Chemistry Experiments

In this lesson, students assess the merits and limitations of historic and modern atomic models. They explore the presence, position, mass, and charge of subatomic particles and use models of an element’s subatomic particles to compare and contrast atoms, ions, and isotopes. 

In this lesson, students analyze and interpret data related to the relative abundance of isotopes to determine the average atomic mass of an element and to identify or describe an element based on its number of protons and isotopic composition.

In this lesson, students analyze and interpret data from light emission spectra and photoemission spectroscopy to identify and describe elements and explain how electron energy levels relate to the light emitted by atoms.

In this lesson, students investigate patterns in the periodic table to construct explanations for trends in atomic radius, ionization energy, and electronegativity and apply those patterns to predict the properties and behavior of elements.

In this lesson, students develop and use Lewis dot diagrams to model the formation of covalent and ionic bonds, then construct explanations describing the change in potential energy that occurs when chemical bonds form. 

In this lesson, students plan and carry out an investigation to identify the physical and chemical properties of ionic, covalent, and metallic compounds and use their observations and data to explain how bonding type influences the properties of substances.

In this lesson, students develop and use models based on valence shell electron pair repulsion (VSEPR) theory to predict molecular geometry for molecules with up to four electron domains and construct explanations of molecular polarity using electronegativity and molecular geometry.

In this lesson, students analyze and interpret data from the periodic table to derive chemical formulas and names for ionic and covalent compounds. By applying systematic naming rules, students will learn to communicate chemical information accurately. 

In this lesson, students analyze and interpret data to compare the strengths of intermolecular forces and explain how these forces affect the physical properties of substances. 

In this lesson, students use qualitative and quantitative reasoning to describe and balance chemical equations, ensuring the law of conservation of matter is satisfied, in order to classify chemical reactions and predict the products of single replacement and double replacement reactions. 

In this lesson, students use ionic equations to represent chemical reactions and apply their understanding of reaction types and ion behavior in solution to explain and predict chemical behavior.

In this lesson, students analyze and interpret temperature and bond energy data to classify reactions as endothermic or exothermic. 

In this lesson, students construct explanations using particle diagrams and collision theory to describe how particle size, concentration, and temperature affect the rate of a chemical reaction.

In this lesson, students quantitatively apply the concepts of the mole and Avogadro’s number to calculate percent composition and determine empirical and molecular formulas of common compounds.

In this lesson, students use mathematical representations of the mole concept to solve reaction stoichiometry problems involving mole-to-mole, mass-to-mole, and mass-to-mass conversions and determine the limiting reactant both qualitatively and quantitatively when given reactant masses.

In this lesson, students develop and use models to illustrate solute-solvent interactions and explain how particle interactions in different types of solutions affect solution properties.

In this lesson, students use mathematics and computational thinking to express solution concentrations in terms of molarity and prepare solutions from solids or concentrated solutions based on a specified molarity and volume.

In this lesson, students analyze and interpret data to explain how temperature and pressure affect the solubility of solid and gaseous solutes and use mathematics and computational thinking to express solution concentrations in terms of molarity.

In this lesson, students design and conduct experiments to evaluate how solute concentration affects the colligative properties of a solution, such as freezing point depression and boiling point elevation. 

In this lesson, students obtain, evaluate, and communicate information about the properties of acids and bases while using the periodic table and computational thinking to derive their chemical formulas and names.

In this lesson, students use multiple models to predict the relative properties of strong, weak, concentrated, and dilute acids and bases. They apply mathematics to calculate pH, pOH, the hydroxide ion concentration, and the hydronium ion concentration for common solutions. 

In this lesson, students plan and carry out a strong acid–strong base titration to determine the concentration of an unknown acidic or basic solution.

In this lesson, students qualitatively and quantitatively relate changes in the temperature and pressure of a gas to particle motion and collision frequency to explain macroscopic gas properties.

In this lesson, students express the relationships among pressure, volume, temperature, and the number of moles of a gas quantitatively, conceptually, and graphically while using mathematics and computational thinking to solve gas stoichiometry problems involving mass, volume, and moles at standard temperature and pressure (STP).