1: Matter and Its Interactions

1: Obtain and communicate information from historical experiments (e.g., work by Mendeleev and Moseley, Rutherford’s gold foil experiment, Thomson’s cathode ray experiment, Millikan’s oil drop experiment, Bohr’s interpretation of bright line spectra) to determine the structure and function of an atom and to analyze the patterns represented in the periodic table.

Bohr Model of Hydrogen

2: Develop and use models of atomic nuclei to explain why the abundance-weighted average of isotopes of an element yields the published atomic mass.

Element Builder

3: Use the periodic table as a systematic representation to predict properties of elements based on their valence electron arrangement.

Electron Configuration
Element Builder
Periodic Trends

3.a: Analyze data such as physical properties to explain periodic trends of the elements, including metal/nonmetal/metalloid behavior, electrical/heat conductivity, electronegativity and electron affinity, ionization energy, and atomic-covalent/ionic radii and how they relate to position in the periodic table.

Electron Configuration
Element Builder
Periodic Trends

3.b: Develop and use models (e.g., Lewis dot, 3-D ball-and-stick, space-filling, valence-shell electron-pair repulsion [VSEPR]) to predict the type of bonding and shape of simple compounds.

Electron Configuration
Element Builder
Periodic Trends

3.c: Use the periodic table as a model to derive formulas and names of ionic and covalent compounds.

Covalent Bonds
Ionic Bonds

5: Plan and conduct investigations to demonstrate different types of simple chemical reactions based on valence electron arrangements of the reactants and determine the quantity of products and reactants.

Covalent Bonds
Ionic Bonds
Periodic Trends

5.a: Use mathematics and computational thinking to represent the ratio of reactants and products in terms of masses, molecules and moles.

Chemical Equations
Limiting Reactants
Stoichiometry

5.b: Use mathematics and computational thinking to support the claim that atoms, and therefore mass, are conserved during a chemical reaction.

Balancing Chemical Equations
Chemical Changes
Chemical Equations
Moles
Stoichiometry

6: Use mathematics and computational thinking to express the concentrations of solutions quantitatively using molarity.

6.b: Analyze and interpret data to explain effects of temperature on the solubility of solid, liquid, and gaseous solutes in a solvent and the effects of pressure on the solubility of gaseous solutes.

Solubility and Temperature

8: Refine the design of a given chemical system to illustrate how LeChâtelier’s principle affects a dynamic chemical equilibrium when subjected to an outside stress (e.g., heating and cooling a saturated sugar-water solution).

Equilibrium and Concentration
Equilibrium and Pressure

2: Motion and Stability: Forces and Interactions

9: Analyze and interpret data (e.g., melting point, boiling point, solubility, phase-change diagrams) to compare the strength of intermolecular forces and how these forces affect physical properties and changes.

Melting Points
Polarity and Intermolecular Forces

3: Energy

10: Plan and conduct experiments that demonstrate how changes in a system (e.g., phase changes, pressure of a gas) validate the kinetic molecular theory.

Boyle's Law and Charles's Law
Energy Conversion in a System
Energy of a Pendulum
Inclined Plane - Sliding Objects
Potential Energy on Shelves

11: Construct an explanation that describes how the release or absorption of energy from a system depends upon changes in the components of the system.

Energy Conversion in a System
Energy of a Pendulum
Inclined Plane - Rolling Objects
Inclined Plane - Simple Machine
Inclined Plane - Sliding Objects

11.a: Develop a model to illustrate how the changes in total bond energy determine whether a chemical reaction is endothermic or exothermic.

Feel the Heat
Reaction Energy

11.b: Plan and conduct an investigation that demonstrates the transfer of thermal energy in a closed system (e.g., using heat capacities of two components of differing temperatures).

Calorimetry Lab
Conduction and Convection
Heat Transfer by Conduction