Effective: 2023-08-01

Course Description

The course outline below was developed as part of a statewide standardization process.

General Course Purpose

The course is designed primarily for non-science majors.

Course Objectives

• Scientific Literacy
• Apply the scientific method of inquiry to analyze data and draw conclusions supported by the data.
• Propose one or more solutions that indicate comprehension of a problem.
• Quantitative Literacy
• Apply mathematical reasoning and techniques in discipline specific ways (including, but not limited to, quantitative analysis of data).
• Matter and States of matter
• Classify matter as an element, compound, heterogeneous mixture or homogeneous mixture.
• Distinguish between physical and chemical properties/ changes.
• Apply kinetic molecular theory (conceptual) to explain/predict the characteristics and behavior of gases, solids and liquids.
• Calculate the pressure, volume or temperature of a gas after a change in conditions.
• Calculate the pressure, volume, temperature or moles of gas from the ideal gas equation.
• Identify and predict how intermolecular forces affect the physical properties of a specific substance.
• Describe the energy changes that accompany changes of state.
• Measurement and Laboratory techniques
• Identify basic units of measurement in the American and metric systems of measurement
• Convert measurements between American and/or metric units using dimensional analysis.
• Express any number in scientific notation.
• Identify the number of significant digits in a given measurement.
• Apply understanding of the inherent precision of laboratory glassware and equipment.
• Perform arithmetic operations, rounding to the correct number of significant digits.
• Calculate the density of a substance and use density to convert between mass and volume of a substance.
• Demonstrate basic laboratory techniques.
• Demonstrate best practices of laboratory safety.
• Atomic Structure and the Periodic Table
• Identify the regions of the Periodic Table related to metal, nonmetals and metalloids.
• Identify groups and periods of elements on the Periodic Table.
• State the charge, location and relative masses of an electron, proton and neutron.
• Write the electron configuration for selected elements.
• Count the valence electrons and draw the electron dot symbols for selected elements.
• Nuclear Chemistry
• Describe the characteristics of alpha, beta and gamma radiation.
• Write and balance nuclear equations.
• Relate the amount of radioactive sample to a given half-life.
• Identify safety issues and health effects associated with radiation exposure.
• Bonding and Nomenclature
• Using the periodic chart, predict the charge on an ion formed by a main group element.
• Draw the Lewis structure for a molecule or polyatomic ion and determine the shape by applying Valence Shell Electron Pair Repulsion (VSEPR) theory.
• Identify bonds and molecules as polar or nonpolar.
• Write names and formulas for ionic and covalent compounds.
• Chemical Reactions including Redox Reactions and Equilibrium
• Write and balance chemical equations.
• Calculate the molar mass of a substance, given its chemical formula.
• Convert between units of moles, mass and particles.
• Perform stoichiometry calculations including limiting reactant and theoretical yield calculations.
• Define oxidation and reduction and recognize the components of a redox reaction.
• Describe energy changes in a reaction and classify reactions as endothermic or exothermic.
• Predict the effect of changes in concentration, temperature and catalyst on reaction rates.
• Use Le Chatelier's principle (conceptual) to predict what happens when equilibrium is disturbed.
• Use the value of the equilibrium constant to qualitatively describe a reaction system.
• Solutions
• Predict how specific changes will affect the solubility of a solute.
• Determine whether a species is soluble or insoluble in a given solvent using solubility rules.
• State whether a solution is saturated, unsaturated, or supersaturated, given its concentration, temperature, and solubility.
• Determine whether solute would be an electrolyte and distinguish between a strong vs weak electrolyte in aqueous solution.
• Perform calculations involving percent concentration and molarity of a solution and dilution of a solution.
• Qualitatively explain colligative properties, osmosis, boiling and melting point of a solution.
• Acid-Bases
• List/identify general properties of acids and bases.
• Classify a solution of given pH as strongly acidic, weakly acidic, neutral, weakly basic, or strongly basic.
• Identify the Br?nsted-Lowry acid and base in a given reaction.
• Convert between pH, [H3O+] ([H+]) and [OH-].
• Identify conjugate acid/base pairs.
• Understand how a buffer works to resist pH changes.

Major Topics to be Included

• Matter and States of matter
• Measurement and Laboratory techniques
• Atomic Structure and the Periodic Table
• Nuclear Chemistry
• Bonding and Nomenclature
• Chemical Reactions including Redox Reactions and Equilibrium
• Solutions
• Acid-Bases