Recommended Textbooks:

• "Chemistry for Changing Times", 10th edition by J.W. Hill & D.K. Kolb.

• Note: Much material from other sources is used, and the book will not be followed closely. Reading a textbook is highly recommended especially for students who have never taken a Chemistry course. Books used in previous years are adequate substitutes.

Sheets:

• Sheets with structures and tables handed out in class may be required for several lectures. You must bring these sheets to class; lectures cannot be understood without them.

Review Sheets:

• Review sheets with questions will be handed out. Some questions on the midterm and final exam will be taken from these sheets, so work through them. You should also work through old exams that are available from the Science Students' Association :Online Examinations.

Grading:

• Mid-term test 1 - TBA 75 min during lecture slot. -------------------------- 25%
• Mid-term test 2 - TBA 75 min during lecture s lot. ------------------------- 25%
• Final Exam 2 Hours. Scheduled by Student Records ---------------------- 50%

The Frank & Donna Hruska Prize:

• My wife & I have set up a scholarship fund (The Frank & Donna Hruska Prize) which awards a seventy-five dollar prize to the student receiving the top grade in 2.100, and a 2nd prize of the same amount to the top student in 2.103, the sequel to 2.100. This award will appear on the winner's university transcript.

Important information in the 'General Calendar':

• Students are reminded that they must remain available until all examination and test obligations are fulfilled. This examination has been held as late as Dec 21.

• Deaths in the immediate family and illness are the only valid reasons for missing tests and exams. A medical certificate must be provided as proof of illness. If the midterm is missed, the final exam will be valued at 75% towards the student's final grade.

QUIRKS & QUARKS:

Quirks and Quarks is a CBC radio program on Saturdays (12:05-1:00 pm) which provides interesting discussions of current issues in chemistry, astronomy, medicine, genetics, the environment, etc, etc. Listen to this informative program while you are eating lunch. You will hear ideas that should impress your colleagues - and professors - the following week.

TOPICS

1. Usefulness of chemistry and the problems it creates. Matter: Substances (elements and compounds) and mixtures of substances. Composition and structure of substances. Physical and chemical properties and changes. Observations and Measurements. Elements and atoms of the ancients.

1. Names and symbols of the elements. The Periodic Table.
2. General features of the Periodic Table: A) States of matter: solids, liquids and gases. States of the elements. Melting points and boiling points. Behaviour of particles in solids, liquids and gases. Refrigerators and air conditioners. B) Metals, nonmetals and metalloids. Density. C) Elemental composition of our bodies. D) Elemental composition of the Earth's crust. E) Etymology of the names of elements.

1. Introduction: A) Mass, weight and gravity. B) Electricity and magnetism. Static electricity. Benjamin Franklin, Humphrey Davy, Mary Shelley and Frankenstein.
2. Structure of atoms. A) Subatomic particles: protons, neutrons and electrons, their charge and mass, and arrangement in atoms. B) Atomic number (Z) and mass number (A). C) Electronic structure of atoms. E) Isotopes.
3. Radioactivity: its discovery by Henri Becquerel. Marie and Pierre Curie. Types of natural radioactivity: alpha (a) particles, beta (b) particles and gamma (g) rays. Half-life. Uses of radioactivity: smoke detectors, medicine. Radon gas, a radioactive health hazard.

1. Electron shells and electron dot structures. Types of chemical bonds: ionic, covalent, metallic.

1. Ionic bonds. The facts on sodium chloride and other salts. Crystal structures.
2. Properties of ionic compounds in the solid state and in water solution. Sodium chloride, a source of chemicals for plastics, manufacture of paper, and water purification.
3. Ions in nutrition. Hemoglobin and chlorophyll. Calcium in teeth and bones (vitamin D, rickets, osteomalacia). Signal conduction by nerve cells. Iodide, thyroid glands and the hormone thyroxine. Diseases of iodide deficiency: goiter.
4. Medical uses of ionic compounds: Fluoride and tooth care. Manic depression: a story of 3 metal ions?
5. Metal ions and disease: lead poisoning, Romans, plumbers, and prostitutes. Why we still use lead and its compounds.

1. Covalent bonds: sharing of electrons between two non-metal atoms to form molecules.
2. The H₂ molecule. The halogens and hydrogen halides. The properties of acids. The H⁺ ion in water solution. Stomach acid for digestion of food.
3. O₂ and N₂ molecules and multiple covalent bonds. Double and triple bonds. Hydrogen derivatives of nitrogen (ammonia, NH₃) and oxygen (H₂O).
4. Molecules with carbon atoms. C compounds with halogens. Tetrafluoroethylene, the precursor from which Teflon is made. Carbon compounds with group 6 elements: carbon dioxide (CO₂) and carbon monoxide (CO).

1. Layers and composition. N₂, O₂, Ar, CO₂, water vapor, and trace gases.
2. The biological importance of the atmospheric gases: A) N₂: Biological nitrogen fixation, the conversion of N₂ to ammonia. Symbiotic and free-living nitrogen fixing bacteria. Fixed nitrogen from electrical storms, the formation of NO (nitric oxide) and NO₂ (nitrogen dioxide). B) O₂: Respiration (similar to the burning of hydrocarbon fuels). Photosynthesis. "Good" ozone in the stratosphere. C) Argon and other group 8 gases: no significant biological importance. D) Carbon dioxide: released during respiration and converted back into biological molecules by photosynthesis.

1. Isolation of the gases from air.
2. N₂ gas and ammonia synthesis. Haber-Bosch process. Haber: the personal side, involvement in World War I, poison gases. Uses of ammonia (fertilizer and explosives).
3. O₂ gas for making steel, antifreeze, polyester, bleaching pulp and paper. Uses of ozone.
4. Argon: metal manufacture, incandescent light bulbs, triple-pane windows. Other noble gases.
5. CO₂ gas: dry ice refrigerant, carbonated drinks, manufacture of aspirin, bullet-proof windows, fertilizer.

1. Carbon monoxide (CO): formation, properties, and how it poisons us. CO is produced naturally in your bodies in small amounts.
2. The nitrogen oxides. Nitric oxide and nitrogen dioxide. Role of our automobiles. "Bad" ozone in the troposphere. The chemical connection between car exhaust and the mechanism of action of Viagra.

Useful Web Sites for Chemistry 2.100:

Global Warming Site

Aspirin

Return to the Chemistry Department Course Descriptions

Return to Dr. Hruska's Home Page

http://home.cc.umanitoba.ca/~joneil/2.100.Course.outline.htm

Maintained by J. O'Neil