AP Chemistry - Ms. Ganz Welcome to AP Chemistry

Transcription

1 AP Chemistry - Ms. Ganz Welcome to AP Chemistry AP is a college level course. The course is designed to be equivalent to the inorganic chemistry course usually taken during the first year of college. This course provides an excellent foundation for further studies in chemistry, and may result in college credit for the course. The general structure of the AP Chemistry program is as follows: Meets 8 periods per 6-day cycle. Units last approximately 2 weeks. Reading of the textbook is REQUIRED before class. Homework, a multiple choice packet, is due before unit exam. Tests occur at the end of each unit, unless units are combined. Unit tests model the AP exam experience. Test will usually be given on a double period day. AP chemistry students are required to take a quarterly and midterm. A final project will replace the final exam. The AP exam is required. An assignment covering Chapter 1-3, , will be completed over the summer. Read these sections carefully. All of this material was introduced in Honors Chemistry. You are required to read the textbook and follow the problems before the class lecture. If the textbook is too difficult, I would recommend that you watch chemistry videos on the website to help you better understand the curriculum. You MUST reread the textbook before each exam. Websites: Khan academy Crash course Bozeman Science Textbook for the summer: Chemistry, Zumdahl, Seventh Edition New textbook to be handed out in the fall 10 th edition Grading will be based on: tests/take home assignments 80%, labs 10%, quizzes and other homework 10%. The assignments within each category will be weighted. Other General Chemistry Sites: Quizzes (multiple choice and free response) Study Cards:

2 The website only includes the summer homework. All other handouts and textbook must be picked up in the guidance office. Chapter 1-3 notes (not online) Chapter 1-3 review (not online) Review material for the summer homework Polyatomic Ions, Chemical Reactions, Periodic Table, Stoichiometry Flow Chart (not online) THE SUMMER HOMEWORK- It covers naming and writing chemical formulas, balancing equations, stoichiometry, gas laws and solutions. Your notebook from Honors chemistry; review book and your AP textbook are good resources for this review. Only the summer homework is due the first day of school. Not the problems in the chapter notes or the review. Your answers must have the same number of significant figures as the word problem. Write a balanced equation for each reaction (where possible), label all units, use dimensional analysis as often as you can. Learning dimensional analysis and using it is a necessity in succeeding in this class. Take your time and carefully read that section of the book. You should look through the Chapter 1-3 review packet and the summer homework before this school year ends in case you need help before the summer. If you have difficulty with the assignment, use your textbook, the online videos, notes, Khan academy, fellow classmate or previous AP student. You are more than welcome to during the summer, after you have read the book and asked a classmate, but do not wait till the last day to work on it. This summer packet will be collected on the first day of school and will be graded. Please take the assignment seriously. I look forward to seeing you next fall. Ms. Ganz ganzw@lakelandschools.org

3 NAME Write the Chemical Formula: 1. Barium sulfate 2. Ammonium chloride 3. Chlorine monoxide 4. Magnesium fluoride 5. Sodium oxide 6. Sodium peroxide 7. Copper ( I) iodide 8. Zinc sulfide 9. Potassium carbonate 10. Hydrobromic acid 11. Lead (II)acetate 12. Sodium permanganate 13. Lithium oxalate 14. Potassium cyanide 15. Iron (II) hydroxide 16. Silicon dioxide 17. Calcium chlorate 18. Cobalt (II) nitrate 19. Ammonium phosphate 20. Potassium chromate Name the following compounds (Give acid names when appropriate): 1. CuSO4 2. PCl3 3. Li3N 4. BaSO4 5. N2F4 6. KClO4 7. NaH 8. (NH4)2Cr2O7 9. HNO2 10. Mg(OH)2 11. Al2S3 12. AgBr 13. HC2H3O2 14. Li2O 15. FeI3 16. Cu3PO4 17. Zn(NO3)2 18. HF 19. NH3 20. N2O

4 Balance the following equations: Fill in the blanks with the coefficients 1. Cu + O2 CuO 2. Fe + O2 Fe3O4 3. Mg + HCl MgCl2 + H2 4. Al + HCl AlCl3 + H2 5. P + O2 P2O5 6. NaHCO3 Na2CO3 + CO2 + H2O 7. NaNO3 NaNO2 + O2 8. Cu(NO3)2 CuO + NO2 + O2 9. PbO + C Pb + CO2 10. C4H8 + O2 CO2 + H2O 11. Na2CO3 + HCl NaCl + H2O + CO2 12. KOH + H2SO4 K2SO4 + H2O 13. Mg + H2O MgO + H2 14. Na + H2O NaOH + H2 15. Fe(OH)3 + Fe2O3 + H2O

5 Predict the product and write a balanced equation State the phase of matter on the products What type of chemical reaction is it? SR, DR, S, D, C Write your answers on this sheet. Do work on separate paper. 1. Ammonium sulfate reacts with barium nitrate 2. Zinc metal is added to a solution of copper (II) chloride 3. Propane gas is burned in excess oxygen 4. Sulfuric acid is combined with solid magnesium hydroxide 5. Solid aluminum hydroxide is added to perchloric acid 6. Solutions of silver nitrate and sodium chromate are mixed 7. A solution of copper (II) chloride is added to a solution of sodium sulfide 8. A solution of manganese (II) sulfate and ammonium sulfide are mixed 9. Aluminum metal is added to a solution of copper (II) chloride 10. Sodium hydroxide is added to potassium nitrate

6 Stoichiometry SHOW ALL WORK!!! Be neat and label with units. Box the final answer. 1. Benzene contains only carbon and hydrogen and has a molar mass of 78.1g/mol. Analysis shows the compound to be 7.74% H by mass. Find the empirical and molecular formulas of benzene. 2. Calcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide gas. a. Write a balanced chemical equation for this reaction b. How many grams of calcium oxide will remain after 12.25g of calcium carbonate is completely decomposed? c. What volume of carbon dioxide gas is produced from this amount of calcium carbonate? The gas is measured at 0.95atm and 10 C. 3. Hydrogen gas and bromine gas react to form hydrogen bromide gas a. Write a balanced equation for this reaction. b. How many grams of hydrogen bromide gas can be produced from 3.2g of hydrogen gas and 9.5g of bromine gas? c. How many grams of which reactant are left unreacted? d. What volume of HBr, measured at STP, is produced in b.?

7 4. When ammonia gas, oxygen gas and methane gas 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 225g of oxygen gas is reacted with an excess of the other two reactants. c. If the actual yield of the experiment in b. is 105g of HCN, calculate the percent yield? 5. A 2.29g sample of an unknown acid is dissolved in 1.00 L of H2O. A titration required 25.0 ml of 0.500M NaOH to completely react with all the acid present. What is the molar mass of the acid? 6. Cinnamic acid contains only carbon, hydrogen, and oxygen, and is found by analysis to be 73.0% carbon, and 5.4% hydrogen. In titration, ml of M NaOH os found to neutralize g of cinnamic acid. a. Find the empirical formula b. Find the molar mass of the compound. c. Write the molecular formula for this compound.

8 7. What mass of aluminum hydroxide is produced when 50.0mL of 0.200M Al(NO3)3 reacts with 200.0mL of 0.100M KOH? 8. Potassium nitrate decomposes when heated forming potassium nitrite and oxygen gas. a. Write a balanced chemical equation for this reaction b. What mass of KNO3 would be needed to produce 18.4L of oxygen gas, measured at 775mmHg and 15 C? c. What mass of KNO2 would also be produced? 9. Heating a 6.862g sample of an ore containing a metal sulfide in excess oxygen produces 1053 ml of SO2 gas measured at 66 C and 739 mmhg. Calculate the percentage by mass of sulfur in the ore.

9 Classify each of the following as units of mass, volume, length, density, energy or pressure a. mg b. ml c. cm3 d. mm e. kg/m3 f. kj g. atm How many significant figures are in each of the following? a b c x d e f. 100 g h i Calculate the following to the correct number of significant figures. a / b / 1.01 c d e. 2.1 X 3.21 f X 120 g

10 You must be able to distinguish: An element from a compound An element from a mixture A compound from a mixture A true solution from a heterogeneous mixture A Bronsted-Lowry acid and base from Arrhenius acid and base Ionic compound from a covalent compound You must be able to define: Molarity, Solution, Electrolyte, Temperature. You must be able to identify the oxidation number of an element and solve for any unknown oxidation numbers.