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Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
Stoichiometry
The M ole and M olar Mass
Students will be expected to:
explain how a major scientific milestone, the mole, changed
chemistry (115-3)
define an isotope and use isotopic notation (carbon-12 or 12 C)6
identify Avagadro’s number (6.02 X 1023), as the mole, the unit for
counting atoms, ions, or molecules
recognize that moles are not a directly measurable quantity
define the mole as the number of atoms (Avagadro’s number) in
exactly 12 g of carbon-12
explain how it allowed chemists to write equations for chemical
reactions
explain how it allowed chemists to make accurate predictions using
balanced chemical reactions
define molar mass and perform mole-mass inter-conversions for
pure substances (323-1)
explain the relative nature of atomic mass
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
calculate the average atomic mass given isotope data
define molar mass
calculate the molar mass of compounds
define STP and the molar volume of a gas at STP
perform calculations converting between the number of particles,
moles, volume of gas at STP and mass of various substances
calculate the percent composition from a compound’s formula
determine the empirical formula from percent composition data
determine the molecular formula from percent composition and
molar mass data
use instruments effectively and accurately for collecting data (213-3)
estimate quantities (213-4)
select and use apparatus and materials safely (213-8)
identify and explain sources of error and uncertainty in
measurement and express results in a form that acknowledges the
degree of uncertainty (214-10)
identify and correct practical problems in the way a technological
device or system functions (214-13)
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
Solutions and the M ole
Students will be expected to:
use solution data and data treatments to facilitate interpretation of
solubility (213-5)
explain and give examples of solutes, solvents, and solutions
use a chart of solubility to determine if an ionic compound will have
high or low solubility
explain and give examples of these terms: electrolytes and non-
electrolytes
provide examples, from living and nonliving systems, of how
dissolving substances in water is sometimes a prerequisite for
chemical change
define the terms “concentrated” and “dilute”
define concentration in terms of molarity (moles per litre of
solution)
use simple calculations to show different ways of expressing
concentration
mass/volume percent
volume/volume percent
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
ppm
ppb
calculate, from empirical data, the concentration of solutions in
moles per litre, and determine mass or volume from such
concentrations
calculate, from empirical data, the concentration of diluted
solutions, and the quantities of a solution and water to use when
diluting
outline the steps required to prepare a solution and a dilution of a
solution, including necessary calculations
define the terms unsaturated, saturated and supersaturated solutions
describe an equilibrium system in a saturated solution in terms of
equal rates of dissolving and crystallization
determine the molar solubility of a pure substance in water (323-6)
define molar solubility quantitatively
Calculations and Chemical Equations
Students will be expected to:
identify mole ratios of reactants and products from balanced
chemical equations (323-10)
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
identify the mole ratios of reactants and products in a chemical
reaction as the coefficients in a balanced equation
define mole ratio, and use mole ratios to represent the relative
amounts of reactants and products involved in a chemical reaction
write dissociation equations for dissolved substances
use the mole ratios from dissociation equations for ionic solids to
calculate the concentration of an ion in solution
understand the Law of Conservation of Mass
do calculations using mole-to-mole stoichiometric problems
perform stoichiometric calculations related to chemical equations
(323-11)
define stoichiometry, gravimetric stoichiometry solution
stoichiometry and gas stoichiometry (at STP)
perform stoichiometric calculations among the following: moles,
mass, volume of a solution, volume of a gas (STP) and
concentration
define theoretical, actual, and percent difference and performing
calculations that involve these terms
perform calculations involving limiting reagents in chemical
reactions
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
Stoichiometric Experimentation
use instruments effectively and accurately for collecting data (213-3)
explain how data support or refute the hypotheses or prediction of
chemical reactions (214-12)
design stoichiometric experiments identifying and controlling major
variables (212-3)
choose an appropriate chemical reaction (produces a gas or a
precipitate)
choose appropriate laboratory equipment necessary for performing
the experiment
determine data table, including sample amounts (masses of reactants
and products)
describe how to carry out the filtration of a precipitate
complete sample calculations of theoretical yield and percent yield
recognize when to use a gravimetric or solution stoichiometry
approach to problem solving
identify safety concerns with sample gravimetric analysis and list
precautions taken
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
identify and explain sources of error and uncertainty in
measurement using precision and accuracy (214-10)
distinguish between precision and accuracy in the context of
gravimetric stoichiometry
communicate questions, ideas, and intentions, and receive, interpret,
understand, support, and respond to the ideas of others (215-1)
predict how the yield of a particular chemical process can be
maximized (323-13)
Applications of Stoichiometry
Students will be expected to
identify practical problems that involve technology where chemical
equations are used (214-13)
state a prediction and a hypothesis based on available evidenceand background information (212-4)
identify various stoichiometric applications (323-12)
analyze a given practical problem, identify the potentialstrengths and weaknesses of solutions, and select one as thebasis for a plan (214-15)
perform percent purity calculations
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
list three factors that affect the viability of an industrialprocess. Include:
raw material quality
cost of process
cost of environmental issues
compare processes used in science with those used intechnology (114-7)
identify various constraints that result in tradeoffs during thedevelopment and improvement of technologies (114-4)
analyze society’s influence on science and technology (117-2)
Unit 2
From Structures to Properties
Identify and describe the properties of ionic and molecularcompounds and metallic substances (321-7)
observe the physical properties of representative samples ofmolecular, ionic and metallic substances
tabulate the properties molecular, ionic and metallicsubstances
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
classify ionic, molecular, and metallic substances according totheir properties (321-9)
use the periodic table as a tool for predicting the formation ofionic and molecular compounds
Molecular Compounds
illustrate and explain the formation of covalent bonds (321-4)
understand that chemical bonds are attractive forces that holdall substances together
define valence electrons, electronegativity, electron pairing,ionic bond and covalent bond
identify the maximum number of electrons that occupy eachenergy level
define valence energy level, bonding (unpaired electrons),nonbonding electrons (lone pairs), and bonding capacity, andbe able to relate these terms to atoms of the representativeelements
draw electron dot diagrams of atoms of the representativeelements
explain why noble gases are unreactive and stable
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
explain the special nature of hydrogen as an exception to theoctet rule
define single, double and triple covalent bonds
given the molecular formula, draw Lewis dot diagrams andstructural formulas for simple molecules containing single,double and triple bonds
explain the structural model of a substance in terms of thevarious bonds that define it (321-11)
explain the three-dimensional nature of molecules usingVSEPR theory
determine the shapes about central atoms in simple moleculesby applying VSEPR theory
build models depicting the shape of simple covalent molecules
explain, in simple terms, the energy changes of bond breakingand bond formation, and relate this to why some changes areexothermic while others are endothermic (114-2)
Molecular Compounds: Intermolecular Forces
Students will be expected to:
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
analyze an example of a Canadian contribution to bondingknowledge, the discovery of Noble Gas compounds (117-11)
explain the evidence from an intermolecular forces experimentand from collected data. (114-2)
illustrate and explain hydrogen bonds and van der Waals’forces (321-5)
compare and contrast intramolecular forces (covalent bonds)with intermolecular forces, simply in terms of strength andspecies involved
define polar and nonpolar covalent bonds
use bond dipoles and the shapes of molecules as predicted byVSEPR to determine if a molecule has a molecular dipole
define London dispersion forces, dipole-dipole forces (van derWaals’ forces), and hydrogen bonding, and explain how theyform
relate the strength of London dispersion forces to themolecular mass (number of electrons) and shape (complexity)
identify trends in electronegativity within periods and familiesof the periodic table
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
illustrate and explain hydrogen bonds and van der Waals’forces (321-5)
identify the relationship between the electronegativitydifference between atoms and the degree of bond polarity
compare the strength of London dispersion forces, dipole-dipole forces, and hydrogen bonding
apply bonding knowledge to a particular problem, thestructure of DNA, and analyze the benefits to society to be ableto solve this problem using bonding knowledge (118-2)
select, evaluate and integrate information from experimental,print and media sources, and to present an understanding ofthis information in a variety of formats such as lab reports,web pages, or posters (213-7, 214-3)
describe how the type of attractions account for the propertiesof molecular compounds (321-8)
identify the types of intermolecular forces between moleculesin a substance
compare the melting points or boiling points of simplemolecular substances by comparing the strengths of theirintermolecular forces
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
Molecular Compounds: Network Covalent Solids
Students will be expected to:
illustrate and explain the formation of network covalentbonding and macromolecules (321-4)
identify three network covalent solids (SiO2, SiC, C(diamond), C(graphite)
explain the high melting points and extreme hardness ofnetwork covalent solids
build/design models or find images to represent networkcovalent bonding in order to distinguish it from ionic andmolecular covalent structures
propose possible technologies which may be developed basedupon bonding (116-4)
explain how bonding theory may evolve and become revised asnew evidence arises, using the discovery of the structure ofBuckminsterfullerenes (115-7)
evaluate and select appropriate instruments for collectingevidence (212-8)
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
compile and organize data, using appropriate formats tofacilitate interpretation of the data (213-5)
compile and display evidence and information, by hand orcomputer, in a variety of formats, including diagrams, tables(214-3)
explain how data support or refute the prediction (214-12)
Ionic Compounds
Students will be expected to:
illustrate and explain the formation of ionic bonds (321-4)
predict the ionic charge for ions in the main group elementsfrom their group number and using the octet rule
explain the importance of electron transfer in ionic bondformation
define ionic crystal lattice, formula unit and empiricalformulae as they apply to ionic compounds
build models or find images to depict the lattice structure of anionic compound, e.g., NaCl
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
explain why formulae for ionic compounds refer to thesimplest whole number ratio of ions that results in a net chargeof zero, while the formulae for molecular compounds refer tothe number of atoms of each constituent element
describe how the type of bonding accounts for the propertiesof ionic compounds (321-8)
use the theory of ionic bonding to explain the generalproperties of ionic compounds: brittleness, high melting andboiling points, and the ability to conduct electricity whenmolten or in aqueous solution
identify limitations of categorizing bond types based ondifferences in electronegativity between the elements ofcompounds (214-2)
recognize the relationship between the electronegativities ofthe atoms and the type of bonding in a compound
describe bonding as a continuum ranging from completeelectron transfer (ionic) to unequal sharing of electrons (polarcovalent) to equal sharing of electrons (non-polar covalent)
compare the strengths of ionic and covalent bonds (321-9)
Solutions and Intermolecular Forces
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
explain the variations in the solubility of various puresubstances, given the same solvent (323-7)
describe the solubility of ionic and molecular compounds inpolar and non-polar solvents
explain how molecular and ionic compounds form solutionsby relating it to intermolecular forces (dipole-dipole) andforces of attraction (ion-dipole), respectively
understand that solutions are mixtures at the particle level anddo not involve a chemical change
state that for different substances, solubility occurs to varyingdegrees
Metallic Compounds
Students will be expected to:
illustrate and explain the formation of metallic bonds (321-4)
define a metallic bond, and use it to explain bonding withinmetals
build models (or find images) to represent metallic bonding inorder to distinguish it from ionic and molecular covalentstructures
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
describe how the type of bond accounts for the properties ofmetallic substances (321-8)
using the theory of metallic bonding, explain why metals aremalleable, ductile, good conductors of heat and electricity, andhave a wide range of melting and boiling points
compare the melting or boiling points of network solids, ioniccompounds, metals, and molecular compounds by comparingthe relative strengths of the forces of attraction between theirparticles (321-8)
Unit 3
Organic Chemistry
So Many Compounds
Students will be expected to:
explain the large number and diversity of organic compoundswith reference to the unique nature of the carbon atom (319-4)
compare organic and inorganic compounds in terms of thepresence of carbon, variety of compounds formed, and relativemolecular size and mass
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
explain the wide diversity of organic compounds in terms ofcarbon’s bonding capacity, ability to form multiple bonds, andability to bond in a variety of stable, relatively unreactivestructures such as chains and rings
list natural sources of organic compounds
briefly describe the origin of the term “organic” and how theconception of organic compounds has changed since the firstsynthesis of an organic compound, urea from an inorganiccompound
Influences of Organic Compounds on Society
explain how synthesizing organic molecules revolutionizedthinking in the scientific community (115-3)
provide organic examples of how science and technology are anintegral part of their lives and their community (117-5)
analyze natural and technological systems to interpret andexplain the influence of organic compounds on society (116-7)
Classifying Organic Compounds
Students will be expected to:
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
classify organic compounds into hydrocarbons andhydrocarbon derivatives based on their names or structures(319-7)
differentiate between pure hydrocarbons and hydrocarbonderivatives on the basis of composition
classify hydrocarbon compounds into aliphatics and aromaticsbased on their names or structures (319-7)
defining aromatics as compounds that contain one (or more)benzene ring
classify aliphatic compounds into alkanes, alkenes and alkynesbased on their names or structures (319-7)
describe and explain the trend in boiling points ofhydrocarbons as the number of C’s increase
describe the solubility of these compounds in polar and non-polar solvents
define and be able to give examples of saturated andunsaturated hydrocarbons
draw Lewis dot diagrams to show the bonding in ethane,ethene, and ethyne
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
describe the bonding shapes around each of the carbon atomsinvolved in a single, double or triple bond
write the general formulae for alkanes, alkenes (1 doublebond), alkynes (1 triple bond), cycloalkanes and cycloalkenesand make predictions based on these formulae
Naming and Writing Organic Compounds
Students will be expected to:
write the formula and provide the IUPAC name for a varietyof organic compounds (319-5)
name all the prefixes for 1 to 10 carbons in a compound oralkyl group
write names and molecular formulae, and draw structuralformulae, complete structural diagrams, condensed structuraldiagrams, skeletal structural diagrams, and line diagramsusing the IUPAC rules for the alkanes, cycloalkanes, alkenes,cycloalkenes, and alkynes.
Isomers in Organic Chemistry
Students will be expected to:
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
define isomers and illustrate the structural formulae for avariety of organic isomers (319-6)
define and give examples of structural isomerism
compare the properties of a pair of organic isomers
define geometric isomers (cis and trans)
draw and/or name geometric isomers (cis and trans) for ethenederivatives
draw and name all structural isomers of alkanes (up to 6carbons)
draw and name all structural isomers (including all cyclic) ofhydrocarbons with general formula CnH2n (up to 4 carbons)
define and delimit problems to facilitate investigation (212-2)
perform an experiment identifying and controlling majorvariables (212-3)
select and use apparatus and material safely (213-8)
Writing and Balancing Chemical Equations
Students will be expected to:
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
write and balance chemical equations to predict the reactionsof alkanes (and cycloalkanes), alkenes (and cycloalkenes) andalkynes (319-8)
define thermal and catalytic cracking
compare hydrocarbon cracking and reforming
draw structural diagrams of all organic reactants for:
addition
substitution
cracking
reforming
complete combustion
incomplete combustion
given the reactants in an organic reaction, determine whichtype of reaction will proceed and predict the products,including the formation of any isomers.
determine the name and structure of a missing compound,given an organic reaction with one reactant or product missing
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
Industrial Processes: Hydrocarbons
Students will be expected to:
evaluate the design of a technology and the way it functions, onthe basis of a variety of criteria that they have identifiedthemselves (118-4)
explain the chemical and physical processes involved in oilrefining (fractional distillation, cracking/reforming)
identify various constraints that result in trade-offs during thedevelopment and improvement of technologies (114-4)
describe how modern oil refineries apply a fractionaldistillation process, and cracking/reforming reactions toproduce petroleum products
distinguish between scientific questions and technologicalproblems (115-1)
compare fractional distillation, cracking/reforming done in alaboratory setting with the same processes carried out in oilrefining
Aromatic Compounds
Students will be expected to:
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
classify various organic compounds as aromatic, based on theirnames or structures (319-7)
define aromatics as compounds that contain at least onebenzene ring structure
describe the bonding in benzene using the term “delocalizedelectrons,” and explain how its unreactive nature and the equalC-C bond lengths in benzene are evidence that it does nothave alternating single and double bonds
draw structures for simple monosubstituted benzenes giventhe name, and vice-versa
explain how organic chemistry evolved as new evidence comesto light (115-6)
explain how Kekulé’s invention of the concept of the ringstructure of benzene revolutionized thinking in organicchemistry
write and balance chemical equations to predict the reactionsof benzene (319-8)
draw structural diagrams of all organic reactants and productsin substitution and complete combustion reactions
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
given the reactants in an aromatic reaction, determine whichtype of reaction will proceed, and predict what the productswill be, including the formation of any isomers
determine the name and structure of a missing reactant ofproduct in a reaction of an aromatic
Hydrocarbon Derivatives
Students will be expected to:
classify hydrocarbon derivative compounds into alcohols,ethers, aldehydes, ketones, organic acids, organic halides,esters, amines and amides based on their names or structures(319-7)
define functional group
define “alkyl group”
identify alcohols, ethers, aldehydes, ketones, organic acids,organic halides, esters, amines and amides from their namesand the functional groups in their structural formulae
name and draw structures for derivatives of hydrocarbons(listed above) with only 1 functional group
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
identify limitations of the IUPAC naming system and identifyreasons for alternative ways of naming (214-2)
describe the relationship between intermolecular forces fororganic structures investigated (214-11)
distinguish between the melting and boiling points ofhydrocarbon derivatives and hydrocarbons (of the same size)
write and balance chemical equations to predict the reactionsof hydrocarbon derivatives (319-8)
define and give examples of elimination, esterification, andcombustion reactions
given reactants, determine the type of reaction that proceeds,and the products, including the formation of any isomers
determine the name and structure of a missing reactant orproduct in a reaction of a hydrocarbon derivative
design an experiment identifying and controlling majorvariables (212-3)
select and use apparatus and material safely (213-8)
identify and evaluate potential applications of findings (214-18)
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
synthesize a carboxylic acid
Polymer Chemistry
Students will be expected to:
describe processes of polymerization and identify someimportant natural and synthetic polymers (319-9)
define and outline the structures of monomers, polymers, andpolymerization
identify addition and condensation
polymerization reactions
build models depicting polymerization
provide examples of polymerization in living and/or non-living systems
solve problems for writing complete balanced chemicalpolymerization reactions (319-8)
define problems to facilitate investigation of polymers (212-2)
given a polymer, draw the monomer reactant(s)
Student’s Name____________________________ Course Name Chemistry 2202Unit 1 StoichiometryUnit 2 From Structures to PropertiesUnit 3 Organic Chemistry
R - retain, D - delete, C - changedOutcomes R D C Changed Outcome
describe environmental/health problems associated with theuse of polymers
select, evaluate and integrate information concerningrecyclable polymers from experimental, print and mediasources, and to present an understanding of this informationin a variety of formats such as lab reports, web pages, orposters (213-7, 215-3)
apply organic polymer knowledge to a particular problem,recycling, and analyze the benefits to society by using organicpolymers as the basis for recyclable materials (118-2)
debate the merits of funding specific scientific endeavours andnot others (117-4)
communicate questions, ideas, and intentions regardingrecycling (215-1)
receive, interpret, understand and respond to the ideas ofothers regarding recycling (215-1)
develop, present and defend your position regarding recycling(215-5)