If you need help with any part of the summer assignment you can contact me via for support on the following dates and times:

Transcription

1 AP Chemistry Summer Assignment 2015 Mrs. Higgins Welcome to AP Chemistry! You already have a background in chemistry from your general chemistry class, but AP Chemistry is very different. Rather than memorizing how to do particular types of problems, you must really understand the chemistry and be able to apply it to different kinds of problems. AP Chemistry is a difficult course. To succeed you must keep up with the assignments and be willing to spend time working through the material. The College Board recommends that students spend one hour outside of class studying and practicing for every hour in class. I think this is an underestimation of what is necessary to be successful. Like most AP classes, AP Chemistry comes with a summer assignment. It is due the first Friday of school and will count as your first quiz grade. We will have a test over the concepts in this summer assignment on approximately the 7 th day of school. The summer assignment is a review of your first year chemistry course. If you do not know how to complete problems in this assignment, use your notes from your first year class or find an online tutorial or website to help you. I have listed some helpful websites on our class website: If you need help with any part of the summer assignment you can contact me via for support on the following dates and times: June 24 from 8am to 11am July 13 from 8am to 11am July 20 from 8am to 11am If I am out of town for some reason during one of the above dates I will post an out of office message with a new date and time. I check my frequently, so feel free to contact me ANYTIME if you are having problems doing the summer assignment. I will be happy to help you! In addition, I will you periodically during the summer to check on your progress and to see if you have any questions or concerns. I hope you will enjoy your AP Chemistry class. Be ready for an academic challenge. I know you will learn a lot in AP Chemistry and it will be an excellent way for you to prepare for college, as it will enhance work-habits, organizational skills and your ability to learn independently and think creatively. Have a great summer. See you in August! Mrs. Higgins

2 You may write your answers on these pages or use notebook paper. Unit One Math and Measurement 1. Write the following measurements in scientific notation. A. 369 g B. 540,000 ml (3 sig figs) C mi D Express the following as whole numbers or decimals. A x 10-3 B. 1.5 x 10 8 C x How many significant figures are there in each of the following values? A B C D E F G Perform the indicated calculations on the following measured values. Give the answer with the correct number of significant figures and units. A m m = B N x 4.4 m 2 = C s 7.52 s = D. 91 g 1.86 cm 3 = 5. Using conversion factors, convert 4.1 liters to: A. kiloliters B. milliliters C. microliters D. cubic centimeters 6. A velocity is 9.21 x 10 4 cm per minute. Use unit analysis (dimensional analysis) to calculate the velocity in meters per second. 7. A team of students determined the density of a sample of wood to be 0.62 grams per centimeter 3. A handbook of tree physiology reported the density to be for the same type of wood. What is the percent error of the student s value?

3 8. A leaky faucet drips at a rate of 1 drop/s. If one drop of water is 0.1 ml, how many gallons of water will be wasted in one day? 9. An aluminum bar is 5.0 cm x 4.0 cm x 10.4 mm and has a mass of g. Find the density of the bar in lb/ft What is the diameter, in Angstroms, of an atom of element X, if 6.89 x 10 7 atoms laid side by side is inches in length? 11. A. Compare and contrast the Kelvin scale and the Celsius scale. B. Convert 450. Kelvin to Celsius C. Convert 200. Celsius to Kelvin D. Convert -230 Celsius to Kelvin In addition to the above items be sure you know The difference between accuracy and precision How to determine the uncertainty of a measurement Metric prefixes (mega, kilo, hecto, deka, deci, centi, milli, micro, nano, pico) Unit Two Basic Atomic Structure, Naming Compounds and Writing Formulas 12. How many protons, neutrons and electrons are in each of the following ions? A. Fe 3+ (mass # 56) p n e B. Ca 2+ (mass # 40) p n e C. F - (mass # 19) p n e D. P 3- (mass# 31) p n e E. I - (mass # 127) p n e

4 13. Name the family or group of the Periodic Table to which each of the following elements belong: A. Ar B. Sr C. Fe D. Cl E. Nd F. Rb 14. Name each of the following compounds: A. PbI2 B. NH4Cl C. Fe2O3 D. LiH E. CsCl F. NaH G. Cr(OH)3 H. NaC2H3O2 I. K2Cr2O7 J. Na2SO4 K. KH2PO4 15. Name each of the following compounds: A. NI3 B. PCl5 C. CO D. P4O10 E. N2O4 F. NH3 16. Write formulas for each of the following compounds: A. iron (III) oxide B. hydrogen iodide C. tin (II) fluoride) D. calcium phosphate E. lead (II) nitrate F. sodium cyanide G. sodium hydrogen sulfate H. sodium bromate

5 17. Write formulas for each of the following compounds: A. rubidium nitrate B. sodium iodate C. dinitrogen tetroxide D. tin (IV) oxide E. potassium carbonate F. iron (III) chloride G. sulfurous acid H. magnesium hydroxide I. carbon tetrachloride J. potassium hydrogen phosphate K. potassium permanganate L. potassium chlorate M. hypoiodous acid N. ammonium acetate O. hydroiodic acid 18. Give the names of the following acids: A. H2SO3 B. HI C. HBr D. HNO2 E. H3PO4 F. HCl 19. Give formulas for the following acids: A. hydrocyanic acid B. hydrofluoric acid C. acetic acid D. sulfuric acid E. nitric acid F. hydrosulfuric acid 20. Give the names of the seven diatomic elements. 21. Define the word isotope. 22. What does the law of definite composition say?

6 23. What does the law of multiple proportions say? In addition to the above items, be sure you read about and understand the following: Dalton s Atomic Theory Thomson s cathode ray tube experiment Rutherford s gold foil experiment The difference between a molecule and an ion Unit Three The Mole, Percent Composition, Empirical and Molecular Formulas 24. An element, E, has only two naturally occurring isotopes. E-10 has a mass of amu and a natural abundance of 19.78%. E-11 has a mass of amu and a natural abundance of 80.22%. What is the average atomic mass of E? 25. Chlorine has two stable isotopes. The mass of one isotope is amu. Its relative abundance is 75.53%. What is the mass of the other stable isotope? 26. How many atoms are in 2.4 moles of neon gas? How many grams? 27. How many grams of zinc are in 1.16 x atoms of zinc? 28. How many mg of Br2 are 4.6 x molecules of bromine?

7 29. How many grams are there in 0.36 moles of cobalt (III) acetate, Co(C2H3O2)3? How many grams of cobalt are in the sample? How many atoms of cobalt? 30. Calculate the mass percent of chlorine in each of the following compounds: A. ClF B. CuCl2 31. Chlorophyll a is essential for photosynthesis. It contains 2.72% magnesium by mass. What is the molar mass of chlorophyll a assuming there is one atom of magnesium in every molecule of chlorophyll a? 32. Which of the following formulas can be empirical? Circle them. A. CH4 F. NH4Cl B. CH2 G. Sb2S3 C. KMnO4 H. N2O D. N2O5 I. CH2O E. B2H8 33. A compound is found to contain % carbon, % chlorine, and 1.39 % hydrogen. The molar mass of the compound is g/mole. Determine the empirical and molecular formulas of the compound.

8 Unit Four Reaction Stoichiometry 34. Calcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide. A. Write a balanced chemical equation for this reaction. B. How many grams of calcium oxide will be produced after grams of calcium carbonate are completely decomposed? C. What is the volume of carbon dioxide gas produced when the grams of calcium carbonate completely decompose at STP? 35. When ammonia gas, oxygen gas and methane (CH4) gas are combined, the products are hydrogen cyanide gas and water. A. Write a balanced chemical equation for the 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.

9 36. DDT, an insecticide harmful to fish, birds and humans, is produced by the following reaction: 2C6H5Cl + C2HOCl3 C14H9Cl5 + H2O chlorobenzene chloral DDT In a government lab, 1142 grams of chlorobenzene is reacted with 485 grams of chloral. A. What mass of DDT is formed? B. Which reactant is limiting? Which is excess? C. What mass of the excess reactant is left over? D. If the actual yield of DDT is grams, what is the percent yield? Unit Five - Solutions 37. Differentiate between what happens when the following are dissolved in water. A. Polar solute versus nonpolar solute B. KF versus C6H12O6 C. RbCl versus AgCl

10 38. Write a reaction to show how solid calcium chloride breaks apart when dissolved in water. 39. What is molarity? 40. Calculate the molarity of the solution made by dissolving grams of NaHCO3 in enough water to make ml of solution. 41. A solution of ethanol (C2H5OH) in water is prepared be dissolving 75.0 ml of ethanol (density = 0.79 g/cm 3 ) in enough water to make ml of solution. What is the molarity of the solution? 42. Which of the following solutions of strong electrolytes contains the largest number of moles of chloride ions? A ml of 0.30 M AlCl3 B ml of 0.60 M MgCl2 C ml of 0.40 M NaCl 43. How would you prepare 2.00 L of M NaOH A. from a 1.00 M stock solution? B. from solid NaOH? In addition to the above, know the following: the difference between an electrolyte and a nonelectrolyte the difference between a strong electrolyte and a weak electrolyte three strong acids and three strong bases one weak acid and one weak base

11 You need to know the following polyatomic ions. You need to know the name, formula and charge of each. Make some flash card. You do need to know these for the first test.