Honors Chemistry
Course Description and Philosophy
Chemistry is the study of matter and the changes it undergoes. This is a comprehensive and intensive course in experimental
and conceptual chemistry. The work includes history and methods of science and ranges over the nature of atoms, molecules and
reactions. Among the major topics are structure, nuclear chemistry, quantum chemistry, bonding, formula and equation writing,
stoichiometry, changes of state, thermochemistry, solutions, kinetics, equilibrium, and electrochemistry. Understanding the periodic
table, developing laboratory techniques, interpreting data, and writing up experiments are stressed. The extensive laboratory work
ranges from investigating the fundamental laws of chemical change to the analytical chemistry of acid-base titration and determination
of reaction rates.
It is expected that students who enroll in this course will be able readers and proficient in basic algebra. Instructional strategies
for this course include lecture, laboratory activities, demonstrations, group discussions and student board work. Student performance
will be evaluated using teacher-generated tests and quizzes, homework assignments, laboratory write-ups, and class participation, as
well as two half-year examinations that will represent 20% of the students’ final grade for the course.
Text Reference:
- Davis, Raymond E., Regina Frey, Mickey Sarquis, Jerry L. Sarquis, Modern Chemistry, copyright 2006 by Holt, Rinehart and
Winston, New York, New York.
Updated July 2007
UNIT I: The Tools For Chemistry
Essential Question: What is the study of chemistry and how can it be applied to our everyday lives?
Objectives – Students will be able to:
-
Describe chemistry and its different branches
Compare basic and applied research
Differentiate between elements and compounds
Describe the difference between intensive and extensive
properties of matter
Distinguish between the physical properties and the
chemical properties of matter
Classify a change of matter as physical or chemical
Describe the solid, liquid and gas states of matter in
terms of particles.
Apply the law of conservation of energy to changes of
matter
Distinguish between a mixture and a pure substance
Use the periodic table to name elements, given their
symbols
Use the periodic table to write the symbols of elements,
given their names
Describe the arrangement of the periodic table
List the characteristics of metals, nonmetals and
metalloids
Describe the scientific method and how it is utilized by
researchers
Differentiate between a theory and a law
-
Distinguish between qualitative and quantitative
observations
Distinguish between a quantity, a unit and a
measurement standard
Utilize the SI units for measurements
Distinguish between mass and weight
Perform density calculations
Convert between metric and nonmetric units of
measurement using dimensional analysis
Distinguish between precision and accuracy
Use and manipulate significant figures in measurements
and calculations
Convert measurements into and out of scientific
notation
Calculate the percentage error of a measurement
Distinguish between inversely and directly proportional
relationships
Topic/Content Skills
Chapter 1: Matter and
Change
- Chemistry is a
Physical Science
- Matter and Its
Properties
- Elements
Assessment
Tests/Quizzes
Lab Activities
Homework
Participation
Resources
Text
Lab Material
LaserDisc
Media Center
Lab Supplies
IBook
Instructional
Method
Lecture
Discussion
Lab Group Work
Individual Research
Tech Infusion
Internet Research
LaserDisc
PowerPoint
IBooks
CBL units
Loggerpro Software
VCR
DVD
SmartBoard
NJCCCS: Unit I
5.1 – A, B, C
5.2 – A
5.3 – A, B, C, D
5.4 – A
5.6 - A
Chapter 2: Measurements
and Calculations
- Scientific Method
- Units of
Measurement
- Using Scientific
Measurements
Differentiated Learning Activities
- Students will use IBooks to research branches of chemistry studied at various universities across the country, and possible
career choices that stem from those areas of studies. Students will then present their findings in class, which will be written on
the board so that all students can record it. The purpose of this activity is to provide the students an opportunity to explore the
possible careers in chemistry, and identify what is required to obtain those careers.
Ethical Decision Making/Character Education
- Discussion about the ethics of data reporting in chemistry; discuss importance in honestly reporting information obtained
during research, and relate real-life examples taken from science news stories
UNIT II: Atomic Theory
Essential Question: How has the theory of the atom changed throughout history?
Objectives – Students will be able to:
- Explain the law of conservation of mass
- Explain the law of definite proportions
- Explain the law of multiple proportions
- Summarize the essential points of Dalton’s atomic
theory
- Summarize the observed properties of cathode rays and
how it led to the discovery of the electron
- Summarize the observations made by the oil drop
experiment and how it characterized the nature of
electrons
- Summarize the work carried out by Rutherford that led
to the discovery of the nucleus
- List the properties of protons, neutrons and electrons
- Describe isotopes
- Determine the number of protons, neutrons and
electrons given a nuclide
- Define the mole, Avogadro’s number, and molar mass,
and describe how these are used to count atoms
- Solve problems involving the relationship between
mass, moles and a number of atoms
- Calculate the average atomic mass of an element given
the properties and abundances of its isotopes
- Explain the relationship between the speed, frequency
and wavelength of electromagnetic radiation
- Describe photoelectric effect and black body radiation
-
-
-
Explain Planck’s theory of quantized energy, and how
this relates to the photoelectric effect
Describe the contributions made to atomic theory by
Bohr, DeBroglie, Heisenberg and Schrödinger
Compare and contrast the Bohr model and the quantum
model of the atom
List and describe the four quantum numbers
Draw energy level diagrams for the electrons in
elements using Aufbau, Hund’s Rule and the Pauli
Exclusion principle
Write out the electron configuration of an element
Explain the roles of Mendeleev and Moseley in the
development of the periodic table
Describe the modern periodic table
Explain how the periodic law can be used to predict the
physical and chemical properties of elements
Describe the periodic trends of atomic radius, ionization
energy, electron affinity, ionic radius and
electronegativity as a function of electron configuration
and position on the periodic table
Define valence electrons, and state how many are
present in atoms of each main-group element
Explain why atoms undergo bonding
Distinguish between an ionic bond and a covalent bond
-
Classify a bond according to electronegativity
differences
Describe a molecule and a molecular formula
Explain the relationships among potential energy,
distance between atoms, bond length and bond energy
Describe the octet rule
Draw Lewis structures when given a molecular formula
Explain why resonance structures are needed to
describe some molecules
Topic/Content Skills
Chapter 3: Atoms – The
Building Blocks of Matter
- The Atom – From
Philosophical Idea to
Scientific Theory
- The Structure of the
Atom
- Counting Atoms
Chapter 4: Arrangement of
Electrons in Atoms
- The Development of a
New Atomic Model
- The Quantum Model of
the Atom
- Electron Configurations
Chapter 5: The Periodic Law
- History of the Periodic
Table
Assessment
Tests/Quizzes
Lab Activities
Homework
Participation
Resources
-
-
Discuss the arrangement of atoms in crystals
Compare the properties of molecular and ionic
compounds
Describe the model of a metallic bond
Explain and use the VSEPR theory to predict the shape,
bond angles, polarity and hybridization of simple
molecules when given a formula
Describe intermolecular forces as a function of polarity
Instructional
Method
Text
Lecture
Lab Material Discussion
LaserDisc
Lab Group Work
Media Center Individual Research
Lab Supplies
IBook
Tech Infusion
Internet Research
LaserDisc
PowerPoint
IBooks
CBL units
Loggerpro Software
VCR
DVD
SmartBoard
NJCCCS: Unit II
5.1 – A, B
5.2 – A, B
5.3 – A, B, C, D
5.4 – A, B, C
5.6 - A
-
Electron Configuration
and the Periodic Table
- Electron Configuration
and Periodic Properties
Chapter 6: Chemical Bonding
- Intro to Chemical
Bonding
- Covalent Bonding and
Molecular Compounds
- Ionic Bonding and Ionic
Compounds
- Metallic Bonding
- Molecular Geometry
Differentiated Learning Activities
- Using IBooks, reference books and texts, students will work in lab groups (2 or 3 students per group) to complete a “Periodic
Table Scavenger Hunt” where they will use clues given to identify unknown elements and place them in their appropriate
location on the periodic table. The purpose of this activity is to allow the students to identify patterns among groups of
elements on the periodic table, as well as utilize their knowledge of electron configurations to further solidify their
understanding of periodic trends.
Ethical Decision Making/Character Education
- Class discussion on the ethical issues surrounding our growing understanding of the atom over time, and how scientists such as
Einstein, Bohr, Heisenberg and others addressed/handled these issues during troubling times in history. This discussion would
allow students to recognize how science contributes to events throughout history as well as current events.
UNIT III – Nomenclature and Chemical Reactions
Essential Question: How is the mole concept used to determine the amount of product made in a chemical reaction?
Objectives – Students will be able to:
-
Identify the name/formula and charge of an element or
ion
Write the formula/name of an ionic or molecular
compound
Write the formula and name of acids
List and utilize the rules for assigning oxidation
numbers
Calculate the formula/molar mass of a compound
Convert between mass, moles and
atoms/molecules/formula units
Calculate the % composition of a compound
Determine the empirical and molecular formula of a
compound when given the composition
Distinguish between an empirical and molecular
formula
List ways of determining that a chemical reaction has
occurred
Write and balance a chemical equation
Define and describe synthesis, decomposition,
combustion, single and double replacement reactions
-
-
Classify a reaction and determine the products when
only given reactants
Utilize an activity series to determine whether a single
replacement reaction will occur
Utilize a solubility table to determine whether a double
replacement reaction will occur
Define stoichiometry
Explain the significance of a mole ratio given by a
balanced chemical equation
Write a mole ratio given a balanced chemical equation
Calculate the amount of moles of reactant/product
needed/produced from a given quantity of another
reactant/product
Calculate the mass of reactant/product needed/produced
from a given quantity of another reactant/product
Calculate the volume of a gas at STP needed or
produced given a quantity of another reactant/product
Determine whether a reactant is a limiting reactant or
excess reactant
Calculate the expected yield and percentage yield of a
reaction
Topic/Content Skills
Assessment
Chapter 7: Chemical Formulas
and Chemical Compounds
- Chemical Names and
Formulas
- Oxidation Numbers
- Using Chemical
Formulas
- Determining Chemical
Formulas
Chapter 8: Chemical Equations
and Reactions
- Describing Chemical
Reactions
- Types of Chemical
Reactions
- Activity Series of the
Elements
Chapter 9: Stoichiometry
- Intro to Stoichiometry
- Ideal Stoichiometric
Calculations
- Limiting Reactants and
Percentage Yield
Tests/Quizzes
Lab Activities
Homework
Participation
Resources
Instructional
Method
Text
Lecture
Lab Material Discussion
LaserDisc
Lab Group Work
Media Center Individual Research
Lab Supplies
IBook
Tech Infusion
Internet Research
LaserDisc
PowerPoint
IBooks
CBL units
Loggerpro Software
VCR
DVD
SmartBoard
NJCCCS: Unit III
5.1 – B
5.3 – A, B, C, D
5.6 – A, B
Differentiated Learning Activities
- Using handheld white-boards, the students will participate in a game to reinforce their understanding of chemical nomenclature.
Instructor will hold up a white board with either a name or formula of a compound. The students will individually determine the
formula or name of the compound, and hold up their answer. If the answer is correct, they earn a point for their team. The activity
allows students to assess their own knowledge of nomenclature before they are tested on it, as well as earn extra points for the test.
UNIT IV: Solids, Liquids, Gases and Solutions
Essential Question: How does the distribution and behavior of particles differ among the 3 states of matter?
Objectives – Students will be able to:
-
-
State the kinetic-molecular theory of matter
Describe how the kinetic-molecular theory explains the
properties of matter
List the five assumptions made by the kinetic molecular
theory about gases
Describe an ideal gas
Describe each of the following properties of gases:
expansion, density, fluidity, compressibility, diffusion,
effusion
Describe the conditions under which a gas will deviate
from idea behavior
Describe the motion and particles of liquids
Describe the properties of liquids according to the
kinetic molecular theory
Define and describe the vaporization and freezing
processes
Describe the properties of a liquid including surface
tension, viscosity and capillary action
Describe the motion of the particles in a solid according
to the kinetic molecular theory
Distinguish between crystalline and amorphous solids
Describe the different types of crystal symmetry
Describe the significance of a unit cell
Describe the state of equilibrium in reference to
changes of state
-
-
-
Read and interpret phase diagrams
Read and interpret heating curves
Calculate the quantity of heat gained/lost by a defined
amount of a substance undergoing one or more phase
changes
Describe equilibrium vapor pressure
Describe the processes of boiling, freezing, melting and
sublimation
Describe the structure of the water molecule and how it
determines the unique properties of water
Define pressure, the units of pressure, and describe how
it is measured
Convert between units of pressure
Use Dalton’s law of partial pressures to calculate partial
and total pressures of gas mixtures
Use the kinetic molecular theory to describe the
relationships between pressure, volume and temperature
of a gas
Describe and perform calculations for Boyle’s Law
Describe and perform calculations for Charles’ Law
Use the combined gas law for calculations
State the law of combining volumes
State Avogadro’s Law and describe its significance
State the ideal gas law and perform calculations
Perform gas stoichiometry calculations
-
-
Describe the processes of effusion and diffusion
State Graham’s law of effusion
Describe the relationship between the average
molecular velocities of two gases and their molar
masses
Calculate the root-mean-square velocity of a given gas
at a given temperature
Distinguish between heterogeneous and homogeneous
mixtures
Compare the properties of suspensions, colloids and
solutions
Describe the properties of electrolytes and
nonelectrolytes
Describe the Tyndall effect
Describe factors that affect the rate at which a solute
dissolves in a solvent
Distinguish among saturated, unsaturated and
supersaturated solutions
Topic/Content Skills
Chapter 10: States of Matter
- The Kinetic-Molecular
Theory of Matter
- Liquids
- Solids
- Changes of State
- Water
Assessment
Tests/Quizzes
Lab Activities
Homework
Participation
Resources
-
Explain the meaning of “like dissolves like” in terms of
polarity
Explain the affects of temperature and pressure on
solubility
Explain the interactions that contribute to enthalpies of
solution
Describe the hydration process of an ionic and a
molecular compound
Calculate the concentration of a solution in units of
molarity, molality and mole fraction
Write equations for the dissolution of ionic compounds
Write net ionic equations for precipitation reactions and
predict whether they will occur
Distinguish between strong and weak electrolytes
List and describe the four colligative properties
Calculate freezing point depression, boiling point
elevation, and osmotic pressure
Determine the van’t Hoff factor for ionic solutes
Instructional
Method
Text
Lecture
Lab Material Discussion
LaserDisc
Lab Group Work
Media Center Individual Research
Lab Supplies
IBook
Tech Infusion
Internet Research
LaserDisc
PowerPoint
IBooks
CBL units
Loggerpro Software
VCR
DVD
SmartBoard
NJCCCS: Unit IV
5.1 – B
5.3 – A, B, C, D
5.6 – A, B
5.7 - B
Chapter 11: Gases
- Gases and Pressure
- The Gas Laws
- Gas Volumes and the
Ideal Gas Law
- Diffusion and Effusion
Chapter 12: Solutions
- Types of Mixtures
- The Solution Process
- Concentration of
Solutions
Chapter 13: Ions in Aqueous
Solutions and Colligative
Properties
- Compounds in Aqueous
Solutions
- Colligative Properties of
Solutions
Differentiated Learning Activities
- Using lab equipment and chemicals provided, students would experimentally determine the value of the ideal gas constant. They
will work in lab groups. This activity will give students to opportunity to take several types of measurements for gases, including
pressure, temperature, volume and mass, and apply these measurements in a calculating involving the idea gas equation
Ethical Decision Making/Character Education
- Class discussion on academic integrity in homework assignments and data reporting for lab activities.
UNIT V: Acid-Base Chemistry
Essential Question: How does one determine the pH of an unknown solution using a titration?
Objective – Students will be able to:
-
List the general properties of aqueous acids and bases
Name and write formulas for common acids and bases
Define acid and base according to Arrhenius’ theory of
ionization
Explain the difference between strong and weak acids
and bases
Define acid and base according to the Bronsted-Lowry
theory
Define a Lewis acid and a Lewis base
Describe and identify conjugate acid-base pairs
Describe amphoteric compounds
Topic/Content Skills
Chapter 14 – Acids and Bases
- Properties of Acids and
Bases
- Acid-Base Theories
- Acid-Base Reactions
Assessment
Tests/Quizzes
Lab Activities
Homework
Participation
Resources
-
Explain the process of neutralization
Define acid rain, and describe how it is formed
Describe the self-ionization of water
Define and calculate pH
Explain and use the pH scale
Find pH when given the concentration of hydrogen ion,
hydronium ion or hydroxide ion
Describe the function of an acid-base indicator
Explain and perform an acid-base titration
Calculate the concentration of an unknown solution
based on titration data
Instructional
Method
Text
Lecture
Lab Material Discussion
LaserDisc
Lab Group Work
Media Center Individual Research
Lab Supplies
IBook
Tech Infusion
Internet Research
LaserDisc
PowerPoint
IBooks
CBL units
Loggerpro Software
VCR
DVD
SmartBoard
NJCCCS: Unit V
5.1 – B
5.2 – B
5.3 – A, B, C, D
5.6 – A, B
Chapter 15 – Acid-Base
Titration and pH
- Aqueous Solutions and
the Concept of pH
- Determining pH and
Titrations
Differentiated Learning Activities
- Using IBooks, CBL units, pH probes and Loggerpro 3 Software, students will experimentally track the pH of a basic solution
as small amounts of acid are added to it.
UNIT VI – The Control of Reactions
Essential Question: How to enthalpy, entropy and free energy changes relate to whether a reaction is likely to occur?
Objectives – Students will be able to:
-
Define temperature and state the units in which it is
measured
Define heat and state its units
Perform specific-heat calculations
Describe enthalpy change, enthalpy of reaction,
enthalpy of formation
Calculate enthalpy of reaction using enthalpies of
formation
Perform Hess’ Law calculations
Perform calorimeter problems
Explain the relationship between enthalpy change and
the tendency of a reaction to occur
Explain the relationship between entropy change and
the tendency of a reaction to occur
-
Discuss the concept of free energy, and explain the
meaning of its value
Describe the use of free energy change to determine
whether a reaction will occur
Calculate the temperature at which a reaction becomes
spontaneous using enthalpy and entropy changes
Explain the concept of a reaction mechanism
Use the collision theory to interpret chemical reactions
Define activated complex
Relate activation energy to enthalpy of reaction
Define chemical kinetics
Describe the conditions needed for a chemical reaction
to occur
Discuss factors that affect reaction rates
-
Define catalyst
Relate the order of a reaction to the rate law for the
reaction
Write a rate law for a chemical reaction
Perform rate law calculations given reaction rate data.
Define chemical equilibrium
Explain the nature of the equilibrium constant
Write equilibrium expressions and carry out
equilibrium calculations
Discuss the factors that disturb equilibrium
Discuss conditions under which reactions go to
completion
Describe the common-ion effect
Topic/Content Skills
Chapter 16 – Reaction Energy
- Thermochemistry
- Driving Force of
Reactions
Chapter 17 – Reaction
Kinetics
- The Reaction Process
- Reaction Rate
Assessment
Tests/Quizzes
Lab Activities
Homework
Participation
Resources
-
Perform reaction quotient calculations to determine
how a reaction will shift
Perform common-ion effect calculations
Explain the concept of acid-ionization constants
Write acid ionization equilibrium expressions
Explain buffering
Compare cation and anion hydrolysis
Explain what is meant by solubility product constants
and calculate their values
Calculate solubilities using solubility product constants
Carry out calculations to predict whether precipitates
will form when solutions are combined
Instructional
Method
Text
Lecture
Lab Material Discussion
LaserDisc
Lab Group Work
Media Center Individual Research
Lab Supplies
IBook
Tech Infusion
Internet Research
LaserDisc
PowerPoint
IBooks
CBL units
Loggerpro Software
VCR
DVD
SmartBoard
NJCCCS: Unit VI
5.1 – B
5.3 – A, B, C, D
5.6 – A, B
5.7 - B
Chapter 18 – Chemical
Equilibrium
- The Nature of
Chemical Equilibrium
- Shifting Equilibrium
- Equilibria of Acids,
Bases and Salts
- Solubility Equilibrium
Differentiated Learning Activities
- Using chemicals provided and lab handouts with detailed instructions, students will make predictions for several equilibrium
reactions utilizing their knowledge of Le Chatelier’s Principle. Then, students will pair up with their lab partners and perform
experiments to determine whether their predictions are correct.
UNIT VII – Electrochemistry
Essential Question: How does one determine the cell potential of an unbalanced redox reaction?
Objective – Students will be able to:
-
Assign oxidation numbers to reactant and product
species
Define oxidation and reduction
Explain what occurs during a redox reaction
Balance a redox reaction using the half-reaction method
Relate chemical activity to oxidizing/reducing strength
Explain the concept of disproportionation
Identify parts of an electrochemical cell and their
functions
-
Write electrode half reactions for cathodes and anodes
Describe how a voltaic cell operates
Identify how corrosion occurs and how to prevent it
Describe the relationship between voltage and electron
movement
Calculate cell potential from standard reduction
potentials
Describe electrolytic cells
Describe the chemistry of a rechargeable cell
Topic/Content Skills
Assessment
Resources
Chapter 19 – OxidationReduction Reactions
- Oxidation and
Reduction
- Balancing Redox
Equations
- Oxidizing and
Reducing Agents
Chapter 20 – Electrochemistry
- Intro to Electrochem
- Voltaic Cells
- Electrolytic Cells
Tests/Quizzes
Lab Activities
Homework
Participation
Text
Lab Material
LaserDisc
Media Center
Lab Supplies
IBook
Instructional
Method
Lecture
Discussion
Lab Group Work
Individual Research
Tech Infusion
Internet Research
LaserDisc
PowerPoint
IBooks
CBL units
Loggerpro Software
VCR
DVD
SmartBoard
NJCCCS: Unit VII
5.1 – B
5.3 – A, B, C, D
5.4 – A, B, C
5.6 – A, B
5.7 - B
Differentiated Learning Activities
- Using lab equipment several electrodes and solutions, students will work in lab groups to predict how to create a cell that produces
the highest voltage with the chemicals provided. They will then determine if their predictions are correct by testing different
electrode/solution pairs.
UNIT VIII – Special Topics in Chemistry
Essential Question: How do the side chains on amino acids determine the properties of the amino acids?
Objectives – Students will be able to:
-
Explain what a nuclide is and how they can be
represented
Relate mass defect and nuclear binding energy
Explain what affects nuclear stability
-
Explain why nuclear reactions occur
Balance a nuclear equation
Define radioactive decay, and discuss the different
types
-
Describe the half-life of a radioactive substance
Compare the penetrating ability of alpha and beta
particles and gamma rays
Describe ways of detecting radioactivity
Describe applications of radioactive nuclides
Distinguish between fusion and fission
Explain how fission reactors produce power
Describe the significance of the bonding and structure
of carbon
Compare the use of molecular and structural formulas
to represent organic compounds
Compare and identify structural isomers
Distinguish among alkanes, alkenes and alkynes
Write and name alkanes, alkenes and alkynes
Relate properties of alkanes, alkenes and alkynes
Define and describe properties of functional groups
Topic/Content Skills
Chapter 21 – Nuclear
Chemistry
- The Nucleus
- Radioactive Decay
- Nuclear Radiation
- Nuclear Fission
and Nuclear
Fusion
Assessment
Tests/Quizzes
Lab Activities
Homework
Participation
Resources
Text
Lab Material
LaserDisc
Media Center
Lab Supplies
IBook
-
Identify and name alcohols, halides, ethers, and other
functional groups
Describe the characteristics of simple and complex
carbohydrates
Explain the role of carbohydrates in living systems
Describe the characteristics and functions of lipids
Describe the basic structure of amino acids and the
formation of polypeptides
Determine the significance of amino acid side chains
Describe the different functions of proteins in cells
Identify the effects of enzymes
Describe the role of ATP
Explain how metabolic reactions release energy
Describe the relationship between anabolism and
catabolism
Describe the structure and functions of DNA and RNA
Describe the applications of modern gene technology
Instructional
Method
Lecture
Discussion
Lab Group Work
Individual Research
Tech Infusion
Internet Research
LaserDisc
PowerPoint
IBooks
CBL units
Loggerpro Software
VCR
DVD
SmartBoard
NJCCCS: Unit
VIII
5.3 – A, C, D
5.4 – A, B, C
5.5 – A
5.6 – A, B
5.7 - B
Chapter 22 – Organic
Chemistry
- Organic
Compounds
- Hydrocarbons
- Functional Groups
- Organic Reactions
Chapter 23 – Biological
Chemistry
- Carbohydrates and
Lipids
- Amino Acids and
Proteins
- Metabolism
- Nucleic Acids
Differentiated Learning Activities
- Using IBooks and reference books in media center, students will work in small groups to research the pros and cons of nuclear
power, and compare these to those of other alternative sources of energy. Students will then return to the classroom to discuss
their findings, and their opinions on whether nuclear power is a sound alternative energy choice.
Ethical Decision Making/Character Education
- Class discussion about gene technology and the ethical issues that have arisen regarding cloning, gene therapy and stem cell
research