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|Description - |
|The course includes basic chemical laboratory techniques and methods, a survey of important chemical principles with emphasis on problem solving, and a description of the elements and their compounds. Intended for students who wish to meet general education requirements in physical science or need background preparation for CHEM 1A.|
|Course Objectives - |
|The student will be able to: |
- understand the scientific method and distinguish between a theory and a scientific law.
- report the correct number of significant figures in measured and calculated quantities.
- use dimensional analysis to set up and solve numerical problems.
- classify matter and describe the properties of matter.
- understand and apply the fundamental assumptions of Dalton's atomic theory and describe the structure of the atom.
- use the periodic table to explain and predict the properties of elements.
- interpret chemical formulas and write the names and formulas for ionic compounds, molecular compounds, and acids.
- understand the meaning and uses of the mole and of Avogadro's number.
- write, balance, and classify chemical equations and recognize patterns of chemical reactivity to predict the products of a chemical reaction.
- perform stoichiometry calculations and understand the concept of a limiting reactant.
- understand the basis of the gas laws and derive the gas laws from the ideal gas law.
- describe the properties of solids and liquids and understand the manifestations of intermolecular forces.
- describe the properties of solutions and define and use molarity in calculations.
- desribe the properties of acids and bases and understand the basis of the pH scale.
|Special Facilities and/or Equipment - |
|A chemistry laboratory, safety goggles or Visorgogs, a scientific calculator, and a Mastering Chemistry access code for online homework. |
|Course Content (Body of knowledge) - |
- Introduction to Chemistry
- Chemistry in the modern world
- Scientific method
- Observations, hypotheses, experiments, theories, and scientific laws
- Mass, length, volume, and temperature
- SI and metric units
- Significant figures and scientific notation
- Problem Solving
- Conversion factors
- Dimensional analysis
- Classification and Properties of Matter
- Physical states of matter
- Pure substances and mixtures
- Physical and chemical properties
- Physical and chemical changes
- Energy, heat, and specific heat capacity
- Early Atomic Theory and Modern Atomic Structure
- Atoms and Dalton's atomic theory
- Subatomic particles and atomic structure
- Atomic number and mass number
- Isotopes and average atomic mass
- The Periodic Table
- Periods and groups
- Elemental symbols
- Metals, nonmetals, and metalloids
- Valence electrons and ion formation
- Composition and Nomenclature of Inorganic Compounds
- Law of definite proportions and law of multiple proportions
- Molecular compounds and molecules
- Ionic compounds and formula units
- Nomenclature of ionic and binary molecular compounds
- Nomenclature of common binary acids and oxyacids
- Quantitative Composition of Compounds
- The mole and Avogadro's number
- Molar mass
- Mass percent composition
- Empirical formulas
- Chemical Reactions
- Combination, decomposition, and single-, and double-displacement reactions
- Solubility of ionic compounds and aqueous reactions
- Exothermic and endothermic reactions
- Quantities in Chemical Reactions
- The concept of stoichiometry and mole ratios
- Mole-mole, mole-mass and mass-mass calculations
- Limiting reactants
- Theoretical yield and percent yield
- Kinetic molecular theory and properties of gases
- Boyle's law, Charles's law, and Avogadro's law
- The combined gas law and the ideal gas law
- Gas density and molar mass of a gas
- Gas stoichiometry
- Liquids and Solids
- Surface tension
- Evaporation and condensation
- Equilibrium vapor pressure and normal boiling point
- Heat of vaporization and heat of fusion
- Common types of solutions
- Solubility and saturation
- Dilution calculations
- Solution stoichiometry
- Acids and Bases
- Properties of acids and bases
- Arrhenius theory and dissociation versus ionization
- Br??nsted-Lowry theory and conjugate acid-base pairs
- Strength of acids and bases
- The pH scale and pH calculations
- Acid-base titration calculations
|Methods of Evaluation - |
- Online homework assignments
- Written laboratory assignments
- Lecture and laboratory quizzes
- Midterm exam
- Comprehensive final exam
|Representative Text(s) - |
- Tro, Nivaldo J., Introductory Chemistry, Essentials 3rd Edition, Pearson Prentice Hall, 2009.
- Signature Labs Series, Fundamentals of Chemistry: Chemistry 25, Custom Published Laboratory Manual, Cengage Learning, 2008
|Disciplines - |
|Method of Instruction - |
|Lecture, Laboratory, |
|Lab Content - |
- Determining Density
- Observe and record mass and volume data
- Explore whether density of a substance depends on sample size
- Determine the density of an unknown object and identify the composition using a provide list of substances
- Resolving a Two-Component Mixture
- Use physical separation methods including decantation, gravity filtration, evaporation, and extraction to separate and recover the components of a binary mixture
- Calculate the percent of each component in the mixture and percent recovery of the components
- Determining the Percent Water in an Unknown Hydrate
- Refine the proper use of a Bunsen burner
- Explore whether the percent water in a hydrate depends on sample size
- Calculate the theoretical percent water to evaluate the accuracy of the experimentally determined percent water
- Determining an Empirical Formula
- Determine an empirical formula from experimental data
- Experimentally evaluate the law of constant composition
- Deduce the impact of several theoretical procedural errors on the experimentally determined empirical formula
- Classifying some Chemical Reactions
- Effectively collaborate with a partner to perform series of chemical reactions and detail the observed results
- Use qualitative observations to predict the products of several chemical reactions and classify each reaction as one of four general types
- Introducing Chemical Equilibrium
- Evaluate the reversibility of several chemical reactions and apply the concepts of chemical equilibrium
- Experimentally evaluate Le Ch?¢telier's principle
- Subject reversible reactions to temperature changes and use the qualitative observations to classify each reaction as either exothermic or endothermic
- Determining the Molar Volume of Carbon Dioxide
- Apply the simple gas laws
- Evaluate the accuracy of the experimentally determined molar volume relative to the accepted value for an ideal gas
- Deduce the impact of several theoretical procedural errors on the experimentally determined molar volume
- Titrating the Acid Content of Fruit Juices
- Apply the concepts of pH and titration using a common household product
- Refine the proper use of a buret
|Types and/or Examples of Required Reading, Writing and Outside of Class Assignments - |
- Homework assignments
- There are 40-60 homework problems for each of the twelve chapters covered in this course, roughly half of which are completed and graded online.
- Laboratory assignments
- There are 8 experiments administered in this course during the weekly two-hour laboratory session for which a pre-laboratory assignment, a data sheet, a calculations sheet, and a post-laboratory assignment are all collected and graded by the instructor.
- Additional course work
- The careful and regular reading and rereading of the text and lecture notes is essential to passing this course.
- There are several practice worksheets provided by the instructor that showcase more challenging problems and may be completed in-class or as additional homework.