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Chemistry, Grade 13. Curriculum S-17E.Ontario Dept. of Education, Toronto.6710p.

EARS Price MF-$O.65*Chemistry, *Curriculum Guides, *Grade 13

GRADES OR AGES: Grade 13. SUBJECT MATTER: Chemistry.ORGANIZATION AND PHYSICAL APPEARANCE: The guide is divided into 15units, each of which is in list form. It is offset printed andstaple-bound with a paper cover. OBJECTIVES AND ACTIVITIES: Noobjectives are mentioned. Topics to be covered are listed in eachunit. Most units also list several experiments to be performed,although no details are giver. Suggestions are made for timing ofunits. INSTRUCTIONAL MATERIALS: One textbook is mentioned in thepreface. STUDENT ASSESSMENT: No mention. (RT)

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CONTENTS

Preface 1

Ur -r 1: Introduction 3

UNIT 2: Energy Effects in Chemical Reactions 4

UNIT 3: The Rates of Chemical Reactions 4

um"- 4: Equilibrium in Chemical Reactions 5

UNIT 5: Solubility Equilibria 5

UNIT 6: Aqueous Acids and Bases 6

UNIT 7: Oxidation-Reduction Reactions 6

UNIT 8: Experimental Basis for theAtomic Theory 7

UNIT 9: Electron ArranLement and thePeriodic Table 7

UNIT 10: Mole' Iles in the Gas Phase 8

UNIT 11: The Bonding in Solids and Liquids 8

UNIT 12: The Chemistry of Carbon Compounds 9

twrr 13: The Third Row of the Periodic Table 9

UNIT 14: The Fourth-row transition Elements 10

tam- 15: Some Sixth -row and Seventh-row

Elements 10

PREFACE

This course is a considerable departure from the one usedtill now for Grade 13 students. This evolution is madepossible in pert by the considerable revision of the coursefor Grade 12 (Curriculum S -17D). It also reflects the sub-stantial efforts made to upgrade and update Chemistrycurricula in other parts of the world, especially by theCHEM Study and CBA projects in the United States.The revision of the courses in Chemistry for Ontariostudents comes at a time when all aspects of chemicaleducation, including university courses, are under inten-sive study.

The inevitable consequence of the continuous increasein the body of chemical knowledge is that the part ofChemistry which can reasonably be Lught ii an intro-ductory cool se must from time to time be reconsidered inthe light of its relevance and importance to the wholesubject. The result of this review is that some topics thathave in the past been regarded as important have had tobe removed or given lesser sigr' icance, and oth..rsbrought into prominence.

This course gives much greater attention to the struc-ture of atoms, the energy associated with atomic andmolecular even, the nature of bonding in molecules andcrystals, the interpretation of redox reactions iu terms ofelectrochemical cells, a quantitative consideration ofequilibrium, and the interpretation of reaction kinetics interms of collision theory. Besides making these changesin content, the new course places some stress on thenature of scientific activity and scientific explanation andthe Lse of models to explain and describe structure andreactions in Chemistry.

The course given here is based on the Chemical Educa-tion Material Study (citest Study) project in the UnitedStates. The textbook issued by this group, Chemistry AnExperimental Science (1963), emphasizes in its title aswell as its content the importance attached to laboratorywork. From experimental work the student discovers forhimself the origin of chemical principles and the limita-tions and the interpretation of scientific measurements.The natnic, and number of the experiments will require,for their performance, laboratory facilities and the provi-sion of adequate time. Wherever possible, two doubleperiods per week should be allowed for laboratoryexpef iments.

COURSE OUTLINE Unit 1:

INTRODUCTION

(3 weeks)

Reference to Curriculum S17D will show that Chapters Ito 6, 13, 19, and 21 of ChemistryAn ExperimentalScience (1963) have been largely covered in the Grade /2course. There are some significant differences in approach,however, between the two courses. Many teachers maywish to use material from these chapters, though notspecifically listed in the following outline, as a review ofGrade 12 work and as on introduction to the moreinductive and deductive approach that characterizes theclitst Study program. Perhaps this could be made clearerby some specific illustrations.

Chanter I of ChemistryAn Experimental Science (1963)(The Activities of Science) contains very little scientific in-formation that will be unfamiliar to a Grade 13 student.It has, however, a discussion, very simply illustrated, ofinductive reasoning; of the :tature of scientific explana-tion in terms of "models"; of significant figure.; of theuncertainty of scientific observations; of the g:.ephicalportrayal of experimental data. None of these is specifi-cally treated in Curriculum S-17D.

Chapter 2 (A Scientific Model: The Atomic Theory)includes some interesting examples of deduction, e.g. ofthe relative weights of molecules, or of the number ofatoms in a molecule. Exerciss of this kind are notspecifically suggested in Curriculum S-17D.

Although material of this sort is not, as such, includedin the following Units, it embodies the philosophy cf thewhole course. The abovementioned chapters thereforeshould be adequately preserited to the students G s back-ground material.

NOTE:Generally speaking, about three weeks should be given toUnit I, whether the time is distributed throughout theyear or spent at the beginning of the course.

4

3

Unit 2:

ENERGY EFFECTS INCHEMICAL REACTIONS

(2 weeks)

I. Heat and Chemical Reactionsa) The water-gas reactionb) The heat content of a substancec) Additivity of reaction heatsd) The measurement of reaction heat: calorimetrye) Calculation of heat of reaction, LH

2. The Law of Conservation of Energya) Conservation of kinetic and potential energyb) Conservation of energy in a chemical reaction

3. The Energy Stored in & Moleculea) The energy of a molecule: molar heat contentb) Energy changes on warming

4. The Energy Stored in a Nucleus

Experiment: The heat of reaction

4

Unit 3:

THE RATES OFCHEMICAL REACTIONS

(2 weeks)

I. Meaning of Rate of Reaction; units for its expression,e.g. moles/litre/second

2. Factors .Affecting Rates of Reactiona) The nature of the reactantsb) Effect of concentration: collision theoryc) Reaction mechanismd) The quantitative effect )f concentratione) Effect of temperature: collision theory

Distribution of kinetic energiesThreshold energy and rate of reaction

3. The Role of Energy in Rates of Reactiona) Activation energyb) Heat of reactionc) Action of catalystsd) Examples of catalysts

Experir tents:

a) Reaction of potassium permanganate with (i) iron(II)ion (ii) oxalic and sulphuric acids, to illustrate theeffect of reactants, concentration ,)f reactants, tem-

eraturc, and catalysis on the rate of reactionb) Reaction to iodate ion and hydrogen sulphite ion in

presence cf starch to illustrate the effect ct concen-tration changes and temperature changes on the rateof reaction.

Unit 4:

EQUILIBRIUM INCHEMICAL REACTIONS

(2 weeks)

1. Meaning of the Equilibrium State

2. Qualitative Aspects of Equilibriuma) Recognition of equilibriumb) The dynamic nature of equilibrium

SolubilityVapour pressureChemical reactions

c) The state of equilibrium3) Altering the state of equilibrium

ConcentrationTemperatureCatalysts

Attainment of equilibriumPredicting new equilibrium concentrations: LeChatelier's PrincipleEffect of changes in

ConcentrationPressureTemperature

Application of equilibrium principles: the Habe:process

3. Quantitative Aspects of Equilibriuma) The equilibrium constantb) The law of chemical equilibriumc) The law of chemical equilibrium derived frum

rates of opposing reactionsd) The factors which determine equilibriume) Simple problems

Experiment: Verification of the equilibrium law for thereaction:

Fe3+(aq.)+SCN(aq.) 4 FeSCN2+ (aq.)

e)

f)

g)

Unit 5:

SOLUBILITY EQUILIBRIA

(1'/2 weeks)

1. Solubility: A Case of Equilibriuma) Solubility of iodine in ethyl alcoholb) The dynamic nature or solubility equilibrium

Rate of dissolvingRate of precipita:ionThe dynamic nature of equilibrium

c) The factors that determine the solubility of a solidEffect of

RandomnessEnergyTemperature

d) Solubility of a gas in a liquidEffect of

RandomnessEnergyTemperature

2. Aqueous Solutionsa) Review of meaning of electrolyte and 11 on-electro-

lyteb) Types of compounds that are electrolytesc) A qualitative view of aqueous solubilitiesd) The equilibrium law: solubility-product constant

(KOe) Calculation of the solubility of copper(1) chloride

in waterf) Prediction of formation of precipitates in chemical

reactionsg) Precipit,ions used for separationsh) Simple problems

Experiment: Determination of the solubility-productconstant of silver .,:rate

5

Unit 6:

AQUEOUS ACIDS

AND BASES

(21/2 weeks)

1. Electrolytesa) Strong and weak electrolytesh) Water: a weak electrolyte

Ion-product constant for waterc) Special roles of H+ (aq.) and OH-(aq.) in water

2. Introduction to Acids and Bases (see CurriculumS-17D, Unit IX, 4)a) Properties of aqueous solutions of acidsb) Properties of aqueous solutions of bases and their

explanationc) The nature of H+(aq.); sow. models to explain itd) Acid-base titrations

Calculation of [H+ ] and [01-1- } at various pointsduring the neutralization of a strong acid or astrong base

e) Definition of pH

3. Strengths of AcidsWeak acidsa) Equilibrium constants for ionizatior of weak acids

Calculations of equilibrium constant for weak acidsUse of equilibrium constant to calculate [H+ ]

b) Competition for protons among weak acidsHydronium ion in the proton-transfer theory ofacids

c) Contrast of acid-base definNons

Experimenb:a) Determination of the approximate hydrogen-ion con-

centration of solutions using indicatorsb) Application of Le Chatelier's Principle to a reversible

chemical reaction; the influence of [11+ ] on thechromate ion-dichromate ion equilibrium

c) Quantitative acidbase titrationsStandardization of a base using a standard acidTitration of an unknown acid

6

Unit 7:

OXIDATION-REDUCTION

REACTIONS

(21/2 weeks)

1. Electrochemical Cellsa) The chemistry of an electrochemical cellb) Oxidation-reduction reactions without electrodes;

competition for electrons (see Curriculum S-17D,Unit IX, 3)

c) The nomenclature of an electrochemical cell

2. Electron Transfer and Prediction of Reactionsa) Electron-losing tendency

Demonstration cf voltages of electrochemical cellsHalf-cell potentials; the hydroget, half-cell as astandard; table of half-cell potentials

b) Prediction of reactions from table of half-cellpotentials; effect of concentration such pre-dictions; validity of predictions

c) Oxidation numbersOxidation and reduction in terms of changes inoxidation numbers

3. Balancing of Oxidation-Reduction Reactionsa) Use of half-reactions (electron balancing)b) Use of oxidation numbers

4. Electrolysisa) Review of Unit IX, 2 of Curriculum S-17Db) Electrolysis as a reverse reaction to that occurring

in an electrochemical cell

Experiments:

a) An introduction to oxidation-rcductionReactions involving metals such as zinc, copper, andlead, when placed in solutions of each metal's salts(see Unit IX, Experiment (g) of Curriculum S-17D)Reactions involving displacement of bromine, iodine,from solutions of halides of metals (sec Unit XI, 2%b)of Curriculum S-17D)

b) Etc.( trochemical cells using pairs of metals such aszinc-copper, silver-copper

c) Reactions between ions in solutionReactions involving solutions containing ions whichwhen mixed produce (I) precipitates and (ii) oxidation-reduction reactions

Unit 8:

EXPERIMENTAL BASIS FOR

THE ATOMIC THEORY

Unit 9:

ELECTRON ARRANGEMENT AND

THE PERIODIC TABLE

(11/2 weeks) (11/2 weeks)

1. Chemical Evidence for the Atomic Theorya) The laws of definite proportions and multiple pro-

portionsb) The law of combining gas volumesc) Faraday's laws of electrolysis (number of coulombs

/mole of elections)

2. Physical Evidence for the Atomic Theorya) Electrical conduction in rarefied gases; properties

of cathode raysb) Deflection of cathode rays by magnetic fields to

measure e/ for electronsc) Millikan's oil-drop experiment to deduct e for

electronsd) Production of positive ions in rarefied gases;

measurement of e the mass spectrographe) Scattering of a-particles by metallic foils; hy-

pothesis or nuclear atom (the mathematical basisneed not be learned)

3. Spectroscopic Information about Atomi. and Molecu-lar Dimensionsa) Light and the frequency spectrumb) X-ray diffraction patterns revealing spacings in

crystalsc) Infrared spectroscopy revealing rotation and vibra-

tion in molecules

Experiment: The relationship between the moles ofcopper, moles of silver, and moles of electrons involvedduring electrolysis

Spectroscopy of the Hydrogen Atoma) Energy associated with light; Planck's relationshipb) The line spectrum of hydrogen atoms; spectral

seriesc) Energy levels in hydrogen atomsd) The quantum jump in electronic transitions; sta-

tionary states in atomse) Quantum numbers: n, principal quantum numberf) Orbitals: a re; resentation of the distribution of an

electron in space about an atomic nucleus. Desig-nation of orbitals s, p, d,f

g) Description of s acid p orbitalsh) The total number of orbitals for each value of n;

the number of s, p, d, and f orbitals within thistotal

2. Many-Electron AtomsEnergy levels of many-electron atoms. Differentia-tion in energy levels of s,p,d, andf orbitals havingsame value of n (cf. hydrogen atom)Build-up of periodic table. Filling of orbitals inorder of ascending energy regulated by the PauliPrinciple (maximum of 2 electrons per ort:tal) anda principle of maximum repulsion (orbitals ofequivalent energy are first filled singly beforer.iring occurs)

3. Ionization Energy and the Periodic Tablea) Definition of ionization energyb) Trends in ionization energies among first 20 ele-

mentsc) Ionization energies (first, second, etc.) and valence

electronsd) Fourth row of periodic table; significance of ten

transition elements

a)

b)

7

Unit 10:

MOLECULES INTHE GAS PHASE

(2 weeks)

I. The Covalent Bonda) The hydrogen moleculeb) Interaction between helium atomsc) Representation of chemical bondingd) The bonding of fluorine

Ponding Capacity of the Elements Lithium to OxygenThe coaelation of ordinary bonding capacities withorbital occupancies of the atoms of these elements

3. Trend in Bond Ty pe Among Some Fluorine Com-poundsa) The bonding in gaseous lithium fluorideb) Ionic character in bond; to fluorine (lithium to

oxygen)c) Ionic character in bonds to hydrogen

4. Molecular Architecturea) The shapes of some molecules: water, diftuorine

oxide, ammonia, nitrogen trifluoride, methane,cai bon tetraftumide, boron trifluoride, teryllium

b) Molecular shape and electric dipoles

5. Double Bondsa) Bonding in the oxygen moleculeb) Ethylene: a carbon-carbon double bond

Experiment: Investigation of some of the properties of apair of cis-trans isomers; e.g., maleic and fumaric adds

8

Unit 11:

THE BONDING INSOLIDS AND LIQUIDS

(2 weeks)

1. The Elementsa) van der Waals' forcesb) Covalent lands and network solidsc) Metallic bonding

2. Compoundsa) van der Waals' forces and inoiecular substancesb) Covalent bonds and network solid compoundsc) Alloysd) Ionic solidse) Effects due to charge separation0 Hydrogen bonds

Experiment: Corstruction of models to show the packingof atoms or ions in crystals

Unit 12.

THE CHEMISTRY OFCARBON COMPOUNDS

(3 weel:s)

I. Sources of Carbon Compounds

2. Moloniar Structures of Carbon Compoundsa) The composition and strut:Uwe of car bon com-

poundsb) Experimental determination of molecular structurec) The ethyl group

3. Some Chemistry of Organic Compoundsa) Ciemical behaviour of ethyl and methyl bromideb) Oxidation of organic compoundsc) The functional groupd) Aminese) Acid derivative s: esters and amides

4. Nomenclature

5. Hydrocarbonsa) Saturated hydrocarbonsb) Ulsatursted hydrocarbonsc) Benzene and its derivatives

6. Polymersa) T3 pes of polymerizationb) "Nylon," a polymeric amidec) Protein, another polymeric amide

Experiments:

a) Some reactions of hydrocarbons and of alcoholsb) The ireparation of some derivatives of organic acids

Unit 13:

THE THIRD ROW OF THEPERIODIC TABLE

(11/2 weeks)

1. Physical Properties of the Elen....mt,s) Sodium, magnesium, and aluminium:

solidsb) Silicon: a network solidc) Phosphorus, sulphur, and chlorine: molecular

solids

2. The Elements as Oxidizing and Reducing AgentsSodium, magnesium, and aluminium: strong re-ci,:.cing agents

Silicon, phosphorus, and sulphur: oxidizing andreducing agents of intermediate strength,hlorine: a strong oxidizing agent

metallic

a)

b)

.!)

3. 'fhe Acidic and Basic Properties of the Hydroxidesn) Sodium and magnesium hydroxides: strong basesh) Aluminium hydroxide: an amphoteric hydroxidec) Silicon, phosphorus, sulphur, and chlorine oxy-

acids

4. Occurrence and Preparation of the Third-rowElements) Occurrence

1) Preparation of the elements

5. -"rends in Some Properties of Second-row and Third-row Elements

Experiment: Comparison of the relative acid-base strengthof t hydroxides of the third row of the periodic table

9

Unit 14:

THE FOURTH-ROWTRANSITION ELEMENTS

(21/2 weeks)

1. Meaning of Transition Elementa) Electron configurationb) General properties

2. Complex Ionsa) Natureb) Geometryc) Bondingd) Arnphoteric complexes

3. Some Properties of Fourth-row Transition Elementsa) General propertiesb) Specific properties of chromium, manganese, iron,

nickel, copper, zinc

Experiments:

a) Separation of iron, cobalt, and nickel ions by ananion exchange resin

b) Corrosion of ironc) Preparation of a complex salt and double saltd) Preparation of potassium dichromate

10

Unit 15:

SOME SIXTH-ROW ANDSEVENTH-ROW ELEMENTS

(1/2 week)

1. The Sixth Row of the Periodic Tablea) The lanthanides, or rare earths

2. The Seventh Row of the Periodic Tablea) The occurrence of the seventh-row elementsb) The elements following ac.iniumc) Nuclear stability and radioactivityd) Types of radioactivitye) Nuclear energy