Division of Math and Science
Arkansas Northeastern College
Departmental Course Syllabus: Survey of Chemistry
CH 14003
I.
Course Prerequisites
Prerequisite or corequisite of MA 14023 Math for Health Science or above. Prerequisite: Grade “C” or above in CP
01113 Advanced Reading Techniques (or appropriate placement test score) and CP 02003 College Writing Skills (or
appropriate placement test score).
II.
Course Catalog Description
This course is designed to introduce the students to the different phases of chemistry: inorganic, organic, and
biochemistry.
III.
Required Texts and Materials
Introductory Chemistry: A Foundation
Stephen S. Zumdahl
Houghton Mifflin Company, Publisher
Calculator (suggested TI 30xa or TI-30XIIS)
IV.
Course Rationale: The natural sciences provide the opportunity for the development of independent, creative, and
logical thinking while they enhance one’s understanding of the effects of the sciences upon the individual, society
and the environment. The information gained from studies in the biological and physical sciences is based upon
acute observations, experimentation, and arriving at logical conclusions. The decision-making processes that are
used daily in coping with life in a modern society are basically those practiced in all science classes. The historical
development of this logical process is an integral part of each science class, and as such, provides the individual with
a foundation for continued personal growth.
V.
Course Objectives
By the end of the course, students will have
 Demonstrated a working vocabulary in chemical nomenclature and fundamental chemical processes
through written and oral communications.
 Demonstrated an overall working knowledge of the scientific method, elements and compounds,
chemical nomenclature and the characteristics of the states of matter.
 Demonstrated the use of a systematic process to solve chemical stoichiometry, conversions and word
problems.
 Demonstrated predicting and writing examples of chemical bonding and predicting, writing and balancing
simple chemical reactions.
 Demonstrate a working knowledge of the behavior of gases and the gas laws.
VI.
Unit and Instructional Objectives
UNIT ONE: CHAPTERS 1-4
Rationale: The basic vocabulary of science is mathematics. Accurate measurements, calculations and observations are
intrinsic to the continuation of commerce, healthcare and innovation. A fundamental understanding of atomic structure
is invaluable in a scientific education.
Objectives: The student will be able to:
CHAPTER 1: CHEMISTRY: AN INTRODUCTION
1.
communicate using appropriate scientific vocabulary at an appropriate level.
2.
develop a strategy using the Scientific Method to solve a word problem.
CHAPTER 2: MEASUREMENTS AND CALCULATIONS
1.
Communicate the differences in quantitative and qualitative observations, and the importance of units.
2.
Discuss why a reference standard is necessary in measurement.
3.
Explain the need for scientific notation and convert ordinary numbers to scientific notation, and vice versa.
4.
Discuss the base units of length, mass and volume in the metric system, and convert using metric prefixes.
5.
Given a measurement in the English system of measurement, convert to appropriate metric system measurement.
6.
Given a measurement in the metric system of measurement, convert to appropriate English system measurement.
7.
Discuss the difference between mass and weight.
8.
Convert between Fahrenheit, Celsius and Kelvin temperature scales.
9.
Identify and utilize units in which density is expressed.
10. Given the mass and volume of a sample, calculate density.
11. Recognize density as a conversion factor.
12. Given the density and volume, convert to mass.
13. Given density and mass, convert to volume.
14. Given a word problem, be able to recognize the given quantities, convert if necessary, and solve for the unknown.
15. Manipulate an algebraic equation to isolate an unknown.
16. Explain the meaning of significant figures and be able to do addition/subtraction, multiplication/division, and scientific
notation and report answers significantly.
CHAPTER 3: MATTER
1.
Identify and discuss matter and the three states of matter.
2.
Name the processes by which matter changes physical states, noting terminology for the points when matter is in the
process of changing. Sublimation, condensation, melting, freezing, deposition and vaporization, and that these phase
changes occur at a constant temperature.
3.
Given the melting point and boiling point, identify the state of matter at a given temperature for a specific substance.
4.
Discuss differences in physical and chemical properties; physical and chemical changes; pure substances and
mixtures; elements and compounds.
5.
Distinguish elements, compounds and mixtures in terms of their atomic makeup.
6.
Discuss the classification of matter, specifically in terms of pure substances and mixtures.
7.
Discuss methods of separation of mixtures.
8.
Describe differences in metals and nonmetals, and identify their general positions on the Periodic Table.
CHAPTER 4: CHEMICAL FOUNDATIONS: ELEMENTS, ATOMS AND IONS
1.
Demonstrate and discuss the structure of atoms and properly write and use atomic symbols.
2.
Discuss Dalton’s Atomic Theory and differentiate between elements and compounds, atoms and molecules.
3.
Identify names and symbols of subatomic particles.
4.
Identify relative charge and mass of subatomic particles.
5.
Form and communicate mental picture of atoms, with arrangement of subatomic particles.
6.
Given the atomic number, determine the number of protons and electrons in an atom.
7.
Given number of protons and electrons, indicate whether atoms are neutral or ions.
8.
Given the atomic mass and mass numbers, determine the number of subatomic particles in the atom.
9.
Given a periodic table and the number of protons and neutrons, write the correct symbol, atomic number and mass
number.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
Discuss how ions (anions and cations) are formed.
Given the number of protons and electrons, calculate the charge on an ion.
Identify and communicate the relationship between symbol for an ion, charge, mass number, atomic number,
number of protons, neutrons and electrons.
Given a periodic table, determine atomic number and atomic mass of a specific element.
Discuss trends on periodic table..
Identify common names of periodic table groups and periods, and how to locate elements by period and group.
Describe differences and trends seen in metals and nonmetals.
List and KNOW the elements that exist as naturally occurring diatomic molecules.
Predict the charge of a monoatomic ion from the element’s position on periodic table.
Define and discuss what is meant by ‘valence’.
Unit Two: Chapters 10 – 12
Rationale: In nature, as well as in business or life in general, the configuration of circumstances which is at the lowest
energy is the most stable. The knowledge that energy isn’t created or destroyed, but rather is transformed from one
form to another, is fundamental to our understanding of our universe. Chemical reactivity is primarily electronic
interactions, therefore a basic knowledge of structure and energetic of electrons is necessary for continuing scientific
education.
Objectives: The student will be able to:
CHAPTER 10: Energy
1.
Differentiate between heat and temperature and contrast exothermic vs. endothermic processes.
2.
Convert between energy units (calorie and Joule).
3.
Discuss how a material’s specific heat relates to its uses.
4.
Given specific heat, mass and temperature change, be able to calculate energy.
5.
Given specific heat, mass and energy, be able to calculate temperature change.
6.
Given specific heat, temperature change and energy, be able to calculate mass.
7.
Given mass, temperature change and energy, be able to calculate specific heat.
8.
Given a word problem, be able to recognize the given quantities, convert if necessary, and solve for the unknown.
CHAPTER 11: MODERN ATOMIC THEORY
1.
Discuss the s,p,d and f orbitals and how they make up the different Principal energy levels.
2.
Identify pictorial representations of the different orbitals and relate the maximum electronic occupancy in each.
3.
Discuss stability with respect to distance from nucleus, including ground state vs. excited state of an electron.
4.
Discuss how the principal energy levels ‘fill’.
5.
Discuss valence electrons and write complete electron configurations. (first 36 elements)
6.
Using box diagrams, show how electrons fill orbitals, pair up (Pauli’s Exclusion Principle) and discuss Hund’s Rule.
7.
Correlate electron configurations with the periodic table.
8.
Recognize and discuss general trends that arise from the periodic table.
CHAPTER 12: CHEMICAL BONDING
1.
Differentiate between ionic and covalent bonding.
2.
Discuss how sharing vs. transfer of electrons between atoms relates to metals and nonmetals, and how the periodic
table is utilized in this discussion.
3.
Discuss the meaning of electronegativity and how it relates to periodic table position.
4.
Identify and discuss polar and nonpolar compounds.
5.
Write Lewis Dot Structures for compounds with single, double and triple bonds, and for polyatomic ions.
Unit Three: Chapters 5-7
Rationale: In order to converse intelligently in many fields, including healthcare, agriculture and science, a student must
be able to identify, write and use chemical names and chemical formulas appropriately. The ability to write, balance and
speak about chemical reactions is vital to the safe and effective production of goods and services.
Objectives: The student will be able to:
CHAPTER 5: NOMENCLATURE
1.
Identify a binary compound.
2.
Name a binary ionic compound given a chemical formula.
3.
Given the name, be able to write the chemical formula of an ionic compound.
4.
Identify and write the names and formulas for common polyatomic ions, and the acids from which they are derived.
5.
Name a molecular compound given the chemical formula, and vice versa.
6.
Define ‘acid’ and ‘oxoacid’, and recognize and supply examples of both.
7.
(located in ch. 8) Given a periodic table and chemical formula, calculate the molecular weight of a molecular
compound and the formula weight of an ionic compound.
8.
(located in ch. 8) Calculate the percentage composition of elements in any compound, molecular or ionic, given the
chemical formula and a periodic table.
CHAPTER 6: CHEMICAL REACTIONS: AN INTRODUCTION
1.
Discuss and write the form of a chemical equation, including phase symbols.
2.
Recognize the difference between reactants and products.
3.
Write and balance a chemical equation for a chemical reaction, starting from formulas, and also starting from words.
CHAPTER 7:
1.
Discuss the factors that cause reactions to occur (driving forces).
2.
Discuss precipitation reactions and solubility rules in order to predict if a precipitate will form (simple examples).
3.
Describe reactions in terms of molecular, complete ionic and net ionic equations.
4.
Identify the difference between acids and bases, and in terms of electrolytes, what a strong acid/base and a weak
acid/base will do.
5.
Assign oxidation numbers to atoms in both monoatomic and polyatomic species.
6.
Identify a simple oxidation reduction reaction, and in doing so, discuss oxidation numbers and how electrons are
transferred. (LEO goes GER = loss of electron is oxidation, gain of electron is reduction).
7.
Discuss why a loss of electron(s) increases oxidation number, and a gain of electron(s) decreases oxidation number.
8.
Identify where a reaction fits in a the simple classifications of reactions.
Unit Four: Chapters 8-9, 13
Rationale: In the same way a cook works from a recipe, a chemist works from a chemical reaction. The ‘kitchen’ is,
however, on a microscopic scale, so it is necessary to determine amounts by mass, or ‘counting by weighing’. To do this,
the student must be knowledgeable about working with moles ratios in all phases of matter. Failure to react correct
amounts of certain chemicals can have disastrous consequences.
CHAPTER 8: CHEMICAL COMPOSITION
1.
Discuss average mass, and how atomic mass is experimentally determined.
2.
Given a periodic table and chemical formula, calculate the molecular weight of a molecular compound and the
formula weight of an ionic compound.
3.
Calculate the percentage composition of elements in any compound, molecular or ionic, given the chemical formula
and a periodic table.
4.
Discuss the mole concept and Avagadro’s number and molar mass.
5.
Convert from moles to grams, and vice versa.
6.
Convert from number of atoms to moles to grams, and vice versa.
7.
Determine the mass percent of elements in a given compound.
8.
Discuss and determine empirical formulas from mass percent, and determine molecular formula given the empirical
formula and molar mass.
CHAPTER 9: CHEMICAL QUANTITIES
1.
Discuss and convert from moles of one compound to moles of another compound using a balanced equation.
2.
Discuss and show how to convert from grams (mass) of one compound to mass (grams) of another compound using a
balanced equation.
3.
Determine the limiting reactant in a chemical reaction.
4.
Differentiate between actual yield and theoretical (calculated) yield.
5.
Given the actual and theoretical yield, determine the percent yield.
6.
Given the percent yield and theoretical yield, determine the actual yield.
CHAPTER 13: GASES
1.
Discuss the concept of pressure, units of pressure, and conversions within those units.
2.
Discuss Boyle’s Law, Charles’s Law to form the Combined Gas Law and when to use it.
3.
Recall and manipulate the Combined Gas Law (equation rearrangement).
4.
Given a word problem, determine known information and calculate for the unknown using the Combined Gas Law.
5.
Discuss Avogadro’s Law and Ideal Gas Law and when to use Ideal or Combined Gas Law.
6.
Recall and manipulate the Ideal Gas Law (equation rearrangement).
7.
Given a word problem, determine known information and calculate for the unknown using the Ideal Gas Law.
8.
Discuss Dalton’s Law of Partial Pressures and when to use it.
9.
Given a word problem, determine known information and calculate for the unknown using Dalton’s Law of Partial
Pressures.
10. Discuss and explain the Postulates of the Kinetic Molecular Theory of Gases.
11. Calculate a stoichiometry problem in the gas phase.
VII.
Course Policies:
Grades of "Incomplete":
The current College policy concerning incomplete grades will be followed in this course. Incomplete grades are
given only in situations where unexpected emergencies prevent a student from completing the course and the
remaining work can be completed the next semester. Your instructor is the final authority on whether you qualify
for an incomplete. Incomplete work must be finished by mid-term of the subsequent semester or the “I” will
automatically be recorded as an “F” on your transcript.
Technology and Media
Email: Arkansas Northeastern College has partnered with Google to host email addresses for ANC students.
myANCmail accounts are created for each student enrolled in the current semester and is the email address your
instructor will use to communicate with you. Access your email account by going to
http://mail.google.com/a/smail.anc.edu and using your first and last names, separated by a period for your
username. Your default password is the last six digits of your Student ID. If you cannot access your student
email, contact the MITS department at 762-1020 ext 1150 or ext 1207 or send an email to
ANChelp@smail.anc.edu.
Internet: This course has a web component on myANC.
Student Expectations
Disability Access: Arkansas Northeastern College is committed to providing reasonable accommodations for all
persons with disabilities. This First Day Handout is available in alternate formats upon request. Students with
disabilities who need accommodations in this course must contact the instructor at the beginning of the semester
to discuss needed accommodations. No accommodations will be provided until the student has met with the
instructor to request accommodations. Students who need accommodations must be registered with Johnny
Moore in Statehouse Hall, 762-3180.
Professionalism Policy:
Per classroom etiquette: mobile phones, iPods, etc. must be silenced during all classroom and lab lectures. Those
not heeding this rule will be asked to leave the classroom immediately so as to not disrupt the learning
environment. Please arrive on time for all class meetings. If you know ahead of time that you will be late, please
contact the instructor ahead of time and provide that information. If a student is late for a lecture, I have no
problem with entering the class as long as it is done in a professional manner (no noise, no talking, etc).
NO TEXTING IN CLASS.
Academic Integrity Policy:
Academic dishonesty in any form will not be tolerated. If you are uncertain as to what constitutes academic
dishonesty, please consult ANC’s Student Handbook (http://www.anc.edu/docs/anc_handbook.pdf) for further
details. Students are expected to do their own work. Plagiarism, using the words of others without express
permission or proper citation, will not be tolerated. Any cheating (giving or receiving) or other dishonest activity
will, at a minimum, result in a zero on that test or assignment and may be referred, at the discretion of the
instructor, to the Department Chair and/or Vice President of Instruction for further action.
VIII.
Assessment
Any tools for institutional assessment will be provided by the Chemistry Department.
Assessment
Lecture – exams/quizzes/assignments
Final Exam
Percent of Final Grade
80%
20%
100%
Calculation of the final grade will be determined by the following grading scale:
Grading Scale (%)
90-100
A
80 – 89
B
70 – 79
C
60 – 69
D
0 – 59
F