1. Introduction to the Chemical Properties of Matter
CHM1111 Section 04
Instructor: Dr. Jules Carlson
Class Time: M/W/F 1:30-2:20

2. Course Materials
Chemistry, Canadian Edition, 1st edition, Olmstead, Williams, Burk
Student Solutions manual to accompany Olmstead et al. (Digital copy with text)
Laboratory Manual
WHIMIS Handbook
I>Clicker 2 or I>Clicker

3. Timeline/Office Hours
Section 04: Classes Mon/Wed/Fri 1:30-2:20 PM Office Hours: Mon/Wed 11 AM – 12 PM No classes: Monday, October 10th or Friday, November 11th Mid-term: Wednesday, October 12th Final Exam: Friday, December 9th

4. Mark Breakdown Mid-term exam: 20 % Laboratory: 25 %
I>clicker questions: 10 %
Final Exam: 45 %
Total: %

5. I>Clickers
Great way to keep up with how well you are understanding lectures
One question per lecture – get mark for voting
Makes up 10 % of your final grade
Come to class and always remember your I>clicker!!!!
Register online at
2 Freebies

6. WileyPlus Make sure to register on WileyPlus
Instruction video on registration found at:
Lecture notes available on the site
Online textbook plus other resources
Practice assignments that are not worth marks but you are strongly encouraged to do

7. Labs
Buy a lab manual this week at the Petrified Sole Bookstore (in the basement of the Bulman Student Centre). Bring it to your first lab next week.
Attend your SCHEDULED first lab, during the week of Monday Sept. 12th to Friday Sept. 16th.
All lab sections are full, so you cannot attend at a different time.
You must attend this first lab in order to find out which experiment or workshop you will be doing the following week. (Not everyone will start with Experiment #1.)
Questions? Contact Theresa Baran
Lab Coordinator

8. To do well in the course
Read ahead in your textbook – don’t get behind.
Do LOTS of problems!!!!!!!! Work together!
Problems will be assigned from the textbook plus feel free to do more on your own.
Also – weekly assignments will be provided on WileyPlus
Feel free to contact me and Theresa, we will be available by and have office hours!!!

9. Chapter 1
Quick review, you are expected to know this material from high school.
Please read Chapter 1 thoroughly for a full review.
Also, work on the Chapter 1 Assignment (Due Friday not for marks) on the WileyPlus site.
Textbook questions:
1.3, 1.5, 1.7, 1.9, 1.11, 1.19, 1.23, 1.25, 1.27, 1.31, 1.33, 1.35, 1.79, 1.85, 1.87

10. Measurement in Chemistry
Smallest fundamental unit of a substance is an atom
Atoms bond together through ionic or covalent bonding to produce molecules
Atoms and molecules are extremely small, so are measured in moles.
1 mole = x 1023 molecules or atoms
Called Avogadro’s number
The mass of 1 mole of atoms is the molar mass
Molar masses given on periodic table

11. Periodic Table What is the mass of 2 moles of Fluorine?
How many moles in 13 g of Chromium?
Molar mass in g/mol

12. Concentrations
Concentrations can be mass per volume or moles per volume
In a gas, use m3 as unit of volume (mol/m3)
In liquids, use L or mL as unit of volume
Moles per litre: Molar (M)
Concentrations can be moles per unit mass
Moles per kg: Molal (m)
See table 1.1 (page 9) for magnitudes
Commonly see M (mega), k (kilo), m (milli) and μ (micro)

13. Dilutions
Say we have CaCl2 solution with a concentration of 50 mM in 100 mL of water
What is the concentration in 500 mL of water?
What are the final concentrations in moles per litre of Ca2+ and Cl- ions?

14. Chemical Reactions and Stoichiometry
Stoichiometry: study of amounts of materials produced and consumed in chemical reactions
Consider the reaction with 4 mol of H2 and 4 mol of O2:
2 H2 + O2  H2O
How many moles of H2O should be produced if the reaction goes to completion and is completely efficient?
If 3.2 moles of H2O are formed, what is the percentage yield for the reaction?

15. Significant figures
How many significant figures do the following numbers have (calculate as necessary)?
3.54 x 10-3 M M + 75 mM
5.5 mol
10.5 m3