Ca 2+, Ba 2+, and Sr 2+ Carbonates (CO3 2 ) NH4 + and Group 1 ions Phosphates (PO4 3 ) NH4 + and Group1 ions Hydroxides (OH ) NH4 +, Group 1 ions, Ca 2+, Ba 2+, and Sr 2+ *By the end of the first week of school, you will be tested on the ions and the solubility rules. For example, given the name of an ionic compound, you should be able to write the correct formula and indicate whether it is soluble or insoluble in water. 2

3 Common Ions and Their Charges A mastery of the common ions, their formulas and their charges is essential to success in AP Chemistry. You are expected to know all of these ions on the first day of class. You will always be allowed to use a periodic table, which makes identifying the ions on the left side of the chart automatic. From the Periodic Table: Ions to Memorize: Cations Name Cations Name H + hydrogen Ag + silver Li + lithium Zn 2+ zinc Na + sodium Hg2 2+ mercury(i) K + potassium NH4 + ammonium Rb + rubidium Cs + cesium Be 2+ beryllium Anions Name Mg 2+ magnesium NO2 nitrite Ca 2+ calcium NO3 nitrate Ba 2+ barium SO3 2 sulfite Sr 2+ strontium SO4 2 sulfate Al 3+ aluminum HSO4 hydrogen sulfate (bisulfate) OH hydroxide Anions Name CN cyanide H hydride PO4 3 phosphate F fluoride HPO4 2 hydrogen phosphate Cl chloride H2PO4 dihydrogen phosphate I iodide CO3 2 carbonate O 2 oxide HCO3 hydrogen carbonate (bicarbonate) S 2 sulfide ClO hypochlorite Se 2 selenide ClO2 chlorite N 3 nitride ClO3 chlorate P 3 phosphide ClO4 perchlorate As 3 arsenide BrO hypobromite BrO2 bromite Type II Cations Name BrO3 bromate Fe 3+ iron(iii) BrO4 perbromate Fe 2+ iron(ii) IO hypoiodite Cu 2+ copper(ii) IO2 iodite Cu + copper(i) IO3 iodate Co 3+ cobalt(iii) IO4 periodate Co 2+ cobalt(ii) C2H3O2 acetate Sn 4+ tin(iv) Cr2O7 2 dichromate Sn 2+ tin(ii) CrO4 2 chromate Pb 4+ lead(ii) O2 2 peroxide Pb 2+ lead(ii) C2O4 2 oxalate Hg 2+ mercury(ii) NH2 amide BO3 3 borate S2O3 2 Thiosulfate MnO4 permanganate 3

4 Text: AP Chemistry Summer Assignment Section B (Reference Material) Chemistry (AP Edition) 10th Edition (2017) by Steven S. Zumdahl; Susan A. Zumdahl; Donald J. DeCoste SI Units, Dimensional Analysis & significant Figure Review Chapter 1 Chemical Foundations Additional Review Questions: Section 1.4: Uncertainty in Measurement o Can you describe accuracy, precision, random error, and systematic error? Section 1.10: Classification of matter o Can you use words and diagrams to distinguish between the 3 common states of matter, homogeneous or heterogeneous mixtures and pure substances? o o Can you describe physical changes such as distillation, filtration, or chromatography Can you use words and diagrams to differentiate compounds from elements and describe chemical changes? Atomic Structure & Electron Arrangement Review Chapter 2 Atoms, Molecules, and Ions (Section ) Chapter 3 Atomic Masses (Section 3.2) Chapter 7 Atomic Structure and Periodicity (only section 7.11) Additional Review Questions: Sections o Can you describe the modern atomic model and relate experimental evidence to changes in the model? Section 2.7: An Introduction to the Periodic Table o Can you identify special areas of the periodic table? Nomenclature Review Chapter 2 Atoms, Molecules, and Ions (Section 2.8) Composition Stoichiometry Chapter 3 Stoichiometry (Sections ) Additional Review Questions: Can you describe what is meant by percent composition? Can you distinguish between an empirical formula and molecular formula for a compound and describe how to determine each? Chemical Reactions Chapter 3 Stoichiometry (Sections ) We will learn a different way to classify types of reactions this year, so you will not need to review the Patterns of Chemical Change handout from Honors Chemistry. You should be able to identify states of reactants and products when writing balanced equations. Reaction Stoichiometry Chapter 3 Stoichiometry (Sections ) Additional Review Question: Can you use diagrams to identify the limiting reactant for a given reaction mixture? Properties and Reactions of Gases Chapter 5 Gases (Sections ) Additional Review Questions: Can you describe the relationships between pressure, volume, temperature, and moles of gases using words, diagrams, graphs, and equations? 4

5 Summer Assignment Section C Practice Problems SI Units, Dimensional Analysis & Significant Figure Review 1) Complete the table by indicating the number of significant figures in each value given below. Value # of sf Value # of sf m 40 ml g 800. cm 1.04 x 10 5 J 3.0 x 10 4 L 1 dozen donuts 2) Complete each calculation and give your answer with correct significant figures and units. (a) 1.27 g cm 3 = (b) 1.01 g ml = 3 cm (c) 12.2 g g = (d) ml ml = 2 (e) ( 2.1 m )( m ) = 3) Classify each of the following units as a measure of mass, volume, length, density, energy, or pressure. (a) kg (e) Joule (b) kj (f) Liter (c) mm (g) atm (d) cm Hg (h) g/ml 4) If you drive 154 miles in 3.0 hours, what is your speed in meters per second? (Given 1 in = exactly 2.54 cm.) 5) A cylindrical rod of silicon is 16.8 cm long and has a mass of 2.17 kg. The density of silicon is 2.33 g/cm 3. What is the diameter of the cylinder? (Given: The volume of a cylinder can be found from 2 V = r h where r is the radius and h is the length.) 5

6 Atomic Structure & Electron Arrangement Review 6) Complete the table below: Symbol Name # of Protons # of Electrons # of Neutrons Fe K O Pb-208 7) What is the average atomic mass of an element if out of 100 atoms, 5 have a mass of 176 amu, 19 have a mass of 177 amu, 27 have a mass of 178 amu, 14 have a mass of 179, and the remainder have a mass of 180 amu? 8) Element X exists in nature as four isotopes: 0.5% is X-84 ( amu, 9.9% X-86 ( amu), 7.0% X-87 ( amu) and 82.6% X-88 ( amu). Without any calculations, identify this element and explain how you know. 9) Write the abbreviated electron configuration for the ground state of each of the following: (a) Strontium atom (b) Silicon atom (c) Selenide ion (d) Mercury(II) ion (e) Argon atom 6

7 Nomenclature Review 10) Name the following compounds (a) CuSO 4 (b) PCl 3 (c) Li 3N (d) BaSO 3 (e) N 3F 4 (f) KClO 4 (g) NaH (h) (NH 4) 2Cr 2O 7 (i) HNO 2 (j) Sr 3P 2 (k) Mg(OH) 2 (l) Al 2S 3 (m) AgBr (n) NaC 2H 3O 2 (o) CaI 2 (p) MnO 2 (q) K 2O (r) Cu 3PO 4 (s) NaCN (t) CsCl (u) Zn(NO 3) 2 (v) N 2O (w) HBr (x) H 2O 2 (y) CaC 2O 4 (z) Na 2S 2O 3 7

8 11) Write the formula for the following compounds (a) Barium sulfate (b) Ammonium chloride (c) Chlorine monoxide (d) Silicon tetrachloride (e) Magnesium fluoride (f) Sodium oxide (g) Sodium peroxide (h) Copper(I) iodide (i) Zinc sulfite (j) Potassium carbonate (k) Hydrofluoric acid (l) Hypochlorous acid (m) Lead(II) acetate (n) Lithium oxalate (o) Potassium cyanide (p) Iron(III) hydroxide (q) Silicon dioxide (r) Nitrogen trifluoride (s) Chromium(III) oxide (t) Calcium chlorate (u) Nitrous acid (v) Potassium chromate (w) Cobalt(III) nitrate (x) Ammonium sulfide (y) Sulfuric acid (z) Sodium permanganate 8

9 AP Chemistry ***All of the work for problems #12-50 should be completed on a separate sheet of paper. Clearly show your problem solving and box your final answer for computational problems.*** Composition Stoichiometry 12) White gold is an alloy that typically contains 45% 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? 13) What mass of methane (CH 4) is equivalent to 5.6 moles of methane? 14) Determine the number of molecules present in 4.56 g of nitrogen gas. 15) Determine the mass of calcium chloride that contains 4.2 x chloride ions. 16) In an experiment, a student gently heated a hydrated copper compound to remove the water of hydration. Use the data that was collected from the table below to determine the percent water in the compound. Mass of empty crucible and lid Mass of crucible, lid, & contents before heating Mass of crucible, lid, and contents after heating g g g 17) Thyroxine, a hormone that is secreted by the thyroid gland, has the formula C 15H 17NO 4I 4. How many milligrams of iodine can be extracted from 15.0 g of thyroxine? 18) How many phosphate ions are contained in a sample of hydroxyapatite, Ca 5(PO 4) 3OH, that contains 5.50 x 10-3 grams of oxygen? 19) Determine the percent by mass of each element present in a sample of ammonium nitrate. 20) What is the empirical formula of a compound that is 53.73% iron and 46.27% sulfur? What is the name of this compound? 21) Arsenic reacts with chlorine to from a chloride. If g of arsenic reacts with excess chlorine to form g of the compound, what is the empirical formula of the compound? 22) Ibuprofen, a headache remedy, contains 75.6% carbon, 8.80% hydrogen, and 15.5% oxygen. If the molar mass of this compound is about 206 g/mole, what is the molecular formula of this compound? 23) A compound containing titanium and chlorine is analyzed by converting all of the titanium into 1.20 g TiO 2 and all of the chlorine into 6.45 g of AgCl. What is the empirical formula for the original compound? 24) A sample of moles of a metal M reacts completely with excess fluorine to form 46.8 g of MF 2. (a) How many moles of F are in the sample of MF 2 that forms? (b) How many grams of M are in this sample of MF 2? (c) What element is represented by the symbol M? Chemical Reactions 25) A solid white substance A is strongly heated in the absence of air. It decomposes to form a new white substance B and a gas. The gas has exactly the same properties as the product obtained when carbon is burned in an excess of oxygen. Based on these observations, can we determine whether solids A and B and the gas C are elements, or compounds? Explain your conclusions for each substance. 26) Draw particle diagrams to illustrate two reactions that produce iron(iii) oxide. In one reaction oxygen gas reacts with iron metal. The other reaction occurs when iron(ii) oxide reacts with oxygen gas. 9

10 AP Chemistry For questions #26-30, convert the descriptions into balanced equations including states. 27) When gallium metal is heated in oxygen gas, it melts and forms solid gallium(iii) oxide. 28) Liquid hexane (C 6H 14) burns in excess oxygen to form carbon dioxide and water vapor. 29) When solutions of calcium chloride and sodium phosphate are mixed, calcium phosphate precipitates and sodium chloride remains in solution. 30) Liquid disilicon hexachloride reacts with water to form solid silicon dioxide, hydrogen chloride gas, and hydrogen gas. 31) When nitrogen dioxide is bubbled into water, a solution of nitric acid forms and gaseous nitrogen monoxide is released. 32) Loss of atmospheric ozone has led to an ozone hole over Antarctica. The loss occurs in part through three consecutive steps: Step 1: Chlorine atoms react with ozone (O 3) to form chlorine monoxide and molecular oxygen. Step 2: Chlorine monoxide forms ClOOCl. Step 3: ClOOCl absorbs sunlight and breaks into chlorine atoms and molecular oxygen. Write a balanced chemical equation for each step and then write an overall balanced equation for the sequence. 33) Solid iodine trichloride is prepared in two steps: first, a reaction between solid iodine and gaseous chlorine to form solid iodine monochloride; then, treatment with more chlorine. Write a balanced equation for each step and then write a balanced equation for the overall reaction. Reaction Stoichiometry 34) The scene below represents a mixture of A 2 and B 2 before they react to form AB 3. What is the limiting reactant? How many molecules of product can form? 35) Calcium oxide and carbon dioxide are produced when calcium carbonate decomposes. What mass of calcium oxide could be produced when grams of calcium carbonate is heated? 36) Sodium hydroxide reacts with carbon dioxide to form sodium carbonate and water. (a) What is the limiting reactant when 1.85 moles of sodium hydroxide reacts with 1.00 moles of carbon dioxide? (b) How many moles of sodium carbonate could be produced? (c) How many moles of excess reactant remain after completion of the reaction? 37) When benzene (C 6H 6) reacts with bromine gas, bromobenzene (C 6H 5Br) along with hydrogen bromide gas is formed. A chemist reacted 30.0 g of benzene was reacted with 65.0 g of bromine in the lab. After the reaction was complete, she collected 56.7 g of bromobenzene. What was the percent yield for this reaction? 38) Elemental phosphorus occurs as tetratomic molecules, P 4. What mass of chlorine gas is needed to react completely with 455 g of phosphorus to form phosphorus pentachloride? 39) When 20.5 g of methane (CH 4) and 45.0 g of chlorine gas undergo a reaction that has a 75.0% yield, what mass of chloromethane (CH 3Cl) forms? Hydrogen chloride gas is also a product of this reaction. 10

11 AP Chemistry ) A massed sample of iron is added to liquid bromine and allowed to react completely. The reaction produces a single product, which can be isolated and massed. The experiment was repeated a number of times with the same mass of bromine (see graph below). (a) Explain the shape of the graph. (b) What mass of bromine is used when the reaction consumes 2.0 g of iron? (c) What is the mole ratio of bromine to iron of the product? (d) What is the empirical formula of the product? (e) Write a balanced equation for the reaction of iron and bromine. Properties and Reactions of Gases (f) What is the name of the reaction product? 41) A balloon filled with carbon dioxide has a volume of 5.75 L at atm. If the temperature remains unchanged and the balloon is kept closed, what is the new volume will the balloon have when the pressure is changed to 955 mmhg? 42) A sample of Freon gas occupies 9.10 L at 198 C. Assuming that the pressure remains the same, what Celsius temperature is needed to reduce the volume to 2.50 L? 43) A gas-filled weather balloon with a volume of 65.0 L is released at sea level conditions of 745 torr and 25 C. The balloon can expand to maximum volume of 835 L. When the balloon reaches an altitude at which the temperature is -5.0 C, and the pressure is atm, will the balloon reach maximum volume? 44) A bedroom that measures 11 ft by 12 ft by 8.0 ft contains kg of air at 25 C. What is the pressure of the air in the room? Since air is essentially 78% nitrogen and 22% oxygen, you may assume that the molar mass of air is 29.0 g/mole. (Given: 1 in 2.54 cm) 45) A drum used to transport crude oil has a volume of 162 L. How many water molecules, as steam, are required to fill the drum at 1.00 atm and C? What volume of liquid water (density = 1.00 g/ml) is required to produce that amount of steam? 46) A 2.00 g sample of gaseous SX 6 has a volume of cm 3 at 1.00 atm and 20.0 C. Identify the element X and name the compound, SX 6. 47) An open flask contains moles of air. The atmospheric pressure is 745 mmhg and the room temperature is 25 C. How many moles of air are present in the flask when the pressure is 1.10 atm and the temperature is 33 C? 48) Hydrogen cyanide is a poisonous gas. It can be produced by the reaction described by the equation given below. NaCN (s) + H + (aq) HCN (g) + Na + (aq) What mass of sodium cyanide is required to make 8.8 L of hydrogen cyanide at 22 C and 751 mm Hg? 49) In one of his most critical studies into the nature of combustion, Lavoisier heated mercury (II) oxide and isolated elemental mercury and oxygen gas. If 40.0 g of mercury (II) oxide is heated in a 502 L vessel and 20.0% (by mass) decomposes, what is the pressure (in atm) of the oxygen that forms at 25.0 C? Assume that the gas occupies the entire volume of the vessel. 50) One way to remove nitrogen monoxide from smokestack emissions is to react it with ammonia as described by the equation given below. What volume of nitrogen gas could be collected at STP when 1.03 kilograms of NO reacts? 4 NH 3 (g) + 6 NO (g) 5 N 2 (g) + 6 H 2O (l) 11