Division of Math and Science
Arkansas Northeastern College
Departmental Course Syllabus: General Chemistry I and Lab
CH 14023 / CH 14031
I.
Course Prerequisites
Prerequisite: Grade of “C” or better in College Algebra (MA 14043). Co-requisite: General Chemistry I Lab (CH
14031) must be taken with this course.
II.
Course Catalog Description
This course is designed to include the basic principles of chemistry, including the correlation between electronic
configurations of their elements and their chemical properties.
III.
Required Texts and Materials
General Chemistry
Ebbing and Gammon
Houghton Mifflin Company
Laboratory Notebook
(carbonless quad notebook)
W.H. Freeman and 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
 Implement a substantial vocabulary in chemical nomenclature and fundamental chemical processes
through written and oral communications.
 Demonstrate an overall working knowledge of the scientific method, elements and compounds, chemical
nomenclature and the characteristics of the states of matter.
 Demonstrate a systematic process to address chemical stoichiometry, conversions and word problems in
all phases of matter.
 Demonstrate a working knowledge of the behavior of gases and the gas laws.
 Demonstrate a working knowledge of thermodynamic processes and application of thermodynamics in
order to predict spontaneity of a reaction.
 Demonstrate the ability to correlate electronic structure to reactivity.
 Demonstrate a working knowledge of molecular geometry and hybridization, leading into Molecular
Orbital Theory.
VI.
Unit and Instructional Objectives
Lecture Topical/Unit Objectives:
I. Unit One
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:
A. Chemistry and Measurement
1. Given a specific situation, discuss and demonstrate how the Scientific Method is utilized.
2. Define and contrast: matter, material, substances, elements, compounds and mixtures
3. Discuss the states of matter, and the transformation from one state to another
4. Given a word problem involving multistep calculations, apply correct significant figures in calculations
5. Describe and apply: conversion from English to Metric system of measurement, units, prefixes, derived units
and dimensional analysis (factor-label method)
B. Atomic Structure: Nuclear Model
1. Given a particular element, explain the atomic structure of the atom, giving names and characteristics to
subatomic particles
2. Identify sections of Periodic Table: metals, nonmetals, groups, periods, halogens, etc.
3. Given a particular isotope, identify the atomic number, mass number, and determine the number of electrons
in that atom.
4. Given a nuclear reaction, identify a radioactive decay and/or a nuclear bombardment reaction.
5. Given a nuclear reaction, classify the type of radioactive decay (alpha emission, beta emission, etc)
6. Given the decay constant for a nucleus, calculate the half-life of the nucleus.
C. Chemical Formulas and Chemical Nomenclature
1. Write the compound name from chemical formula, and write chemical formula from compound names
2. Differentiate between a molecular and ionic compound, and determine molecular weight and formula weight.
3. Calculate the mass of an atom or molecule, convert moles to grams (and grams to moles), and calculate the
number of molecules in a given mass.
4. Calculate percentage composition from a chemical formula, and calculate the mass of an element in a given
mass of compound.
5. Determine empirical formula from percent composition, and determine molecular formula from percent
composition and molecular weight.
II. Unit Two
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:
A.
Chemical Reactions and Stoichiometry
1. Given a chemical equation (word form) and masses of reactants, identify and utilize the limiting reactant.
2. Using solubility rules, predict precipitation reactions
3. Given the reactants only, predict and complete the molecular equation, the complete ionic equation and the
net ionic equation.
4. Given a reaction, classify it as precipitation, acid-base or oxidation-reduction reactions.
5. Assign oxidation numbers, recognize redox reaction, and balance
6. Calculate dilutions of solutions, and preparations of required molar concentrations
7. Calculate the volume of a reaction solution necessary in a given reaction, and calculate the quantity of
substance in a titrated solution.
B. The Gaseous State and Kinetic Theory
1. Define pressure, utilize pressure unit conversions, and calculate pressure problems
2. Utilize the empirical gas laws and explain the relationship between pressure, temperature and volume.
3. Given a word problem, recognize which gas law applies, and calculate accordingly.
4. Given a word problem, demonstrate the relationship between gas density and molecular weight
5. Discuss and do calculations using the Law of Partial Pressures
6. Given a ‘real-gas’, calculate pressure or volume accordingly using van der Waals equation.
7. Given a particular gas, calculate the root-mean-square (rms) speed.
8. Discuss Maxwell’s distribution of molecular speeds.
III. Unit Three
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 energetics of electrons is necessary for continuing scientific
education.
Objectives: The student will be able to:
A. Thermochemistry
1. Given the mass and speed of an object, calculate the kinetic energy
2. Compare and contrast: heat and energy.
3. Differentiate and calculate using heat of reaction, standard enthalpy and standard enthalpies of formation
4. Define and apply Hess’s Law
5. Given a thermochemical reaction, calculate the heat of reaction from stoichiometry
6. Discuss the difference between heat and specific heat
7. Calculate the heat of phase transition from standard enthalpies of formation
8. Calculate the enthalpy of reaction from standard enthalpies of formation
B. Electron Configurations and Periodicity
1.
Given an orbital diagram or electron configuration, apply the Pauli exclusion principle in locating electrons.
2.
Determine the configuration of an atom using the building-up principle
3.
Determine the configuration of an atom using the period and group numbers
4.
Given a particular atom, write the configuration and apply Hund’s rule, and discuss
5.
Identify periodic trends and predict characteristics of elements by their position on the periodic table
C. Quantum Theory of the Atom
1.
Calculate wavelengths and frequency using the speed of light in a vacuum.
2.
Given either wavelength or frequency, calculate the energy of a photon
3.
Given a particular hydrogen atom transition, determine the wavelength, frequency and energy.
4.
Discuss the Bohr Theory of the Hydrogen Atom
5.
Given a set of quantum numbers, state whether the set is valid
6.
Define the four quantum numbers which describe any electron
IV. Unit Four
Rationale: An understanding of the bonding within a molecule is the basis on which further chemical education is based.
Objectives: The student will be able to:
A. Ionic and Covalent Bonding
1.
Define chemical bonding, and given various compounds, identify types of bonds involved.
2.
Given a polyatomic ion or compound, draw Lewis dot structures to represent bonding in the compounds,
including exceptions to the octet rule.
3.
Given two disparate elements, use periodic trends to compare relative ionic radii
4.
Write electron configurations of ions
5.
6.
7.
Describe covalent bonds, and how they differ with ionic bonds
Discuss polarity and electronegativity
Explain bond length, bond energy and bond order
B. Valence Bond Theory and Molecular Geometry
1.
Given the number of bonds and lone pairs around an atom, determine the probable molecular geometry
around that atom.
2.
Given a compound, draw Lewis Dot structures to determine hybridization
3. Given a compound, utilize VSPER Model to predict the shape, geometry and hybridization involved.
4.
Given a compound, describe (in words using correct grammar) the bonding – including hybridization, sigma
and pi bonds, and molecular geometry using the VSPER Model.
C. Molecular Orbital Theory
1. Given a simple diatomic molecule, describe the molecular orbital configuration.
2. Given a simple diatomic molecule, determine the bond order, diamagnetic or paramagnetic properties, and the
molecular configuration.
3. Discuss the advantage of Molecular Orbital Theory with respect to delocalized bonding (resonance).
Laboratory:
Rationale: The ability to work safely and efficiently in a laboratory setting is essential. The laboratory, taken
concurrently with the lecture, illustrates and reinforces the material and principles in General Chemistry I. The skills
developed in a controlled laboratory setting, including documentation, computer skills, and chemical handling, will
translate into a myriad of settings and prepare the student for further educational and career opportunities.
Objectives: The student will be able to:
Experiment 1: Lab Safety and Correct Documentation Techniques
1. Locate and utilize all safety equipment in the laboratory.
2. Write a prelab after reading an experimental procedure.
3. Record data in a laboratory notebook in the correct manner, and plan data sheets and post labs.
Experiment 2: Evaluation of Data
1. Recognize and correctly use a triple beam balance, measuring and recording masses to the 0.01 g.
2. Correctly complete volume readings from graduated cylinders.
3. Utilize a graduated pipette correctly.
4. Use EXCEL spreadsheet to record, manipulate and graph data.
5. Begin mastering the skill of producing a ‘work-product’ level lab report.
Experiment 3: Chemical Nomenclature – Study Lab
1. Classify ionic and covalent compounds.
2. Name compounds from formulas.
3. Write formulas from chemical names.
4. Write and balance a chemical reaction given words only (not given formulas).
Experiment 4: Household Chemicals
1. Identify a precipitation reaction (microscale).
2. Identify a reaction in which a gas is formed.
3. Collect qualitative information on a series of reactions, and then identify an unknown based on this.
Experiment 5: Copper Lab
1. Given the series chemical reactions, calculate the necessary amounts of each reactant in order to insure copper
is the limiting reactant in each step.
2. Calculate the necessary volumes of solutions required for the series of reactions, and then preparing the correct
concentration of all solutions.
3. Complete the reactions in lab, collecting and recording data in lab notebook (correct documentation).
4. Identify and classify different types of reactions (precipitation, redox) which are part of the reaction scheme.
5. Produce a ‘work-product’ level lab report.
Experiment 6: Titration #1
1. Demonstrate the correct procedure for setting up the apparatus for a titration.
2. Demonstrate the correct titration procedure.
3. Determine an endpoint using phenolphthalein indicator.
4. Calculate the percent of a compound in a solution from data collected.
Experiment 7: Titration #2
1. Set up titration apparatus.
2. Calculate and prepare all solutions necessary for standardization of a NaOH solution using oxalic acid dehydrate
as the primary standard.
3. Use an analytical balance and perform titrations to standardize NaOH solution.
4. Use standardized NaOH solution to determine the molarity of an unknown acid solution.
5. Produce a ‘work-product’ level lab report.
Experiment 8: Alum from Aluminum
1. Safely use NH4OH reagent in a chemical reaction.
2. Dry product by correctly utilizing a Buchner funnel.
3. Produce a ‘work-product’ level lab report.
Experiment 9: Hess’s Law
1. Correctly read a thermometer.
2. Utilize a graduated pipette correctly.
3. Set up a ‘macro’ program in EXCEL to complete calculations
4. Produce a ‘work-product’ level lab report.
Experiment 10: Specific Heat
1. Correctly read a thermometer.
2. Calculate specific heat using method of mixtures.
3. Set up a ‘macro’ program in EXCEL to complete calculations
Experiment 11: Lewis Dot Structures
1. Draw Lewis dot structures for a series of molecules.
2. Determine correct Lewis dot structure using formal charges.
Experiment 12: Molecular Geometry
1. Draw Lewis dot structure, and determine VSPER class and molecular geometry.
2. Using ball and stick model, build molecules in 3-D.
3. Predict hybridization.
4. Discuss (using complete sentences and correct grammar) the bonding in a molecule.
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.
Calculation of the final grade will be determined by the following:
Assessment
Lecture – exams/quizzes/assignments
Final Exam
Laboratory
Final grades will be assigned according to the following:
Grading Scale (%)
90-100
A
80 – 89
B
70 – 79
C
60 – 69
D
0 – 59
F
Percent of Final Grade
55%
20%
25%
100%