DOCUMENT RESUME

ED 084 083 SE 014 896

AUTHOR Mary, Charlotta B.; Feuer, JeroldTITLE Physical Chemistry, Science (Experimental):

5318.60.INSTITUTION Dade County Public Schools, Miami, Fla.PUB DATE 71NOTE 14p.; An Authorized Course of Instruction for the

Quinmester Program

EDRS PRICE MF-$0.65 HC-$3.29DESCRIPTORS *Chemistry; *Instruction; Laboratory Experiments;

*Objectives; Science Education; Secondary SchoolScience; *Teaching Guides; Thermodynamics; Units ofStudy (Subject Fields)

IDENTIFIERS *Quinmester Program

ABSTRACTPerformance objectives are stated for this secondary

school instructional unit concerned with aspects of physicalchemistry, involving the physical properties of matter, and laws andtheories regarding chemical interaction. Lists of films andstate-adopted and other texts are presented. Included are enrollmentguidelines; an outline summarizing the unit content; a list ofdiscussion questions; and numerous suggestions for experiments,demonstrations, field trips, and reading assignments. A master sheetshoving the relationship of each suggested activity to the objectivesof the unit is ai pended in this booklet. (CC)

U S DEPARTMENT OF HEALTH,EDUCATION &WELFARENATIONAL INSTITUTE OF

EDUCATIONt0( 'I N T N PI 01(0

,r1 f A( Y 141 ( 41-11 11(0/,f1 PSON ()1(,,A1otA r109100,G1P1A 1 (OP ()PA,00.45

A 1 F DO ( t...,Af(if 1(101(1

A 'if ,A if l'(!(-:Af Ae,111LIf 00I t),,( A 1`0 `9.

AUTHORIZED COURSE OF INSTRUCTION FOR THE U

41-5>d\4

PHYSICAL CHEMISTRY

5318.60

SCIENCE

(Experimental)

FILMED FROM BEST AVAILABLE COPY

Om

C.

...c

r"Cro,C")

4=2Or--Cr,

'DIVISION OF INSTRUCTION1971

PHYSICAL CHEMISTRY

5318.60

SCIENCE

(Experimental)

Written by Charlotta B. Mary and Jerold Feuer

for the

DIVISION OF INSTRUCTIONDade County Public Schools

Miami, Florida1971

DADE COUNTY SCHOOL BOARD

Mr. William Lehman, ChairmanMr. G. Holmes Braddock, Vice-Chairman

Mrs. Ethel BeckhamMrs. Crutcher Harrison

Mrs. Anna Brenner MeyersDr. Ben Sheppard

Mr. William H. Turner

Dr. E. L. Whigham, Superintendent of SchoolsDade County Public Schools

Miami, Florida 33132

Published by the Dade County School Board

Copies of this publication may be obtained through

Textbook Services2210 S. W. Third StreetMiami, Florida 33135

TABLE OF CONTENTS

Page

COURSE DESCRIPTION 1

ENROLLMENT GUIDELINES 1

STATE ADOPTED TEXTS 1

PERFORMANCE OBJECTIVES 2

COURSE OUTLINE 3

EXPERIMENTS 5

DEMONSTRATIONS 6

FIELD TRIPS 6

FILMS

SUGGESTED DISCUSSION QUESTIONS 8

REFERENCES 9

MASTER SHEET 10

PHYSICAL CHEMISTRY

COURSE DESCRIPTION

Physical chemistry is that branch of chemistrywhich deals with the study of the physical propertiesof matter,the structure of matter and the laws andtheories regarding chemical interaction. Physicalchemists seek to codify the data and formulate the basicprinciples of descriptive chemistry as usually taughtin the introductory courses.

ENROLLMENT GUIDELINES

The student should have finished four quinmestercourses of chemistry before electing physical chemistry.Progress in physical chemistry is tested largely by thestudent's ability to solve specific problems. It isrecommended that he have a good grasp of the alge-braic processes, and that he be able to relate thesymbols of a mathematical expression to chemicalrealities.

STATE ADOPTEL TEXT

1. Physical Sciences Study Committee, Physics, 2ded. Boston: D. C. Heath and Co., 1965.

PERFORMANCE OBJECTIVES

The student will:

1. Given problems involving the pressure, volumeand temperature of an ideal gas, show his com-prehension of Charles' Law, Boyle's Law and theideal gas equation by using the correct relation-ship to solve problems.

2. Plot a graph of pressure versus volume of anideal gas.

3. Given the above graph, identify the variousisotherms, isobars and isometric curves.

4. Synthesize from experimental data a cycleutilizing the pressure versus volume graph(Carnot cycle).

5. Distinguish between Cv (heat capacity at constantvolume) and Cp (heat capacity at constantpressure).

6. Differentiate between enthalpy (p H), energy(AE), entropy (LIS), and Gibbs' free energy(AG) .

7. Specify how these state functions are relatedto C and C.

8. Discover the relationships between4 E,41G,AL H, AS, and the equations for chemicalequilibriums.

9. Derive the rate law and the molecularity for agiven equation.

10. Identify the variables in the Boltzmann expression,the Arrhenius equation and the absolute reactionrate.

2

PERFORMANCE OBJECTIVES (CONT'D)

11. Examine the deviations from solution ideal-ity involved in Raoult's Law and Her.ry's Law.

12. Cite evidence for the failure of NewtonianMechanics to explain atomic spectra, black bodyradiation, and the behavior of elementaryparticles.

13. Discuss critically the conclusions of De Broglie,Heisenberg, Planck and Schroedinger, relativeto the quantum theory.

14. Describe an electron cloud conception of bothcovalent and ionic chemical bonds.

15. Propose reasons for dipole moments, bond strengths,bond angles, bond lengths in terms of electroncloud model and overlap.

16. Describe the bonding in Fn and LiF in terms ofsimple molecular orbital .

COURSE OUTLINE

I. Gases

A. Charles' Law

B. Boyle's Law

C. Ideal Gas Law

D. pv = nRT (Pressure- Volume Relationships)

E. Carnot Cycle

II. Thermodynamics

A. Heat Capacity

3

COURSE OUTLINE (CONT'D)

1. C (Constant Volume)2. C

v(Constant Pressure)

B. State Functions1. Enthalpy2. Energy3. Entropy4. Gibbs Free Energy

C. Chemical Equilibrium1. Mass Action Law2. Sojubility Expressions

III. Kinetics

A. Rate Laws and Molecularity

B. Kinetic Theories1. Boltzmann Expression2. Arrhenius Equation3. Absolute Rate Theory

IV. Solutions

A. Ideal Solutions1. Raoult's Law2. Henry's Law

B. Nonideal Solutions

V. Quantum Theory

A. History1. Failure of Newtonian Mechanics to Explain

Observed Phenomena.2. De Broglie3. Heisenberg4. Planck5, Schroedinger

B. Wave Mechanics

4

COURSE OUTLINE (CONT'D)

C. Orbital Overlap and Bonding1. Dipole Moments

Bond Angles3. Bond Lengths4. Bond Strengths

D. Molecular Orbital Theory1. Linear Combination of Atomic Orbitals2. Resonance

EXPERIMENTS

Curriculum Bulletin, 8-D. Chemistry 2. Miami, Florida:Dade County Public Schools, 1966.

1. Boyle's Law (Ex. 18, p. 105)2. Charles' Law (Ex. 19, p. 107)3. Molecular Weight of a Gas (Ex. 20, p.. 109)4. Solubility (Ex. 21, p. 113)5. Solubility Product Constants (Ex. 22, p. 116)6. Reaction Principles (Ex. 27, p. 132)

Salzberg, Morrow, Cohen, Laboratory Course in PhysicalChemistry. New York: Academic Press, 1966.

7. Cv/Cp Ratio of a Gas (Ex. 2, p. 179)8. Standard Free Energy, Enthalpy, and Entropy

of Reaction, (Ex. 20, p. 221)9. Energies and Heats of Combustion and For-

mation (Ex. 13, p. 217)10. Rate of the Acid-Catalyzed Inversion of

Sucrose (Ex. 30, p. 250)11. Effect of Ion Strength on Rate of Reaction

(Ex. 31, p. 252)12. Vapor Pressure Versus Temperature (Ex. 6,

p. 188)13. Bond Moments, Bond Angles and Dipole Moments

(Ex. 37, p. 272)14. Dipole Moment of a Polar Liquid (Ex. 36,

p. 268)

5

DEMONSTRATIONS

Shoemaker and Garland. Experiments in PhysicalChemistry. New York: McGraw Hill Book Co.,1962.

1. The teacher will build and demonstrate a gaseousthermometer (p. 38)

2. The teacher will demonstrate calorimetricallythe measurements of heat and relate thisgeneral method to the measurements of Cp,Cv, H, etc. (p. 107)

3. Iodine Clock experiment (p. 214)4. The teacher will demonstrate the measurer.:nt of

the vapor pressure of a solution (p. 1.)9)

Salzberg, Morrow and Cohen, Laboratory r.,urse in PhysicalChemistry. New York: .iclademic Press, 1966.

5. Constant-Volume Ideal. Gas Thermometers (p. 43)6. Kinetics of the Iodine- -catalyzed Decomposition

of H202. (Ex. 29, p. 246)

FIELD TRIPS

1. To the University of Miami to observe thecalorimetry lab.

2. To Florida Atlantic University to observe therunning of infra-red, ultra-violet and nuclearmagnetic resonance spectra.

6

DADE COUNTY 16 mm FILMS

1. Demonstrating the Gas LawsAV#1-10740, 21 min. C

2. Gas Pressure and Molecular CollisionsAV#1-10849, 21 min. BW

3. ThermodynamicsAV#1-05588, 11 min., BW

4. Introduction to Reaction KineticsAV#1-10959, 13 min., C

5. EquilibriumAV#1-10829, 22 min., C

6. Photoelectric EffectAV#1-30317, 28 min., C

7. PhotonsAV#1-10794, 25 min., BW.

8. Atomic RadiationAV#1-01921, 11 min., BW

SUGGESTED DISCUSSION QUESTIONS

1. What observaticns do you think Boyle and Charlesmade that led them to formulate their gas laws?

2. Given that pressure times volume gives unitsof energy, how do you think that temperatureis related to energy?

3. What types of things contribute to the values ofCv and C ?

p

4. For many chemical reactions, the rate of reactiondoubles for a 100 temperature rise. How wouldyou explain this?

5. What would a solution's cohesive properties haveto do with its observance of Raoult's Law orHenry's Law?

6. What do you think causes chemical bonds tohold together?

7. How do you feel that quantum theory fits intothe evolutionary scheme of sciencr?

8. Using the same type of arguments as givenfor the strength of chemical bonds, why do youthink that different substances melt and boilat different temperatures?

9. DeBroglie was laughed at when he first proposedhis hypothesis. Can you give examples of howthe evolution of scientific discovery was markedby skeptics and closed-minded scientificcommunities?

8

REFERENCES

1. Curriculum Bulletin 8-D. Chemistry 2. Miami,Florida: Dade County Public Schools, 1966.

2. Daniels, Farrington and Alberty, Robert.Physical Chemistry, 3d ed. New York:Wylie and Sons, 1966.

3. Kittsley, Scott L. Physical Chemistry, 3d ed.New York: Barnes and Noble, Inc., 1969.

4. Lewis, Gilbert N. Chemistry. 7th ed. New York:Barnes and Nobles, Inc., 1962.

5. Mahan, Bruce. Elementary Chemical Thermo-dynamics. New York: W. A. Benjamin, Inc.1964.

6. Nash, Leonard K. Elements of Chemical Thermo-dynamics, Reading, Mass: Addison-WesleyPublishing Co., Inc., 1962.

7. Physical Sciences Study Committee. Physics,2d ed. Boston: D. C. Heath and Co., 1965.

8. Ryschkewitsch, George E. Chemical Bonding andthe Geometry of Molecules. New York:Reinhold Publishing Corporation, 1963.

9. Salzberg, Hugh W. Morrow, Jack I. and Cohen,Stephen. Laboratory Course in PhysicalChemistry. New York: Academic Press, 1966.

10. Shoemaker, David and Garland, Carl. Experimentsin Physical Chemistry. New York: McGraw HillBook Company, 1962.

9

oz

Z6I'd s R 00I489'dd 8

Z6T -E9E.dd E 91

I6E'd s u z .deu o

Z0S'd Z E8-Wdd ry

861.d z '11 'ET ST

ItT'd s L t I ISI-6/I'dd £ Z 'duLIO 8 I

VT

6 '9 C

1LI -OSI'dd E

EE'du40 4 ET

9 8 '9 Z ZT 'dug., Z 7E 'duLID 4 ZT

' 1

SL 4994EL

.04Tg.dd 9 L 'de40 E ZI II

7 9 OT 'deLID E 9 OT

ICI -0Erdd g 1 Z 7 01 'clu40 Z or 'dv40 E

z

IT 40I 6

901 -s0/.dd 9

E

S . St 'd 9

94E'du4D Z

68 4zL.Ldd g

g 'de40 E

IV 'd E 6 4S 47 8

09 d g C z .deq3 z Z 'dell0 s L

E T E Z

Z .deqo z

SL .d 9

OR 'd E

Z 'de40 S

SZ 'duLIO L 8 9

09 .d q

57..07 dd s ZI1411I

4ES4LI'dd 9

z .dailo z

gy .d E / S

/Ord 8 7E 'd 9 7

E dailo z gz-Ez.dd 9 E

tvd g Z Z 'I T Z4I'd1340 s Z '1 Z

trd g 1 S Z 4I r *45.40 z

6 'd940 t

ZS -67'44 7 E 4Z 4T I

SUIO [ gala SUOT3eanO uoTesnosT0

suopeals wily -uowa0 PTaid

swlid saJualajoll

10430 s ulpsau

71.1apn7g

paiTnba

s3uawilo a BOA17 -00[4o

XHISIWAHD VOISAIld - laAHS H31SVW