C.1: Properties and States of Matter

C.1.2: Observe and describe chemical and physical properties of different types of matter and designate them as either extensive or intensive.

 Density Experiment: Slice and Dice
 Density Laboratory

C.1.3: Recognize observable indicators of chemical changes.

 Chemical Changes
 Identifying Nutrients

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

 Density Laboratory

C.2: Atomic Structure and the Periodic Table

C.2.1: Describe how models of atomic structure changed over time based on available experimental evidence and understand the current model of atomic structure.

 Bohr Model of Hydrogen
 Bohr Model: Introduction

C.2.2: Describe how the subatomic particles (i.e., protons, neutrons and electrons) contribute to the structure of an atom and recognize that the particles within the nucleus are held together against the electrical repulsion of the protons.

 Element Builder

C.2.9: Understand that the radioactive decay process is random for any given atom but that this property leads to a predictable and measurable exponential decay of a sample of radioactive material. Know how to calculate the initial amount, the fraction remaining or the half-life of a radioactive isotope when given two of the other three variables.

 Half-life

C.2.3: Determine the number of protons, neutrons, and electrons in isotopes and in those isotopes that comprise a specific element. Relate these numbers to atomic number and mass number.

 Element Builder

C.2.4: Calculate the average atomic mass of an element from isotopic abundance data.

 Element Builder

C.2.5: Write the electron configuration of an element and relate this to its position on the periodic table.

 Electron Configuration

C.2.6: Use the periodic table and electron configuration to determine an element's number of valence electrons and its chemical and physical properties.

 Electron Configuration
 Element Builder

C.3: Bonding and Molecular Structure

C.3.1: Describe, compare and contrast the characteristics of the interactions between atoms in ionic and covalent compounds.

 Covalent Bonds
 Ionic Bonds

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

 Covalent Bonds
 Ionic Bonds

C.4: Reactions and Stoichiometry

C.4.1: Predict products of simple reactions such as synthesis, decomposition, single replacement and double replacement.

 Equilibrium and Concentration

C.4.2: Balance chemical equations using the law of conservation of mass and use them to describe chemical reactions.

 Balancing Chemical Equations
 Chemical Equations

C.4.3: Given mass of the sample, use the mole concept to determine the number of moles and number of atoms or molecules in samples of elements and compounds.

 Chemical Equations

C.4.4: Using a balanced chemical equation, calculate the quantities of reactants needed and products made in a chemical reaction that goes to completion.

 Balancing Chemical Equations
 Chemical Equations

C.4.5: Describe, classify and give examples of various kids of reactions-synthesis (i.e., combination), decomposition, single displacement, double displacement and combustion.

 Chemical Changes

C.4.7: Perform calculations to determine the composition of a compound or mixture when given the formula.

 Chemical Equations

C.5: Behavior of Gases

C.5.1: Use kinetic molecular theory to explain changes in gas volumes, pressure, moles and temperature.

 Temperature and Particle Motion

C.5.2: Using the ideal gas equation of state PV = nRT, calculate the change in one variable when another variable is changed and the others are held constant.

 Boyle's Law and Charles' Law

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: Solve problems involving heat flow and temperature changes by using known values of specific heat, phase change constants (i.e., latent heat values) or both.

 Phase Changes

C.7: Solutions

C.7.5: Explain how the rate of a reaction is qualitatively affected by changes in concentration, temperature, surface area and the use of a catalyst.

 Collision Theory

C.7.6: Write equilibrium expressions for reversible reactions.

 Equilibrium and Concentration
 Equilibrium and Pressure

C.8: Acids and Bases

C.8.1: Use Arrhenius and Brønsted-Lowry definitions to classify substances as acids or bases.

 pH Analysis
 pH Analysis: Quad Color Indicator

C.8.2: Describe the characteristic properties of acids and bases.

 pH Analysis
 pH Analysis: Quad Color Indicator

C.8.5: From acid-base titration data, calculate the concentration of an unknown solution.

 Titration

C.9: Organic Chemistry and Biochemistry

C.9.1: Use structural formulas to illustrate carbon atomsÂ? ability to bond covalently to one another to form many different substances.

 Covalent Bonds
 Ionic Bonds

Correlation last revised: 5/11/2018

This correlation lists the recommended Gizmos for this state's curriculum standards. Click any Gizmo title below for more information.