Chemistry II is a laboratory course that builds on topics taught in Chemistry I. This course investigates chemical bonding and how the kinetic molecular theory and by intermolecular forces explain the physical and chemical characteristics of matter. Additional aspects of chemical reactions including limiting reactants, percent yield, equilibrium, reaction rates, and thermochemistry are considered. Students explore chemistry concepts through an inquiry approach.

Chemistry II students investigate:

3222.Inq.2 Identify an answerable question and formulate a hypothesis to guide a scientific investigation.

3222.Inq.3 Design a simple experiment including appropriate controls.

�3222.Inq.4 Perform and understand laboratory procedures directed at testing hypothesis.

3222.Inq.5 Select appropriate tools and technology to collect precise and accurate quantitative and qualitative data.

3222.Inq.6 Correctly read a thermometer, balance, metric ruler, graduated cylinder, pipette, and burette.

3222.Inq.7 Record observations and/or data using correct scientific units and significant figures.

3222.Inq.8 Export data into the appropriate form of data presentation (e.g., equation, table, graph, or diagram).

3222.Inq.9 Translate data into the correct units and dimension using conversion factors and scientific notation.

3222.Inq.10 Analyze information in a table, graph or diagram (e.g., compute the mean of a series of values or determine the slope of a line).

3222.Inq.11 If accepted values are known, calculate the percent error for an experiment.

3222.Inq.12 Determine the accuracy and precision of experimental results.

3222.Inq.13 Analyze experimental results and identify possible sources of bias or experimental error.

3222.Inq.14 Recognize, analyze, and evaluate alternative explanations for the same set of observations.

3222.Inq.15 Design a model based on the correct hypothesis that can be used for further investigation.

CLE 3222.T/E.2 Differentiate among elements of the engineering design cycle: design constraints, model building, testing, evaluating, modifying, and retesting.

CLE 3222.T/E.3 Explain the relationship between the properties of a material and the use of the material in the application of a technology.

CLE 3222.T/E.4 Describe the dynamic interplay among science, technology, and engineering within living, earth-space, and physical systems.

3222.T/E.1 Distinguish among tools and procedures best suited to conduct a specified scientific inquiry.

3222.T/E.2 Apply the engineering design process to construct a prototype that meets developmentally appropriate specifications.

3222.T/E.3 Evaluate a protocol to determine the degree to which an engineering design process was successfully applied.

3222.T/E.4 Explore how the unintended consequences of new technologies can impact human and non-human communities.

3222.T/E.5 Evaluate the overall benefit to cost ratio of a new technology.

3222.T/E.6 Present research on current bioengineering technologies that advance health and contribute to improvements in our daily lives.

3222.T/E.7 Design a series of multi-view drawings that can be used by other students to construct an adaptive design and test its effectiveness.

CLE 3222.Math.2 Utilize appropriate mathematical equations and processes to solve chemistry problems.

3222.Math.1 Use a variety of appropriate notations (e.g., exponential, functional, square root).

3222.Math.2 Select and apply appropriate methods for computing with real numbers and evaluate the reasonableness of the results.

3222.Math.3 Apply algebraic properties, formulas, and relationships to perform operations on real-world problems such as: solving for density, determining the concentration of a solution in a variety of units (e.g., ppm, ppb, molarity, molality, and percent composition), calculating heats of reactions and phase changes, and manipulating gas law equations.

3222.Math.4 Interpret rates of change from graphical and numerical data (e.g., phase diagrams, solubility graphs, colligative properties, nuclear decay or half-life).

3222.Math.5 Analyze graphs to describe the behavior of functions (e.g., concentration of a solution, phase diagrams, solubility graphs, colligative properties, nuclear decay half-life).

3222.Math.6 Model real-world phenomena using functions and graphs.

3222.Math.7 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).

3222.Math.8 Apply and communicate measurement units, concepts and relationships in algebraic problem-solving situations.

3222.Math.9 Select appropriate units, scales, and measurement tools for problem situations involving proportional reasoning and dimensional analysis.

3222.Math.10 Choose, construct, and analyze appropriate graphical representations for a data set.

3222.Math.11 Identify and solve different types of stoichiometry problems (e.g., volume at STP to mass, moles to mass, molarity).

3222.Math.12 Calculate the amount of product expected in a lab experience and determine percent yield.

3222.Math.13 Convert among the quantities of a substance: mass, number of moles, number of particles, molar volume at STP.

CLE 3222.1.2 Relate the arrangement of electrons surrounding an atom with observed periodic trends.

CLE 3222.1.3 Describe the structure, shape, and characteristics of polyatomic ions, ionic and molecular compounds.

3222.1.1 Calculate the wavelength, frequency and energy of a photon of electromagnetic radiation.

3222.1.2 Determine the energy level transition of an electron for a particular wavelength of electromagnetic radiation.

3222.1.3 Correlate emission spectra lines of the hydrogen atom to their respective energy-level transitions.

3222.1.4 Describe the arrangement of electrons in an atom using orbital diagrams, electron configuration notation, and Lewis structures.

3222.1.5 Explain the periodic trends of the main group elements including atomic and ionic radii, ionization energies, and electron affinities.

3222.1.6 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.

3222.1.7 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.

3222.1.8 Use Lewis structures to illustrate the structure, shape, and characteristics of polyatomic ions, ionic and molecular compounds.

3222.1.9 Illustrate the shape of molecular compounds using VSEPR theory.

3222.1.10 Determine the polarity of a molecular compound by examining its bond dipoles and shape.

3222.1.11 Apply Lewis structures and formal charge analysis to determine if a compound or polyatomic ion forms resonance structures.

3222.1.12 Explain the formation of hybridized bond orbitals in molecular compounds using VSEPR and valence bond theory.

3222.1.13 Illustrate how sigma and pi bonds form between atoms in a molecular compound.

3222.1.14 Draw the basic functional groups found in organic molecules.

3222.1.15 Draw the structural formulas of simple organic molecules.

CLE 3222.2 Determine the intermolecular forces that exist between ions and molecules.

CLE 3222.3 Explain how the physical characteristics of matter are governed by kinetic molecular theory and intermolecular forces.

3222.2.1 Correlate the kinetic-molecular theory with the motion of particles within a substance.

3222.2.2 Explain the effect of heat on temperature in terms of the motion of the particles within the substance.

3222.2.3 Explain how the motion of gas molecules affects the pressure.

3222.2.4 Explain the effects of temperature changes on the pressure of a gas.

3222.2.5 Explain the effects of pressure changes on the volume of a gas.

3222.2.6 Solve complex combined and ideal gas law problems to quantitatively explain the behavior of gases.

3222.2.7 Determine the rates of effusion of gas molecules using Graham’s Law of Effusion.

3222.2.8 Describe conditions that cause real gases to deviate from their ideal behavior.

3222.2.9 Determine the types of intermolecular interactions that occur in a pure substance or between the components of a mixture.

3222.2.10 Compare the strengths of intermolecular forces between ions, molecules, and ion-molecule mixtures.

3222.2.11 Correlate the strength of intermolecular force with the viscosity, surface tension and physical state of the substance at a given temperature.

3222.2.12 Explain the role of intermolecular forces in determining the vapor pressure, volatility and boiling point of a substance.

3222.2.13 Use a phase diagram to identify the triple-point, critical temperature, and pressure of a substance.

3222.2.14 Apply a phase diagram to interpret the effects of temperature and pressure on the phase of a substance.

3222.2.15 Calculate the effect of solute concentration on vapor pressure using Raoult’s Law.

3222.2.16 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.

3222.2.17 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.

CLE 3222.3.2 Fully analyze the quantitative aspects of a chemical reaction in terms of the amounts of products and reactants.

CLE 3222.3.3 Analyze the kinetics of a chemical reaction.

CLE 3222.3.4 Describe parameters of chemical equilibria.

CLE 3222.3.5 Explain the thermodynamics of a chemical reaction.

3222.3.1 Apply an activity series to predict products and write net ionic reactions that identify spectator ions in a single-replacement reaction.

3222.3.2 Use a solubility chart to predict products and write net ionic reactions that identify spectator ions in a double-replacement reaction.

3222.3.3 Identify the oxidation states of ions in an oxidation-reduction reaction.

3222.3.4 Balance an oxidation-reduction reaction performed in neutral, acidic, or basic environments.

3222.3.5 Use reduction potentials to determine the anode and cathode reactions in an electrochemical cell, and calculate its standard reduction potential.

3222.3.6 Apply reduction potentials to identify oxidizing and reducing agents and determine their relative strengths.

3222.3.7 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.

3222.3.8 Calculate the amount of remaining reactants and products in which one of the reactants is limiting.

3222.3.9 Calculate the rate of a chemical reaction based on elapsed time and amount of remaining reactant or product.

3222.3.10 Use the rate law and rate of reaction to calculate and interpret the rate constant of a chemical reaction.

3222.3.11 Calculate and interpret the reaction order based on the rate constant and concentration of reactants or products at various times during the reaction.

3222.3.12 Draw energy profiles for catalyzed and uncatalyzed chemical reactions in terms of activation energy.

3222.3.13 Write an equilibrium expression and calculate the equilibrium constant based on the concentration of reactants and products at equilibrium.

3222.3.14 Interpret the magnitude of the equilibrium constant to determine equilibrium concentrations and direction of a chemical reaction that has yet to reach equilibrium.

3222.3.15 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.

3222.3.16 Calculate the percent ionization and pH of a solution given the identity, concentration, and acid/base dissociation constant of an acid or base.

3222.3.17 Prepare a buffer of a specific pH and calculate the change in pH in response to addition of additional acid or base.

3222.3.18 Perform a titration of a weak acid or weak base identifying the K_{a or Kb and the pH at the equivalence point.}

3222.3.24 Interpret the magnitude of free energy change in terms of spontaneity of the chemical reaction.

3222.3.25 Relate the magnitude of the free energy change to the equilibrium condition and reduction potential of a chemical reaction.