AP Chemistry



AP Chemistry Fall 1819Chapters 1-4, 10: Introduction; Atoms, Molecules and Ions; Stoichiometry; Reactions in Aqueous Solutions & GasesYou should be able to…(Chapters 1 and Intro Unit: and past material from Honors Chemistry) Describe matter using properties: incl. physical and chemical, intensive and extensiveCompare and contrast the three states of matterClassify chemical reactions and physical changes as endothermic or exothermicIdentify and classify physical/chemical changes and properties of matter, with examplesWrite the symbols of common elements, and write the element given its symbolRead a chemical formula for type of elements and number presentDifferentiate between an element and a compoundDistinguish among pure substances, mixtures, and compounds on the particle levelClassify a mixture as homogeneous or heterogeneous Describe methods of separating the components of a mixtureState the difference between mass and weight of a substanceCalculate density Distinguish among hypothesis, theory, and law - with examplesDistinguish between the accuracy and precision of a measurementUse significant figures in measurements and calculationsUse metric prefixes to convert metric unitsConvert temperatures from Kelvin to Celsius and vice-versaDetermine percent errorDetermine percent composition by mass (Law of Definite Proportions, Law of Multiple Proportions)Determine percent yield Draw and interpret graphs(Chapter 2 and Atomic Theory and Periodicity Units, including Honors Chemistry)Use the atomic number and mass number to find the number of protons, electrons, and neutrons in an atom Describe how the isotopes of an atom differ Calculate the average atomic mass of an element from isotope data using weighted averages Classify the elements into four categories according to the configuration of their outermost electrons (s,p,d,f; representative, transition and inner transition elements, noble gases) and their properties (metal, metalloid, nonmetal)Use the periodic table to find the number of valence electrons in an atom and the charge on an ionWrite the chemical formula of an ionic compound when given the name of the compound, vice versaName an acid, ionic compound or molecular compound when given the formula, vice versaName common compounds when given the formula, vice versaCompare and contrast ionic and covalent compoundsNo organic chem. at this time (i.e. no Sec. 2.9)(Chapter 3 and Moles and Stoichiometry Units, including Honors Chemistry)Perform conversions between moles and # particlesDetermine molar masses of elements Determine molar masses of compounds, given the chemical formulaPerform conversions between moles and molar mass of elements or compoundsPerform conversions between molar mass and # particlesPerform conversions involving the # atoms of an element in a compoundSolve problems involving any combination of the above-listed conversionsDetermine percent composition of elements in a compoundDetermine empirical formula of a compound from the masses or percent composition of elements in a compoundDetermine molecular formula of a molecule from mass or percent composition and molecular molar massDetermine chemical formulae of hydratesDetermine empirical formula of a compound from combustion analysisInterpret a balanced equation in terms of interacting moles, representative particles, masses, and volumes of gases (at STP)Construct mole ratios from balanced chemical equations for use as conversion factors in stoichiometric problemsPerform stoichiometric calculations with balanced equations using mass, moles, representative particles, and/or volumes of gases (at STP, and non-standard conditions with the use of PV = nRT)Identify the limiting reactant in a reactionKnowing the limiting reactant in a reaction, calculate the maximum amount of product(s) produced (theoretical yield) and amount of unreacted excess reactantGiven information from which any two of the following may be determined, calculate the third: theoretical yield, actual yield, and percentage yield(Chapter 4, and Chemical Reactions Unit, including Honors Chemistry)Identify the reactants and products in a chemical equationWrite word, skeleton (formula, unbalanced) and balanced chemical equationsUse appropriate symbols when writing an equation to accurately describe the chemical reaction, including reaction conditions and states of matterWrite a balanced chemical equation when given the names or formulas of all the reactants and products in a chemical reactionClassify a reaction as synthesis (combination), decomposition, double replacement (metathesis) or combustionPredict the products of simple synthesis (combination) and decomposition reactionsClassify a reaction as exothermic or endothermicDistinguish among strong, weak and non-electrolytesDefine acids and bases as proton donors/acceptors; distinguish between strong and weak acids and basesDefine oxidation and reduction, with examplesIdentify and write oxidation-reduction reactions as molecular formulas and net ionic equationsAssign oxidation numbers to atoms in a chemical formulaIdentify the substances undergoing oxidation and reduction in a chemical reactionWrite molecular and net ionic equations for synthesis, decomposition, combustion, oxidation-reduction, and the various kinds of metathesis reactions, identify the type(s) of reaction, apply solubility rulescalculate the molarity of a solution from mass and/or moles and volume and related calculationsapply stoichiometry to reactions occurring in aqueous solutionperform a dilution calculation determine the molarity of a solution from titration data and perform other titration-related calculationsdistinguish between endpoint and equivalence point in acid-base reactions(Chapter 10 Gases, and gases Unit, including Honors Chemistry4general properties of gases STP and 1 mol = 22.4 L at STP gas pressure, including atmospheric pressure, conversions amongst pressure units manometer problems Combined Gas Law (which include Boyle’s, Charles’and Gay-Lussac’s, don’t need to know them by name) Ideal Gas Law application of the Ideal Gas Law (Equation) to gas densities and finding molar masses of gases application of the Ideal Gas Equation to stoichiometry problemsDalton’s Law of Partial Pressuresapply partial pressures to mole fractions of gases, and collecting gases by water displacement use the Kinetic Molecular Theory to predict and explain gas behavior Graham’s Law (in theory) define and compare effusion and diffusion deviations from ideal gas behavior ................
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