Differentiate between physical and chemical changes and properties.
Compare solids, liquids, and gasses in terms of:
Compressibility
Structure
Shape
Volume
Classify matter as pure substances or mixtures through investigation of their properties.
Explain everyday examples that illustrate the four laws of thermodynamics.
Investigate the process of heat transfer using calorimetry.
Classify processes as:
Exothermic
Endothermic
Represent energy changes that occur in chemical reactions using:
Thermochemical equations
Graphical analysis
Perform calculations involving:
Heat
Mass
Temperature change
Specific heat
Unit 2
Construct an argument to support how periodic trends such as electronegativity can predict bonding between elements.
Name and write the chemical formulas for ionic and covalent compounds using International Union of Pure and Applied Chemistry (IUPAC) nomenclature rules.
Classify and draw electron dot structures for molecules with:
Linear
Bent
Trigonal planar
Trigonal pyramidal
Tetrahedral molecular geometries as explained by Valence Shell Electron Pair Repulsion (VSEPR) theory
Analyze the properties of ionic, covalent, and metallic substances in terms of intramolecular and intermolecular forces.
Unit 3
Describe the characteristics of alpha, beta, and gamma radioactive decay processes in terms of balanced nuclear equations.
Compare fission and fusion reactions.
Give examples of applications of nuclear phenomena such as:
Nuclear stability
Radiation therapy
Diagnostic imaging
Solar cells
Nuclear power
Unit 4
The Moles and The Solutions
Define mole and apply the concept of molar mass to convert between moles and grams.
Calculate the number of atoms or molecules in a sample of material using Avogadro’s number.
Calculate percent composition of compounds.
Differentiate between empirical and molecular formulas.
Describe the unique role of water in solutions in terms of polarity.
Distinguish among types of solutions, including:
Electrolytes and nonelectrolytes
Unsaturated, saturated, and supersaturated solutions
Investigate how solid and gas solubilities are influenced by temperature using solubility curves and how rates of dissolution are influenced by temperature, agitation, and surface area.
Investigate the general rules regarding solubility and predict the solubility of the products of a double replacement reaction.
Calculate the concentration of solutions in units of molarity.
Calculate the dilutions of solutions using molarity.
Unit 5
Chemical Reactions & Stoichiometry
Interpret, write, and balance chemical equations, including:
Synthesis
Decomposition
Single replacement
Double replacement
Combustion reactions using the law of conservation of mass
Perform stoichiometric calculations, including determination of:
Mass relationships
Gas volume relationships
Percent yield
Describe the concept of limiting reactants in a balanced chemical equation.
Unit 6
Gas Laws
Describe the postulates of the kinetic molecular theory.
Describe and calculate the relationships among volume, pressure, number of moles, and temperature for an ideal gas.
Define and apply Dalton’s law of partial pressure.
Unit 7
Acids & Bases
Name and write the chemical formulas for acids and bases using IUPAC nomenclature rules.
Define acids and bases and distinguish between Arrhenius and Bronsted‐Lowry definitions.
Differentiate between strong and weak acids and bases.
Predict products in acid‐base reactions that form water.
Define pH and calculate the pH of a solution using the hydrogen ion concentration.
Unit 8
Redox & Thermal Chemistry
Differentiate among:
Acid‐base reactions
Precipitation reactions
Oxidation‐reduction reactions
Explain everyday examples that illustrate the four laws of thermodynamics.
Investigate the process of heat transfer using calorimetry.
Classify processes as exothermic or endothermic and represent energy changes that occur in chemical reactions using thermochemical equations or graphical analysis.
Perform calculations involving heat, mass, temperature change, and specific heat.