2: Properties of Matter and Energy

2.1: Describe how the nature of the interactions between atoms and molecules are reflected in physical and chemical properties of matter. Distinguish between different forms of matter. Compare and contrast chemical and physical changes and be able to predict when a chemical or physical change will occur.

Chemical Changes

3: Atomic and Molecular Structure

3.1: Describe the numbers and types of subatomic particulates and how they contribute to the structure of an atom. Describe the arrangement of the elements in the periodic table and use it to identify repeating patterns of physical and chemical properties of the atoms within it. Explain how these properties reflect the electronic structure of the atoms that make up the elements. Describe the process of radioactive decay and explain the concept of half-life for an isotope.

Electron Configuration
Nuclear Decay

4: Bonding

4.1: Describe how electronic structure determines the nature and extent of bonds between atoms and interactions between molecules. Compare and contrast formation of covalent, ionic and hydrogen bonds. Name and write chemical formulas for ionic and molecular compounds, and draw structural formulas for simple molecules and ionic compounds.

Chemical Equations
Covalent Bonds
Electron Configuration
Ionic Bonds

5: Reactions and Stoichiometry

5.1: Recognize and classify various types of chemical reactions. Interpret, write and balance chemical equations. Apply the law of conservation of mass in balancing chemical equations. Use the balanced chemical equation and the mole concept to determine the numbers of atoms, moles and molecules of the reactants and products. Determine empirical and molecular formulas and percent compositions.

Balancing Chemical Equations
Chemical Changes
Chemical Equations
Equilibrium and Concentration
Limiting Reactants

6: Kinetic Molecular Theory and States of Matter

6.1: Using the kinetic molecular theory, model the behavior of ideal gas molecules and describe what happens when matter in one phase undergoes transition into another phase. Use the ideal gas law to calculate measurable properties of gases, such as pressure and temperature. Use examples to describe how the speed at which gas particles move is proportional to the square root of the absolute temperature of the gas.

Phase Changes
Temperature and Particle Motion

7: Thermochemistry

7.1: Recognize that the reorganization of atoms in chemical reactions results in either the release (exothermic) or absorption (endothermic) of heat energy. Apply the law of conservation of energy by performing specific heat calculations and explaining heats of reaction, formation, combustion and enthalpy. Explain the importance of energy and entropy in chemical reactions and why systems tend to move in the direction of disorder or entropy.

Chemical Changes
Energy Conversion in a System

9: Acids, Bases and Salts

9.1: Compare and contrast the dissociation of acids, bases and salts in solution. Explain that when acids dissociate they donate hydrogen ions, and when bases dissociate they accept hydrogen ions or form hydroxide ions. Explain how the pH scale indicates the hydrogen ion concentration in a solution.

pH Analysis
pH Analysis: Quad Color Indicator

10: Organic Chemistry and Biochemistry

10.1: Use structural formulas to show that carbon atoms are unique due to their ability to bond to one another and to form up to four stable covalent bonds. Describe how this feature allows carbon to bond with a variety of atoms to form different molecules, ranging from simple hydrocarbons to complex polymers, which provide the biochemical basis of life.

Covalent Bonds

Correlation last revised: 5/11/2018

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