C.1: Properties and States of Matter

C.1.3: Recognize observable macroscopic indicators of chemical changes.

Chemical Changes

C.1.6: Demonstrate an understanding of the law of conservation of mass through the use of particle diagrams and mathematical models.

Chemical Changes
Chemical Equations

C.1.7: Perform calculations involving density and distinguish among materials based on densities.

Density Experiment: Slice and Dice
Density Laboratory

C.2: Atomic Structure and the Periodic Table

C.2.1: Using available experimental data, explain how and why models of atomic structure have changed over time.

Bohr Model of Hydrogen
Bohr Model: Introduction

C.2.3: Write the full and noble gas electron configuration of an element, determine its valence electrons, and relate this to its position on the periodic table.

Electron Configuration

C.2.4: Use the periodic table as a model to predict the relative properties of elements based on the pattern of valence electrons and periodic trends.

Electron Configuration

C.2.6: Describe nuclear changes in matter, including fission, fusion, transmutations, and decays.

Nuclear Decay

C.2.7: Perform half-life calculations when given the appropriate information about the isotope.

Half-life

C.3: Bonding and Molecular Structure

C.3.2: Compare and contrast how ionic and covalent compounds form.

Ionic Bonds

C.3.5: Use laboratory observations and data to compare and contrast ionic, covalent, network, metallic, polar, and non-polar substances with respect to constituent particles, strength of bonds, melting, and boiling points and conductivity; provide examples of each type.

Circuit Builder

C.4: Reactions and Stoichiometry

C.4.1: Describe, classify, and give examples of various kinds of reactions: synthesis (i.e., combination), decomposition, single displacement, double displacement, acid/base, and combustion.

Balancing Chemical Equations
Chemical Equations
Dehydration Synthesis
Equilibrium and Concentration
Titration

C.4.4: Apply the mole concept to determine the mass, moles, number of particles, or volume of a gas at STP, in any given sample, for an element or compound.

Chemical Equations
Limiting Reactants
Stoichiometry

C.4.5: Use a balanced chemical equation to calculate the quantities of reactants needed and products made in a chemical reaction that goes to completion.

Chemical Equations
Limiting Reactants
Stoichiometry

C.5: Behavior of Gases

C.5.1: Use the kinetic molecular theory with the combined and ideal gas laws to explain changes in volume, pressure, moles, and temperature of a gas.

Temperature and Particle Motion

C.6: Thermochemistry

C.6.1: Explain that atoms and molecules are in constant motion and that this motion increases as thermal energy increases.

Temperature and Particle Motion

C.6.2: Distinguish between the concepts of temperature and heat flow in macroscopic and microscopic terms.

Calorimetry Lab

C.6.4: Perform calculations involving heat flow, temperature changes, and phase changes by using known values of specific heat, phase change constants, or both.

Calorimetry Lab
Energy Conversion in a System
Phase Changes

C.8: Acids and Bases

C.8.1: Classify solutions as acids or bases and describe their characteristic properties.

pH Analysis
pH Analysis: Quad Color Indicator