ofb chapter 1 lecture notes - georgia institute of...

OFB Chapter 1 11/3/2003

Subject: new element

A major research institution has recently announced the discovery of the heaviest element yet known to science. This new element has been tentatively named "Administratium". Administratium has I neutron, 12 assistant neutrons, 75 deputy neutrons, and III assistant deputy neutrons, giving it an atomic mass of 312. These 312 particles are held together by a force called "morons", which are surrounded by vast quantities of lepton-like particles called "peons". Since Administratium has no electrons, it is inert. However, it can easily be detected as it impedes every reaction with which it comes into contact. A minute amount of Administratium causes one reaction to take over 4 days to complete when it would normally take less than an hour. Administratium has a normal half-life of 3 years; it does not decay but instead undergoes a reorganization, in which a portion of the assistant neutrons and deputy neutrons and assistant deputy neutrons exchange places. In fact, Administratium's mass will actually increase over time, since each reorganization causes some morons to become neutrons forming "isodopes." This characteristic of moron-promotion leads some scientists to speculate that Administratium is formed whenever morons reach a certain quantity in concentration. This hypothetical quantity is referred to as "Critical Mass". You will know it when you see it.


Chem 1310 Spring 2003

William J. Baron, Ph.D.– GaTech School of Chemistry and Biochemistry

• Director of the Freshman Chemistry Program– 1310, 1311, 1312, 1313– Office Boggs 1-59A (temporary) inside Main

Chemistry office Boggs – Office Chem Annex Room 47– E-mail preferred

[email protected]– Phone 404-385-2808– Mailbox in Chemistry Office

– Lucent Technologies, Bell Laboratories (retired)

• Director, Optical Products Technology –Norcross

– Fiber Optics, R&D, product design and development

• Director, Advanced Materials Development –New Jersey

– Semiconductor crystals and devices– Circuit board fabrication and assembly

– Ph.D. Princeton, Postdoctoral work at Ruhr Universität Bochum and Columbia

– Specialties: Physical Organic Chemistry, reaction mechanism, reactive intermediates, photochemistry, polymers


Chem 1310 Spring 2003 Sections AB

• Course Objectives– Semester Schedule (later slide)

• Problems, Exercises• Exams

– Friday, January 24– Wednesday, February 12– Wednesday, March 19– Monday, April 14– Friday, ,May 2 2:50 PM to 5:40 PM

Room CoC 16)

• Grading– Hour Exams 45% (5%. 10%, 15%, 15%)– Final Exam 25%– Homework 10%– Laboratory 20%


Chem 1310 Spring 2003 Sections AB

• Lectures– MWF, 10:05 - 10:55 – Will use ppt, suggest downloading

lecture notes, print 1, 4, 6 per slide

• Recitations and Labs– Recitations: (50 minutes)

• Wednesdays, either 1:05, 2:05, or 3:05 PM

– Labs: (2 hours 50 minutes)• Tuesdays, either 12:05 or 3:05

• Office Hours – MWF following lecture in Chem Annex

47 office– Or by appointment

• Study– ask questions, memorization not the

whole answer, study everyday, stay limber, can’t cram


www.chemistry.gatech.edu/class/1310/1310ab/

Instructor

Teaching Assistants

Required Course materials

Course Description

Grading Policies

Syllabus

Homework

Lecture Notes

Exams

Exam 1

old exams

answer key

Exam 2

Exam 3

Exam 4

Final Exam

CHEM 1310 SECTION AB SPRING 2003 GENERAL CHEMISTRY

Class Meetings Classes begin on Monday, January 6 and end on Friday April, 25. Holidays are Monday, January 20 (MLK Day), and Monday through Friday, March 3 to 7 (Mid- Semester Break).

Lectures: Monday, Wednesday, and Friday, 10:05 − 10:55

Recitations: Wednesday, either 1:05 to 1:55, or 2:05 to 2:55, or 3:05 to 3:55 or 4:05 to 4:55.

First meeting is January 8.

Labs: Tuesday, either 12:05 to 2:55, or 3:05 to 5:55.

First Lab meeting is Tuesday January 14.

Instructor Dr. William J. Baron Office: 1-59A Boggs Bldg. (will be moving in early semester to Boggs 1-108)

Phone: 404-435-2808

e-mail: [email protected]

Office Hours: Monday, Wednesday, and Friday, 11:00 − 12:00 in Chem Annex 47 or by

appointment

Teaching Assistants SECTION NAME LOCATION

OFFICE HOURS

E-MAIL

A1 Tumpa Sarkar [email protected] A2 Berhane Temelso [email protected] A3 Victoria Mariani [email protected] B1 Frankie Onyemauwa [email protected] B2 Kristin Shepperd [email protected] B3 Asmerom Hagos [email protected]

Required Course Materials Lecture Text: Chemistry: Science of Change, 4th Ed., by Oxtoby, Freeman, & Block. Lab Text: Laboratory Experiments for General Chemistry, 4th Ed., by Hunt, Block, & McElvey

Other Materials (GT bookstore)

• Calculator (+, -, *, /, ln, and log)

• Key-controlled combination lock. Locks can be purchased at the bookstore (must be "chemistry locks"). Used locks may be purchased (at a discount price) from the stockroom in the Chem Annex.

• Safety glasses or goggles

• Lab Apron (recommended)

• NOTE: You should maintain a balance of at least $30 on your BuzzCard so that you can pay for any fees you might incur in lab (breaking glassware, renting safety goggles, etc). Payment will be made at the Annex stockroom. You will not be permitted to work in lab unless you are wearing safety glasses or goggles and closed shoes.

Course Description The course covers fundamental observations, laws, and theories of chemistry at the introductory level. Topics include atoms/molecules, stoichiometry, acids/bases, solutions, equilibria, gases, solids, liquids, thermodynamics, electrochemistry, kinetics, quantum theory, the periodic table, and chemical bonding. Grading Policies Attendance: Attendance is expected in lecture, required in laboratory and highly

beneficial in recitation. Material on exams may be taken from assigned reading, homework, lecture material, or problems similar to those at the end of each chapter in the course text.

Recitation: The weekly recitation section is meant to give students a chance to ask

questions and see sample problems worked. Each recitation section will be directed by a teaching assistant (TA) who is usually a chemistry graduate student.

Exams: Four closed-book exams will be given during the semester. The exam

dates are Friday, January 24, Wednesday February 23, Wednesday March 19, and Monday April 14, 2003.

Final Exam: A three-hour final exam will be given at the time and place determined for

this course by standard Georgia Tech procedures. The final exam for this course is tentatively scheduled for Friday, May 2 at 2:50 PM in Room 16 CHEM Annex.

Homework: Homework problems will be assigned weekly and will be graded on a 0, 1, 2 basis. Many exam questions will be analogous to assigned homework

problems, so working homework problems is an essential part of exam

preparation. Assigned homework problems are taken from the textbook. It is OK for students to collaborate on homework, but each student should turn in their own homework in their own writing. Homework will be collected each week during.

Laboratory Grade: You must pass Laboratory to pass the overall course. Teaching

Assistants will have the responsibility for establishing laboratory grades. Students are graded on pre-lab quizzes, formal lab reports, summary reports, report accuracy, lab technique and attitude, Lab Midterm exam, and Lab Final exam. A grade of 70% or better in the lab is considered passing. Grades between 60% and 65% will be considered, if documentation is provided for any extenuating circumstances.

Grade Changes: Re-grades of hour exams must be requested within one week of the date

that the graded exams are returned to students. Only re-grades that could add four or more points to the score will be considered.

Make-up Exams: There will be no make-up exams. If a student has a valid excuse for

missing an exam, his/her grade for that exam will be calculated from his/her performance on that part of the final exam that covers topics from the missed exam..

Honor Code: Students are expected to adhere to the Georgia Tech honor code during all

aspects of this course (see http://www.honor.gatech.edu/ for details). The basis for course grades will be as follows: Hour Exam 1 5%

Hour Exam 2 10%

Hour Exam 3 15%

Hour Exam 4 15%

Final Exam 25%

Homework 10%

Laboratory 20%

Course Webpage

Information of interest to students will be posted on the course webpage: http://www.chemistry.gatech.edu/class/1310/1310ab/

Students should consult the webpage at frequent intervals throughout the semester.

Dr. William J. BaronDepartment of Chemistry and Biochemistry

Chem 1310General ChemistrySections A1-3, B1-3MWF 10:05 to 10:55

Monday, Wednesday and Friday Course Schedule Recitation on WednesdaysCollege of Computing Room 16 Homework Assignments, due at Recitation

Date Topic Reading Problems for HomeworkMonday, January 06, 2003 Course Introduction & OFB Chapter 1 Chapter 1Wednesday, January 08, 2003 Lab Introduction (Dr. George McKelvy) Appendices A-C Meet TAs, discuss Labs, recitations, etc.Friday, January 10, 2003 The Atomic Nature of MatterMonday, January 13, 2003 Stoichiometry Chapter 2Wednesday, January 15, 2003 OFB 1: # 9, 10, 11, 17, 19, 20, 29, 37, 38, 55, 68Friday, January 17, 2003 Chemical Periodicity & Formation of Simple Compounds Chapter 3Monday, January 20, 2003 HolidayWednesday, January 22, 2003 OFB 2: # 2, 5, 33, 42, 43, 44, 81Friday, January 24, 2003 Exam 1 (Chapters 1-3)Monday, January 27, 2003 Review & Types of Chemical Reactions Chapter 4Wednesday, January 29, 2003 OFB 3:# 8, 9, 18, 34, 45, 57, 59, 60, 69, 70Friday, January 31, 2003 Monday, February 03, 2003 The Gaseous State Chapter 5Wednesday, February 05, 2003 OFB 4: # 1, 6, 12, 50, 54, 55, 59, 71Friday, February 07, 2003 Condensed Phases and Phase Transitions Chapter 6Monday, February 10, 2003 Wednesday, February 12, 2003 Exam 2 (Chapters 4-6) OFB 5: # 34, 38, 48, 62, 70, 81Friday, February 14, 2003 Review & Chemical Equilibrium (Last Day to Drop) Chapter 7Monday, February 17, 2003 Wednesday, February 19, 2003 OFB 6: # 4, 20, 26, 38, 44, 62Friday, February 21, 2003 OFB Acid-Base Equilibria Chapter 8Monday, February 24, 2003 Wednesday, February 26, 2003 OFB 7: # 1, 2, 7, 9, 12, 15, 18, 24, 31, 42, 45Friday, February 28, 2003 Dissolution and Precipitations Equilibria (mid-Term Grades Due) chapter 9Monday, March 03, 2003 BreakWednesday, March 05, 2003 Break OFB 8: # 5, 9, 11, 12, 26, 31, 42, 43, 44, 46Friday, March 07, 2003 BreakMonday, March 10, 2003 Wednesday, March 12, 2003 Thermochemistry Chapter 10 OFB 9: # 16, 19, 23, 30, 39, 41, 42, 51, 52, 54Friday, March 14, 2003 Monday, March 17, 2003 Wednesday, March 19, 2003 Exam 3 (Chapters 7-10) OFB 10: # 11,13,19, 23,33,37,40, 43,49,53,59,63Friday, March 21, 2003 Review & Spontaneous Change and Equilibrium Chapter 11Monday, March 24, 2003 Wednesday, March 26, 2003 OFB 11: # 13, 15, 23, 29, 31, 37, 39, 43, 49, 53, 57, 63, 69Friday, March 28, 2003 Redox reactions and Electrochemistry Chapter 12Monday, March 31, 2003 Wednesday, April 02, 2003 Electrochemistry and Cell Voltage Chapter 13 OFB 12: # 1, 3, 7 ,9, 11, 13, 29, 31, 33Friday, April 04, 2003 Monday, April 07, 2003 Chemical Kinetics Chapter 14Wednesday, April 09, 2003 OFB 13: # 3, 5, 9, 11, 15, 19, 29, 31, 35, 37, 41, 45Friday, April 11, 2003 Monday, April 14, 2003 Exam 4 (Chapters 11-14)Wednesday, April 16, 2003 Review & Quantum Mechanics & The Hydrogen Atom Chapter 16 (note skip OFB 15) OFB 14: # 7, 9, 11, 15, 19, 21, 23, 25, 37, 41, 43, 45, 51, 53Friday, April 18, 2003 Monday, April 21, 2003 Wednesday, April 23, 2003 Many-Electron Atoms and chemical Bonding Chapter 17 OFB 16: # 14, 16, 22, 28, 34, 41 Friday, April 25, 2003 Friday, May 02, 2003 Tentative Final 2:50 PM to 5:40 PM OFB 17 don’t turn in: # 1, 3, 5, 7Monday, May 05, 2003 All grades due to Registrar's Office by 12 noon

Phone: 404-398-2808

E-mail [email protected] Boggs

Mailbox in Chemistry Department Main Office

CHEM 1310 SECTION AB Spring 2003 GENERAL CHEMISTRY

Homework Problems (to be turned in at Recitation) December 17, 2002 update ______________________________________________________________________________ Chapter Problems Due Date ______________________________________________________________________________

1 9, 10, 11, 17, 19, 20, 29, 37, 38, 55, 68 Jan-15

2 2, 5, 33, 42, 43, 44, 81 Jan-22

3 8, 9, 18, 34, 45, 57, 59, 60, 69, 70 Jan-29

4 1, 6, 12, 50, 54, 55, 59, 71 Feb-05

5 34, 38, 48, 62, 70, 81 Feb-12

6 4, 20, 26, 38, 44, 62 Feb-19

7 1, 2, 7, 9, 12, 15, 18, 24, 31, 42, 45 Feb-26

8 5, 9, 11, 12, 26, 31, 42, 43, 44, 46 Mar-05

9 16, 19, 23, 30, 39, 41, 42, 51, 52, 54 Mar-12

10 11,13,19, 23,33,37,40, 43,49,53,59,63 Mar-19

11 13, 15, 23, 29, 31, 37, 39, 43, 49, 53, 57, 63, 69 Mar-26

12 1, 3, 7 ,9, 11, 13, 29, 31, 33 Apr-02

13 3, 5, 9, 11, 15, 19, 29, 31, 35, 37, 41, 45 Apr-09

14 7, 9, 11, 15, 19, 21, 23, 25, 37, 41, 43, 45, 51, 53 Apr-16

16 14, 16, 22, 28, 34, 41 Apr-23

17 1, 3, 5, 7 don’t turn in

______________________________________________________________________________

Spring 2003 Tutorial Room

Place: Chem Annex Room 50 Days: Tuesday, Wednesday, Thursday Hours: 12 Noon to 2:00 PM


Reading

• OFB Chapter 1• Appendices A, B, and C• Read, Read, Read• Work Problems, Work

Problems, Work Problems


Chapter 1The Atomic Nature of Matter

• 1-1 Chemistry: Science of Change• 1-2 The Composition of Matter• 1-3 The Atomic Theory of Matter• 1-4 Chemical Formulas and Relative

Atomic Masses• 1-5 The Building Blocks of the

Atom• 1-6 Finding Atomic Masses the

Modern Way• 1-7 The Mole Concept: Counting

and Weighing Atoms and Molecules• 1-8 Finding Empirical and

Molecular Formulas the Modern Way

• 1-9 Volume and Density


Definitions• Analysis (Take things apart)• Synthesis (Put things together)• Physical Properties (Color, odor, taste,

boiling point, etc.)• Chemical properties (with respect to

other materials, e.g., uniformity)• Substance (refer to elements and

compounds, never mixtures)• Elements (cannot be decomposed into

simpler substances)• Compounds (contain two or more

elements bonded together, e.g., NaCl)• Molecule (a few atoms connected together,

e.g., CO2)• Mixtures (can be separated into two or

more substances)• Homogenous (uniform throughout,

solutions)• Heterogeneous (properties vary from

region to region)• Phase (liquid, gas, solid)


Examples• Table Salt

– Heterogeneous (mixture of NaCl and small amounts of other substances)

• Wood– Heterogeneous (mixture of tree cells, and thousands

of other substances)• Mercury

– A substance and an element• Air

– Homogenous mixture of gases– Also a Heterogeneous mixture of gases and dust

• Water– A substance that is a compound with molecular

formula H2O• What is an example of a homogenous sample that

would gradually become heterogeneous if left to itself?– E.g., A solution of sugar in water– 1st Homogeneous– 2nd allow evaporation to start, becomes

heterogeneous– 3rd, complete evaporation, becomes homogeneous


Atomic Theory of Matter• Law of conservation of mass:

Mass is neither created nor destroyed in a chemical reaction

• Dalton’s Atomic Theory of Matter (1808):

1. All matter consists of solid and indivisible atoms

2. All atoms of a given chemical element are identical in mass and in all other properties

3. Different elements have different kinds of atoms; these atoms differ in mass from element to element

4. Atoms are indestructible and retain their identity in all chemical reactions

5. The formation of a compound from its elements occurs through the combination of atoms of unlike elements in small whole-number ratio.


Chemical Formulas and Relative Atomic Masses

• Chemical Formulas display symbols for the elements and the relative number of atoms– E.g., NH3, CO2, CH3CO2H or

C2H4O2

• Molecules are groupings of two or more atoms bound closely together by strong forces that maintain them in a persistent combination


Exercise 1-1 • Problem: Every 100.00 g of

the compound SiH4 contains 87.45 g of Si and 12.55 g of H. Find the ratio of the atomic mass of S to the atomic mass of H.

• Strategy: 1. Take the ratio of S/H2. Account for the 1:4 ratio of S:H


Exercise 1-1• Problem: Every 100.00 g of the

compound SiH4 contains 87.45 g of Si and 12.55 g of H. Find the ratio of the atomic mass of S to the atomic mass of H

• Solution:


Building Blocks of the Atom

• Electrons, Protons and Neutrons– Electrons discovered in 1897 by

Thomson– Rutherford proposed that the

atomic nucleus was composed of neutral particles called Neutrons and positively charged particles called protons

– Neutron number = N– Atomic number = Z = number of

Protons– Atomic mass number = A

A = Z + N


1530.794

PPhosphorus

1428.086

SiSilicon

714.007

NNitrogen

612.011

CCarbon


612.011

CCarbon

Atomic NumberAtomic

Mass

A = Z + N

Atomic Mass = # Protons + # Neutrons

For Carbon, 12 = 6 + Neutrons

Neutrons = 6

Every Carbon atom has 6 electrons, 6 protons and 6 neutrons


Mass Spectrometry and Isotopes

• Mass Spectrometeraccelerates ions (or molecular ions) in an electric field and then separates those ions by relative mass in a magnetic field

Mass Spectrometer Separation of Chlorine

020406080

100

35 37

Relative Mass

Rel

ativ

e A

mou

nt

17

35.453

ClChlorine


Atoms• Avogadro’s Number is the

number of 12C atoms in exactly 12 grams of carbon

• N0 = 6.0221420 X 1023

• The mass, in grams, of Avogadro's number of atoms of an element is numerically equal to the relative atomic mass of that element


• Relative Molecular Mass of a molecule equals the sum of the relative atomic masses of all of the atoms making up the molecule

Molecules


Moles• A mole measures the chemical amount of a

substance• Mole is an abbreviation of gram molecular

weight• One mole of a substance equals the

amount that contains Avogadro's number of atoms, molecules.

• One mole = Molar mass (M) of that element or molecule


Exercise 1-6

• Molecules of isoamyl acetate have the formula C7H14O2. Calculate (a) how many moles and (b) how many molecules are present in 0.250g of isoamyl acetate.

• Strategy:1. Calculate molar mass of C7H14O2

2. Calculate the number of moles in 0.250 grams

3. Using Avogadro’s number to calculate the number of molecules in X moles of C7H14O2


Exercise 1-6• Molecules of isoamyl acetate have

the formula C7H14O2. Calculate (a) how many moles and (b) how many molecules are present in 0.250g of isoamyl acetate.

• Solution:1. Calculate molar mass of C7H14O2

2. Calculate the number of moles in 0.250 grams

3. Using Avogadro’s number calculate the number of molecules in X moles of C7H14O2


Percentage Composition from Empirical or Molecular Formula

Exercise 1-8

• Tetrodotoxin, a potent poison found in the ovaries and liver of the globefish, has the empirical formula C11H17N3O8. Calculate the mass percentages of the four element in this compound.

Strategy:1. Calculate molar mass of C11H17N3O,

by finding the mass contributed by each element

2. Divide the mass for each element by the total mass of the compound.


Exercise 1-8

• Tetrodotoxin has the empirical formula C11H17N3O8. Calculate the mass percentages of the four element in this compound.

Solution:1. Calculate molar mass of

C11H17N3O, by finding the mass contributed by each element

2. Divide the mass for each element by the total mass of the compound.


Finding an Empirical FormulaExercise 1-9

• Heating a 150.0mg dose of a compound used to treat rheumatism decomposes it to its constituent elements, which are separated. There are 60.29 mg of gold, 21.10 mg of sodium, 29.37 mg of oxygen, and 39.24 mg of sulfur. Determine the empirical formula of this compound.

• Strategy:1. Calculate the chemical amount (in

moles) of each element in the sample using the table of atomic masses.

2. Find the ratios of the moles for each element by dividing each by the smallest one, i.e., normalize to the smallest.

3. If necessary, multiply smallest factor that clears any fractions that they contain.


Exercise 1-9• Heating a 150.0mg dose of a compound used to treat

rheumatism decomposes it to its constituent elements, which are separated. There are 60.29 mg of gold, 21.10 mg of sodium, 29.37 mg of oxygen, and 39.24 mg of sulfur. Determine the empirical formula of this compound.

Solution:1. Calculate the chemical amount (in moles) of each

element in the sample using the table of atomic masses.




Exercise 1-9Determine the empirical formula of this compound.

Solution:1. Calculate the chemical amount (in moles) of each element

in the sample using the table of atomic masses.




Exercise 1-10• Moderate Heating of 97.44 mg of a

compound containing nickel, carbon and oxygen and no other elements drives off all of the carbon and oxygen in the form of carbon monoxide (CO) and leaves 33.50 mg of metallic nickel behind. Determine the empirical formula of the compound.

Strategy:1. Write the reaction2. Use the conservation of mass to

find the amount of CO3. Find the number of moles of CO

and Nickel4. Find the ratios of the moles for

each substance by dividing each by the smallest one, i.e., normalize to the smallest.


Exercise 1-10• Moderate Heating of 97.44 mg of a compound

containing nickel, carbon and oxygen and no other elements drives off all of the carbon and oxygen in the form of carbon monoxide (CO) and leaves 33.50 mg of metallic nickel behind. Determine the empirical formula of the compound.

Solution:1. Write the reaction

2. Use the law of conservation of mass to find the amount of CO

3. Find the number of moles of CO and Nickel

4. Find the ratios of the moles for each substance by dividing each by the smallest one, i.e., normalize to the smallest.


Exercise 1-10• Moderate Heating of 97.44 mg of a compound containing

nickel, carbon and oxygen and no other elements drives off all of the carbon and oxygen in the form of carbon monoxide (CO) and leaves 33.50 mg of metallic nickel behind. Determine the empirical formula of the compound.

Solution:1. Write the reaction

2. Use the law of conservation of mass to find the amount of CO

3. Find the number of moles of CO and Nickel



Combustion AnalysisExercise 1-11

• A sample of a liquid hydrocarbon weighing 142.70 mg is burned in a combustion train to give 477.0 mg of carbon dioxide, 111.60 mg of water and no other products. What is the empirical formula of this hydrocarbon?

Strategy:1. Calculate the chemical amount (in

moles) of carbon dioxide and water using the table of atomic masses.




Exercise 1-11

• A sample of a liquid hydrocarbon weighing 142.70 mg is burned in a combustion train to give 477.0 mg of carbon dioxide, 111.60 mg of water and no other products. What is the empirical formula of this hydrocarbon?

Solution:1. Calculate the chemical amount (in moles) of

carbon dioxide and water using the table of atomic masses.




Exercise 1-11Solution:

1. Calculate the chemical amount (in moles) of carbon dioxide and water using the table of atomic masses.




Volume and DensityExercise 1-13

• The density of liquid mercury at 20 deg C is 13.594 g cm-3. A chemical reaction requires 0.560 mol of mercury. What volume (in cubic centimeters) of mercury should be measured out at 20°C?

Strategy:1. Use density and mass to find

volume. Rearrange

2. Density is given, can find mass from the number of moles of mercury which is given

3. Solve for volume.

Vmd =

dmV =


Exercise 1-13• The density of liquid mercury at 20 deg C is

13.594 g cm-3. A chemical reaction requires 0.560 mol of mercury. What volume (in cubic centimeters) of mercury should be measured out at 20°C?

Solution:1. Use density and mass to find volume.

2. Density is given, can find mass from the number of moles of mercury which is given

3. Solve for volume.

dmV =


Chapter 1The Atomic Nature of Matter

Examples / Exercises– All (1-1 thru 1-13)

Problems– 9, 10, 11, 17, 19, 20, 29, 37, 38,

55, 68

ofb chapter 1 lecture notes - georgia institute of...

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