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Chemistry 2015: Semester 1 – Final Exam Study SheetJunior/Senior Science Fri, January 16, 2015 8:00 amSophomore Science Fri, January 16, 2015 10:30 amThe test contains 86 multiple choice problems and 12 short answer problems.Know the symbols and names of the following elements: 1-20, 26, 29, 30, 47, 50, 79, 80, 82, 92, all of groups 17 and 18. Be familiar with the memorized polyatomic ions (the seven –ates).CHAPTER 1Be able to define the following terms:scientific methodinferencestheoryexperimenthypothesisobservationlawCHAPTER 2 / MATTERObjectives:List the three states of matter and understand their properties.Distinguish between chemical and physical changes.Distinguish between a compound and an element and explain how this is related to a chemical change.State and explain the law of conservation of mass.Write simple chemical equations in both words and symbols.Distinguish between homogeneous and heterogeneous mixtures and give examples of each.Classify matter using the PYRAMID OF MATTER.Define the following terms:chemical property and chemical changechemical symbolcompoundelementgasliquidsolidheterogeneous mixturehomogeneous mixturephysical property and physical changesubstancesolutionsolutesolventCHAPTER 3 / MEASUREMENTObjectives:Distinguish between qualitative and quantitative measurements and give examples of each.Convert between measurements.Be skilled in scientific notation.Distinguish between accuracy and precision and calculate percent error.Identify the number of significant figures in measurement and calculation.Know the base units of length, volume, temperature, and mass in the metric system.State the prefix, symbol, and scientific notation factor of kilo-, centi-, milli-, and micro-.Calculate mass, volume, or density of a substance given any two of the three parameters.Convert between Kelvin and Celsius temperatures.Terms:absolute zeroaccepted valueaccuracyprecisiondensityquantitativequalitativeexperimental valuepercent errorsignificant figureProblems:A. Determine the number of significant figures in each of the following:1. 0.0008 cm2. 2.0000080 mm3. 356 L4. 0.020 g.5. 3.678 x 102 ml6. 35 baseballsB. Give the answer to each of the following problems in the correct number of significant figures.1. 4.66 m x 0.45 m2. 34 cm x .000000000002 cm3. 0.365 m + 0.200 m4. 3.998 cm + 200 cm + 3.2 cm5. 4.999 m + 5.8765 m + 2.3 mC. A student finds a piece of metal that she thinks is lead. In the lab, she determines that the metal has a volume of 122 cm3 and a mass of 1.39 kg. Calculate the density of this metal. Is it lead?D. Write the following numbers in scientific notation:1. 40867542. 0.00000387E. Convert 45?C to Kelvin.F. Convert 0 K to Celsius.G. Order these lengths from smallest to largest: centimeter, meter, nanometer, decimeter, micrometer, kilometer, millimeter, picometer.H. the teacher told the class that a sample of gold should have a mass of 33.8 g. A student made 4 measurements of the sample using the same balance. the measurements were: 33.9 g, 33.5 g, 34.0 g, and 33.9 g. Were the student’s measurements precise? Were they accurate? Can you have precision without accuracy? Can you have accuracy without precision?I. A student determines the density of a piece of solid aluminum to be 3.2 g/ml by measuring its mass and volume in the lab. The actual density of aluminum is 2.7 g/ml. What is the percent error of the student’s measurement?CHAPTER 3 / PROBLEM SOLVINGObjectives:Use conversion factors.Apply dimensional analysis (conversion cross) in solving conversion problems.Convert density and other complex units between different units.Problems:A. Convert:1. 642 mg to grams2. 261 mm to km3. 4.5 m/s to km/hCHAPTER 9 / CHEMICAL BONDINGObjectives:Distinguish between ionic and molecular compounds.Interpret chemical formulas in terms of numbers of atoms in a molecule or formula unit.Distinguish between anions and cations.Name and write formulas for monatomic and polyatomic ions.Write chemical formulas for binary and ternary ionic compounds using the criss-cross method.Give the charge of an ion, given the ion in a compound, using the reverse criss-cross method.Write the names of ionic compounds given the chemical formula.Name any molecular compound given the formula.Write the formula for any molecular compound.State the formula and name of the common acids.Terms:anioncationbinary compoundternary compoundionic compoundmolecular compoundformula unitmoleculeionmonatomic ionpolyatomic ionProblems:A. State the number of electrons lost or gained in forming each ion. Name each ion.1. Br-2. Na+3. As3-4. Ca2+5. Cu+B. How many oxygen atoms are in 6 Cr2(SO4)3?C. Name the 5 common acids and give their formulas.D. Write the formulas for the following compounds.1. tin (IV) cyanide2. calcium nitride3. aluminum oxide4. barium phosphate5. ammonium nitrate6. lead (III) oxideE. Write the names of the following compounds. Identify whether each is ionic or molecular.1. SO22. P4O103. KHSO44. Mg(NO3)25. FeCl36. Ag3PO4F. Describe the role of roman numerals in naming compounds.G. How can the periodic table assist you in determining the charges of ions?CHAPTER 11 / CHEMICAL EQUATIONS AND NET IONIC EQUATIONSObjectives:Translate chemical equations from words to symbols and vice versa.Define a skeleton equation.Balance chemical equations and interpret the coefficients in terms of atoms, molecules, and moles.Describe the 5 types of chemical reactions.Predict products or reactants of chemical equations.Determine precipitates by predicting the solubility of products in reactions using the solubility rules.Write ionic and net ionic equations.Determine the spectator ions in ionic equations.Terms:skeleton equationbalanced equationcatalystcoefficientsubscriptcombination reactioncombustion reactiondecomposition reactionsingle replacement reactiondouble replacement reactionionic equationnet ionic equationspectator ionProblems:A. Write balanced chemical equations for the following. What kind of reaction is this?1. chlorine gas reacts with a solution of potassium iodide to produce iodine and a solution of potassium chloride2. a piece of steel wool is placed in sulfuric acid and a reaction results.3. C4H8 undergoes combustion.4. iron reacts with oxygen5. potassium metal reacts with magnesium nitrateB. Write the following reactions in words.1. Fe(OH)3 + NaOH ? + ?2. Mg(s) + KNO3(aq) K(s) + Mg(NO3)2(aq)3. PbSO4(aq) + NaI(aq) PbI2 + Na2SO4 What states are the products of this reaction in?C. Write ionic and balanced net ionic equations for number 3 above. Remember that ionic equations do not have to be balanced. When writing both kinds of equations you must indicate the state of matter of all ions and other substances.CHAPTER 10 / THE MOLEObjectives:Calculate the mass of a mole of any substance.Memorize Avogadro’s number and describe how it is related to a mole of a substance.Convert between moles, grams, volume, and number of particles.Calculate percent composition.Distinguish between empirical and molecular formula.Calculate the empirical formula of a compound given its percent composition.Calculate the molecular formula of a compound given its empirical formula and molar mass.Terms:moleAvogadro’s numbermolar massmolar volume of gasmole conversionspercent compositionempirical formulamolecular formulastandard temperature and pressure (STP)Problems:A. How many atoms are there in 2.45 moles of propane (C3H8)?B. Find the molar mass of1. PCl3.2. K2SC. How many moles is 4.89 x 1024 atoms of Li?D. Mind the mass of 1.50 moles of C5H12.E. Convert 82 grams of Kr gas to liters.F. Determine the empirical formula for a compound with this percent composition:32.0 % C, 42.66 % O, 18.67 % N, and 12.12% HG. What is the molecular formula for a compound that has a molar mass of 90 g/mol and an empirical formula of CH2O?H. What is the percent composition of each element in the compound AgNO3?****Important Information**** You must bring pencils and a calculator if you want one for the test. You may not use a phone as a calculator, nor may you share calculators.Bring your old tests to the final for extra credit. You should have 3 tests/2 quizzes.You will be allowed (1) 3x5 inch notecard on the final. It can be double sided, but it must be hand written BY YOU. The note card may not contain names and symbols of polyatomic ions or old test questions. All decisions on card content are at the discretion of Mr. Moser.In order to use the notecard on the final it MUST be turned in to Mr. Moser by 3:00 pm (PST) on Thurs January 15, 2015.You will receive a periodic table to help you on your test. ................
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