College in the Schools
Course Syllabus
501West College Drive
Brainerd, MN 5640
CHEM 1414
Fundamentals of Chemistry
Pierz Healy High School
112 Kamnic Street
Pierz, MN 56364
Instructor: Dr. Randy S. Fischer
Email: [email protected]
Office: Room 200
Office Phone: 320-468-6458 x1263
Office Hours: Monday through Friday Sem 1 [7:30-8:00 AM, 8:12-8:59 AM, 3:30-4:00 PM]
Sem 2 [7:30-8:00 AM, 10:43-11:30 AM, 3:30-4:00 PM]
Course Information:
Course Title: CHEM 1414 – Fundamentals of Chemistry
Term: Fall → Spring (2016-2017)
CLC Credits: 4
Transfer Curriculum Goal: 3
Prerequisites:
High School: 2
● Introduction to Chemistry 9, Algebra I, Algebra II
● Junior with a 3.0 GPA or a Senior with a 2.5 GPA.
Course Description:
This course involves the general study of chemistry, periodicity, atomic and molecular structure, and physical
and chemical changes.
Course Purpose:
This course gives a general and practical introduction to chemistry. The theoretical portion of the course will be
complemented by the use of projects and laboratory exercises to develop deeper understanding of the concepts.
This course is intended for non-science majors as well as providing a foundation for those planning to enter
medical, engineering, or scientific fields in college.
Course-Specific Learning Outcomes: Upon completion of this course the student will be able to:
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Use dimensional analysis to solve problems related to converting one size measuring unit or dimension into
another.
Use the periodic table and atomic theory to describe the basic structure of any element.
Apply the Lewis structure theory to predict the covalent bonding properties in molecules or polyatomic ions
consisting of nonmetal elements.
Predict the formula resulting from the combination of a type I metal and nonmetal.
Determine the quantitative relationships between reactants and products for any chemical reaction.
Use kinetic molecular theory to predict how the volume and pressure of a gas change with temperature.
College-Wide Learning Outcomes: The students will be measured in their individual ability to:
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Demonstrate understanding of scientific theories and the ways in which scientists develop, express, and
question theories in the field of chemistry.
Formulate and test hypotheses by performing chemistry experiments requiring collection of data, its
statistical and or/graphical analysis, and an appreciation of uncertainty and sources of error.
Communicate their findings, analysis, and interpretations with other students and the instructor orally and
in writing.
Topical Outline:
1. Lecture Sessions
I. Matter and Measurement
A. State the steps of the scientific method.
B. Explain the difference between a fact and an inference.
C. Recognize qualitative verses quantitative data.
D. Define the term scientific law.
E. Explain the difference between a hypothesis and a theory.
F. State the two properties matter must possess.
G. Define and recognize a physical verses a chemical change.
H. Recognize the three states of matter.
I. Define the terms homogeneous verses heterogeneous.
J. Describe how matter can be classified by attempting to separate it by physical changes.
K. Describe how matter can be further classified by attempting to separate it by chemical changes
once it has been completely separated by physical changes.
L. Express decimal numbers in scientific notation and vice versa.
M. Express the results of multiplication and division of scientific numbers in scientific notation.
N. Perform multiplication and division of scientific numbers on a scientific calculator.
O. Write unit paths and solve any problem that involves converting from one unit of measurement
to another—given a table of conversion factors.
P. Interpret the meaning of proportionality and of a proportionality constant.
Q. Solve problems that involve the use of a proportionality constant as a conversion factor.
R. Convert Fahrenheit temperatures to Celsius and vice versa.
S. Convert Celsius temperatures to Kelvin and vice versa.
T. Distinguish between units of the English system and Metric system.
U. List the standard metric units of measurement and their abbreviations for length, mass and
volume.
V. Write equivalencies, with their correct abbreviations, between any standard metric unit and a
prefixed metric unit of kilo, centi, or milli.
W. Write equivalencies between metric units when utilizing a table of prefixed metric units.
X. Determine the number of significant figures in a number by having memorized the rules for
counting significant numbers.
Y. Determine the uncertainty in a given measured value.
Z. Determine the correct number of significant figures after adding and subtracting measured
values.
AA. Determine the correct number of significant figures after multiplying and dividing measured
values.
II. Atoms and Elements
A. Identify three subatomic particles by name, relative mass, and charge, and describe the
structure of the atom.
B. Write and name a given isotope and determine the number of subatomic particles it contains.
C. Define an atomic mass unit, amu.
D. Calculate the atomic mass of an element given a set of isotopes, masses and abundances.
E. Distinguish between periods and families or groups in the periodic table.
F. Describe why groups or families of elements have similar chemical and physical properties.
G. Locate the alkali metals, halogens, and noble gases in the periodic table.
H. Predict the relative sizes of atoms within a group or family and period.
I. Identify the metals, nonmetals, and metalloids by their positions in the periodic table.
J. Identify representative and transition elements by their positions in the periodic table.
III. Molecules, Ions and Compounds
A. Name molecules.
B. Recognize the seven elements that form stable diatomic molecules.
C. Name and know the charges of the polyatomic ions asked to memorize.
D. Name the two types of ionic formulas that contain polyatomic ions.
E. Describe how scientists arrived at Avogadro’s number.
F. Define a mole in terms of mass and Avogadro’s number.
G. Convert grams of a given substance to moles and vice versa.
H. Convert grams of a given substance to numbers of atoms, molecules, or formula units or vice
versa.
I. Calculate the percentage by mass of each element in a given formula.
J. Determine the empirical formula from percentage data.
K. Determine the true molecular or ionic formula from percentage data and formula weight.
IV. Chemical Equations and Stoichiometry
A. Balance chemical equations.
B. Identify the abbreviations used in chemical equations for solids, liquids and gases.
C. Classify balanced equations into one of the six types discussed in class.
D. Identify common acids and bases.
E. Solve the four types of possible stoichiometry problems.
F. State the definitions of endothermic and exothermic reactions.
G. Draw energy level diagrams for endothermic and exothermic reactions.
H. Calculate percentage yield for a given stoichiometric reaction.
V. Atomic Structure
A. Describe the wave nature of electromagnetic radiation and how wavelength plays a role in its
character.
B. Describe how observations of a discharge tube can be used to make of model of electron energy
levels.
C. List the two types of energy an electron possesses.
D. Describe how the total energy of an electron changes with increased average distance from the
nucleus.
VI. Atomic Electron Configuration
A. Describe the shapes of the s and p orbitals.
B. List the various orbitals, sublevels, and principal energy levels and their capacities for
electrons.
C. Write the electron configuration for any element in the periodic table using the short-hand
notation.
D. Define valence electrons.
E. Write electron-dot structures for any representative element.
VII.Bonding and Molecular Structure
A. Define the terms cations and anions.
B. Predict the number of electrons representative metals and nonmetals tend to loss or gain so as
to acquire a noble gas electron configuration when they are involved in an ionic bond.
C. Predict the charge the representative metals and nonmetal acquire when they are involved in
an ionic bond.
D. Use electron-dot structures to draw the electron transfers necessary between metals and
nonmetals to form ionic bonds.
E. Predict ionic formulas from those metals and nonmetals that have only one charge.
F. Calculate the charge a transition metal when contained in an ionic bond.
G. Name the nonmetal anions.
H. Name ionic formulas that contain metals that have only one oxidation state and those that
contain metals that can have more than one oxidation state.
I. Draw electron-dot structures for covalently bonded substances.
J. Draw electron-dot structures for polyatomic ions.
K. Define electronegativity and apply it to determine if a formula contains ionic or covalent bonds.
L. Define polar, nonpolar or essentially nonpolar covalent bonds and be able to use
electronegativities to determine the type found in a formula.
M. State the elements which disobey the octet rule.
N. Predict the geometry of a molecule.
O. Determine if a molecule is polar or nonpolar.
VIII.Gases and Their Properties
A. State the properties of gases.
B. Describe the model for ideal gases.
C. Describe a barometer and open ended monometer and how to make pressure measurements
from each.
D. Convert one pressure measurement to another given the relationship between the pressure
measurements.
E. State Boyle’s and apply it to solve applicable problems.
F. State Gay-Lussac’s Law, Charles’ Law, and the combined gas law and apply them to solve
applicable problems.
G. State Avogadro’s Law.
H. State the ideal gas law and apply it to solve applicable problems.
I. State or derive the gas density equation from the ideal gas equation and apply it to solve
applicable problems.
J. State or derive the molar volume equation from the ideal gas equation and apply it to solve
applicable problems.
K. Define STP.
IX. Intermolecular Forces, Liquids, Solids
A. Predict how vapor pressure, molar heat of vaporization, boiling point, viscosity, and surface
tension varies with intermolecular forces of attraction.
B. Identify the intermolecular forces of attraction in a substance from its formula.
C. Draw an kinetic energy distribution curve for molecules in a liquid.
D. Explain how escape energy of molecules in a liquid is related to the intermolecular forces of
attraction and how its value relates to the liquids vapor pressure.
E. Explain how the kinetic energy distribution curve changes with temperature and how that
affects the vapor pressure of the liquid.
F. Write a reversible equation to represent the equilibrium between a liquid and its vapor state.
G. Define boiling point of a liquid in terms of the liquids vapor pressure and the total gaseous
pressure exerted on the liquid and explain how the boiling point of a liquid can be changed.
H. Identify the five types of solids and their respective physical properties.
I. Define heats of vaporization, condensation, fusion, and solidification.
J. Calculate the amount of energy required to vaporize a given mass of liquid at its boiling point
or condense the same amount of gas at its condensation temperature.
K. Calculate the amount of energy required to melt a given mass of solid at its melting point or
freeze the same amount at its freezing point.
L. Identify melting, freezing, boiling, or condensation as endothermic or exothermic processes.
M. Define specific heat.
N. Calculate the amount of energy required to be added or removed to change the temperature of
a given amount of solid, liquid, or gas.
O. Calculate the amount of energy required to be added or removed to make any variation in
temperature including any combination of phase changes.
X. Solutions and Their Behavior
A. Explain the electric properties of polar and nonpolar molecules.
B. Know what hydrogen bonding is and when it occurs.
C. Know the definitions of homogeneous and heterogeneous mixtures, solutions, solute, and
solvent.
D. Know how polar and nonpolar molecules affect the mixing process between solute and solvent.
E. Know how to calculate % wt., ppm, and molarity of a solute in a solution.
F. Know how to use molarity as a conversion factor to solve the four types of molarity problems
discussed in class.
G. Know how to calculate dilution problems.
2. Tentative Laboratory Activities (in proposed order)
1. Working With Glass
2. Physical and Chemical Changes
3. Compounds and Elements
4. SI Measurement
5. Precision and Accuracy
6. Developing A Logical Model
7. Mole and Molar Mass
8. Spectroscopy
9. Periodic Tendencies
10. Alkaline Earth Metals
11. Halogens
12. Difference Between Ionic and Covalent Compounds
13. Determination of An Empirical Formula
14. Types of Chemical Reactions
15. Activity Series of Metals
16. Stoichiometry
17. % Yield
18. Boyle’s Law
19. Charles’ Law
20. Molar Volume of A Gas
21. Chromatography
22. Solutions
23. Reactions Between Ions in Solution
24. Preparing a Standard Solution
25. pH Indicators
26. pH Titrations
27. Variations in Carbohydrates
28. Developing A Novel Laboratory Procedure
Required/Recommended Textbook and Learning Materials:
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Required Text: Modern Chemistry, Davis et al. (ISBN-0-03-051389-8, Holt, Rinehart and Winston).
Chapters proposed to be covered in this course: 1-16, 18-22. Some sections may be omitted.
Scientific Calculator: Must have scientific notation function.
Laboratory Notebook: A chemistry lab notebook (3-ring binder) will be used to compile all laboratory reports.
Grading Criteria/Course Evaluation:
Course Evaluation: Quarter grades will be based upon the following categories and scale:
 Tests and Quizzes:
 Labs:
 Projects and Papers:
55%
30%
15%
The letter grade given will be directly based upon a percentage of points earned compared to the total points
possible. The Semester Grade is the sum of the two quarters (50% each). A COMPREHENSIVE SEMESTER
FINAL WILL BE GIVEN!
Grading Scale Will Be:
100-94% = A
93-90% = A89-88% = B+
87-84% = B
83-80% = B79-78% = C+
77-74% = C
73-70% = C-
69-68% = D+
67-64% = D
63-60% = D59-Below = F
Student Requirements:
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Attendance: Missing this class, even for just one day, may have a negative impact on your grade. Be prudent
when it comes to absences, regardless of whether it is for personal or school-related reasons.
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Assignments: All work must be completed by the time you get to class on the day it is due.
LATE WORK WILL ONLY RECEIVE 50% CREDIT. IF THE ASSIGNMENT HAS BEEN GRADED &
HANDED BACK TO YOUR PEERS, ZERO CREDIT WILL BE GIVEN.
◊ WRITE NEATLY! IF I CAN’T READ IT, I WON’T GRADE IT!
◊ LABORATORY REPORTS will be generally be due two days after completion of the lab. Follow the
specific instructions of each lab and the laboratory report handout.
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Extra Help: If you need help, see me during my office hours. When you come in be prepared to ask specific
questions rather than just saying you don’t understand anything we have done.
◊ GENERAL HELP SESSIONS WILL BE SCHEDULED AS NEEDED
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Studying: Study chemistry each day. Go over your notes after each class and complete your own assignments.
YOU ARE LESS LIKELY TO SUCCEED IF YOU CRAM FOR TESTS AND TRY TO MEMORIZE
YOUR WAY THROUGH THIS COURSE!
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Tests and Quizzes: Four to five unit tests are scheduled each quarter (dates will be assigned at least 5 days prior
to each test).
◊ ALL TESTS WILL BE COUNTED TOWARDS THE FINAL GRADE. You are responsible for taking a
scheduled test even if you were absent the day before. If you miss one of the scheduled tests, a make-up
test will be given only if you:
1) have a verifiable medical or immediate family emergency.
2) are gone on a school sanctioned activity.
NOTE: If you know you are to be absent for a school-sanctioned activity, you must take the test the day before.
◊ QUIZZES MAY OR MAY NOT BE ANNOUNCED AHEAD OF TIME.
◊ SETTING UP THE PROBLEM BY WRITING OUT THE CORRECT EQUATION,
DEFINITION OF THE VARIABLES, and SHOWING YOUR WORK AND UNITS WILL
TYPICALLY BE WORTH 50-80% OF THE TOTAL POINTS
Lab Etiquette:
The next lab section would appreciate your cooperation with the following : 1) please cleanup your station
before you leave; 2) clean and return equipment, glassware, tools and other materials to their proper places;
3) throw garbage in the wastebasket; 4) observe lab safety rules; and 5) replace chairs to proper positions.
Academic Integrity:
Academic integrity is one of the most important values in higher education. This principle requires that each
student’s work represents his or her own personal efforts and that the student acknowledges the intellectual
contributions of others. The foundation for this principle is student academic honesty. Central Lakes College
and Pierz Healy High School expect all students to uphold the highest standards of academic integrity and acts
of dishonesty will not be tolerated. See your student handbooks for more detailed information.
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Professional Conduct and Communication Are Expected.
Formal and professional conduct is expected of you at all times in lecture, lab and on campus. Your practice
of study, communication, politic, inter-personal and group interaction skills, generally accepted and
expected of a professional, begins and / or continuously improves in this class. Pro-actively shared,
cooperative assistance is highly valued in the professional setting because it is a critical factor in providing
quality science. Because unprofessional, disruptive, and / or rude behavior demonstrated by you is harmful
to the quality of the professional setting to which you aspire, its demonstration in this educational setting
toward anyone, including me, is unacceptable and will result in your immediate discharge from the
classroom / lab. Your grade and your continued membership in the course will be negatively affected based
upon the severity of the offense. Unauthorized cell phone use during class is not permitted. I DO
NOT WISH TO SEE ANYONE’S CELL PHONE!
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Cheating / Plagiarism - Cheating / Plagiarism are not tolerated in any form.
Cheating Defined:
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Copying, in part or in whole, from another’s test or other evaluation instrument or obtaining answers
from another person during the test
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Submitting work previously presented in another course, if contrary to the rules of either course.
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Using or consulting sources or materials not authorized by the instructor during an examination
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Altering or interfering with grading or grading instructions
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Sitting for an examination by a surrogate, or as a surrogate
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Any other act committed by a student in the course of his or her academic work, which defrauds or
misrepresents, including aiding or abetting in any of the actions defined above
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Talking or consulting during the test with another person
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Giving / providing in any way, information to other students that allows the student an undeserved
advantage on an exam or quiz, such as telling a peer what to expect on a make-up exam or prepping a
student for a test in another section of the same class
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Plagiarism Defined:
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The act of incorporating the ideas, words, sentences, paragraphs or parts thereof, or the specific
substance of another’s work, without giving appropriate credit, and representing the product as one’s
own work
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Representing another’s artistic/scholarly or similar works as one’s own
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Plagiarism may either be deliberate or unintentional, but it must be avoided with all due diligence
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Consequences of Academic Dishonesty or Unacceptable Behavior:
Upon the first infraction of academic dishonesty, the instructor may do one or more of the following:
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Give a lower or failing grade on the assignment or exam
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Give a lower or a failing grade in the course
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Refer the student to high school administrators and the Vice President of Student Services for student
disciplinary action.
In the event of a second infraction, upon consultation with administration, the instructor may do one or
more of the following:
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Fail the student from the course
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Refer the student to high school administrators and the Vice President of Student Services for student
disciplinary action
Statement of Accommodation - ADA:
As an affirmative action, equal opportunity employer and educator, Central Lakes College and Pierz Healy High
School are committed to a policy of nondiscrimination in employment and education opportunity and will
work together to provide reasonable accommodations for all persons with disabilities. Accommodations are
provided on an individualized, as-needed basis, determined through appropriate documentation of need. The
accommodations authorized in your plan should be discussed with your instructor. All discussions will remain
confidential.
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Students with learning disabilities, who believe they may need accommodations in this class, are
encouraged to contact Pierz Healy High administration.
Support Services:
The ACE center at both Brainerd and Staples is available for students who need outside help with
understanding their course material. Tutors are present for many disciplines. Accommodations can also be
made for students with special needs. (e.g. wheelchairs, motorized carts, interpreters, audiotapes)
Affirmative Action:
Central Lakes College and Pierz Healy High School are committed to a policy of nondiscrimination in
employment and education opportunity. No person shall be discriminated against in terms and conditions of
employment, personnel practices, or access to and participation in programs, services, and activities with
regard to race, sex, color, creed, religion, age, national origin, disability, marital status, status with regard to
public assistance, or sexual orientation. If you have any concerns see the Student Handbook or contact the
Human Resources Department.
Emergency Procedures:
Emergency information and procedures can be found in each classroom. Please take time to review these
procedures. Ask the instructor if you have any questions.
Academic Standards:
This course is part of the College in the Schools program through CLC. If you are taking this course for
college credit you are required to meet CLC’s academic standards. This means that you must maintain a 2.0
GPA and complete 67% of the college courses that you enroll in or you will be placed on academic probation.