DELAWARE TECHNICAL AND COMMUNITY COLLEGE 
CAMPUS COURSE SYLLABUS
Campus:
Wilmington
Department: Allied Health/Science
Course Number and Title: CHM 110 - General Chemistry
Instructor Name: Ray Lynch, MD Telephone:
302-571-5320
E-mail:
wlynch@dtcc.edu
Web
Site: http://physics.dtcc.edu
Pre-requisites: ENG 051, RDG 051, MAT 015/016
Course Hours and Credits: 3:2:4
Course Description: This course is designed for students
majoring in technical areas other than chemistry. It includes chemical
reactions, the metric system, structure of matter, nomenclature, gases,
solutions, acids, bases and nuclear chemistry. A laboratory sequence illustrates
theory.
Text: Introduction to General Organic and
Biochemistry, 7th ed., Frederick A. Bettelheim and Jerry March, Harcourt
College Publishers (2004).
CHM 110 Lab Manual,
Wilmington
Campus Bookstore
Materials: Scientific calculator
Method of Instruction: Lecture/Lab
Manuals: Allied Health/Science Department Policy Manual
2008-2009
CORE COURSE PERFORMANCE OBJECTIVES
-
Convert between English and SI measurements. (CCC7,9)
-
Describe the structure of matter at the atomic and molecular
level. (CCC1,5,9)
-
Outline types of chemical reactions and balance equations.
(CCC1,2,7,9)
-
Contrast the properties of gases, liquids, solids, and
solutions. (CCC5,7,9)
-
Perform stoichiometric calculations; perform calculations
using the gas laws. (CCC 7,9)
-
Describe acids, bases, and buffers, and perform calculations
used to evaluate them. (CCC5,7,9)
-
Describe simple organic compounds (alkanes), including names,
structures, formulas and example reactions. (CCC5,9)
-
Discuss nuclear radiation, including nomenclature. (CCC9)
-
Perform laboratory exercises demonstrating basic chemical
principles. (CCC2,7,9)
MEASURABLE PERFORMANCE OBJECTIVES
Upon completion of various teaching methods, which may include:
lecture presentations, assigned readings, class discussions, independent study
and laboratory exercises, the student will demonstrate 75% proficiency in each
of the following objectives:
1. Convert between English and SI measurements.
1.1 Name the metric base units and SI units for mass, length,
volume, and temperature and their abbreviations.
1.2 Interpret scientific notation and prefixes for units of
measure and convert numbers to and from scientific notation.
1.3 Convert physical quantities from one unit to another by
using conversion factors.
1.4 Apply the factor-label method, problem analysis, and
estimation techniques to solving problems.
1.5 Convert a temperature in oC, oF, or K to the other scales.
2. Describe the structure of matter at the atomic and molecular
level.
2.1 Define matter, energy, and chemistry.
2.2 Distinguish among mixtures, pure substances, elements, and
compounds.
2.3 Name and give the symbols for the most important elements.
2.4 Differentiate the different types of energy.
2.5 Distinguish between the calorie, kilocalorie, and Joule.
2.6 Define heat, specific heat, density, and specific gravity
and use these quantities in calculations.
2.7 Name the major assumptions of modern atomic theory.
2.8 Name the 3 subatomic particles and their symbols, relative
masses, charges, and location.
2.9 Explain the composition of different atoms in terms of the
number of protons, neutrons, and electrons.
2.10 Identify isotopes of an element from their atomic
composition.
2.11 Define and distinguish atomic number, mass number, and
atomic weight.
2.12 Describe the arrangement of electrons within shells and
subshells of an atom and write the electron configuration of an atom.
2.13 Explain the relations between atomic energy and electronic
arrangement.
2.14 Describe the relationship between absorption and release of
energy by an electron and changes in energy level.
2.15 Explain the relationship between the energy of radiation
and its wavelength.
2.16 Describe the arrangement of elements in the periodic table.
2.17 Define and distinguish period, group, metal, nonmetal,
alkali metal, alkaline earth metal, halogen, and noble gas.
2.18 Discuss the periodic law and relate the position of an
element in the periodic table to its electronic structure.
2.19 Define ion, cation, anion, ionic bond.
2.20 Draw electron dot structures for the first 20 elements.
2.21 Describe how a given ion differs from its parent neutral
atom.
2.22 Describe the octet rule and discuss its significance.
2.23 Discuss the properties of ionic compounds.
2.24 Given an element from a main group (A groups) give the
symbol of the ion that element forms.
2.25 Define covalent bond and describe its formation.
2.26 Name the elements which exist as diatomic molecules.
2.27 Predict the numbers of covalent bonds usually formed by the
more common main group elements.
2.28 Interpret molecular formulas, structural formulas, and
Lewis structures.
2.29 Recognize and distinguish single, double, and triple
covalent bonds.
2.30 Draw Lewis structures and use them to predict molecular
geometry.
2.31 Define electronegativity and describe the trends in
electronegativity within periods and groups of the periodic table.
2.32 Indicate the polarity of polar bonds with the partial
charge notation:∂+,∂-
2.33 Given two elements that are bonded and their
electronegativities, determine whether the bond is ionic, polar covalent, or
nonpolar covalent.
2.34 Use electronegativity and molecular geometry to predict
bond and molecular polarity.
3. Outline types of chemical reactions and balance equations.
3.1 Name and write formulas for ionic compounds containing
polyatomic ions.
3.2 Explain the significance of formula units in describing
ionic compounds.
3.3 Calculate the formula weight of any given ionic compound and
explain what the formula weight represents.
3.4 Name and write formulas for molecular compounds.
3.5 Discuss the properties of molecular compounds.
3.6 Describe the differences in structure, composition, and
properties of ionic and molecular compounds.
3.7 Describe how ions are formed from certain molecular
compounds by loss or addition of hydrogen.
3.8 Translate a written description of a chemical reaction into
a balanced chemical equation and vice versa.
3.9 Balance a chemical equation.
3.10 Explain the meaning and uses of the mole and Avogadro's
number.
3.11 Given the formula of a compound, calculate its formula
weight (molar mass).
3.12 Convert between molar and mass quantities of any element or
compound.
3.13 Given an equation, identify the reaction as either
combination, decomposition, single, double replacement, or redox.
3.14 Write the net ionic equation for a given exchange reaction.
3.15 Recognize and distinguish oxidizing agents and reducing
agents.
3.16 Explain the factors that influence energy changes in
chemical reactions.
3.17 Define heat of reaction and calculate the quantity of heat
absorbed or released in a given reaction.
3.18 Define and distinguish endothermic and exothermic
processes.
3.19 Explain the significance of spontaneity and entropy in
chemical reactions.
3.20 Explain how collisions and activation energy determine
reaction rate.
3.21 Describe what is occurring in a reaction that is at
equilibrium.
3.22 Predict the effects of changes in conditions on reaction
rates and chemical equilibria.
4. Contrast the properties of gases, liquids, solids, and
solutions.
4.1 State the assumptions of the kinetic theory of gases and use
them to explain gas behavior.
4.2 Name and define the common units of pressure.
4.3 Define partial pressure and use Dalton's Law of partial
pressures.
4.4 Apply the concepts of heat exchange, equlibrium and vapor
pressure to changes of state.
4.5 Define and distinguish the principal intermolecular forces.
4.6 Discuss the significance of hydrogen bonding.
4.7 Describe the relations among vapor pressure, temperature,
and boiling point.
4.8 Describe how boiling point is affected by changes in
atmospheric pressure.
4.9 Perform calculations with heat of fusion and heat of
vaporization.
4.10 Distinguish solids, liquids, and gases.
4.11 Describe the properties of solutions and distinguish them
from ordinary mixtures.
4.12 Define and distinguish solution, suspension, and colloid.
4.13 Explain how the nature of solute and solvent affect
solubility.
4.14 Describe the influence of temperature and pressure on
solubility.
4.15 Define, use, and convert between the most common ways of
expressing solution concentration; percent concentration and molarity.
4.16 State the result of a dilution and explain how to make a
desired dilution.
4.17 Define and distinguish strong, weak, and nonelectrolytes
and use electrolyte concentrations in equivalents.
4.18 Define and distinguish diffusion, osmosis, and dialysis.
4.19 Define osmotic pressure and discuss its significance.
5. Perform stoichiometric calculations; perform calculations
using the gas laws.
5.1 Perform mole and mass calculations using chemical equations.
5.2 Calculate percent yield for a reaction.
5.3 State Boyle's Law, Charles' Law, and Avogadro's Law; explain
them in terms of the kinetic theory, and use them in calculations.
5.4 State the universal gas law and use it in calculations.
6. Describe acids, bases, and buffers, and perform calculations
used to evaluate them.
6.1 Describe the properties of acids, bases, and salts.
6.2 Discuss the dual acid-base character of water and explain
its origin.
6.3 List the common types of acid-base neutralization
reactions and write equations for them.
6.4 Write the names and formulas for the most common acids and
bases.
6.5 Define and distinguish strong and weak acids and bases in
terms of their electrolyte character.
6.6 Discuss the ionization of water.
6.7 Define pH and perform calculations with pH.
6.8 Discuss the techniques used for measuring pH.
6.9 Describe the composition and action of buffer solutions.
6.10 Calculate the equivalent weight of a substance and
perform calculations with equivalents.
6.11 Define normality.
7. Describe simple organic compounds (alkanes), including
names, structures, formulas and example reactions.
7.1 Explain the significance of carbon compounds.
7.2 Identify the principal functional group families of
organic compounds.
7.3 Draw structural formulas for organic compounds.
7.4 Define and distinguish structural isomers.
7.5 Name alkanes using the IUPAC system.
7.6 Compare the properties and reactions of organic and
inorganic compounds.
7.7 Define and distinguish aliphatic and aromatic compounds.
7.8 Describe the composition of polymers.
7.9 Name and distinguish the principal types of biomolecules.
7.10 Discuss the properties of enzymes.
8. Discuss nuclear radiation, including nomenclature.
8.1 Define radioactivity and the terms used to describe it.
8.2 List the characteristics of alpha, beta, and gamma
radiation.
8.3 Describe the important factors in protection from radiation.
8.4 Describe the processes of alpha, beta, and gamma decay.
8.5 Define half-life, and use it to calculate the radioactive
material remaining after a period of time.
8.6 Define ionizing radiation, and describe the properties of
its different forms.
8.7 List and define the common units for measuring radiation.
9. Perform laboratory exercises demonstrating basic chemical
principles.
9.1 Interpret the number of significant figures in a
physical quantity and round off numbers in calculations involving physical
quantities.
9.2 Distinguish between physical and chemical changes.
9.3 On a heating-cooling graph, identify the parts of the
graph that correspond to changes in temperature and changes in state.
9.4 Describe a titration experiment.
Evaluation
Criteria / Policy:
Students will demonstrate proficiency
on all measurable performance objectives at least to the 75% level to
successfully complete the course. The
grade will be determined using the college grading system:
92-100 =
A
83- 91 =
B
75- 82 =
C
0 -
74 = R
Students should refer to the DTCC
Student Handbook and the Allied Health/Science Department Policy Manual
for information on Academic Standing Policy, Academic Honesty Policy, Student
Responsibilities and Student Rights, and other policies relevant to their
academic progress.
