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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



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)



Solutions and the M ole


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



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


identify mole ratios of reactants and products from balanced

chemical equations (323-10)



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



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



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



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



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



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




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



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



Molecular Compounds: Network Covalent Solids


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)



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


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



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



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


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



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


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



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




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



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


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




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




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



Industrial Processes: Hydrocarbons


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




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



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


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



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)



synthesize a carboxylic acid

Polymer Chemistry


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)



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)

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