Please send me a quick to provide me with your address.

Transcription

1 AP Chemistry Rampart High School Welcome to AP Chemistry! I hope you have a fun and restful summer. I look forward to seeing you in August. Please send me a quick (sandra.vuletich@asd20.org) to provide me with your address. Tips for Success: 1. Read the chapters, once is great and twice is better. 2. When practice problems in class are given, do them. 3. Do the assignments on time. 4. Form study groups that meet regularly to discuss and practice your chemistry. 5. Don t fall behind! If you must miss a class make sure you make up the work ASAP! If you know you are going to be absent talk to the teacher and get the work before you leave. 6. Ask for help. Don t wait until the day before the exam if something does not make sense, get help. 7. Be engaged in class, bring your book, calculator or outlines to every class. 8. Be prepared for labs, you are required to complete a prelab and read over the procedures before you can participate in the lab. Time is limited so if you come unprepared you may not be able to participate in the lab or you may not finish the lab in the time allotted. What to Expect: 1. AP Chemistry is challenging and requires dedication. Students who work hard, ask for help, and follow the tips given above have the best opportunity to do well. 2. Read your syllabus when you receive it next fall. Don t expect exceptions to be made. This is a college level course offered in high school. I realize you are high school students and however I expect you to strive to work to college expectations. Communication is imperative between students and teachers. I want you to enjoy your social life, athletics, and other extracurricular activities, but they cannot become an excuse for not completing your work. Balance your time and set aside dedicated time each day to complete your coursework. 3. The College Board who oversees AP coursework determines the amount of content needed to be covered and other requirements for this to be considered an AP level course. They state it is to be expected to spend at least an additional 5 hours per week studying, reading and completing assignments for an AP level course as compared to a high school level course. 4. The pace of AP Chemistry is more accelerated than regular high school courses. There are occasions where we may cover a chapter in one week. 5. Labs are conducted at least every two three weeks. Lab content is on the AP Exam, pay attention to details as well as how the content applies to your lab. You will have at least 4 formal lab write ups during the year. 6. Your semester in progress grade is 65% Exams and quizzes, 25% labs, and 10% homework. This will make up 70% of your final course grade. a. Lab grades include a laboratory portfolio check at least once each semester. 7. Comprehensive finals are 30% of your grade and given at the end of each semester. The final is composed of two parts: written (75%) and lab practical (25%). a. All students take the final at the end of 2 nd semester including those who take the AP exam. 8. I want all of you to be successful in AP Chemistry and I will do my part to help you. If you find you are struggling, please be proactive and schedule time to work with me! 1

2 Summer Review Assignment The purpose of the review assignment is to remind you of and sharpen your current skills, so I recommend you wait until the end of July to complete the problems. The review assignment is due August 28th, approximately 1.5 weeks after the first day of school. Memorization Become very familiar with the periodic table. Know the names and locations of the first 36 elements. Memorize common ions and polyatomic ions (see attached list). Know the names and formulas of common compounds, common acids and bases (see attached list) SI system. Know your base units and prefixes (see attached) Reading Although you do not have your AP Chemistry books yet here is a link to a pdf version you can download to Apple or PC. This is the 12 th edition, however, we use the 11 th edition. This will get you through the summer until you can pick up your textbook this fall. If you want a textbook early you can check one out, but there is a $110 deposit required (ouch!). I highly recommend you read chapters 1 and 2. Not just for fun and joyful reading, but to review and learn the material presented in these chapters. There is a lot of material to cover in the school year so we start at chapter 3 in the fall. I also highly recommend finding a strategy to learn the vocabulary. There will be a lot of vocabulary next school year and knowing your vocabulary will help in understanding the content. On ALEC you will find some quizzes to check you understanding for chapters 1 and 2. ALEC will be available to you over the summer. I will post videos, comments, and quizzes for you to explore in preparation for this fall. Assignment Complete the 31 problems. Please do your work on a separate sheet of paper. Keep your work neat and organized, carry units and labels throughout problems and please check your spelling for accuracy. Reference the online textbook for help and to identify proper techniques for showing work in problems. 2

3 SI System Base Units and Prefixes Memorization Tasks 3

4 Names and Charges of Some Common Ions and Polyatomic Ions AP Chemistry ammonium, NH 4 + hydrogen or hydronium, H + or H 3O + lithium, Li + potassium, K + rubidium, Rb + silver, Ag + sodium, Na barium, Ba 2+ beryllium, Be 2+ calcium, Ca 2+ magnesium, Mg 2+ strontium, Sr 2+ zinc, Zn 2+ aluminum, Al acetate, C 2H 3O 2 bromate, BrO 3 bromide, Br chlorate, ClO 3 chlorite, ClO 2 chloride, Cl cyanide, CN fluoride, F hydrogen carbonate, HCO 3 (bicarbonate) dihydrogen phosphate, H 2PO 4 hydride, H hydrogen sulfide, HS (bisulfide) hydrogen sulfate, HSO 4 (bisulfate) hydrogen sulfite, HSO 3 (bisulfite) hydroxide, OH hypochlorite, ClO iodate, IO 3 iodide, I nitrate, NO 3 nitrite, NO 2 perchlorate, ClO 4 permanganate, MnO 4 carbonate, CO 3 2 chromate, CrO 4 2 dichromate, Cr 2O 7 2 hydrogen phosphate, HPO 4 2 oxide, O 2 peroxide, O 2 2 sulfate, SO 4 2 sulfide, S 2 sulfite, SO 3 2 nitride, N 3 phosphate, PO 4 3 phosphide, P 3 phosphite, PO 3 3 4

5 Polyatomic Elements, Acids, and Common Compounds Polyatomic Elements Br2 Bromine Cl2 Chlorine F2 Fluorine H2 Hydrogen I2 Iodine N2 Nitrogen O2 Oxygen Acids CH3COOH or HC2H3O2 Acetic (Vinegar) HBr Hydrobromic HCOOH Formic H2CO3 Carbonic HCl Hydrochloric HClO Hypochlorous HClO2 Chlorous HClO3 Chloric HClO4 Perchloric HF Hydrofluoric HI Hydroiodic HNO2 Nitrous HNO3 Nitric H2SO3 Sulfurous H2SO4 Sulfuric Common Compounds CH4 Methane CH3OH Methyl alcohol (Methanol) C2H5OH Ethyl Alcohol (Ethanol) CH3COCH3 Acetone H2O Water NH3 Ammonia NaCl Table salt NaHCO3 Baking soda 5

6 Descriptive Chemistry Colors (FYI good stuff with which to be familiar) Flame Test Colors Li + Deep red (crimson) Na + Yellow K + Violet Ca 2+ Orangered Sr 2+ Red Ba 2+ YellowGreen Cu 2+ Bluegreen Aqueous Ion Colors Cu 1+ Green Cu 2+ Blue Fe Yellow to redorange (depending on anion and charge of Fe); in rare cases, can form complex ion with a deep blue color Fe 2+ Yellowgreen (depending on the anion) Fe 3+ Orangered (depending on the anion) Co 2+ Pink Cr 3+ Violet (Cr(NO 3) 3 to Green (CrCl 3) Ni 2+ Green Mn 2+ Pink Pb 3+ Bluegreen (Pb 2+ and Pb 4+ are colorless) V 2+ Violet V 3+ Bluegreen MnO 4 Purple (Mn w/ +7 oxidation state is purple) 2 CrO 4 Yellow Cr 2O 2 7 Orange Cu(NH 3) 2+ 4 Dark Blue; produced when ammonia is added to Cu 2+ solutions FeSCN 2+ Redbrown, Winered to dark orange 2 CoCl 4 Blue (Co 2+ 2 with HCl will form a CoCl 4 complex that is blue) Ti(H 2O) 3+ 6 Purple Al, K, Li, Mg, Na, Ca, Ba, Sr, Zn are colorless aqueous ions and most of their solid salts are white. Transition element ions with partially filled d orbitals tend to release colored light. Assorted Compounds F 2 Paleyellow gas Cl 2 Greenyellow gas Br 2 Redbrown liquid I 2 Darkviolet vapor & dark metallic looking solid S 8 Yellow, odorous solid NO Colorless gas; associated with reactions between metals and dilute HNO 3 NO 2 Brown gas; associated with reactions between metals and concentrated HNO 3 PbI 2 Bright yellow precipitate Metallic sulfides Sulfides of transition metals tend to be black Fe 2O 3 Reddish brown (rust) Metallic oxides Oxides of colored transition metal ions tend to be colored AcidBase Indicators Phenolphthalein Red Litmus (paper) Blue Litmus (paper) Colorless (ph<7) to Pink (ph>8; when OH is present, i.e. turns bring fuschia pink in basic/alkaline solution) Turns purple/blue in alkaline solution Turns pink in acidic solution 6

7 Review Questions from Brown and LeMay: Chemistry the Central Science Chapter 1 Introduction: Matter and Measurement Assignments Classification and Properties of Matter: 1. Classify each of the following as a pure substance or a mixture; if a mixture, indicate whether it is homogeneous or heterogeneous: a) rice pudding b) seawater c) magnesium d) gasoline 2. A solid white substance A is heated strongly in the absence of air. It decomposes to form a new white substance B and a gas C. 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. 3. In the process of attempting to characterize a substance, a chemist makes the following observations: The substance is a silvery white, lustrous metal. It melts at 649 o C and boils at 1105 o C. Its density at 20 o C is g/cm 3. The substance burns in air, producing an intense white light. It reacts with chlorine to give a brittle white solid. The substance be pounded into thin sheets or drawn into wires. It is a good conductor of electricity. Which of these characteristics are physical properties, and which are chemical properties? Units of Measurement: 4. What decimal power do the following abbreviations represent? a) d b) c c) f d d) M e) k f) n g) m h) p 5. a) A sample of carbon tetrachloride, a liquid once used in dry cleaning, has a mass of g and a volume of 25.0 ml at 25 o C. What is its density at this temperature? Will carbon tetrachloride float on water? b) The density of platinum is g/cm 3 at 20 o C. Calculate the mass of cm 3 of platinum at this temperature. c) The density of magnesium is g/cm 3 at 20 o C. What is the volume of g of this metal at this temperature? Uncertainty in Measurement: 6. What is the number of significant figures in each of the following measured quantities: a) 358 kg b) s c) cm d) L e) x 10 3 m 3 7

8 7. Carry out the following operations, and express the answers with the appropriate numbers of significant figures: a) b) c) (6.21 x 10 3 )(0.1050) d) /75.3 Dimensional Analysis: 8. The Morgan silver dollar has a mass of g. By law, it was required to contain 90% silver, with the remainder being copper. a) When the coin was minted in the late 1800s, silver was worth $1.18 per troy ounce (31.1 g). At this price, what is the value of the silver in the silver dollar? b) Today, silver sells for $13.25 per troy ounce. How many Morgan silver dollars are required to obtain $25.00 worth of pure silver? Chapter 2 Atoms, Molecules and Ions Assignments The Atomic Theory and The Discovery of Atomic Structure: 9. A negatively charged particle is caused to move between two electrically charged plates, as illustrated below a) Why does the path of the charged particle bend? b) As the charge on the plates is increased, would you expect the bending to increase, decrease, or stay the same? c) As the mass of the particle is increased while the speed of the particles remains the same, would you expect the bending to increase, decrease, or stay the same? d) An unknown particle is sent through the apparatus. Its path is deflected in the opposite direction from the negativelycharged particle, and it is deflected by a smaller magnitude. What can you conclude about this unknown particle? The Modern View of Atomic Structure and Atomic Weights: 10. The radius of an atom of krypton (Kr) is about 1.9 Å (10 10 m). a) Express this distance in nanometers (nm) and in picometers (pm). b) How many krypton atoms would have to be lined up to span 1.0 mm? c) If the atom is assumed to be a sphere, what is the volume in cm 3 of a single Kr atom? 11. Determine whether each of the following statements is true or false; if false, correct the statement to make it true: a) The nucleus has most of the mass and comprises most of the volume of an atom; b) Every atom of a given element has the same number of protons; c) The number of electrons in an atom equals the number of neutrons in the atom; d) The protons in the nucleus of the helium atom are held together by a force called the strong nuclear force. 8

9 12. How many protons, neutrons, and electrons are in the following atoms: a. 40 Ar b. 65 Zn c. 70 Ga d. 80 Br e. 184 W f. 243 Am 13. Fill in the gaps in the following table assuming each column represents a neutral atom: Symbol 52 Cr Protons Neutrons Electrons Mass number a) What isotope is used as the standard in establishing the atomic mass scale? b) The atomic weight of boron is reported as 10.81, yet no atom of boron has the mass of amu. Explain. 15. Only two isotopes of copper occur naturally, 63 Cu (atomic mass = amu; abundance 69.17%) and 65 Cu (atomic mass = ; abundance 30.83%). Calculate the atomic weight (average atomic mass) of copper. The Periodic Table and Molecules and Molecular Compounds: 16. Locate each of the following elements in the periodic table; indicate whether it is a metal, metalloid, or nonmetal; and give the name of the element: a) Ti b) Ga c) Th d) Se e) Kr 17. The elements of group 4A show an interesting change in properties with increasing period. Give the name and chemical symbol of each element in the group, and label it as a nonmetal, metalloid, or metal. 18. Write the empirical formula corresponding to each of the following molecular formulas: b) C 8H 10 c) C 4H 8O 2 d) P 4O 10 f) B 3N 3H Each of the following elements is capable of forming an ion in chemical reactions. By referring to the periodic table, predict the charge of the most stable ion of each: a) Mg b) Al c) K d) Se e) F 9

10 Ions and Ionic Compounds: 20. Using the periodic table to guide you, predict the formula and name of the compound formed by the following elements: a) Ga and F b) Li and H c) Al and I d) K and S 21. Predict the empirical formula for the ionic compound formed by a) Ca 2+ and Br b) K + and CO 3 2 c) Al 3+ and C 2H 3O 2 d) NH 4 + and SO 4 2 e) Mg 2+ and PO Predict whether each of the following compounds is molecular or ionic: a) B 2H 6 b) CH 3OH c) LiNO 3 d) Sc 2O 3 e) CsBr Naming Inorganic Compounds: 23. Give the chemical formula for each of the following ionic compounds: a) aluminum hydroxide b) potassium sulfate c) copper(i) oxide d) zinc nitrate e) mercury(ii) bromide f) iron(iii) carbonate g) sodium hypobromite 24. Give the chemical formula for each of the following acids: b) hydrobromic acid c) phosphoric acid d) hypochlorous acid e) iodic acid f) sulfurous acid 25. Write the chemical formula for each substance mentioned in the following word descriptions. a) Zinc carbonate can be heated to form zinc oxide and carbon dioxide. b) On treatment with hydrofluoric acid, silicon dioxide forms silicon tetrafluoride and water. c) Sulfur dioxide reacts with water to form sulfurous acid. d) The substance phosphorus trihydride, commonly called phosphine, is a toxic gas. e) Perchloric acid reacts with cadmium to form cadmium (II) perchlorate. f) Vanadium (III) bromide is a colored solid. 10

11 Chemistry Review for MYP and/or Analytical Some Simple Patterns of Chemical Reactivity: 26. Write a balanced chemical equation for the reaction that occurs when f) solid magnesium reacts with chlorine gas; g) barium carbonate decomposes into barium oxide and carbon dioxide gas when heated; h) the hydrocarbon styrene, C 8H 8(l), is combusted in air; i) dimethylether, C 3OCH3 (g), is combusted in air. 27. Balance the following equations, and indicate whether they are combination (synthesis, decomposition, or combustion reactions: a) C 3H 6(g) + O 2(g) CO 2(g) + H 2O (g) b) NH 4NO 3(s) N 2O (g) + H 2O (g) c) C 5H 6O (l) + O 2(g) CO 2(g) + H 2O (g) d) N 2(g) + H 2(g) NH 3(g) e) K 2O (s) + H 2O (l) KOH (aq) Formula Weights: 28. Calculate the percentage by mass of the indicated element in the following compounds: a) carbon in acetylene, C 2H 2, a gas used in welding b) hydrogen in ascorbic acid, HC 6H 7O 6, also known as vitamin C c) hydrogen in ammonium sulfate, (NH 4) 2SO 4, a substance used as a nitrogen fertilizer The Mole: 29. Without doing any detailed calculations (but using a periodic table to give atomic weights), rank the following samples in order of increasing number of atoms: 0.50 mol H 2O; 23 g Na; 6.0 x N 2 molecules. 30. a) What is the mass, in grams, of 2.50 x 10 3 mol of ammonium phosphate? b) How many moles of chloride ions are in g of aluminum chloride? c) What is the mass, in grams, of 7.70 x molecules of caffeine, C 8H 10N 4O 2? d) What is the molar mass of cholesterol if mol weighs g? 31. The molecular formula of allicin, the compound responsible for the characteristic smell of garlic, is C 6H 10OS 2. a) What is the molar mass of allicin? b) How many moles of allicin are present in 5.00 mg of this substance? c) How many molecules of allicin are in 5.00 mg of this substance? d) How many S atoms are present in 5.00 mg of allicin? 11