Introductory Chemistry - CHM 101 at Southside Virginia Community College
https://courses.vccs.edu/colleges/svcc/courses/CHM101-IntroductoryChemistry
Effective: 2023-08-01
Course Description
Explores the experimental and theoretical concepts of general chemistry while emphasizing scientific reasoning, critical and analytical thinking. Designed for the non-science major. This is a Passport and UCGS transfer course.
Lecture 3 hours. Laboratory 3 hours. Total 6 hours per week.
4 credits
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