Mercer County Community College
Course Number: CHE 100
Lecture Hours: 3
Length of Semester: 15 Weeks and a Final Exam Week
Cumulative Final Exam given in the 16th week.
Objectives - Topics covered in this course
Required Materials - what you must buy
College Catalog Description
Prerequisite and Corequisite
Evaluation and Grading
General Course Objectives -
Specific Course Objectives -
Topics covered in this course
Program Textbook - additional help if you want it
Mid-semester Evaluation Procedure
Topic Schedule and Homework Assignments
Introductory Chemistry 7th Ed.
Authors: Charles H. Corwyn
Publisher: Prentice Hall
Course Outline and Overhead Transparency Notes for CH100,
It is also required that the student purchase a ring binder type of
notebook and that these Transparency Note be placed therein.
Students must have a simple calculator that adds, subtracts, multiplies
and divides. Calculators that can store, in memory, formulas or other
are not allowed. Calculators that can convert from one type of units to
another are not allowed.
Selected fundamental principles of general chemistry. The course is
designed for students who have not had high school chemistry and for
who need a review of chemistry before taking other chemistry courses.
course does not include laboratory instruction. 3 lecture
Prerequisite - MAT 034 Basic Algebra
or equivalent proficiency.
Corequisite - placement in ENG 101 English Composition I
Course Coordinator: Michael Dorneman, Office MS 120,
Phone: 609-586-4800 x3369
Attendance is required at all classes. A missed test or quiz will
as zero. Students are also expected to be in class on time.
Homework consists of your reading the textbook, memorizing certain
and information, and doing homework problems. Additional studying must
be done on a continuing basis so that information needed to solve
and problem solving methods are remembered for quizzes and exams. It is
expected that you will write out all assigned homework in a neat and
fashion. All written homework is due the meeting after the
material is covered in class.
HOMEWORK WILL BE COLLECTED AT VARIOUS TIMES THROUGHOUT THE SEMESTER!
It is useful to note that the textbook generally gives more
than you need to know for this course.
It is required that the student purchase a ring binder type of
and that these Transparency Notes be placed therein. The notebook must
include additional blank loose-leaf (three-hole punched) paper between
pages of the Transparency Notes so that the student can take notes
lecture. Homework must be written out, also on loose-leaf paper, and
in the notebook in a section exclusively for homework. Additional blank
sheets should be included at the front of the notebook for important
such as exams, deadlines, etc.
Students must have a simple calculator that adds, subtracts,
and divides. Calculators that can store, in memory, formulas or other
are not allowed. Calculators that can convert from one type of units to
another are not allowed.
Evaluation and Grading:
The course grade will be based on exams, quizzes, class attendance,
and homework assignments.
There will be 3 hour exams given in class at approximately the time
indicated in the Homework Schedule, with the exact date to be
when the material on the exam is completed. Additionally, a cumulative
final exam will be given during the Final Exam period in the 16th week
of the semester. You must be present for the exams, including the Final
Quizzes will be given every week. In addition surprise quizzes will
Homework assignments will be collected and graded several times
the semester. For credit, homework must be written in a neat and
fashion, showing work and explaining your answers.
The course grade will be determined by the total number of points
The following table describes the point value for each component.
Exam I, 100 % score
Exam II, 100 % score
Exam III, 100 % score
Exam IV, 100 % score
(Given in Finals Week and is cumulative)
Quizzes (Total of 12 best) 120, 10 points each
Attendance (see below), 20 for no absences
Total possible 540 Cut off scores for each letter grade are listed below.
Attendance Points: There are no excused absences. It
expected that all students will attend all classes. Points are lost for
missing classes: -0 for the first absence; -0 for the second; -0 for
third; -0 for the fourth; and -5 for the fifth subsequent absences to a
total of -20 points for missing 8 classes.
Course Grade: Although the majority of the course grade comes from
scores, attendance in class is critical to learning. A student that
substantial portions of the course will receive a failure grade. Missed
exams cannot be "made up", and Incomplete grades will not be given.
Course Grade Calculation: A student must pass the final exam
pass the course. For course grade assignment, see the chart
1. Total your percentage scores from all four exams.
2. Add in your Attendance points:
20 points if you missed 4 or fewer classes
15 points if you missed 5
10 points if you missed 6
5 points if you missed 7
0 points if you missed 8 or more
3. Add in your 12 best quiz scores.
4. Add in any points for homework or bonus.
5. Look up your point total here:
503 - 540 =
A (more than 93%)
486 - 502 =
A- (more than 90%-93%)
470 - 485 =
B+ (more than 87%-90%)
449 - 469 =
B (more than 83%-87%)
432 - 448 = B-
411 - 431 =
C+ (more than 77%-80%)
368 - 410 =
C (more than 70%-77%)
303 - 368 =
D (more than 60%-70%)
Less than 303 = F
General Course Objectives:
This course will take the place of a high school chemistry course
a curriculum at MCCC that requires such a course for entrance. You must
therefore learn the technical terms and the principles that will be
in courses in Nursing, Mortuary Science, etc. that have to do with
This course, then, will be helpful to students taking the chemistry
courses in the Nursing programs, or taking CHE 101, General Chemistry.
Since CHE 100 is a fundamental science course, it will be helpful if
take such courses as BIO 101 or PHY 101 (biology or physics).
Introductory Chemistry is not an adequate course in the physical
for a student majoring in business or the liberal arts.
- Define Chemistry, give its two major subdivisions, and define
describe the other subdivisions of chemistry, define matter.
- Describe what each of the following societies or individuals had
with the history of chemistry:
Ancient Egyptians, Ancient Greeks, Alchemists,
Robert Boyle, Antoine
Lavoisier, Neils Bohr, Albert Einstein.
- Know the four steps in the
scientific method and define and
between an observation, a hypothesis, a theory, and a scientific law.
- Define and differentiate between qualitative measurements and
measurements; give examples of each.
- Know and describe the 3 parts of a measurement.
- Define and contrast accuracy and precision.
- Define the term significant digits and, given a measurement,
number of significant digits in the number. (Know and use the rules for
- Define and give at least 3 examples of fundamental quantities and
- Use the technique for rounding off numbers.
- Use the rules for keeping the proper number of significant digits
answer when doing a calculation involving multiplication and/or
and when doing a calculation involving addition or subtraction.
- For a number written in Scientific Notation, identify its parts
and the order of magnitude) and be able to convert a number from the
it is normally written (decimal notation) to scientific notation or
scientific notation to decimal notation.
- Define length, mass, weight, and volume and state the difference
mass and weight.
- Know the metric units and measuring device for length and mass.
- Know the metric units for volume (cm3 , ml and L) and convert
- Define and convert between metric units with prefixes milli,
and kilo, and give examples of objects of these sizes.
- Know what unit factors are, how to make them, and be able to use
solving problems and when converting between different units.
- Define temperature, Fahrenheit, Celsius, and Kelvin temperatures,
the formulas for conversion between Fahrenheit and Celsius. Be able to
tell if a temperature is cold, room temperature, hot or very hot in
system. Be able to list the Freezing point and melting point of water,
room temperature, and body temperature in both Fahrenheit and Celsius.
- Define heat, calorie, Calorie, kilocalorie, joule and specific
- Define density, know the formula for density (D=M/V), be able to
density, know how a change in M or V affects D, and tell which
will float or sink in a liquid and why. Define specific gravity and
how it is related to density.
- Define physical properties, give 6 examples, and identify
of a substance.
- Define and describe the four physical states of matter, including
description volume and shape, attraction between, motion of, and
between the elementary particles in that state, and identify the state
of a substance.
- Identify and define the various types of matter (pure, compound,
mixture, homogeneous, heterogeneous, phases of mixture, substance) and
- Define chemical properties, give 6 examples and identify the
of a substance.
- Describe and differentiate between physical and chemical
physical and chemical changes, and identify which occur during an event.
- Define energy, potential energy, kinetic energy, heat energy,
potential energy, and, in a particular situation, identify energy as
potential or kinetic, and describe how these are related to chemical or
- State the law of conservation of matter and the law of
energy, give examples of where and how these laws are important, and
this is related to chemical changes. Describe the roles of Lavoisier
Einstein with respect to these laws.
- Define an element, give examples, identify them from a list of
and state how elements are related to atoms.
- List (not necessarily in order) the 6 most common elements in the
body, and the 4 most common elements in the earth's crust.
- Define and identify the symbol for an element, given the name of
write the symbol and given a symbol, write the name for selected
- Define, differentiate between, and give examples of compounds,
molecular compounds, ions, cations, anions, and molecules. State what
of bond holds different types of compounds together, and which type of
elements form which kind of compound.
- State how an element, compound, and mixture differ; identify
as either a compound, mixture, or element.
- Calculate the % of a component in a mixture, or the amount of a
in a mixture given its percent.
- Define chemical formula and subscript, given a formula, state the
involved and how many atoms of each element; also use parenthesis in
- Know the classes of elements and properties of each class; where
located in the periodic table, which elements are gaseous at room
which are diatomic, which elements are monatomic gasses, and what the
diatomic and monatomic mean.
- Define a binary compound; give examples; given a formula,
binary or not, and give its name (if binary).
- Define a chemical equation (reaction), define and identify
coefficients; given the reactants and products, balance a chemical
state the coefficient on each formula in a chemical equation.
- State the name, charge, relative mass, and location in an atom of
types of sub-atomic particles in an atom.
- Define atomic number, state how it is related to the sub-atomic
in an atom, and how it is related to different atoms.
- Describe the arrangement of the periodic table and note the
importance of families or groups, periods, A and B subgroups, alkali
Halogens, Noble Gasses, metals, non-metals, semi-metals, Transition
and Representative elements.
- For the representative elements, from their position on the
give the correct formula for a binary compound.
- Describe Rutherfords's picture of an atom in detail.
- Describe Bohr's theory of atomic structure. Define energy levels
and relate them to Bohr's theory.
- Describe the quantum mechanical theory of the structure of the
how this differs from the Bohr structure. Define energy levels.
- Describe electron structure, define Principal Quantum Shell and
each represents. State how many electrons the Principal Quantum Shell
hold, and define valence shell.
- Define orbitals; state where they are located, how each is
how they are related to principal quantum levels, how many electrons
can contain, and how they are related to energy levels.
- State what importance sub-orbitals have and how many electrons a
can hold; draw and describe the s and p sub-orbitals.
- Given a periodic table, give the electronic structure (or
for an element. Give the Valence Configuration for an element.
- State what is special about the Noble Gasses and why, with
electron configuration. Define stability.
- Define atomic weight, mass number, atomic number and isotopes and
how they are related. Given a periodic table, give the atomic number or
atomic weight of any element. Relate these concepts to the subatomic
that are contained in a specific atom.
- Describe how and why the size of the atoms changes in relation to
position on the period table. Given a list of elements, state which
have a larger or smaller atom.
- Describe in detail how the periodic table is related to electron
- Define ionization and ionization energy and state how and why the
of ionization changes in relation to an elements' position in the
table. Given a list of elements, state which will be easier or harder
ionize, and which will have the higher (or lower) ionization energy.
- Define electron affinity, state how it is related to ionization
the electronic structure of an atom.
- State the octet rule; given a periodic table, tell which elements
and which elements lose electrons to complete their octets; state what
happens to an atom when it completes its octet.
- Use the octet rule to give the charge on the monatomic ion for
- Describe ionic bonding, including what type of elements form this
how the electrons are involved, and the nature of the attractive force.
Give the properties of ionic compounds.
- Draw Lewis Dot structures for elements, ionic compounds, and
compounds (such as water, ammonia, carbon dioxide, methane, HCl).
Lewis Dot structures to valence electron configuration and the octet
- Determine the correct formula for an ionic compound, given the
or polyatomic ions involved.
- Describe covalent bonding including what type of elements form
how the electrons are involved, and the nature of the attractive force
- describe a bonding orbital, how it is made and how many electrons it
contains. Describe a single, double, and triple bond. Give the
of covalent compounds.
- Define electronegativity, state which element is most and which
electronegative and where they are on the periodic table. Given a list,
select the most and least electronegative elements. Tell how
is related to bonding, bond type, and polarity of a molecule or
of a bond. List the four most electronegative elements in order.
- Define a polar molecule and a polar bond; given a series of
decide which is most or least polar. State why H2O or NH3 are polar and
CO2 or CH4 are not; state what elements are involved in non-polar bonds.
- Define polyatomic ion. State the name, formula and charge of
ions (sulfate, sulfite, nitrate, carbonate, phosphate, cyanide,
hydroxide, bicarbonate, and ammonium).
- Define oxidation number and state how it relates to the charge of
Given a periodic table, give the oxidation number for any
element alone or as part of any compound. Give examples of elements
can have more than one oxidation state. Give the formula and oxidation
numbers of selected elements that have more than one oxidation state
Fe, Sn, Pb, Hg).
- Given the elements or ions involved in a compound, give the
of that compound.
- Given the formula for any of the following types of compounds,
correct chemical name for that compound, and given the name, give the
formula. Binary - metal and non-metal, i.e., PbCl4, FeCl3, Binary - 2
i.e., CO2, SO2, SO3,P205, Binary - with hydrogen cation, i.e., HCl,
Ternary - oxy-acids, i.e., H2SO4, HNO3, H2CO3, Ternary - bases
Ternary - metal and polyatomic anion.
- Define a salt; given an acid or base, give examples of its salts;
a salt, name the corresponding acid. Define neutralization reaction.
- Define a mole in terms of atoms or molecules, and grams of a
- Given a number of moles, using unit factors, calculate a number
or molecules; given a number of atoms or molecules, calculate a number
- Given a number of grams of an element or compound,
(using unit factors) the number of moles. Given a number of moles of an
element or compound, calculate the number of grams.
- Given a number of grams, calculate using unit factors a number of
- Given a name or formula of a compound, calculate the formula
- Given a formula or name of a compound, calculate the percent
Given 2 or more compounds that all contain a particular element,
which has the largest or smallest % of that element.
- Define empirical formula, describe its relation to and difference
- Define chemical equation and balanced equation. Given a chemical
identify the reactants, products, and coefficients, and balance the
- Given the reactants only, give the 3 steps in completing and
a chemical equation, and complete and balance the equation.
- Describe a synthesis reaction, give examples of the 4 types of
reactions (metal and non-metal, element and oxygen, water and metal
water and non-metal oxide), complete and balance all these types of
- Describe decomposition reactions, give examples and complete and
this type of reaction.
- Describe single displacement reactions and give examples. Define
the activity series and how this relates to single displacement
Give examples of common metals more or less active than iron. Define
and reduction, state how this relates to reactions and give examples.
and balance single displacement reactions.
- Describe double displacement reactions, complete and balance
and describe a neutralization reaction, give the general formula for a
neutralization reaction, complete and balance neutralization reactions.
- Tell why chemical reactions occur, define exothermic and
and give examples of each.
- Identify a reaction as a combustion reaction, state the products
of a hydrocarbon, and given only the reactants, complete and balance a
- Given a balanced reaction, give all the mole ratios (unit
that reaction, and tell which are used to calculate moles of one
from moles of another.
- Given a balanced reaction, and (for one compound in the reaction)
of moles of a compound, calculate the moles of all other compounds used
or produced. (Perform mole - mole calculations from balanced chemical
- Given a mass (or moles) of one participant in a balanced
the mass (or moles) of all other substances used or produced in the
- Define stoichiometry.
- Define evaporation, heat of vaporization, boiling point, heat of
freezing, sublimation, condensation. State which processes are
and which are endothermic.
- State how water differs from H2S, H2Se, H2Te and why. Define
what elements are involved in hydrogen bonding, and how hydrogen
affects the physical properties of water.
- Write a reaction for the formation of water from its elements,
of water, the reaction of a metal oxide or non-metal oxide with water.
List 3 non-metal oxides in Acid Rain, and where they come from.
- Define a hydrate; given a hydrate, write the balanced
for its dehydration. Define anhydrous salt.
- Describe ozone, give its formula, state how it is formed, how it
why it is important, where it is pollution, where it is not pollution,
- Define and identify solution, solute and solvent, give examples.
- Define concentration, dilute, concentrated, unsaturated,
- Describe (generally) why things dissolve in water (and why things
dissolve in water), what affects the amount that dissolves, and how
- Define molarity and molar solution, given a volume of solution
of solute or grams of solute, calculate molarity. Given molarity and a
volume, calculate moles of solute.
- Define percent by weight, given a mass of solute and solvent (or
calculate the percent concentration, define a weight/volume percent,
a weight/volume percent define a volume/volume percent.
- Define PPM (parts per million); give examples of things measured
Given the mass of solute and solvent, calculate a concentration of PPM.
- Know and be able to use the formula M1V1=M2V2 to solve dilution
- Define, describe, and explain colligative properties, osmosis,
and osmotic pressure, including examples.
"Chemical Problem-Solving by Dimensional Analysis"
Author: Loebel, Arnold B.
This book is in the library on reserve under Professor Dorneman's
DO NOT WRITE IN THE TEXTBOOK!
This is a programmed textbook, that is, it leads you through a
of material and requires you to answer questions on the material as you
proceed. It takes you through a particular type of problem in a
manner, asking questions that you will answer and checking your answers
at every step.
This book does not do everything exactly as done in lecture, but
are done in a very similar fashion. The major difference is in
Specifically, what your course manual calls unit factors, this book
conversion factors and what this book calls gram molecular weight (or
atomic weight) your course manual shortens to molecular weight (or
The sections of this book are independent and can be used if you are
having problems with a specific topic or need review.
||Chapter and Section
|Rounding Off Numbers
||2 A B, 4 A
|Temperature Scales and Conversions
|Balancing Chemical Equations
(skip meta, ortho, pyro)
|9 A C D F
|Salts of Acids
Number, and Mass Calculations
|Mole Ratios and Calculations
from Chemical Equations
|10 A B
- use the following proceedure:
Calculate the percentage of points that you have acquired to date and
compare that to the chart below.
(total your quiz scores) + (your score on the first exam) = part you
(amount of quizzes given to date x 10) + 100 = total possible
Your % = (part you care about) x 100
If your % is: Your grade is:
91% - 100% = A
81% - 90.9% = B
70% - 80.9% = C
60% - 69.9% = D
- See the directions on pages 2 and 3 of this Course Outline.
Topic Schedule and Homework Assignments (approximately by week)