Dear Students, +JMJ+ Advanced Placement Chemistry Summer Work May 16 th, 2016 Congratulations on enrolling in AP Chemistry for the 2016-2017 School Year! I am eagerly anticipating a great year for AP Chemistry. In order to ensure the best start for everyone next fall, I have prepared a summer assignment that reviews basic chemistry concepts. This summer assignment is derived from what the College Board expects for AP Chemistry students to have as prior knowledge, meaning it will not be taught in class. There is a multitude of tremendous chemistry resources are available via the internet and elsewhere. With access to hundreds of websites either in your home or at the local library, I am confident that you will have sufficient resources to prepare adequately for the fall semester. I also encourage you to work with your classmates as talking with one another about the material will help you recall and remember the material in preparation for class. If you kept your Chemistry textbook, it will be a helpful resource for you. Much of the material in the summer assignment should be familiar to you. The problems will help you review the foundational skills you acquired in chemistry and insure that all students are on a relatively even plane. Keep in mind that the AP Chemistry (along with many other AP science courses have or will) curriculum has changed to a more conceptual understanding of the course material. There are fewer algorithmic calculations and more emphasis is placed on an understanding of what the formulas and results mean rather than just calculating them. It will be important for everyone to come to class on the first day prepared. While I review, extensive tutoring is not an option as we work towards our goal of being 100% prepared for the AP Exam in early May 2017. There will be a test covering the basic concepts included in the summer assignment on the second day of school. This test will cover all the material you will review by successfully completing the summer assignment; it will be worth 100 points and counts toward your quarter 1 grade. It is also important that you realize up front how your performance in this course will be measured. Grades will mainly depend on quizlettes (almost daily), homework and test scores, multiple lab reports, and a few special topic assignments or projects. Be aggressive in pursuit of knowledge not just the grades. As you work on the summer assignment, you may contact me via email: martinezc@stcecilia.edu this summer. I will do my best to answer your questions ASAP. Finally, I recommend that you spread out the summer assignment. Please do not try to complete it all in the final week of the summer. Chemistry takes time to process and grasp at a level necessary for success in AP Chemistry. Working a few problems each day will prove to be an excellent practice in developing the study skills for any college science class. Remember, AP Chemistry is an equivalent course to Introductory Chemistry in college. Continue having a great summer and enjoy the chemistry! +Ad majorem Dei gloriam+ Mr. Martinez
Assignment #1 Using your school email address, email Mr. Martinez to confirm that you have received a copy of the summer assignment. Assignment #2 Obtain the AP Chemistry textbook NOW and begin reading and reviewing chapters 1-4, these subjects are expected prior knowledge and are covered in your summer work: Book info: Chemistry, 9 th Edition (2014) by Zumdahl and Zumdahl (ISBN 978-1-1-133-61110-3) Choose and purchase an AP Chemistry review book. Make sure you get a new version as the course and exam format changed in 2013. Assignment #3 Complete the vocabulary/problems beginning on page 3 of this assignment. SHOW ALL WORK (handwritten and/or typed responses are both acceptable). These are DUE the FIRST DAY OF CLASS. Late work will not be accepted. Assignment #4 To familiarize yourself with some of the periodic trends I would like you to know, please print out the AP approved periodic table and label and/or color code it to indicate the following periodic trends: 1. Number of valence electrons for the main groups elements in groups 1A-8A. 2. Group ion charge 3. Group number of bonds 4. Atomic radius 5. Electronegativity *note: it may be helpful to print out more than one periodic table and color/label one chart for each trend. Assignment #5 Start your AP Chemistry binder, complete with: o Paper o Tabs for sections on: Notes and Vocabulary, Quizlettes, Tests, Labs, Reports, and Special Topics. *note: I do not want to force you to study in a way that is not helpful for you, so if you d prefer to make flashcards for vocabulary or keep it in a separate section or include it in your notes for each chapter, that is ok with me! If you use Quizlet for online vocabulary, make sure to have a printout of your vocabulary lists for me as proof.
AP CHEMISTRY 2016-2017 SUMMER VOCABULARY and PROBLEMS 1) Write the most common guidelines to determine significant figures (digits) with an example for each rule. 2) Use conversion factors to convert the following: a. 200 meters = miles. b. 650 in = meters c. 4 years= seconds. d. 200 liters = ml 3) Classify each of the following as units of mass, volume, length, density, energy, or pressure. a.kg b. Liter c. m 3 d. mm e. kg/m 3 f. Joule g. atm h. cal. i. Torr J. g/ml 4) How many significant figures are in each of the following? a. 1.9200 mm b. 0.0301001 kj c. 6.022 x10 23 atoms d. 460.000 L e. 0.000036 cm 3 f. 10000 g. 1001 h. 0.001345 i. 0.0101 j. 3.02 x 10 4 k. 3.21 x 10-2 5) Re-write each of the following in correct scientific notation: a. 4050,000,000 cal b. 0.000123 mol c. 0.00345 Ǻ d. 700,000,000 atoms 6) Calculate the following to the correct number of significant figures. a. 1.270 g / 5.296 cm 3 b. 12.235 g / 1.010 L c. 12 g + 0.38 g d. 170g + 2.785 g e. 2.1 x 3.2102 f. 200.1 x 120 g. 17.6 + 2.838 + 2.3 + 200 7) Give the chemical symbols for the following elements: a. Carbon b. sulfur c. Titanium d. Nitrogen e. Helium f. Krypton g. Fluorine h. Scandium i. Arsenic j. Potassium k. Sodium l. chloride m. Iron n. Zinc 8) Write the latin names for each of the elements symbols: a. Na b. Au c. Ag d. Sn e. Fe f. Hg g. K h. Pb
9) Label each of the following as either a physical process or a chemical process. a. Corrosion of aluminum metal. b. Melting of ice. c. Pulverizing an aspirin. d. Digesting a candy bar. e. Explosion of nitroglycerin. f. Milk turning sour. g. Burning of paper. h. Forming of frost on a cold night. i. Bleaching of hair with hydrogen peroxide. j. A copper wire is hammered flat. 10) Why do we call Ba(NO 3 ) 2 barium nitrate, but we call Fe(NO 3 ) 2 iron (II) nitrate? Explain. 11) Write the formula for each of the following compounds: a. Calcium sulfate. b. Ammonium Phosphate c. Lithium Nitrite d. potassium perchlorate. e. Barium Oxide f. Zinc sulfide. g. Sodium Perbromate h. Calcium Iodide i. Aluminum Carbonate 12) What is the difference between: a. Chlorine and Chloride? b. Sodium atom and sodium ion. 13) How many grams of methane (CH 4 ) are present in 5.6 moles of methane gas? (use conversion factors) 14) 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 atoms of neon. 15) 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: 18.82 g 3. mass of crucible, cover, and contents after heating to constant mass: 20.94 g Calculate the experimental percent of water in the compound. 16) Mercury has an atomic mass of 200.59 amu. Calculate the a. Mass of 3.0 x 10 10 atoms. b. Number of atoms in one nanogram of Mercury.
17) Calculate the molar masses (g/mol) of a. Ammonia ( NH 3 ) b. Baking soda ( NaHCO 3) ) c. Osmium Metal (Os) 18) Convert the following to moles a. 3.86 grams of Carbon dioxide. b. 6.0 x 10 5 g of Hydrazine (N 2 H 4 ), a rocket propellant. 19) The molecular formula of morphine, a pain-killing narcotic, is C 17 H 19 NO 3. a. What is the molar mass? b. What fraction of atoms in morphine is accounted for by carbon? c. Which element contributes least to the molar mass? 20) Write the name or formula of the following compounds as appropriate: a. Cupric Hydroxide b. Strontium Chromate c. Ammonium Per chlorate d. NaHCO 3 e. Fe 2 (CO 3 ) 3 f. Sodium Hydroxide. g. Potassium Chloride. 21) The hormone, thyroxine is secreted by the thyroid gland, and has the formula: C 15 H 17 NO 4 I 4. How many milligrams of Iodine can be extracted from 15.0 Grams of thyroxine? 22) Determine the formula weight for the following: a. N 2 O 5 b. CuSO 4 C. Ca(HCO 3 ) 2 d. CaSO 4. 2 H2 O 23) Calculate the percentage by mass of the following compounds: a. SO 3 b. CH 3 COOCH 3 c. Ammonium Nitrate. 24) Determine the empirical formula of the compounds with the following compositions by mass: a. 10. 4% C, 27. 8% S, 61. 7 % Cl b. 21.7% C, 9.6 % O, and 68.7 % F 25) What is the molecular formula of each of the following compounds? a. empirical formula CH 2, molar mass =84g/mol b. empirical formula NH 2 Cl, Molar mass = 51.5g/mol 26) Write balanced chemical equations for the reactions of sodium with the following nonmetals to form ionic solids. a. Nitrogen b. Oxygen c. Sulfur d. Bromine
27) Write a balanced equation for the following: a. Reaction of boron trifluoride gas with water to give liquid hydrogen fluoride and solid boric acid,(h 3 BO 3 ). b. Reaction of magnesium Oxide with Iron to form Iron (III) Oxide and Magnesium. c. The decomposition of dinitrogen Oxide gas to its elements. d. The reaction of Calcium Carbide solid with water to form calcium hydroxide and acetylene (C 2 H 2 ) gas. e. The reaction of solid calcium cyan amide (CaCN 2 ) with water to from calcium carbonate and ammonia gas. f. Ethane burns in air (Oxygen). g. Hydrogen reacts with oxygen to form Water. h. Nitrogen gas reacts with Hydrogen to form Ammonia. i. Hydrogen reacts with Iodine gas to form Hydrogen Iodide. j. Sodium reacts with Iodine gas to form Sodium Iodide. k. Sodium Oxide reacts with water to form sodium hydroxide and hydrogen. 28) DEFINE limiting reagent, theoretical yield, and actual yield. 29) Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO 2 (g) Na 2 CO 3 (s) + H 2 O(l) Which reagent is the limiting reactant when 1.85 mol of sodium hydroxide and 1.00 mol carbon dioxide are allowed to react? How many moles of sodium carbonate can be produced? How many moles of the excess reactant remain after the completion of the reaction? 30) What is an Activity series of metal? How does it help us in studying properties of elements? 31) Identify each of the following as being most like an observation, a law, or a theory. a. All coastal areas experience two high tides and two low tides each day. b. Tides in Earth s oceans are caused mainly by the gravitational attraction of the moon. c. Yesterday, high tide in San Francisco Bay occurred at 2.43 a.m. and 3.07 P.m. d. Tides are higher at the full moon and new moon than at other times of the month. 32) What is a solute and solvent?
33) DEFINE and compare & contrast Molarity and Molality 34) Calculate the molarity of a solution that contains 0.0345 mol NH 4 Cl in exactly 400 ml of solution? 35) Calculate the molarity of a solution that contains 20.0 grams of sodium hydroxide in 200mL? 36) How many grams of solute are present in 50.0 ml of 0.360 M sodium chloride? 37) What is Avogadro s number and what does it represent? 38) Briefly, in a table, compare/contrast the Law of definite composition with the Law of multiple proportions. 39) What is an isotope? Explain how an atom can have an isotope. 40) Choose any element on the periodic table and draw a full-page sketch/picture of that atom in the form of an advertisement. Be sure to include the name of the element, the mass and atomic number, the amount of all the subatomic particles, and at least one version of the electron configuration (your choice of full-length electron configuration, orbital notation, or noble gas notation. Vocabulary Kinetic molecular theory Homogeneous Heterogeneous Solution Endothermic Exothermic Polarity Electronegativity Octet rule Lewis dot structures VSEPR theory Ionic bond Covalent bond Polar Non-polar Catalyst Entropy Enthalpy Precision Accuracy Mass Density Cation Anion Mole Meniscus Stoichiometry Polyatomic Ions (consider these vocabulary and memorize formulas AND charges) Name Formula Name Formula a) Acetate b) Ammonium c) Carbonate d) Chlorate e) Chlorite f) Chromate g) Cyanide h) Dichromate i) Dihydrogen Phosphate j) Dihydrogen Phosphate k) Hydrogen Carbonate l) Hydrogen Sulfate m) Hydrogen Sulfite n) Hypochlorite o) Hydroxide p) Nitrate q) Nitrite r) Oxalate s) Perchlorate t) Permanganate u) Perioxide v) Phosphate w) Sulfate x) Sulfite y) Thiosulfate