CH 121 College Chemistry 1

Lecture Hours: 3
Lab Hours: 2
Credits: 5

Introduces the fundamentals of chemistry for students majoring in fields other than chemistry. Examines the interrelationships of chemistry to all disciplines of science. Covers scientific method, atomic theory, stoichiometry, energy, periodicity, atomic structure, and bonding. First of a three term sequence.

Prerequisite: Placement into WR 115 (or higher), or completion of WR 090 (or higher); and placement into MTH 111Z (or higher), or completion of MTH 095 (or higher, except MTH 098 and MTH 105Z); or consent of instructor. (All prerequisite courses must be completed with a grade of C or better.)
Student Learning Outcomes:

Describe chemical reactions and chemical change.
Define matter and energy and discuss the properties of matter.
Differentiate between elements, compounds and mixtures.
Interpret chemical symbols, formulae and equations.
Apply the scientific method.
Utilize the metric and international systems of measurement.
Utilize significant figures and scientific notation.
Use the factors label method for calculations.
Calculate density and specific gravity.
Name inorganic compounds.
Differentiate between metals, non-metals, and metalloids.
Describe substances by means of chemical and physical properties.
Identify the subatomic particles; proton, neutron and electron.
Describe the Bohr atomic theory.
Predict electronic configuration.
Determine atomic and ionic sizes.
Describe ionization energy and electron affinity.
Describe ionic and covalent bonding.
Draw Lewis structures.
Explain coordinate covalent bonding.
Describe polar bonds and electronegativity.
Use the periodic table.
State Dalton’s atomic theory and the laws of chemical combination.
Calculate formula and molecular weights.
Define and apply the mole and molar concepts.
Determine empirical and molecular formulas.
Utilize percentage composition.
Balance equations.
Discuss stoichiometry.
Perform stoichiometric calculations.
Determine percentage yield and limiting reactants.
Describe energy and its sources and units.
Calculate specific heat and heat capacity.

Additional General Education Outcomes

Gather, comprehend, and communicate scientific and technical information in order to explore ideas, models, and solutions and generate further questions.

Apply scientific and technical modes of inquiry, individually, and collaboratively, to critically evaluate existing or alternative explanations, solve problems, and make evidence-based decisions in an ethical manner.

Assess the strengths and weaknesses of scientific studies and critically examine the influence of scientific and technical knowledge on human society and the environment.

Content Outline

Introduction
- Nature and the history of chemistry
- Branches of chemistry and relationship to other sciences
- Scientific method and study skills development
Standards for Measurement
- Mass and weight
- Scientific notation, significant figures and rounding
- The metric system
- Mass, length, and volume
- Heat and temperature measurements
- Density and specific gravity
Properties of Matter
- Matter defined
- Substances, mixtures and their properties
- Physical and chemical changes
- Laws of conservation of mass and energy
Elements and Compounds
- Elements, names, and symbols
- Compounds and their formulae
- Mixtures
- Metals, non-metals, metalloids
- Chemical equations and nomenclature
Atomic Theory and Structure
- Dalton’s atomic theory
- The nuclear atom and the subatomic particles
- Energy levels and sub-levels
- Atomic numbers and electron configuration
- Electron dots and the octet rule
- Atomic weight and the mole
The Periodic Arrangement of the Elements
- Periodic law and arrangement of the periodic table
- Periods and groups
- Group nomenclature
- Predicting formulae by use of the periodic table
Chemical Bonds
- Chemical bonds: ionic and covalent
- Electronegativity
- Lewis electron dot structures
- Polyatomic ions
- Oxidation numbers
Nomenclature of Inorganic Compounds
- Common names
- Systematic nomenclature
- Binary and ternary compounds
- Complex salts and bases
Quantitative Composition of Compounds
- Formula and molecular weights
- Gram-formula weight and the mole
- Percent composition of compounds
- Empirical and molecular formulae
Chemical Equations
- The chemical equations
- Writing and balancing chemical equations
- Information from equations
- Types of chemical equations
- Heat in chemical equations
Calculations from Chemical Equations
- Review
- The mole method
- Mole-mole calculations
- Mole-mass calculations
- Limiting reagents

Laboratory Outline and Objectives:

Laboratory Technique and Glass Blowing lab
- Safety procedures
- Indoctrination
- Selection of laboratory equipment
- Laboratory techniques
  - Glass working
  - The laboratory burner
  - Evaporation
  - Filtration
Densities lab
- - - Measurements
The metric system
Mass, length, volume
- Temperature
  - 3 . Density and specific gravity
Separation of Mixture lab
- Physical vs. chemical properties
- Melting points and boiling points
- Solubilities
Oxygen and Hydrogen lab
- Preparation of Oxygen
  - Generation of oxygen from KClO3
  - Properties of oxygen
  - Reactions of metals and nonmetals with oxygen
- Preparation of Hydrogen
  - Methods of preparation
  - Collection of hydrogen
  - Reactions with hydrogen
Atomic spectra lab
- Atomic fingerprints
- Chemical Periodicity
  - Patterns in the periodic table
  - Group characteristics
  - Predictions of “new” elements
- Trends and relationships in the periodic table
Molecular Models lab
- Covalent Bonding
- Lewis dot structures, two & three dimensional structures 
- Bond angles
- Resonance structures
Naming Ionic and Covalent Compounds lab
- Structure of Compounds
  - Formation of compounds
  - Properties of compounds
Formula of a Hydrate lab
- Qualitative determination of water
- Quantitative determination of water in a hydrate
Identification of a Compound -Analyzing liquids based on their b.p. and density
- Physical vs. chemical properties
- Melting points and boiling points
- Solubilities
- Combustion
Silver analysis lab
- Quantitative determination of silver ion in solution
- Single displacement reactions
  - Reactivity
  - Determining reaction factors
  - Balancing the single- displacement equation
- Relationship of Mole Ratios in chemical reactions
Inorganic Synthesis-limiting reagents and filtering using a Buchner funnel
- Limiting reagents
- Cold temperature synthesis
- Using gases as reactants
- Use of the Buchner funnel
- Recrystallization from a solvent

Required Texbook for college credit: Open Stax Chemistry 2e. ISBN 978-1-947172-62-3