Chem100

CAMOSUN COLLEGE

DEPT. OF CHEMISTRY & GEOSCIENCE

CHEMISTRY 100-INTRODUCTORY CHEMISTRY

FALL 2017

Instructor: Dr. Nasr Khalifa, Fisher 348C, Phone: 250-370-3201, E-mail: khalifa@camosun.bc.ca

Texts: “Chemistry100 Notes,  Lab Manual, and Problem Sets (2017). This is a required in-house textbook and is available at the Camosun bookstore.

 

Course Description:

This course is a basic introduction to chemistry and is intended for students with little or no background in chemistry. Topics include: chemical formulae and equations, simplest formula, atomic mass, mole concept, molarity, periodic table, molecules and chemical bonding, and some descriptive chemistry. Experiments will emphasize basic lab techniques.

 

Credits: 4

Mode and Hours of Delivery: 4 hours of lectures and 2 hours of labs. Duration: 15 weeks, Estimated out-of-class: at least 4 hours per week.

Pre-requisites:

“C” in Principles of Math 10, or Foundations of Math & Pre-calculus 10, or MATH 053, or 057, or MATH 072, or MATH 135, or MATH 137, or assessment.

Prior Learning Assessment Available: Yes

 

Intended Learning Outcomes:

Upon completion of this course, the student will be able to:

1. Use dimensional analysis, metric and SI units in performing chemical calculations.
2. Utilize the specialized vocabulary and nomenclature of chemistry and name chemical compounds, and identify and construct chemical formulas.
3. Summarize the characteristics of electrons, protons and neutrons, and identify their roles as components of atoms, ions and isotopes, including radioisotopes.
4. Describe atomic structure, the differences between elements, and the role of the periodic table in organizing elements within a coherent theoretical and empirical system.
5. Describe and account for the periodic table trends concerning atomic number, atomic radius, ionization energy and electronegativity.
6. Compare the formation and characteristics of ionic and molecular compounds.
7. Perform mathematical calculations involving chemical formulas, molecular weights, moles, Avogadro’s number and Molarity.
8. Balance chemical equations, including use of the mole concept, and solve stoichiometry problems.
9. Account for the general characteristics of the gas, liquid, and solid states.
10. Conduct experiments in basic chemistry, utilizing common chemistry laboratory equipment with an enhanced knowledge and practice in basic lab skills.

 

Detailed Course Outline:

 

1. Measurements and Calculations:

-SI units, Si prefixes, metric conversions, scientific notation

-measurements, calculations using measurement, density calculations,

-energy and energy calculations.

 

2. Introductory Terminology:

-the scientific method, physical and chemical changes

-elements and compounds, mixtures

-metals and non-metals

-Dalton’s atomic theory, atoms and molecules, subatomic particles, the nuclear atom

-isotopes, ions and atomic masses.

 

3. Chemical Formulas and names:

-composition of a compound, number of units of a compound, formulas of compounds

-naming compounds, chemical formulas for some common compounds.

 

4. Calculations Based on Chemical Formulas:

-molecular and formula masses, percentage by mass composition

-the Mole concept, interconversions between moles and grams

-moles of molecular and ionic substances

-calculations involving numbers of particles, grams and moles, mass of an atom in grams.

 

5. Stoichiomerty:

-writing balanced equations, interpreting and using equations

-stoichiometry calculations using equations

-limiting reactant concept, percentage yield

-heat and chemical reactions.

 

6. The Periodic Table and The Distribution of Electrons in Atoms:

-chemical families

-electron energy levels, energy sublevels and orbitals, electron arrangements in atoms

-electron dot formulas

-atomic size and periodic trends, ionization energy and periodic trends

-chemical properties of elements and periodic trends.

 

7. Chemical Bonding:

-ionic compounds and the ionic bond

-molecular compounds and the covalent bond, multiple bonds

-electronegativity concept and bond polarities

-molecular geometry and polarity.

 

8. Gases:

-why gases exist

-gas volume and pressure, units of pressure, gas volume and temperature

-absolute temperatures and the Kelvin scale

-standard temperature and pressure (STP)

-partial pressures, relating gas volume to the number of molecules

-reaction stoichiometry for gases.

 

9. Liquids and Solutions:

-the liquid state

-hydrogen bonding, vapour pressure and boiling point

-liquid solutions, solubility, concentrations of liquid solutions, dilution of a solution

-electrolytes, ion concentrations, ionization

-pH scale, stoichiometry of reactions in solution.

 

10. Organic Reactions:

-why so many organic compounds

-structural formulas, condensed structural formulas, isomers

-hydrocarbons, alkanes, alkenes, alkynes, cycloalkanes, aromatic compounds, alcohols

-selected organic chemical reactions

-polymerization reactions.

 

Basis of Student Assessment:

(a)	Labs	Lab Experiments	25%
(b)	Quizzes	Quiz #1 (September 27)	5%
		Quiz #2 (October 25)	5%
		Quiz #3 (November 29)	5%
(c)	Exams	Test #1(October 16th, 2 hours)	15%
		Test #2 (November 20th, 2 hours)	15%
		Final Exam (December, 3 hours)	30%
(d)	Other

 

Chem. 100 Lab Schedule (Fall 2017)

(Subject to change)

 

Sep. 4	Labour Day
Sep. 11	Safety introduction. Attendance is mandatory
Sep. 18	Experiment 1: Density
Sep. 25	Experiment 2: Identifying liquid compounds
Oct. 2	Experiment 3: Separating mixtures
Oct. 9	Thanksgiving Day
Oct. 16	Test #1 (test will be written during the lab period)
Oct. 23	Experiment 4: Heat of combustion
Oct. 30	Experiment 5: Recycling copper
Nov. 6	Experiment 7: The copper and silver nitrate reaction
Nov. 11	Remembrance Day
Nov. 13	No Lab (Remembrance Day observed)
Nov. 20	Test #2 (test will be written during the lab period)
Nov. 27	Experiment 11: The magnesium and HCl reaction
Dec. 4	Experiment 13: Synthesis of Aspirin
Dec. 18	Last day of instruction

*Final exam at the end of the course will cover all course material.

*You must pass (50% or more) both the lecture and the laboratory portions of the course independently in order to pass overall.

*If any of the term tests or the quizzes is missed due to illness or other justifiable reason with accompanying documentation, the percentage value of that term test (15%) or of that quiz (5%) will be added to the percentage value of the final exam.

*You must provide your own safety glasses. Prescription glasses are OK, but sunglasses are NOT. You must wear these safety glasses at all times while you are in the lab. You will not be allowed to carry out experiments without safety glasses.

*Office hours are posted on the door. You can, however, drop by the office any time. You will not be wasting my time if you come for help. I’m here to help you learn.

 

Grading System:

Standard Grading System (GPA)

Percentage	Grade	Description	Grade Point Equivalency
90-100	A+		9
85-89	A		8
80-84	A-		7
77-79	B+		6
73-76	B		5
70-72	B-		4
65-69	C+		3
60-64	C		2
50-59	D	Minimum level of achievement for which credit is granted; a course with a “D” grade cannot be used as a prerequisite.	1
0-49	F	Minimum level has not been achieved.	0

 

LEARNING SUPPORT AND SERVICES FOR STUDENTS

There are a variety of services available for students to assist them throughout their learning. This information is available in the College Calendar, Registrar’s Office or the College web site at http://camosun.ca

 

ACADEMIC CONDUCT POLICY

There is an Academic Conduct Policy including plagiarism. It is the student’s responsibility to become familiar with the content of this policy. The policy is available in each School Administration Office, Registration, and on the College web site in the Policy Section.

http://camosun.ca/about/policies/policies.html