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Use a variety of appropriate notations (e.g., exponential, functional, square root). Math.1
Select and apply appropriate methods for computing with real numbers and evaluate the reasonableness of the results. Math.2
Apply algebraic properties, formulas, and relationships to perform operations on real-world problems (e.g., solve for density, determine the concentration of a solution in a variety of units: ppm, ppb, molarity, molality, and percent composition) calculate heats of reactions and phase changes, and manipulate gas law equations. Math.3
Interpret rates of change from graphical and numerical data (e.g., phase diagrams, solubility graphs, colligative properties, nuclear decay or half-life). Math.4
Analyze graphs to describe the behavior of functions (e.g., concentration of a solution, phase diagrams, solubility graphs, colligative properties, nuclear decay half-life).
Math.5
Model real-world phenomena using functions and graphs. Math.6
Apply and interpret algebraic properties in symbolic manipulation (e.g., density, concentration of a solution, chemical equations, effect of volume, temperature or pressure on behavior of a gas, percent composition of elements in a compound, molar mass, number of moles, and molar volume, amount of products or reactants given mole, molarity, volume at STP or mass amounts, heat loss or gain using mass, temperature change and specific heat, and half-life of an isotope). Math.7
Apply and communicate measurement units, concepts and relationships in algebraic problem-solving situations. Math.8
Select appropriate units, scales, and measurement tools for problem situations involving proportional reasoning and dimensional analysis. Math.9
Select, construct, and analyze appropriate graphical representations for a data set. Math.10
Identify and solve different types of stoichiometry problems (e.g., volume at STP to mass, moles to mass, molarity). Math.11
Calculate the amount of product expected in an experiment and determine percent yield. Math.12
Convert among the quantities of a substance: mass, number of moles, number of particles, molar volume at STP. Math.13
Calculate the wavelength, frequency and energy of a photon of electromagnetic radiation. 1.1
Determine the energy level transition of an electron for a particular wavelength of electromagnetic radiation. 1.2
Correlate emission spectra lines of the hydrogen atom to their respective energy-level transitions. 1.3
Describe the arrangement of electrons in an atom using orbital diagrams, electron configuration notation, and Lewis structures. 1.4
Explain the periodic trends of the main group elements including atomic and ionic radii, ionization energies, and electron affinities. 1.5
Explain the role of electron shielding and effective nuclear charge in determining the atomic and ionic radii, ionization energy, and electron affinities of an atom or ion. 1.6
Describe to correlation between the principle quantum number of the valence electrons and the atomic and ionic radii, ionization energy, and electron affinities of an atom or ion. 1.7
Use Lewis structures to illustrate the structure, shape, and characteristics of polyatomic ions, ionic and molecular compounds. 1.8
Illustrate the shape of molecular compounds using VSEPR theory. 1.9
Determine the polarity of a molecular compound by examining its bond dipoles and shape. 1.10
Apply Lewis structures and formal charge analysis to determine if a compound or polyatomic ion forms resonance structures. 1.11
Explain the formation of hybridized bond orbitals in molecular compounds using VSEPR and valence bond theory. 1.12
Illustrate how sigma and pi bonds form between atoms in a molecular compound. 1.13
Draw the basic functional groups found in organic molecules. 1.14
Draw the structural formulas of simple organic molecules. 1.15
Correlate the kinetic-molecular theory with the motion of particles within a substance. 2.1
Explain the effect of heat on temperature in terms of the motion of the particles within the substance. 2.2
Explain how the motion of gas molecules affects the pressure. 2.3
Explain the effects of temperature changes on the pressure of a gas. 2.4
Explain the effects of pressure changes on the volume of a gas. 2.5
Solve complex combined and ideal gas law problems to quantitatively explain the behavior of gases. 2.6
Determine the rates of effusion of gas molecules using Graham’s Law of Effusion. 2.7
Describe conditions that cause real gases to deviate from their ideal behavior. 2.8
Determine the types of intermolecular interactions that occur in a pure substance or between the components of a mixture. 2.9
Compare the strengths of intermolecular forces between ions, molecules, and ion-molecule mixtures. 2.10
Correlate the strength of intermolecular force with the viscosity, surface tension and physical state of the substance at a given temperature. 2.11
Explain the role of intermolecular forces in determining the vapor pressure, volatility and boiling point of a substance. 2.12
Use a phase diagram to identify the triple-point, critical temperature, and pressure of a substance. 2.13
Apply a phase diagram to interpret the effects of temperature and pressure on the phase of a substance. 2.14
Calculate the effect of solute concentration on vapor pressure using Raoult’s Law. 2.15
Calculate the freezing point depression and boiling point elevation of a solution based on appropriate constants, quantities of solute and solvent, and type of solute. 2.16
Use the freezing or boiling points of the solution, appropriate constants, and the amount solute or solvent to calculate the molar mass of a solute. 2.17
Apply an activity series to predict products and write net ionic reactions that identify spectator ions in a single-replacement reaction. 3.1
Use a solubility chart to predict products and write net ionic reactions that identify spectator ions in a double-replacement reaction. 3.2
Identify the oxidation states of ions in an oxidation-reduction reaction. 3.3
Balance an oxidation-reduction reaction performed in neutral, acidic, or basic environments. 3.4
Use reduction potentials to determine the anode and cathode reactions in an electrochemical cell, and calculate its standard reduction potential. 3.5
Apply reduction potentials to identify oxidizing and reducing agents and determine their relative strengths. 3.6
Calculate the number of moles, mass, number of ions, atoms, and molecules, volume, and pressure of reactants and products in a chemical reaction based on appropriate constants and quantitative information about reaction components. 3.7
Calculate the amount of remaining reactants and products in which one of the reactants is limiting. 3.8
Calculate the rate of a chemical reaction based on elapsed time and amount of remaining reactant or product. 3.9
Use the rate law and rate of reaction to calculate and interpret the rate constant of a chemical reaction. 3.10
Calculate and interpret the reaction order based on the rate constant and concentration of reactants or products at various times during the reaction. 3.11
Draw energy profiles for catalyzed and uncatalyzed chemical reactions in terms of activation energy. 3.12
Write an equilibrium expression and calculate the equilibrium constant based on the concentration of reactants and products at equilibrium. 3.13
Interpret the magnitude of the equilibrium constant to determine equilibrium concentrations and direction of a chemical reaction that has yet to reach equilibrium. 3.14
Apply Le Chatelier’s Principle to predict shifts in the direction of a chemical reaction in response to changes in temperature, pressure and concentration of reactants or products. 3.15
Calculate the percent ionization and pH of a solution given the identity, concentration, and acid/base dissociation constant of an acid or base. 3.16
Prepare a buffer of a specific pH and calculate the change in pH in response to addition of additional acid or base. 3.17
Perform a titration of a weak acid or weak base identifying the Ka or Kb and the pH at the equivalence point. 3.18
Characterize the strength of acids and bases by exploring their chemical structures. 3.19
Calculate the solubility product constant based on the concentration of soluble ions. 3.20
Interpret the magnitude of the solubility product constant in terms of the solubility of the substance. 3.21
Apply thermodynamic data to calculate the change in enthalpy, entropy, and Gibb’s free energy of a chemical reaction. 3.22
Interpret the magnitude of the enthalpy and entropy change of a chemical reaction in terms of heat changes and order of the reaction components. 3.23
Interpret the magnitude of free energy hange in terms of spontaneity of the chemical reaction. 3.24
Relate the magnitude of the free energy change to the equilibrium condition and reduction potential of a chemical reaction. 3.25
a site for teachers | 
a PowerPoint show | 
Adobe Acrobat document | 
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sound | 
video format | 
interactive lesson | 
a quiz | 
to print
