• Chemical Reactions

  • Write and balance chemical equations based on chemical reactions.

  • Identify and characterize the types of reactions, including synthesis, decomposition, single replacement, double
    replacement, and combustion.

  • Recognize and write balanced chemical equations for synthesis, decomposition, single replacement, double replacement, or combustion reactions.

  • Use the activity series to determine whether a single replacement reaction will occur.

  • Write ionic equations, net ionic equations, and recognize spectator ions based on reactions with aqueous solutions.

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• Stoichiometry

  • Understand and use stoichiometry in balanced chemical equations (particularly regarding molar quantities of mass, volume, and number).

  • Explain and calculate the interconversion of reactants and products using mole ratios.

  • Identify the limiting and excess reactants for a given reaction.

  • Use the limiting reactant to predict the theoretical yield of a reaction.

  • Calculate the percent yield of a reaction.

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• The Behavior of Gases

  • State Boyle’s law, Charles’s law, Gay-Lussac’s law, and Avogadro's law and apply these laws to calculate the relationships between volume, temperature, and pressure.

  • Derive the combined gas law from Boyle’s law, Charles’s law, and Gay-Lussac’s law and calculate for pressure, volume, or temperature.

  • Define partial pressure and apply Dalton’s law of partial pressures to describe the composition of gases.

  • State the Ideal Gas Law (PV = nRT) and calculate moles of a gas, understanding the difference between ideal and real gases.

  • Understand Graham's Law which states that gases of lower molar mass diffuse and effuse faster than gases of higher molar mass.

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• Water & Solutions

  • Describe how the structure of water accounts for its polarity

  • Explain why water has unique properties including high surface tension and high boiling point

  • Describe the unique role of water as the “universal solvent”

  • Identify factors affecting solubility and the rate at which a substance dissolves

  • Define solubility and differentiate between saturated, supersaturated, and unsaturated solutions

  • Define & calculate concentration in terms of mass, volume, & molarity, and molality

  • Describe the relationship of the molality of a solute in solution and the solution’s depressed freezing point or elevated boiling point. Calculate freezing point depression & boiling point elevation.

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• Thermochemistry

  • Distinguish aspects of heat flow (endothermic, exothermic, potential energy, kinetic energy, heat and temperature).

  • Identify heat flow, potential and kinetic energy, phase changes, and heating or cooling for phase diagrams of a substance.

  • Calculate heat flow for heating and cooling of substances using mass, specific heat, and the change in temperature or heat of fusion or heat of vaporization.

  • Define and calculate the specific heat of a substance and the heat flow related to calorimetry.

  • Identify reactants, products, heat of reaction, and heat flow in potential energy diagrams.

  • Calculate heat flow in thermochemical equations using heat of reaction, standard heats of formation, and Hess's Law

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• Reaction Rates and Equilibrium

  • Explain the concept of reaction rate.

  • Describe collision theory and explain how various factors, including concentration, temperature, and pressure affect the rate of a chemical reaction.

  • Interpret reaction pathways (PE diagrams) to identify exothermic versus endothermic reactions and to define and explain the role of the activation energy in a chemical reaction.

  • Explain what a reaction mechanism is and understand the concept of rate determining step for a reaction.

  • Write equilibrium expressions, distinguishing molar concentrations of reactants and products for reactions.

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• Ksp and Free Energy

  • Use Le Chatelier’s principle to predict shifts in equilibrium caused by changes in pressure, concentration, and temperature.

  • Write expressions for the solubility product constant (Ksp) and solve problems involving Ksp and ion concentrations.

  • Use Ksp to predict the solubility of compounds.

  • Compare spontaneous and nonspontaneous reactions.

  • Describe and give examples of entropy and describe how enthalpy and entropy affect a reaction's spontaneity.

  • Define free energy and use Gibbs free energy equation to determine whether a reaction is spontaneous.

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• Acids, Bases and Salts

  • Explain Arrhenius acids and bases based on the dissociation of water.

  • Define pH and pOH. Use the pH scale to characterize the acidity and basicity of solutions and properties of acids and bases.

  • Convert between pH, pOH, hydrogen ion concentration and hydroxide ion concentration.

  • Describe Bronsted-Lowry acids and bases.

  • Identify conjugate acids and conjugate bases as well as conjugate pairs in a Bronsted-Lowry acid–base reaction.

  • Describe Lewis acids and bases. [Enrichment]

  • Differentiate between strong and weak acids and bases based on dissociation and ionization.

  • Explain how the acid-dissociation constant, Ka, and the base dissociation constant, Kb, relate to the acid & base strength.

  • Differentiate between the concentration & strength of solutions.

  • Predict the products of acid-base neutralization reactions, and calculate the molar concentrations of acid or base needed.

  • Explain the use of titration in chemistry, and describe the steps of the titration process. Recognize & describe titration graphs for strong and weak acids & bases.

  • Explain hydrolysis (reverse reaction of neutralization). Show how salt solutions can be acidic, neutral, or basic.

  • Explain buffers and write the resulting chemical equations when an acid or base is added to the system.

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• Oxidation-Reduction (REDOX) Reactions

  • Follow rules to assign oxidation numbers to atoms in compounds.

  • Recognize oxidation-reduction (REDOX) reactions and define oxidation and reduction, distinguishing oxidized & reduced species and oxidizing & reducing agents in a REDOX reaction.

  • Write half reactions for oxidation-reduction reactions.

  • Use the half-reaction method to balance oxidation-reduction equations.

  • Use the Electron transfer method/Oxidation number method to balance oxidation-reduction equations.

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• Electrochemistry

  • Define electrochemistry and describe the components of an electrochemical cell.

  • Identify the types of electrochemical cells based on spontaneity.

  • Use the relative strengths of oxidizing and reducing agents to make predictions of an oxidation/reduction reaction.

  • Describe voltaic cells and explain how voltaic cells work.

  • Give examples and a brief description of common voltaic cells.

  • Describe electrolytic cells and compare electrolytic cells with voltaic cells.

  • Describe the electrolytic processes that happens during electroplating and recharging batteries.