Posted: Tue, 03/22/2016 - 1:53pm Updated: Tue, 12/08/2020 - 7:56am

This Teacher Resource Guide has been developed to provide supporting materials to help educators successfully implement the Indiana Academic Standards for Science. These resources are provided to help you in your work to ensure all students meet the rigorous learning expectations set by the Academic Standards. Use of these resources is optional – teachers should decide which resource will work best in their school for their students.

The resources, clarifying statements, and vocabulary provided are for illustrative purposes only, to promote a base of clarity and common understanding. Each item illustrates a standard but please note that the resources, clarifying statements, and vocabulary are not intended to limit interpretation or classroom applications of the standards.

The links compiled and posted in this Resource Guide have been provided by classroom teachers, the Department of Education, and other sources. The DOE has not attempted to evaluate any posted materials. They are offered as samples for your reference only and are not intended to represent the best or only approach to any particular issue. The DOE does not control or guarantee the accuracy, relevance, timeliness, or completeness of information contained on a linked website; does not endorse the views expressed or services offered by the sponsor of a linked website; and cannot authorize the use of copyrighted materials contained in linked websites. Users must request such authorization from the sponsor of the linked website.

Standard Specific Resource/Activity for the Standard
Standard 1: Properties and States of Matter  
C.1.1 Differentiate between pure substances and mixtures based on physical and chemical properties.

Quizlet Pure Substances

C.1.2 Use chemical properties, extensive, and intensive physical properties to identify substances.  
C.1.3 Recognize observable macroscopic indicators of chemical changes.


Chemical Reactions

C.1.4 Describe physical and chemical changes at the particle level.  
C.1.5 Describe the characteristics of solids, liquids, and gases and changes in state at the macroscopic and microscopic levels.

States of Matter PBS

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

Reactants Products and Leftovers

C.1.7 Perform calculations involving density and distinguish among materials based on densities.  
Standard 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. Atomic models: Resource 1
C.2.2 Determine the number of protons, neutrons, and electrons in isotopes and calculate the average atomic mass from isotopic abundance data.

Build an atom


Chemistry interactive atom

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.  
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.

Octet Rule Song - YouTube

Periodic Table Trends

C.2.5 Compare and contrast nuclear reactions with chemical reactions



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

Nuclear fission

C.2.7 Perform half-life calculations when given the appropriate information about the isotope. Radioactive decay: Resource 1
Standard 3: Bonding and Molecular Structure
C.3.1 Investigate the observable characteristics of elements, ionic, and covalent compounds.


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

Octet Rule Video and Quiz

C.3.3 Draw structural formulas for simple molecules and determine their molecular shape.

VSPER theory

Molecular Geometry simulation

C.3.4 Write chemical formulas for ionic compounds and covalent compounds given their names and vice versa. Ionic Formula Naming (Who wants to be a millionaire?)
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.  
C.3.6 Use structural formulas of hydrocarbons to illustrate carbon's ability to form single and multiple bonds within a molecule.  
Standard 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. Chemical equations. Resource 1, Resource 2, Resource 3, Resource 4
C.4.2 Predict products of simple reactions as listed in C.4.1.


C.4.3 Balance chemical equations and use the law of conservation of mass to explain why this must be true.

Balancing Chemical Equations

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. Mole Calculations: Resource 1
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.

Balancing Chemical Equations

C.4.6 Perform calculations to determine the composition of a compound or mixture when given the necessary information.


C.4.7 Apply lab data to determine the empirical and molecular formula of a compound.

Formula Lab

Standard 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. Kinetic Molecular Theory: Resource 1
C.5.2 Apply the ideal gas equation (PV = nRT) to calculate the change in one variable when another variable is changed and the others are held constant. Gas Laws: Resource 1, Resource 2, Resource 4, Gas Laws Unit
C.5.3 Use lab data and a balanced chemical equation to calculate volume of a gas at STP and non STP conditions, assuming that the reaction goes to completion and the ideal gas law holds.

Gas Properties

Standard 6: Thermochemistry
C.6.1 Explain that atoms and molecules are in constant motion and that this motion increases as thermal energy increases.


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

Heat and Thermodynamics

C.6.3 Classify chemical reactions and phase changes as exothermic or endothermic based on enthalpy values. Use a graphical representation to illustrate the energy changes involved



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.

Specific Heat Capacity

Enthalpy Lab

Standard 7: Solutions
C.7.1 Describe the composition and properties of solutions. Solutions/molarity: Resource 3, Resource 4, Resource 5
C.7.2 Explain how temperature, pressure, and polarity of the solvent affect the solubility of a solute.

Concentration phet

C.7.3 Describe the concentration of solutes in a solution in terms of molarity. Perform calculations using molarity, mass, and volume. Prepare a sample of given molarity provided a known solute.

Molarity phet

Standard 8: Acids and Bases
C.8.1 Classify solutions as acids or bases and describe their characteristic properties.

Acid Base Activity

C.8.2 Compare and contrast the strength of acids and bases in solutions.

Acid Base Solutions phet

Acid Base Lab

C.8.3 Given the hydronium ion and/or the hydroxide ion concentration, calculate the pH and/or the pOH of a solution. Explain the meanings of these values.

Acid Base Solutions phet

Possible Websites for Science: