Syllabus Chemistry 101 Fall 2008 Sec. 501 (MWF 8:00-8:50) Sec 505 (MWF 12:40-1:30) RM 100 HELD Professor: Dr. Earle G. Stone Office: Room 123E Heldenfels (HELD) Telephone: (no voice mail) or leave a message at (put CHEM 101-Sec. # + subject in subject line of your ) Office Hours: HELD 123E: Tue. And Thur. 8:00-10:50 AM I.A. TBA S.I. Leader: TBA CHEM 101 and 102 are the first-year chemistry sequence in the core curriculum. These are 3-credit courses. All lecture sections strive to cover common content. The lecture component of Chemistry 101 covers stoichiometry, atomic and molecular structure, inorganic and organic nomenclature and structure, chemical bonding, fundamental acid/base chemistry, solution chemistry, properties of liquids and solids, and the gas laws. Additionally, it is the goal of my lecture section to help you develop the skill set to successfully complete your undergraduate degree and as most in this class are pre-something to prepare you for your professional school entrance exam.

All College498100% BIMS17635% Science12625% GEST6413% Ag BICH, NUSC, GENE286%20094 Engineering214%20081 Education306% Geosciences51% Liberal Arts102% Agriculture other255% 78% Science or Pre-something Architecture71% 22% This is a great way to learn how to survive college Business61% College249100%College249100% BIMS6024%BIMS11647% Science8032%Science4618% Ag BICH, NUSC, GENE2013%Ag BICH, NUSC, GENE83% GEST328%GEST3213% Engineering146%Engineering73% Education156%Education156% Geosciences21%Geosciences31% Liberal Arts52%Liberal Arts104% Agriculture other114%Agriculture other83% Architecture62%Architecture10% Business42%Business21%

Top Ten Most Repeated Comments 8a. Well organized notes with the problems available online. 8b. (Wish the material was available so I did not have to write down the problems.) 3. Tell us what to know and don’t expect us to figure it out on our own. Teach how to do the problems in class not just theory. Actually work through the problems, rather than say the rest is math. 5. I felt like I was seeing much of the material for the first time on the tests. The instructor should relate class to exams to encourage attendance. 9. His teaching methods make it easy to learn. 10. He needs to take a class in teaching. 1. But I did not have to study in High School. 6. The information covered did not pertain to my major as much as BIMS or others. 4. Used material from tests earlier in the semester on later exams. The Free Response was very random and not at all like the problems worked in class. The material in class was simpler than the material on the exam. 2. The instructor places too much responsibility on the student by not requiring homework which I feel would have helped me if I had done it promptly. Give a few quizzes to make sure we are doing the required work outside of class 7. Very good at concentrating on important material and concepts and explaining them, while spending little time on extraneous issues.

Tutoring Supplemental Instruction Courses Texas Success Initiative About Us Contact UsAbout UsContact Us 118 Hotard North of Sbisa, between Neeley Hall and the Northside Post Office (979) The Student Learning Center has won the 2008 National College Learning Center AssociationNational College Learning Center Association Frank L. Christ Outstanding Learning Center Award! The award recognizes the center's commitment to supporting and strengthening the Academic experience of students at Texas A&M University by providing a variety of programs and services that promote retention and success. Read more...Read more... The Student Learning Center provides Supplemental Instruction and tutoring free of charge to allSupplemental Instructiontutoring Texas A&M University students. The SLC oversees the STLC courses (formerly CAEN), which teachSTLC courses students how to improve their study skills and prepare for the job market. The SLC manages Developmental programs for students who have not yet passed the assessment tests required by the state.assessment tests Study Tips General Time Management Reading Textbooks Setting Goals Preparing for Exams Success Tips from Fellow AggiesSuccess Tips from Fellow Aggies Tutoring During the Fall 2008 semester, drop-in tutoring will be offered Sunday nights 5-8pm and Monday through Thursday nights from 5-10pm. Tutoring will begin on Monday, September 1st. Tutor Zones are currently planned for Studio 12 of The Commons. Look for our table and tutors and just ask for help! See the schedule... Drop-in tutoring is available for most lower level math and science courses on the first floor of Hotard Hall. Tutors are also available to help out with many other courses. If you need help in a particular course and would like to check to see if a tutor is available for that course, you can contact our tutor coordinator, Linda Callen, at See the schedule...

Suggested Course Materials: “Chemistry and Chemical Reactivity, Any Edition”, by Kotz, Treichel, and Weaver or Mastering the Fundamental Skills – General Chemistry I as a Second Language Helpful Dictionary of Chemistry Useful As A Second Language Organic Chemistry I (There is a O-chem II also for those who will have to take the class. Ebook includes Online tutorial Solution manual $45 per semester Hardbound ~$150 Solution Manual ~$40 Online Tutor ~$45

Week Date End of Chapter Questions 1 25-AugSyllabus Chapter 1–11,13,30,43,45,78,80 Chapters 1, 2, 9 27-Aug 1,2,3Chapter 2 – 1,27,29,57 Chapter 3 – 7, 8, 19, 21, 23, 27, 29, 31, 33, 39, 47, 51, 56, 61, Aug Sept 3,4 3-Sept 4Chapter 4 – 5, 6, 7, 17, 19, 23, 29, 41, 53, 83 5-Sept 3 8-Sept Exam #1 Chapters 1,2,3,4 10-Sept 7,8,9Chapter 7 – 49, 65, 69, 79 Chapter 8 – 1, 3, 5, 7, 17, 31, 39, 47, 71 Chapter 9 – 19, 23, 27, 29, 33, 43, 55, 95 Chapters 3,6 12-Sept 4 15-Sept 17-Sept 19-Sept 5 22-Sept 10Chapter 10 – 5, 7, 11, 13, 23, 29, 33, 51, Sept Exam #2 Chapters 7,8,9,10 26-Sept 11Chapter 11 – 5, 7, 12, 15, 19, 25 Klein Organic Chapters 5, 7; Traynham 6 29-Sept 1-Oct 3-Oct 7 6-Oct Chapter ,15, 17,19,21 8-Oct 10-Oct 8 13-Oct 5Chapter 5 – 3, 7, 11, 15, 19, 29, 31, 35, 37, 39, 41, 47, 49, 55, 57, 59, 61, 67, 69, 73, 83, 85, 103, 115, 125 Chapters 7,8; Organic 3,4 15-Oct 17-Oct 9 20-Oct 22-Oct 24-Oct Oct Exam # 3 Chapters 5,11,22 29-Oct 6Chapter 6 – 9, 27, 33, 39, 43, 45, 47, 51, 59, 61, 71, 79, 83, 89 Chapter 5 31-Oct 11 3-Nov 5-Nov 7-Nov Nov 13Chapter 13 – 1, 3, 7, 13, 19, 33, 35, Nov 14-Nov Nov 12Chapter , 5, 7, 9, 15, 19, 25, 31, 37, 59, 63, 75, 77, 81, 91, 99 Chapter 4 19-Nov 21-Nov Nov Exam # 4 Chapter 6,12,13 26-Nov Reading Day 28-Nov Thanksgiving Holiday 15 1-Dec Reading Day 2-Dec Reading Day 5-Dec Final morning Sec a.m. - Noon 16 8-Dec Final afternoon Sec :30AM-12:30 PM

Grading: Your grade will be based on Four one-hour examinations (each worth 200 points) A final examination (400 points) There are no bonuses, no extra credit, no soft points Major Examination Schedule Fall 2005: Mon. Sept. 8 Major Exam No.1 Wed. Sept. 24 Major Exam No.2 Mon. Oct. 27 Major Exam No.3 Mon. Nov. 24 Major Exam No. 4 Fri. Dec. 5 Section 501 Final Exam 10:00 to 12:00 Mon. Dec. 8 Section 505 Final Exam 10:30 to 12:30

A BCD,F,Q,W 46% 63% 80% 97% 29% 100% 90% 80% 70% 60% What you are used to The way the real world works +3% approximate points needed for letter grade 100%ABCD after Exam after Exam after Exam after Exam after Final

Problem - A situation that presents difficulty, uncertainty, or perplexity: The mere formulation of a problem is far more often essential than its solution, which may be merely a matter of mathematical or experimental skill. To raise new questions, new possibilities, to regard old problems from a new angle requires creative imagination and marks real advances in science. Albert Einstein Question - A request for data: inquiry, interrogation, query. Answer - A spoken or written reply, as to a question. Solution - Something worked out to explain, resolve, or provide a method for dealing with and settling a problem.

 (m) c (ms -1 ) E =  1.Numbers – Significant Figures, Rounding Rules, Accuracy, Precision, Statistical Treatment of the Data 2.Units – 5 of the 7 1.Time – seconds 2.Length – Meters Density? 3.Mass – grams Molecular Weight (Mass) 4.Amount – Moles Mole Ratio, Molarity, molality 5.Temperature – Kelvins 3.Vocabulary – Approximately 100 new terms or words and applying new or more rigid definitions to words you may already own. 4.Principles (Theories and Laws) – Stoichiometry, Quantum Theory, Bonding, Chemical Periodicity, Solutions, Thermodynamics, Intermolecular Forces, Gas Laws c p = q/m  Trate = k[A] m [B] n ∆E = q + w c p = q/m  Trate = k[A] m [B] n ∆E = q + w  G =  H – T  SE o cell = E cathode = E anode PV = nRT%yield = actual/theoretical * 100%K =  T = Kmi [C] c [D] d [A] a [D] b

Use of Numbers Exact numbersExact numbers – 1 dozen = 12 things for example AccuracyAccuracy –how closely measured values agree with the correct value PrecisionPrecision –how closely individual measurements agree with each other Significant Figures – start at the left and proceed to the rightSignificant Figures – start at the left and proceed to the right –If the number does not have a decimal point count until there are no more non zero numbers –If the number has a decimal point start counting at the first non-zero number and continue counting until you run out of decimal places Scientific notation – use it.Scientific notation – use it.

Use of Numbers Addition & Subtraction ruleAddition & Subtraction rule More subtle than the multiplication rule Answer contains smallest decimal place of the addends. When a 5 appears. Is there anything to the right of the 5 greater than zero? Is the number to the left of the 5 odd? Is the number to the left of the 5 even? (Treat 0 as even.) Multiplication & Division ruleMultiplication & Division rule Easier of the two rules Product has the smallest number of significant figures of multipliers

How many sig figs? How many sig figs in the answer? 472x x x / / /472x /475.0x0.30/ x Round off to two sig figs (1.68) [ ] – x 10 3 =

Scientific Method 1.Observation 2.Hypothesis 3.Experiment 4.Theory 5.Law

Matter and Energy - Vocabulary Chemistry – –Science that describes matter – its properties-composition-structure, the changes it undergoes, and the energy changes that accompany those processes Matter – –Anything that has mass and occupies space. Energy – –The capacity to do work or transfer heat. Chemical Properties - chemical changes – –rusting or oxidation – –chemical reactions Physical Properties - physical changes – –changes of state – –density, color, solubility Extensive Properties - depend on quantity Intensive Properties - do not depend on quantity Scientific (natural) law – –A general statement based the observed behavior of matter to which no exceptions are known.

Natural Laws Law of Conservation of Mass – The notion that mass, or matter, can be neither created nor destroyed.Law of Conservation of Mass – The notion that mass, or matter, can be neither created nor destroyed. Law of Conservation of Energy – A law that states that in any system not involving nuclear reactions or velocities approaching the velocity of light, energy cannot be created or destroyed. The First Law of Thermodynamics.Law of Conservation of Energy – A law that states that in any system not involving nuclear reactions or velocities approaching the velocity of light, energy cannot be created or destroyed. The First Law of Thermodynamics. Law of Conservation of Mass – Energy - Einstein’s Relativity - E=mc 2 – The special theory of relativity, which has been verified by experiment, has shown that the mass of a body changes as the energy possessed by the body changes. Such changes in mass are too small to be detected except in subatomic phenomena. Matter may be created by the materialization of a photon into an electron-positron pair; or it may be destroyed, by the annihilation of this pair of elementary particles to produce a pair of photons.Law of Conservation of Mass – Energy - Einstein’s Relativity - E=mc 2 – The special theory of relativity, which has been verified by experiment, has shown that the mass of a body changes as the energy possessed by the body changes. Such changes in mass are too small to be detected except in subatomic phenomena. Matter may be created by the materialization of a photon into an electron-positron pair; or it may be destroyed, by the annihilation of this pair of elementary particles to produce a pair of photons. Law of Definite Proportions – When two or more elements combine to form a compound, their masses in that compound are in a fixed and definite ratio. This data helps justify an atomic view of matter.Law of Definite Proportions – When two or more elements combine to form a compound, their masses in that compound are in a fixed and definite ratio. This data helps justify an atomic view of matter. Law of Multiple Proportions – When two elements combine to form more than one compound, the mass of element A which combines in the first compound with a given amount of element B has a simple whole number ratio with the mass of element A which combines in the second compound with the same given mass of element B.Law of Multiple Proportions – When two elements combine to form more than one compound, the mass of element A which combines in the first compound with a given amount of element B has a simple whole number ratio with the mass of element A which combines in the second compound with the same given mass of element B.

Dr. Stone’s patent pending chemistry problem solver 1.Write down everything you are given VocabularyVocabulary NumbersNumbers UnitsUnits 2.Write down what you want to know VocabularyVocabulary NumbersNumbers UnitsUnits 3.Write down mathematical equation(s) that include(s) these values and units Principles Principles 4.Write a balanced stoichiometric equation Mole conceptMole concept 5.Convert everything to moles Dimensional analysisDimensional analysis 6.Convert everything to the unknown’s units Rounding, significant figures, accuracy and precisionRounding, significant figures, accuracy and precision

Compounds & Molecules COMPOUNDS are a combination of 2 or more elements in definite ratios by mass.COMPOUNDS are a combination of 2 or more elements in definite ratios by mass. The character of each element is lost when forming a compound.The character of each element is lost when forming a compound. MOLECULES are the smallest unit of a compound that retains the characteristics of the compound.MOLECULES are the smallest unit of a compound that retains the characteristics of the compound. Composition of molecules is given by a CHEMICAL FORMULA CHEMICAL FORMULA C 8 H 10 N 4 O 2 - caffeine H2OH2OH2OH2O

MOLECULAR FORMULAS Formula for glycine is C 2 H 5 NO 2Formula for glycine is C 2 H 5 NO 2 In one molecule there areIn one molecule there are –2 C atoms –5 H atoms –1 N atom –2 O atoms

WRITING FORMULAS Can write glycine chemical formula asCan write glycine chemical formula as –H 2 NCH 2 COOH to show atom ordering to show atom ordering or in the bond-line structural formulaor in the bond-line structural formula Chemical Formula – chemical symbols and number of each representing composition Empirical Formula – simplest ratio of elements that does not represent the actual number and is non-positional number and is non-positional Molecular Formula – chemical symbols and number of each representing composition representing actual number but not position composition representing actual number but not position Structural Formula - chemical symbols and number of each representing composition representing actual number and position composition representing actual number and position

MOLECULAR MODELING Ball & stick Space-filling Bond-line Structural formula of glycine

STRUCTURAL FORMULA BOND-LINE FORMULA

IONS are atoms or groups of atoms with a positive or negative charge. Taking away an electron from an atom gives a CATION with a positive charge Adding an electron to an atom gives an ANION with a negative charge. PREDICTING ION CHARGES In general metals (Mg) lose electrons ---> cationsmetals (Mg) lose electrons ---> cations nonmetals (F) gain electrons ---> anionsnonmetals (F) gain electrons ---> anions Charges on Common Ions CATION + ANION → COMPOUND A neutral compound requires equal number of + and - charges. A neutral compound requires equal number of + and - charges.

MonovalentDivalentTrivalent HydroniumH3O+H3O+ MagnesiumMg 2+ AluminiumAl 3+ (or hydrogen)H+H+ CalciumCa 2+ Antimony IIISb 3+ LithiumLi + StrontiumSr 2+ Bismuth IIIBi 3+ SodiumNa + BerylliumBe 2+ PotassiumK+K+ Manganese IIMn 2+ RubidiumRb + BariumBa 2+ CesiumCs + ZincZn 2+ FranciumFr + CadmiumCd 2+ SilverAg + Nickel IINi 2+ AmmoniumNH 4 + Palladium IIPd 2+ ThaliumTl + Platinum IIPt 2+ Copper ICu + Copper IICu 2+ Mercury IIHg 2+ Mercury IHg 2 2+ Iron IIFe 2+ Iron IIIFe 3+ Cobalt IICo 2+ Cobalt IIICo 3+ Chromium IICr 2+ Chromium IIICr 3+ Lead IIPb 2+ Tin IISn 2+ Table of Common Ions Common Positive Ions (Cations)

MonovalentDivalentTrivalent HydrideH-H- OxideO 2- NitrideN 3- FluorideFl - PeroxideO 2 2- ChlorideCl - SulfideS 2- BromideBr - SelenideSe 2- IodideI-I- OxalateC 2 O 4 2- HydroxideOH - ChromateCrO 4 2- PermanganteMnO 4 - DichromateCr 2 O 7 2- CyanideCN - TungstateWO 4 2- ThiocynateSCN - MolybdateMoO 4 2- AcetateC2H3O2-C2H3O2- tetrathionateS 4 O 6 2- NitrateNO 3 - ThiosulfateS 2 O 3 2- BisulfiteHSO 3 - SulfiteSO 3 2- BisulfateHSO 4 - SulfateSO 4 2- BicarbonateHCO 3 - CarbonateCO 3 2- Dihydrogen phosphateH 2 PO 4 - Hydrogen phosphateHPO 4 2- PhosphatePO 4 3- NitriteNO 2 - AmideNH 2 - HypochloriteClO - ChloriteClO 2 - ChlorateClO 3 - PerchlorateClO 4 - Table of Common Ions Common Negative Ions (Anions)