Description:

This course is an introduction to the fundamentals of chemistry, with emphasis on general concepts of inorganic chemistry and sufficient study of organic chemistry to introduce the student to biochemistry. The student will learn basic definitions and theories of chemistry, solve numerical problems related to chemical principles and apply chemical concepts in laboratory work. 4 hrs. lecture, 3 hrs. lab/wk.

Associated Costs: These are additional (out-of-pocket) expense considerations that students should expect in addition to the course tuition, fees, and textbooks. $60.

Supplies: Refer to the instructor's course syllabus for details about any supplies that may be required.

Prerequisites: NONE

Textbook(s): For information see - http://bookstore.jccc.net

Course Fees: NONE

Course Objectives:

Course Rationale:
Principles of Chemistry is required to supply chemical background for
students with a desire to pursue a career in a medical related field such
as nursing, dental hygiene, respiratory care, etc., or a need for a lab
science credit in a physical science.  These individuals need a general
understanding of selected portions of the vocabulary, theories and
practices of chemistry with an emphasis on those areas which are
applicable to the functions of the human body.

Content Outline & Competencies:

LECTURE

I. Conversion Problems and Atomic/Nuclear Structure
   A. Measurements
      1. Write the names and abbreviations for the metric (SI) units used
in measurements of length, volume and mass.
      2. Determine the number of significant figures in measured numbers.
      3. Adjust calculated answers to the correct number of significant
figures.
      4. Use the numerical values of prefixes to write a metric equality.
      5. Use a conversion factor to change from one unit to another.
      6. Calculate the density or specific gravity of a substance and use
the density or specific gravity to calculate the mass or volume of a
substance.
      7. Use units from mega to nano in conversion problems.
      8. Define terms associated with measurement.
      9. Compare and contrast related chemical terms.
   B. Atoms and elements
      1. Given the name of an element, write its correct symbol or vice
versa.
      2. Use the periodic table to identify the group and the period of an
element and whether it is a metal or a nonmetal.
      3. Describe the electrical charge, mass (amu) and location in an
atom for a proton, neutron and electron.
      4. Give the atomic number and mass number of an atom, state the
number of protons, neutrons and electrons.
      5. Give the number of protons, electrons and neutrons in the
isotopes of an element.
      6. Given the name or symbol of one of the first 20 elements in the
periodic table, write the electron arrangement and use it to explain the
periodic law.
      7. Indicate on the periodic table the appropriate families, groups,
periods or sections which are referred to by the following names: alkali
metals, alkaline earth metals, halogens, rare gases, transition metals,
rare gases, transition metals, rare earth metals, semiconductors and
representative elements.  Given an element, indicate which term is
appropriate for the element.
      8. Describe the electromagnetic spectrum, including relationships
between wavelength, frequency and energy.
      9. Define terms associated with atomic structure and the periodic
table.
      10.   Distinguish between related chemical terms.
   C. Nuclear radiation
      1. Describe alpha, beta and gamma radiation.
      2. Write an equation showing mass numbers and atomic numbers for
radioactive decay.
      3. Write an equation for the formation of a radioactive isotope.
      4. Given a half-life, calculate the amount of radioisotope remaining
after one or more half-lives.
      5. Describe the processes of nuclear fission and fusion.
      6. Define terms associated with nuclear radiation.
      7. Distinguish between related chemical terms.

II. Compounds, Reactions and Energy
   A. Compounds and their bonds
      1. Using the periodic table, write the electron dot structure for a
representative element.
      2. Using the octet rule, write the symbols of the simple ions for
the representative elements.
      3. Using charge balance, write the correct formula for an ionic
compound.
      4. Given the formula of an ionic compound, write the IUPAC name;
given the IUPAC or common (older) name, write the correct formula.
      5. Diagram the electron-dot structure for a covalent molecule.
      6. Given the formula of a covalent compound, write its correct name;
given the name of a covalent compound, write its formula.
      7. Using electronegativity values, classify a bond as nonpolar
covalent, polar covalent or ionic.
      8. Write a formula of a compound containing a polyatomic ion; given
the formula of a compound containing a polyatomic ion, write the correct
name.
      9. Define terms associated with chemical compounds and bonding.
      10.   Distinguish between related chemical terms.
   B. Chemical quantities and reactions
      1. State a chemical equation in words and determine the number of
atoms in the reactants and products.
      2. Write a balanced chemical equation from the formulas of the
reactants and products for a reaction.
      3. Define oxidation and reduction as it occurs in inorganic
compounds (Loss or gain of electrons) and give an example.
      4. Given the chemical formula of a substance, calculate its molar
mass.
      5. Given the number of moles of a substance, calculate the mass in
grams; given the mass, calculate the number of moles.
      6. Define terms associated with chemical quantities and reactions.
      7. Distinguish between related chemical terms.
   C. Energy and matter
      1. Describe some forms of energy.
      2. Identify the physical state of a substance as a solid, liquid or
gas.
      3. Describe the change of state between solid and liquid and also
between solid and gas.
      4. Describe the change of state between gas and liquid.
      5. Describe the energy in exothermic and endothermic reactions;
describe the function of a catalyst.
      6. Describe energy changes in chemical reactions in terms of energy
diagrams for endothermic, exothermic, catalyzed and uncatalyzed
processes.
      7. Define terms associated with energy changes.
      8. Distinguish between related chemical terms.
   D. Gases
      1. Describe the kinetic theory of gases.
      2. Describe the units of measurement used for pressure and change
from one unit to another.
      3. Define terms associated with gases and pressure.
      4. Distinguish between related chemical terms.

III. Introduction to Organic Chemistry
   A. Alkanes and aromatic hydrocarbons
      1. From its properties, classify a compound as organic or
inorganic.
      2. Draw the complete and the condensed structural formula for an
alkane.
      3. Write the names and condensed and structural formulas of the
first ten unbranched alkanes.
      4. Write balanced chemical equations for the combustion of
hydrocarbons.
      5. Use the IUPAC system to write the names of branched-chained
alkanes.
      6. Write the structural formulas of alkanes and their isomers.
      7. Give the name for a cycloalkane and draw the condensed structural
and geometric formulas.
      8. Describe the bonding in benzene, name aromatic compounds and
write their structural formulas.
   B. Haloalkanes, alkene and alkynes
      1. Classify alkanes, alkenes, alkynes and aromatics according to
their functional groups.
      2. Give the name for a haloalkane or draw the structural formula
from the name.
      3. Write the IUPAC names for the structural formulas of alkenes,
cycloalkenes and alkynes or write their structural formulas from their
names.
      4. Write the names and structural formulas of alkenes that have
cis-trans isomers.
      5. Write the structural formulas and names for the products of the
addition reactions of alkenes.
      6. Given the name of common substituents, write the structure and
vice versa.
      7. Distinguish between complete and incomplete combustion and write
balanced equations for each.
      8. Define terms associated with hydrocarbons.
      9. Distinguish between related chemical terms.

IV. Organic Functional Groups and Reactions
   A. Alcohols, phenols, ethers, aldehydes and ketones
      1. Name simple alcohols, phenols and thiols, draw their condensed
structural formulas and describe their solubility in water.
      2. Give the name of an ether and write the condensed structural
formula from the name.
      3. Name aldehydes and ketones and draw the condensed structural
formula from the name.
      4. Write the reactions and/or products for the oxidation and
reduction of alcohols, aldehydes and ketones.  Classify an alcohol as
primary, secondary or tertiary.
      5. Identify and name compounds containing difunctional groups (diol,
dial, dione).
   B. Carboxylic acids, esters, amines and amides
      1. Give the common names, IUPAC names and condensed structural
formulas of carboxylic acids.
      2. Give the common names, IUPAC names and condensed structural
formulas of esters.
      3. Write equations for the formation of an ester (esterification).
      4. Classify amines and give their names and condensed structural
formulas.
      5. Write equations for the formation of an amide (amidation).
      6. Write the common names, IUPAC names and condensed structural
formulas of amides.
      7. Identify and name compounds containing difunctional groups (Dioic
acid, diamine).
      8. Define terms associated with organic functional groups.
      9. Distinguish between related chemical terms.

V. Solutions, Acids and Bases
   A. Solutions
      1. Describe hydrogen bonding in water.
      2. Define solute and solvent and describe the formation of a
solution.
      3. Describe the solution process for electrolytes and
nonelectrolytes in water.
      4. Convert between grams, moles and equivalents.
      5. Define solubility and distinguish between an unsaturated and a
saturated solution.
      6. Identify an insoluble salt.
      7. Calculate the percent concentration of a solute in a solution and
use percent concentration to calculate the amount of solute or solution.
      8. From its properties, identify a mixture as a solution, a colloid
or a suspension.
      9. Calculate the molarity of a solution and use molarity as a
conversion factor to calculate the moles of solute or the volume needed to
prepare a solution.
     10. Complete and balance precipitation reactions.
     11. Write a balanced equation to show the deionization or
dissociation of electrolytes (salts) in water.
     12. Define terms associated with solutions.
     13. Distinguish between related chemical terms.
   B. Acids and bases
      1. Describe acids and bases using the Arrhenius and Bronsted-Lowry
concepts.
      2. Use the ion product of water to calculate the [H3O+] and [OH-] in
a solution.
      3. Calculate pH from [H3O+] and given the pH, calculate [H3O+] and
[OH-] of a solution.
      4. Write an equation for the ionization of strong and weak acids.
      5. Given the molarity or percent concentration of the solution
describe the preparation 
of a dilute solution.
      6. Write a balanced equation for the neutralization reaction between
an acid and a base.
      7. Describe the role of buffers in maintaining the pH of a
solution.
      8. Define terms associated with acids and bases.
      9. Distinguish between related chemical terms.
   C. Carboxylic acids, amines
      1. Write equations for the ionization and neutralization of
carboxylic acids.
      2. Write equations for the ionization of an amine in water and
neutralization of an amine.

VI. Introduction to Biochemistry
   A. Carbohydrates
      1. Classify carbohydrates as monosaccharides, disaccharides and
polysaccharides.
      2. Classify a monosaccharide as an aldose or ketose and indicate the
number of carbon atoms.
      3. Given a Fischer Projection of a monosaccharide, draw the
corresponding mirror image and indicate whether it is a D or L isomer.
      4. Draw the open chain structures for D-glucose, D-ribose and
D-fructose.
      5. Identify alpha and beta structures of Haworth projections for
monosaccharides.
      6. Given the Haworth structure of a disaccharide, identify the type
of glycosidic bond.  For the disaccharides maltose, lactose and sucrose,
identify the monosaccharides 
and type of glycosidic bonds.
      7. Describe polysaccharides, alpha and beta bonds and the
monosaccharide units in polysaccharides.
      8. Define terms associated with carbohydrates.
      9. Distinguish between related chemical terms.
   B. Lipids
      1. Identify a fatty acid as saturated or unsaturated.
      2. Describe the structure and functional groups of waxes, fats and
oils.
      3. Draw the structure of the product from the reaction of a
triglyceride with hydrogen, an acid or a base or an oxidizing agent. 
Write the products of the saponification reaction.
   C. Amino acids, proteins and enzymes
      1. Write the general structural formula of an amino acid and given
the structural formula of the R group; be able to classify as nonpolar,
polar, acidic or basic based upon their R group side chains.
      2. Given the structure of two amino acids, write the structure of
the resulting dipeptide.
      3. Distinguish between the primary and secondary structures of a
protein.
      4. Distinguish between the tertiary and quaternary structures of a
protein.
      5. Describe denaturation of proteins.
      6. Describe the function of an enzyme as a catalyst.
      7. Define terms associated with proteins.
      8. Distinguish between related chemical terms.

LAB

I. Safety, Measurement, Conversions
   A. Safety
      1. State the safety rules for working in a chemistry lab.
      2. Know the location of safety equipment in the lab and state when
and how it is to be used.
      3. Learn the appropriate names of equipment and glassware in the
lab.
   B. Measurement
      1. Measure length of an object, estimating between the lines of the
measuring device.
      2. Measure volume of a liquid using a graduated cylinder, estimating
between the lines.
      3. Measure mass to the nearest milligram using a laboratory
balance.
      4. Determine the volume of a solid by direct measurement or volume
displacement.
      5. Read the specific gravity from a hydrometer.
      6. Given a table with two sets of data, plot the points on a graph.
   C. Conversions
      1. Use significant figures properly in all calculations.
      2. Convert between different units of length, volume or mass.
      3. Using two measured volumes or two measured masses, calculate the
conversion factor.
      4. Given items in a mixture, calculate percent of each.
      5. Calculate the density of an object.
      6. Use density or specific gravity to calculate the mass or volume
of a substance.
      7. From density values, identify an unknown solid or liquid.
      8. Calculate percent error from an experimental value and an
accepted value.
      9. Given percent and component(s), calculate total amount or
individual items in a mixture.

II. Atoms, Chemical Formulas and Chemical Reactions
   A. Atomic Structure
      1. Given the atomic number and mass number of an atom, state the
number of protons, neutrons and electrons.
      2. Light a Bunsen burner and adjust the flame to get a "noisy" light
blue cone indicating a hot flame.
      3. Identify an unknown cation from flame tests.
      4. Give the electron arrangement for the first 20 elements.
      5. Using the octet rule, write electron configurations of ions.
   B. Chemical Formulas
      1. Write the formula and name of representative ions, transition
metal ions and polyatomic ions.
      2. Write the formula and name of ionic compounds.
      3. Write the formula and name of covalent compounds.
      4. Using electron dot structures, diagram the bonds in covalent
compounds.
      5. Identify a compound as ionic or covalent.
      6. Calculate the molar mass of a substance from the chemical
formula.
      7. Work conversion problems between grams and moles.
      8. Given the mole: mole ratio of elements in a compound, determine
the formula.
   C. Chemical Changes
      1. Distinguish between a chemical and a physical change.
      2. Carry out a reaction according to directions and note evidence of
a chemical change.
      3. Balance a chemical reaction.
      4. Determine if a reaction is endothermic or exothermic using a
thermometer.

III. Organic Chemistry
   A. Simple Hydrocarbons
      1. Given a model of an organic compound, write the complete formula,
condensed formula and name.
      2. Compare the properties of organic and inorganic compounds.
      3. Use the CRC handbook to look up the properties of a compound.
      4. Given the molecular formula of an organic compound, write and
name all the isomers.
      5. Write and balance a combustion reaction for a hydrocarbon.
   B. Oxidation Reactions
      1. Know which alcohols are soluble in water.
      2. Classify an alcohol as primary, secondary or tertiary.
      3. Determine which aldehydes and ketones are soluble in water.
      4. Demonstrate the proper technique of smelling a chemical in lab.
      5. Draw the organic product of an oxidation reaction.
   C. Dehydration Reactions
      1. Given an alcohol and an acid, make a model of the resulting ester
and give the name.
      2. Write the structure of the sodium salt obtained by adding NaOH to
a carboxylic acid.
      3. Complete and balance a neutralization reaction involving a
carboxylic acid.

IV. Properties of Solutions
   A. Solution Concentrations
      1. Define saturated, unsaturated or supersaturated solutions.
      2. Given solubility, determine whether a solution is saturated or
not.
      3. Given a graph of solubility versus temperature, determine the
solubility for a given temperature or vice versa.
      4. Given volume and mass data for a solution and solute, calculate
the concentration as mass/mass percent, mass/volume percent and molarity.
   B. Qualitative Analysis
      1. Test an unknown solution for the presence or absence of the
following cations: Na+, K+, Ca+2, NH4+, Fe+3.
      2. Test an unknown solution for the presence or absence of the
following anions: Cl-, Br-, I-, PO4-3, CO3-2, SO4-2.
      3. Given a cation and anion in an unknown, write the formula and
name of the compound.
   C. Electrolytes and pH
      1. Given a solution and a conductivity meter, decide whether the
solution is a strong, weak or non-electrolyte.
      2. Write the equation for the dissociation of a strong, weak or
non-electrolyte.
      3. Use the pH meter to determine the pH of an unknown solution.
      4. Given [H+] and/or [OH-], calculate the other and determine the
pH.
      5. Decide whether an unknown solution is a buffer by adding small
amounts of acid or base and observing the pH change.
      6. Read a buret.
      7. Write a balance equation for an acid - base neutralization
reaction.

Methods of Evaluation of Competencies:

Evaluation of student mastery of course competencies will be accomplished using the following methods:

Chemistry is a science requiring the application of problem-solving
techniques to a wide variety of different situations. Students must be
able to demonstrate a mastery of the vocabulary, theories and processes of
chemistry. In addition, they must be able to demonstrate an ability to
apply abstract and real logic through both verbal and mathematical
communication skills to the analysis and solution of selected problems.

Tests (75%)
  Unit Exams (all equal in value)
  Cumulative Final (equal in value to two unit exams, 50% covering Unit
VI)
  Announced and unannounced quizzes (not to exceed 15%)
Labs (20%)
Reports (10%)
Lab Tests (10%)
Reports (5%)
 
Grade Scale:
  A =  90% - 100% 
  B =  80% -  89%
  C =  70% -  79%
  D =  60% -  69%
  F =   0% -  59%

Caveats:

1. Computer Literacy Expectations: Students will need basic word processing and Internet searching skills for the completion of some papers, exercises and projects.
2. Attendance: Students are normally expected to be present and participate in scheduled class periods; there is no opportunity to make up missed labs after the week scheduled.
3. Safety: Students entering physical science classes should be aware that they may be in close contact with potentially hazardous chemicals and equipment. The students should assume responsibility for conducting themselves in a manner to minimize such hazards.
4. It is in the best interest of students who are pregnant to defer laboratory classes until after delivery.
5. Safety: Chemical hazards dictate that goggles, shoes and protective covering will be worn whenever chemicals are used in the laboratory.
6. Consumption of food, beverages or tobacco is strictly prohibited and will not be tolerated. Unauthorized experiments are prohibited.

Disabilities:

If you are a student with a disability, and if you will be requesting accommodations, it is your responsibility to contact Access Services. Access Services will recommend any appropriate accommodations to your professor and his/her director. The professor and director will identify for you which accommodations will be arranged.

JCCC provides a range of services to allow persons with disabilities to participate in educational programs and activities. If you desire support services, contact the office of Access Services for Students With Disabilities (913) 469-8500, ext. 3521 or TDD (913) 469-3885. The Access Services office is located in the Success Center on the second floor of the Student Center.