Orange County Public Schools



AP ChemistrySummer AssignmentApopka HSWelcome to AP Chemistry!I am excited that you decided to take on the challenge that AP Chemistry has to offer. This packet contains review materials that are necessary for your success in this course. It covers the first 3 chapters in the text which is review of important concepts from 1st year chemistry. Major topics include chemical formulas, chemical reactions and equations and stoichiometry. Your chemistry notes from Chemistry 1 Honors is a good resource for this review. You can also look at you tube video clips from the following sites to help with this review:Bozeman ScienceCrash Course ChemistryKhan AcademyWhat should you purchase to get you off to a great start? “The Princeton’s Review” AP Chemistry study guide. You will need to have this in August. It is strongly recommended that you buy it in the summer so that you can use it to help review the topics from 1st year chemistry. This book is a supplement to the course and will help you review and prepare for the AP test.This review packet will be collected during the first week of school. There will be a series of quizzes during the first few weeks of school in August covering the review topics. Please take this assignment seriously and do not procrastinate. You can email me if you have any questions. I look forward to see you in August.Mr. JadonathEmail: yado.jadonath@Chapter 1 Matter and MeasurementSectionLearning Targets (Objectives)1.11.3 Classification, PropertiesKnow the difference between elements, compounds and mixtures.Know the difference between physical and chemical properties and changes.Be able to classify matter into pure substances or mixtures.Understand how to separate mixtures through different techniques (filtration, distillation, chromatography)1.4 Units of MeasurementUse SI units for measurement.Be able to convert temperature units & do density calculations.1.5 Uncertainty in MeasurementDemonstrate the use of significant figures, scientific notation, and SI units in calculations.1.6 Dimensional AnalysisAttach appropriate SI units to defined quantities, and use dimensional analysis in calculations and conversions.Questions on Classification & PropertiesWhite gold used in jewelry contains 2 elements, gold and palladium. Two different samples of white gold differ in relative amounts of gold and palladium that they contain. Both sample are uniform in composition throughout. How would you classify white gold? (element, compound, homogeneous mixture, heterogeneous mixture)Aspirin is composed of 60.0% carbon, 4.5% hydrogen and 35.5% oxygen by mass regardless of its source. How would you classify it? (compound, homogeneous mixture, heterogeneous mixture)Describe what is involved in each process below and tell if the process involve physical or chemical changes.FiltrationDistillationChromatographyelectrolysisQuestions on Significant Figure & CalculationsState how many significant figures are in each:20.0105 m ___________________4.0500 x 10-6 s ________________5.000 cm ________________.06090 g _________________7000 m ___________________260 L __________________Perform the following calculations and express your results to the proper number of significant figures. (5.24 x 107)(3.27 x 10-4) = _____________________________8.67/4.1 = _________________________ 3.64 x 10-4 + 8.29 x 10-6 = ______________________ 13.478 – 15.4 = _________________________Questions on DIMENSIONAL ANALYSISAs chemistry students, you have two goals with problems. First, get the correct answer. Second, be able to show others WHY your answer is correct. Dimensional analysis meets both of these goals.Dimensional analysis is always a Given value and one or more conversion factors that allow you to determine the Desired value.Any mathematical fact can serve as a conversion factor. 1 hour = 60 minutes 1.Convert 2.83 days into seconds.2.Convert 7.72 years into days.3.Convert 0.0035 weeks into seconds.4.Convert 180 days into minutes.5.Convert your age into seconds Density is often used as a conversion factor between the mass and volume of a sample. For example, the density of liquid mercury is 13.6 g/mL.6.What is the volume of a 175 gram sample of mercury?7.What is the mass of 1.00 gallon of mercury? [1 cup = 236.588 ml]8. When I carry in a 5-gallon container of water from my car, I always wonder its weight. I looked up on the web and found that 1 lb = 0.453542 kg and 1 qt = .946353 Liter. Calculate its weight in pounds.AP Chemistry Chapter 2 Atoms, Molecules, and IonsSectionLearning Targets (Objectives)2.12.4 Atomic TheoryBe able to compare and contrast Dalton’s atomic theory with the modern atomic theory.Describe the structure of the atom in terms of protons, neutrons and electrons.Use chemical symbols with atomic # and mass # to express the subatomic composition of atoms, isotopes, ions.Calculate the atomic weight of an element from the masses of individual atoms and a knowledge of natural abundances.Periodic TableDescribe how elements are organized in the periodic table by atomic number and similarities in chemical behavior.Identify the locations of special groups or rows on the periodic table.2.62.9 Molecular & Ionic CompoundsDistinguish between molecular substances and ionic substances in terms of their composition.Distinguish between empirical and molecular formulas.Write formulas and name compounds for molecular compounds.Write formulas and name compounds for binary and ternary ionic compounds. INCLUDEPICTURE "" \* MERGEFORMATINET INCLUDEPICTURE "" \* MERGEFORMATINET INCLUDEPICTURE "" \* MERGEFORMATINET Questions on Ch 2 Atomic TheoryALL of the answers to this worksheet can be logically figured out by looking at the the Periodic Table. 1.How many protons are found in 12C?13C?13C??2.How many neutrons are found in 12C?13C?13C??3.How many electrons are found in12C?13C?13C??4.Based on the model,a)what do all carbon atoms (and ions) have in common?b)what do all hydrogen atoms (and ions) have in common?5.What is the significance of the atomic number in the periodic table?6.What do all nickel (Ni) atoms have in common?7.How is the mass number determined?8.What is different in isotopes of a particular element?9.a)What feature distinguishes a neutral atom from an ion?b)How is the charge on an ion determined?10.Where is most of the mass of an atom, within the nucleus or outside of the nucleus?Explain your reasoning.plete the following table:IsotopeAtomicNumberZMassNumberANumber ofelectrons31P1518O819391858Ni2+58Calculate the average atomic mass for the element chlorine if it has the following isotopes with the given relative abundances:75 % chlorine-35 (mass = 35)25 % chlorine-37 (mass = 37)Questions on the Periodic TableIdentify the following groups of elements by giving their location on the periodic table and list some unique properties of each.Alkali metalsAlkaline earth metalsTransition metalsHalogensNoble gasesPredict the ionic charges for the group A columns on the periodic table.Questions on Chemical Formulas Write formulas for the following substances:Barium sulfateAmmonium chlorideChlorine monoxideSilicon tetrachlorideMagnesium fluorideSodium oxideSodium peroxideCopper (I) iodideZinc sulfidePotassium carbonateHydrobromic acidLead (II) acetateSodium permanganatePotassium cyanideIron (III) hydroxideNitrogen trifluorideChromium (III) oxideCalcium chlorateSodium thiocyanateNitric acidName each of the following compoundsCuSO4PCl3Li3NBaSO3N2F4KClO3NaH(NH4)2Cr2O7HClSr3P2Mg(OH)2Al2S3AgBrP4O10HC2H3O2CaI2MnO2Li2OFeI3Cu3PO4Questions on Molecular (covalent) and Ionic CompoundsDefine molecular compound. Give an example.Define ionic compound. Give an pare and contrast molecular compounds and ionic compounds using a double-bubble map. Give at least 3 similarities and 3 differences.If you are given a compound, how could you tell if it is molecular or ionic?AP Chemistry Chapter 3 Chemical Reactions & Reaction StoichiometrySectionLearning Targets (Objectives)3.13.2 Equations & Reaction TypesWrite balanced chemical equations for reactions.Classify reactions into different types and predict products.3.33.5 Formula & Moles CalculationsCalculate formula mass and percent composition.Convert grams to moles and vice versa using molar masses.Convert # of atoms or molecules to moles and vice versa using Avogadro’s #.Calculate the empirical and molecular formulas of a compound from the percentage composition and molecular mass.3.63.7 Reaction Stoichiometry Identify limiting reactants and calculate amounts, in grams or moles, of reactants consumed and products formed for a reaction.Calculate the percent yield of a reaction.Questions on Chemical Reactions and EquationsFor each reaction below, write a balanced chemical equation and identify the type of reaction.Ex. Solutions of silver nitrate and magnesium iodide are combined.2AgNO3 + MgI2 2AgI(s) + Mg(NO3)2 double replacement reactionAmmonium sulfate reacts with barium nitrate.Zinc metal is added to a solution of copper (II) chloride.Propane gas is burned in excess oxygen.Solid calcium chlorate is heated strongly.Sodium hydroxide solution is added to a solution of iron (III) bromide.Chlorine gas is bubbled through a solution of sodium bromide.Magnesium is burned in air.Solid sodium carbonate is heated in a crucible.Potassium metal is added to distilled water.Barium combines with fluorine.Questions on StoichiometryBenzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol. Analysis shows the compound to be 7.74 % H by mass. Find the empirical and molecular formulas of benzene.Find the mass percent of nitrogen in each of the following compounds:NONO2N2O4N2OCalcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide gas.Write a balanced chemical equation for this reaction.How many grams of calcium oxide will remain after 12.25 g of calcium carbonate is completely decomposed?What volume of carbon dioxide gas is produced from this amount of calcium carbonate? The gas is measured at 0.95 atm and 10oC.Hydrogen gas and bromine gas react to form hydrogen bromide gas.Write a balanced chemical equation for this reaction.How many grams of hydrogen bromide gas can be produced from 3.2 g of hydrogen gas and 9.5 g of bromine gas?How many grams of which reactant is left unreacted?What volume of HBr, measured at STP, is produced in part b?When ammonia gas, oxygen gas and methane gas (CH4) are combined, the products are hydrogen cyanide gas and water.Write a balanced chemical equation for this reaction.Calculate the mass of each product produced when 225 g of oxygen gas is reacted with an excess of the other two reactants.If the actual yield of the experiment in part b is 105 g of HCN, calculate the percent yield.A 2.29 g sample of an unknown acid is dissolved in 1.0 liter of water. A titration required 25 ml of 0.5 M NaOH to completely react with all the acid present. What is the molar mass of the acid? ................
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