Course Description
This course is a general survey of first-year chemistry designed for students in applied science. Topics include a brief review of stoichiometry and the treatment of experimental data, the modern view of atomic structure, theories of bonding and molecular structure, liquids, solids, solutions, electrochemistry, the laws of thermodynamics, equilibrium, and acids and bases. A practical laboratory component is an integral part of the course.
Course Content
- Review: Reaction stoichiometry, chemical reactions and solution chemistry, gas pressure, ideal gas law, partial pressure and Dalton’s law
- Atomic Structure: Quantum numbers, orbital shapes, sizes and energies, electronic configurations, periodic properties
- Bonding and Molecular Structure: Ionic bonding, covalent bonding; Lewis structures: electronegativity, polarity, resonance; VSEPR theory and molecule shapes; Molecular Orbital Theory of hydrogen: shapes and energies of molecular orbitals, bond order
- Intermolecular Forces: Dipole-dipole forces, London dispersion forces and hydrogen bonding
- Liquids and Solids: Simple phase diagrams, melting point, boiling point, phase changes such as evaporation, condensation and sublimation
- Equilibrium: Equilibrium constant, direction of chemical reactions, applications of equilibrium constant, Le Chatalier’s principle, acid-base theories, acid-base equilibria, pH
- Thermodynamics: Basic concepts of thermochemistry, heat capacity, First Law of Thermodynamics, calorimetry, enthalpy, Hess’s Law, standard enthalpies of formation, entropy, standard molar entropies, Third Law, Second Law and derivation of Gibbs free energy, standard free energies of formation, free energy and spontaneity, relationship between free energy and equilibrium, thermodynamic equilibrium constants, temperature dependence of equilibrium constants
- Kinetics: Basic factors affecting reaction rates, concept and definitions of chemical reaction rates, differential rate law and rate constant
- Electrochemistry: Nernst equation, electrochemical cells, relationship between Ecell and delta G and K, oxidation and reduction, cell potential, simple batteries
Laboratory Content
Laboratory experiments will be similar to ones included in the following list and will be performed during the lab period:
- Laboratory Safety
- Volumetric Techniques: A Review of Titration
- Recycling Aluminum
- Atomic Spectra
- Oxidation/Reduction Analysis
- Thermochemistry
- Equilibria
- pH and Indicators
- Electrochemistry
- Acids and Bases
- Spectrophotometric Determinations
- Synthesis Lab
- Lab Project
Learning Activities
The course will be presented using lectures, problem sessions and class discussions. Videos and other audio-visual aids, as well as programmed material, will be used where appropriate. Problems will be assigned on a regular basis. The laboratory period will be used to illustrate the practical aspects of the course material.
Close coordination will be maintained between laboratory and classroom work whenever possible. This will be accomplished by discussing laboratory experiments in class and, when necessary, by using the lab period for problem solving.
Means of Assessment
Evaluation will be carried out in accordance with the Douglas College Evaluation Policy. The instructor will present a written course outline with specific evaluation criteria at the beginning of the semester. Evaluation will be based on the following criteria:
Lecture Material (75%)
- One or more in-class tests will be given during the semester (20-30% in total)
- A final exam covering the entire semester’s work will be given during the final examination period (30% in total)
- Any or all of the following evaluations at the discretion of the instructor: assignments, quizzes, class participation (5% maximum), presentations, research assignments, group work (15-25% in total)
Laboratory (25%)
Written reports for each experiment or activity will be handed in and graded. These reports may be of various types: complete reports, short reports (handed in on report sheets) or written research assignments. In addition, pre-lab activities, such as written quizzes or online assignments, may be evaluated. Qualitative and quantitative results of experiments performed on unknown samples may be graded.
Note:
- A student who misses three or more laboratory experiments will earn a maximum P grade.
- A student who achieves less than 50% in either the lecture or laboratory portion of the course will earn a maximum P grade.
Learning Outcomes
Upon completion of this course, the successful student should be able to:
- Carry out measurements using the correct number of significant figures, and demonstrate an understanding of precision and accuracy.
- Carry out calculations involving the ideal gas equation.
- Solve stoichiometry problems of the following types: gram-gram or gram-volume (of a gas), solution stoichiometry, limiting reactant, problems involving two simultaneous or two sequential reactions.
- Explain the Bohr Theory of atomic structure.
- Provide the electronic configuration of any of the common elements in the periodic table.
- Determine relative sizes, ionization energies, and electron affinities of elements using the periodic table.
- Explain and apply the concepts of dipole moment and electronegativity to covalent bonds.
- Draw Lewis structures for a given molecule, including those exhibiting resonance or expanded valence shells.
- Use the VSEPR theory to predict the geometry of any polyatomic molecule.
- Use the Molecular Orbital Theory of bonding to describe the bonding in any diatomic molecule involving hydrogen atoms.
- Predict the most likely intermolecular forces present in a bulk sample of a compound.
- Predict trends in boiling point and heat of vaporization among a group of two or more compounds.
- Determine whether chemical reactions will occur spontaneously under standard conditions by using a table of standard electrode potentials.
- Determine the relative strengths of oxidizing agents or reducing agents by using a table of standard electrode potentials.
- Distinguish between various types of heats of reaction and write the corresponding chemical equation.
- Interpret the signs of enthalpy changes.
- Describe both qualitatively and quantitatively the contributions of delta H and delta S to reaction spontaneity.
- Predict the sign of delta S for various chemical and physical processes.
- Interpret equilibrium in terms of thermodynamic driving forces.
- Write the chemical equation for equilibrium involving weak acids and bases in aqueous solution.
- Define any of the chemical terms or describe any of the chemical processes used in the course (e.g. anode, state function)
- Solve problems of the following types:
- Determination of the amount of material produced in an electrolytic cell;
- Calculation of the E.M.F of a galvanic cell;
- Calculation of delta G from electrochemical data;
- Calculations involving the First Law of Thermodynamics;
- Calculation of enthalpy change in a chemical or physical process;
- Calculation of any quantity in a Hess’s Law equation;
- Calculation of delta S from absolute entropies;
- Calculation of delta G for a chemical reaction;
- Calculation of K from delta G°;
- Calculation of quantities relating to aqueous acid-base equilibria (e.g. pH, weak acid ionization constant) and;
- Determination of the order and rate law of a chemical reaction.
Laboratory Objectives:
- State the name and describe the use of common laboratory equipment.
- Accurately perform standard laboratory procedures, such as titration, weighing, pipetting, using accepted methods and techniques.
- Identify the random and systematic errors inherent in common quantitative techniques used in the laboratory.
- Write a report based on observations and data obtained in the laboratory using a standard report format.
- Apply appropriate mathematical techniques (e.g. graphical analysis, solution of equations, etc.) to obtain a numerical result when given a set of experimental data (obtained in the laboratory or otherwise).
- Determine the relationship between experimental variables using the data, observations or results of an experiment.
- Identify the theory upon which an experiment is based.
Textbook Materials
Consult the Douglas College Bookstore for the latest required textbooks and materials. Example textbooks and materials may include:
Chemistry, A Molecular Approach by Tro, Fridgen and Shaw, current edition
Chemistry 1150 Laboratory Manual, Douglas College