1. Introduction and Review
Scientific Measurements: Measurements, errors, precision and accuracy, uncertainty, significant figures.
Atoms, Molecules, and Ions: Isotopes, mole, formulas, percentage composition, nomenclature.
Stoichiometry Review: Determining oxidation states, balancing redox reactions, calculation of percentage yield, limiting reactant problems, solutions: concentration units and stoichiometry, titrations
2. Structure and bonding
Valence and core electrons, Lewis symbols for elements and ionic compounds, drawing Lewis structures, octet rule, bond length and strength, trends in electronegativity, non-polar and polar bonds and consequences of polar bonds on physical properties.
3. Principles of Reactivity: Thermochemistry
Energy units, heat capacity, energy transfer, enthalpy, calorimetry, phase changes, Hess’s Law, standard heats of formation.
4. Chemical Equilibrium
The equilibrium constant, interpretation of equilibrium constant values, calculations involving Kc, Le Chatelier’s Principle, controlling chemical reactions.
5. Gases and Liquids
Properties of gases, Ideal Gas equation, calculations, gas mixtures and Dalton’s Law of partial pressures.
6. Introduction to Acids and Bases
Properties, definitions, conjugate acid/base pairs, autoionization of water, pH scale, relative acid strengths, Ka and Kb, calculations, salts and hydrolysis, common ion effect.
Laboratory experiments will be selected from the following list and will be performed during the lab period:
- Analytical balance and metric conversions
- Density measurements
- Acid-Base Titrations
- Redox: Determination of Water of Hydration
- Chemical Equilibrium
- Molar Mass of Magnesium
- Ideal Gas Constant
- Redox: Water of hydration of Copper (II) Sulfate
- Acid Dissociation Constant
The course will be presented using lecture, problem sessions and class discussions. In-class demonstrations of computer-based educational materials and videos will be used where appropriate. The laboratory consists of experiments performed by students, either individually or in pairs, which illustrate the lecture material, or encourage good experimental technique. 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. Alternately, the course may be offered in a hybrid format in which some of the lecture material is replaced with online activities.
Evaluation will be carried out in accordance with Douglas College policy. The instructor will present a written course outline with specific evaluation criteria at the beginning of the semester.
Lecture Material (75%)
- Two or three in-class tests will be given during the semester (30% in total).
- A final exam covering the entire semester’s work will be given during the final examination period (30%).
- Any or all of the following evaluations, at the discretion of the instructor: problem assignments, quizzes, class participation (5% maximum). (15% in total)
- Written reports for each experiment which will be handed in on report sheets and graded. There will also be several written quizzes based on the procedure and theory of the various experiments.
- Quantitative results of experiments performed on unknown samples will be graded.
- A practical laboratory exam will be given in the last lab period of the semester.
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.
- Express the precision of a calculated quantity given the uncertainties in the measurements used in the calculation.
- Use significant figures in calculations.
- Given the mass of a substance, calculate the number of moles, and the number of particles in the sample.
- Given the percent composition of a compound and the molar mass, find the empirical and molecular formulas.
- Name ionic compounds, including those that involve polyatomic ions.
- Determine oxidation states and balance any redox reaction that occurs under acidic conditions.
- Given the balanced equation for a chemical reaction, carry out the required stoichiometric calculations. The substances in the reaction may be gases, solids, liquids, or solutions.
- Carry out calculations involving the ideal gas equation including density and molar mass.
- Define any of the terms used in the course, for example: mole, specific heat capacity, ideal gas, common ion effect, etc.
- Distinguish between core and valence electrons.
- Draw Lewis structures, explain how electronegativity difference results in polar bonds and the consequences of this polarity.
- Carry out thermochemical calculations based on data obtained in calorimetric measurements.
- Use thermochemical tables to calculate H° for a given chemical reaction.
- Use the Principle of Le Chatelier to predict the direction of change in a system in equilibrium as the result of a given change in temperature or change in concentration of the species in the system.
- Solve problems involving the use of the concentration equilibrium constant, Kc, for gaseous and aqueous systems.
- Write balanced equations for all reactions or equilibria involving acids and bases.
- Calculate the pH of a given solution of any strong acid or base.
- Calculate the pH of a solution of given concentration of a weak acid or base (or the salt of a weak acid or base).
Textbooks and Materials to be Purchased by Students
Textbook varies, please see the College Bookstore for the current requirement. The typical text is Principles of Chemistry by N. J. Tro or equivalent as selected by the department.
Chemistry1108 Laboratory Manual, Douglas College
CHEM 1104 (C or better) AND BC PRECALCULUS 11 (C or better) or equivalent
CHEM 11 (C or better) AND BC PRECALCULUS 11 (C or better) or equivalent
Courses listed here must be completed either prior to or simultaneously with this course:
- No corequisite courses
Courses listed here are equivalent to this course and cannot be taken for further credit:
- No equivalency courses
Course Guidelines for previous years are viewable by selecting the version desired. If you took this course and do not see a listing for the starting semester / year of the course, consider the previous version as the applicable version.
These are for current course guidelines only. For a full list of archived courses please see https://www.bctransferguide.ca
|Institution||Transfer Details for CHEM 1108|
|Alexander College (ALEX)||ALEX CHEM 100 (4)|
|Camosun College (CAMO)||CAMO CHEM 110 (4)|
|Capilano University (CAPU)||CAPU CHEM 101 (4)|
|Coast Mountain College (CMTN)||CMTN CHEM 1XX (3)|
|Kwantlen Polytechnic University (KPU)||KPU CHEM 1105 (4)|
|Langara College (LANG)||LANG CHEM 1118 (4)|
|Okanagan College (OC)||No credit|
|Simon Fraser University (SFU)||SFU CHEM 111 (4)|
|Thompson Rivers University (TRU)||TRU CHEM 1XXX (3)|
|Thompson Rivers University (TRU)||DOUG CHEM 1108 (4) & DOUG CHEM 1110 (4) = TRU CHEM 1500 (3) & TRU CHEM 1510 (3)|
|Trinity Western University (TWU)||TWU CHEM 1XX (3)|
|University of British Columbia - Okanagan (UBCO)||UBCO CHEM 1st (3)|
|University of British Columbia - Vancouver (UBCV)||UBCV CHEM 1st (3)|
|University of Northern BC (UNBC)||UNBC CHEM 1XX (3)|
|University of the Fraser Valley (UFV)||UFV CHEM 110 (4)|
|University of Victoria (UVIC)||No credit|
|Vancouver Island University (VIU)||No credit|