Course

Physical and Inorganic Chemistry

Important Notice

This course is not active. Please contact Department Chair for more information.

Faculty
Science & Technology
Department
Chemistry
Course code
CHEM 2410
Credits
5.00
Semester length
15
Max class size
18
Method(s) of instruction
Lecture
Lab
Typically offered
To be determined

Overview

Course description
This course investigates several topics in physical chemistry, including phase equilibria, spectroscopy, kinetics, and the thermodynamics of electrolyte solutions, and then applies the principles of thermodynamics and bonding to the study of coordination compounds. The laboratory stresses instrumental methods in inorganic chemistry.
Course content

Applications of Spectroscopy

Electromagnetic spectrum and molecular transitions; UV/Visible spectroscopy: instrumentation, use and limitations of Beer's Law; Infrared Spectroscopy: instrumentation, interpretation of spectra; NMR: theory and instrumentation, prediction and identification of spectra; atomic absorption; gas-liquid chromatography.

Phase Equilibria

One and two component systems, Gibbs phase rule, review of ideal solutions, tie-line rule, P vs X and boiling point diagrams for two liquid components, distillation, partially miscible pairs, binary phase diagrams for condensed phases.

Solutions of Electrolytes

Theories of strong and weak electrolytes, ionic strength, activity and activity coefficient; use of activities of electrolytes in pH and equilibrium calculations.

Chemical Kinetics - Elementary Reactions

Rate, rate law, half-life, integrated rate equation for zero, first, and second order reactions, determination of order, rate and activation energy; collision theory and transition state theory.

Chemical Kinetics - Composite Reaction Mechanisms

Parallel and consecutive reactions, steady-state treatment, rate-determining steps, equilibrium constants, free radical mechanisms, enzyme catalyzed reactions.

Coordination Compounds

Nomenclature, Werner Coordination Theory, bonding: Valence Bond Theory, Crystal Field Theory, Molecular Orbital Theory; isomerism, stability constants: factors effecting stability, determination of stability constants; kinetics and mechanisms of reactions of coordination complexes.

Laboratory Content

The following experiments will be performed during the laboratory period:

  1. Quantitative UV/Vis Spectroscopy
  2. Determination of Keto-Enol Equilibrium Constants by NMR
  3. Binary Solid-Liquid Phase Diagram
  4. Geometric Isomers of a Cr(III) Complex
  5. Gas Chromatography
  6. Kinetics of H2O2 Decomposition
  7. Kinetics of the Iodination of Acetone
  8. Preparation and Identification of Co(III) Complexes
  9. Paramagnetic Susceptibility: (a) Gouy Balance (b) NMR
  10. Inorganic Term Project
Learning activities

The course will be presented using lectures, classroom demonstrations, problem sessions and class discussions. Films and audio-visual materials will be used where appropriate. Problem sets will be assigned regularly to be handed in and marked. The laboratory consists of performance of ten experiments and a two-week inorganic chemistry project.

Means of assessment

Lecture Material (70%)

  • Three tests will be given, each worth 20%. These tests will cover (a) spectroscopy, phase equilibria, and electrolytes, (b) kinetics, and (c) coordination chemistry. The last of these tests will be given during the final examination period.
  • Problem assignments will be assigned on a regular basis (about seven) to be handed in and marked (10%).

Laboratory (30%)

  • The laboratory grade will be based on the written report (including accuracy of any experimentally obtained values) of each experiment performed (24%). The report for the inorganic project must be written in the style appropriate for submitting to a scientific journal (conforming to the ACS Style Guide) (6%).
Learning outcomes

With the aid of the relevant thermodynamic data, a periodic table, an equation sheet, and a calculator, the student will be able to:

  1. solve problems of the following general types:
    • interpretation of NMR, IR, and UV/VIS spectra
    • use of Beer-Lambert Law for systems containing one or two absorbing species
    • calculation of activities of strong electrolytes in solution.
    • use of activity coefficients in the calculation of pH, K, and Ksp.
    • calculations involving one or two component phase equilibria
    • calculation of the order and rate constant of a chemical reaction
    • calculation of the rate, amount of decomposition, and activation energy of a reaction
    • derivation of the rate law for a reaction given the mechanism
    • calculations involving use of the formation constants of a coordination compound.
  2. explain or define any of the terms used in the course
  3. compare the Collision and Transition State theories of chemical kinetics with the basic assumptions and interpretation of experimental rate data
  4. derive some of the simpler formulas used in the course (eg. integrated rate equations for zero, first, and simple second order reactions)
  5. given experimental data, draw and interpret the phase diagram for a two component system
  6. given the phase diagram of a two-component system, interpret the diagram (eg. what phases are present at a given T, and P, compound formation etc)
  7. give the systematic name of any coordination compound
  8. explain the bonding in coordination compounds using the Valence Bond Theory, the Crystal Field Theory, or the Molecular Orbital Theory.
  9. draw and name all of the possible isomers of a given coordination compound
  10. given the formulas of two coordination compounds, predict their relative kinetic and thermodynamic stabilities
  11. describe and explain the two limiting mechanisms for substitution in octahedral complexes.
Textbook materials

Textbooks and Materials to be Purchased by Students

  • Laidler, K.J.; Meiser, J.H. and Sanctuary, B.C. Physical Chemistry, 4rd Edition, Houghton Mifflin, Boston, New York, 2003
  • Douglas College, Chemistry 410 Laboratory Manual, 2000.
  • Basolo, F.; Johnson, R.C.; Coordination Chemistry; Science Reviews, 1986.

Requisites

Prerequisites

CHEM 1210 (C or better)

Corequisites

No corequisite courses.

Equivalencies

No equivalent courses.

Course Guidelines

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.

(Current)

Course Transfers

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 2410
There are no applicable transfer credits for this course.

Course Offerings

Winter 2025