1 Chemistry 1A Syllabus Winter 2018 Welcome to Chemistry 1A, the first semester of General chemistry. Dr Kime Office: MTSC building Welcome to Chemistry 1A. This course in the first half of the General Chemistry course offered at RCC. Course Schedule: Lecture: M-Th: 12:00 pm-2:15pm MTSC 437 Lab M-Th 2:30 pm- 7:05 pm MTSC 407 Required Textbooks: Required: Lecture: Chemistry, The Molecular Nature of Matter and Change. Silberberg-Amateis.(8 edition, older editions are okay).isbn Laboratory: Experiments in General Chemistry, by Amrich et.al. I will post the lab on the website so you don't have to purchase the lab manual. Periodic Table, Scientific Calculator with Exponential and Log functions (You may NOT use a programmable calculator or a cell phone.) You will need to bring a pencil, paper and calculator to class each day. If you are not willing to do the practice problems in class, I will tell you to leave class. f Objective: In general chemistry you are going to increase your knowledge and understanding of chemistry and math by doing many word problems, often requiring multi-step mathematical solutions. You will work on applying knowledge you have learned in different situations, this is to help you learn to reason logically. You will work alone in the laboratory, by doing so you will gain confidence in your laboratory abilities. You will learn more in this class if you stay involved by coming to class on time, paying attention and participating in class discussion and in-class work. Learning Outcomes Upon successful completion of the course, students should be able to: 1. Solve multi-step problems (using formulae and unit-analysis) relating to atoms and elements, chemical bonding and molecular geometry, chemical reactions and Stoichiometry, properties of the states of matter, phase changes and solutions. Analyze the nature of chemical bonding and reactions. 2. Collect and analyze data from chemical experiments, including graphing, calculations and qualitative understanding of how data relates to the concept studied. Compose standard operating procedures (SOPs) and/or papers in appropriate scientific format for these experiments. Design experiments that minimize sources of error for concepts studied in the course. Demonstrate laboratory safety protocols, including proper waste management.
2 3. Construct and manipulate equipment to secure reasonably accurate measurements. 4. Describe, analyze, and apply chemical concepts of atoms and elements, chemical bonding and molecular geometry, chemical reactions and stoichiometry, properties of the states of matter, phase changes and solutions. 5. Describe and apply a chemical vocabulary of approximately 500 words and apply the IUPAC system of chemical nomenclature. and Quizzes: is shown on the syllabus; I gave problems only for edition 8 of the textbook. The problems in the different editions are the about same so if you do the problems with answers in the back of the books shown under the heading assigned you should be fine. There will be a quiz some days and worksheets on others. If you are late to class you will not be able to make-up the quiz. Worksheets: There will be class worksheets that you can work on as a group; no text books can be used. These will be included in with your quiz grades Exams There will be 2-50 minute exams during the 6 weeks, each worth 100 points. NO EXAM GRADES WILL BE DROPPED. Exams are multiple choice, fill in, true/false and any other kind of questions I find interesting. On the last day of class there will be a comprehensive final exam worth 200 points. Schedule: The schedule on the syllabus may change. If the instructor feels that more time needs to be spent on a topic one or more of the worksheets may be dropped. Missed work: Missed quizzes and worksheets CANNOT BE MADE UP. If you miss an exam call me IMMEDIATELY, to schedule a make-up, if you call me after I have handed back the graded exam to the class you cannot make up the exam. If you miss more than 1 exam I suggest you drop the class because that exam cannot be made up. NOT MATTER WHAT THE CIRCUMSTANCES. Laboratory: Lab attendance is mandatory; there is no way to make up a lab so if you miss it you will not get credit no matter what the excuse. If you are more than 10 minutes late to lab without prior approval by the instructor you will not receive credit for lab. If you miss the instructions for the lab you may not do the lab. You are required to bring your lecture book to lab each day as we may use some of the time to go over topics from lecture and some homework maybe required. You will turn in a lab report or work sheet each day and this will account for 30% of your course grade. If you miss three labs you will be dropped from the course or if it is after the drop date you will receive an F grade in the lab. Cell phones: If you use your cell phones FOR ANY REASON during class, you will be asked to leave for the entire day. This includes lecture and laboratory. YOU MAY NOT USE A CELLPHONE CALCULATOR EVER, in this class. Grading: 55% exams 15% quizzes and worksheets, 30% lab A % B % C % D % F<55% You must receive 65% of possible lecture points and 65% of possible lab points to pass the class. You must pass both lecture and the laboratory portion of the course to earn a C grade Problems: The Riverside has a tutoring center, get help early. If you have a learning disability please call Disabled Student Services at Cheating equals 0 on the paper and a trip to the dean (not fun).
3 Schedule Week 1* *Schedules are subject to change. Monday 1/1 HOLIDAY Tuesday 1/2 Ch 1Physical vs Chemical Expt 1. properties, Extensive vs. Exploding intensive, Density, Percent, particles Dimensional Analysis 1:15-2:15 Ch. 2 Atoms, atomic theory, history of the atom, Law of multiple proportions, Law of conservation of matter, Atomic number, mass number, isotopes, mass spectrometry Ch. 1.2,4,6,11,13,15,19,20,21, 23, 24,26,30,34,38,40,44,46,54,58,60,62, 66,70,72,78 Ch , Wednesday 1/3 Expt. 3 Density Natural abundance, the mole, Elements vs. compounds. Allotropes, Review of the periodic table 1:15-2:15 Ch. 3 Carbon, diatoms, molecules and compounds, models, ions, chemical formulas. Moles, molar mass Ch. 2 39,41, 43,45, 47, 52, 56,58, Ch. 2. Ch3. 11,14,18, Thursday1/4 Expt. 4 Hydrates Quiz 1 Ionic bonds, formula units, electrolyte, Percent composition. Empirical formula, nomenclature 1:15-2:15 Empirical formula, molecular formulas, hydrates. Monday 1/8 Expt 5 Determination of formula of a compound Schedule Week 2 Ch. 3 Balancing chemical equations, mole ratio, stoichiometry Ch ,22, 24,26,63, 74, 76, 82, 120, Ch 3 20,29,30, Ch. 2 88,90, 92,98, 100,102,104,106,108,110, 124, 128 Ch.3 36,40,42,44,46, 48,51, Ch.3 58,60,62,67,69,71,75,77, 1:15-2:15 Limiting reagents, % yield. Ch ,83,87,89,95,97,117
4 Tuesday 1/9 Combustion analysis. Ch ,127,138,144 Expt 7 Stoichiometry 1:15-2:15 Ch. 4 solubility, precipitation reactions, Double replacement reactions Ch. 4-43,45,115, Wednesday 1/10 WORKSHEET 1 Expt 27, The 8 Acid base rxns, redox reactions, gas solution problem forming rxns. 1:15-2:15 Single replacement reactions, redox reactions, net ionic equations Ch. 8 (354)metal and nonmetal oxides Ch. 2 94, 95 Ch , 65,67, Ch. 4.,79,82,,84,88, 90,92, 94, 103, 105,107,109,111, 119, 131 Ch 8. 73, 74 Thursday 1/11 EXAM 1 Expt 13 the Acid content in food 1:15-2:15 Concentration and dilution of solutions. (titration in lab), solution stoichiometry, Schedule Week 3 Ch. 4-14,16,18,20,22,24, 26, 28, 33, 47,49,53, 63, 69, 71,96, Tuesday 1/16 MONDAY IS A HOLIDAY Ch. 5 Gas laws, combined gas law Ch. 5 6, 10,18,20,22, 26,28, 36, 41, Expt. 8 Molar volume 1:15-2:15 Ch. 5. Avogadro's Law (STP), Ideal Gas law, density, molar mass Ch. 5 47,49 Wednesday 1/17 Stoichiometry, Dalton s Law, Expt. 10 Antacid Non ideal gases analysis 1:15-2:15 Ch. 6. Thermodynamics, energy types, endothermic, exothermic, enthalpy, heat capacity, specific heat capacity, calorimetry Thursday 1/18 Ch. 5.51, 53, 55,64,84,89, 98, 99,145 Ch. 6-18,21,26, 35,37,39, 41,
5 Quiz 2: Expt. 18 Al analysis Calorimetry 1:15-2:15 Ch. 6 changes in state, enthalpy of formation or Direct method for finding enthalpy Schedule Week 4 Monday 1/22 Ch. 6. Hess s Law (Indirect method Expt 3 (II) for finding enthalpy) Specific heat 1:15-2:15 REVIEW DIRECT vs INDIRECT METHODS Ch. 6.43,45, Ch. 6 55, 57, 59,61, 65, , 86, Ch. 6 70, 72, 74, 105, 106 Tuesday 1/23 Ch. 7 Electromagnetic radiation, visible spectrum, Energy, line spectrum, Expt.11 Calorimetry 1:15-2:15 Ch. 7 De Broglie s equation, Uncertainty principle, Schrodinger, Quantum numbers Ch. 7 2, 5, 13,20, 23,27, 31,34, 78, 86, Ch. 7 37, 39, 41, 43, 48, Wednesday 1/24 Expt 12. Emission Spectrum Quantum numbers cont. orbitals Ch. 7 Ch. 8. electron configuration. Magnetism, Ch. 7 51,53,55, 57, 59,68, 72, 75, Ch (odd)75, 77, 81, 83,85,94, 101, 1:15-2:15 Worksheet 2 Thursday 1/25 Exam 2 Expt. 14 Beer s Law Electron dot structures 1:15-2:15 Ch 10 Lewis dot structures, Ch. 9 6, 10,14 Ch. 10 (Lewis structures) 3, 5, 7, 19, 21, 62
6 Monday 1/29 Expt. 15 VSEPR Schedule Week 5 Resonance structures, formal charges, Ch 9. Born Haber cycle, bond length, bond strength, lattice energy, metallic bonds. 1:15-2:15 VSEPR Ch. 10 geometric shapes, electronegativity, (Ch 9), polar vs nonpolar compounds Ch. 10 9, 11, 13, 15, 17,26, 75, Ch. 9 22,26,30,33,35,39, 45, 47, 49, 56, 58, 73, 75, 81 VSEPR Ch , 32, (odd) Ch ,55, 57,59,61, 64, 66, 72, 86, 92, 95 Ch (even) Tuesday 1/30 Valence bond theory Ch. 11 Valence bond theory Valence bond theory Ch.11. 1,3, 5, 7, 10, 13, 15, 20, 21, 23,38, 40, 42,44, 56 Expt 2 Paper Chromatography 1:15-2:15 Ch.8 Zeff, atomic radii, ion sizes, isoelectronic ions, Ionization energy, Ch. 8 46,50,53, 55, 57,59, 61, 62, 65, 87, 89,98, 100 Wednesday1/31 Ch 11: Molecular orbital Theory Ch , 28, 32, 34, 37 M.O. Theory 1:15-2:15 Ch 12 Intermolecular forces, vaporization, vapor pressure, boiling point, surface tension, Ch. 12 : 37, 39, 43, 45, 49, 51, 53, 55, 59, 63, Thursday 2/1 Expt 9 Flame test Quiz 3 Ch 12 capillary action, viscosity. adhesion vs cohesion 11:10-12:10 Ch. 12 Heat of fusion, heat of vaporization, Ch 12Phase diagrams Critical temperature and pressure. Triple point. Ch 12 65, 135 Ch 12 4,9,19, 21, 23,25, 27,28, 30
7 Schedule Week 6 Monday 2/5 Ch. 13 Solutions, Expt 21: Molarity, molality, mole fraction, Determination of weight percent molar mass 1:15-2:15 Ch. 13. Factors affecting solubility, Colligative properties. Raoult s law Tuesday 2/6 Boiling Point elevation, Freezing H.O. Thermal point depression, Osmosis degradation of mixed Dissacharides 1:15-2:15 WORKSHEET 3 Wednesday 2/7 Solid state chemistry H.O. Solid state Crystal structures 1:15-2:15 REVIEW WORKSHEET For COMPREHENSIVE FINAL Ch. 13 7,9,11,13, (even) 165 Ch , 44, 46, 49, Ch , 85, (even), 126, 132 Ch 12. Solid state chemistry. 86,88, 92, 96, 146 Thursday 2/8 12:05-2:15 Final Exam
8 Chemistry 1A Lab Schedule, Winter, 2018 Date Day Experiment 1/1 M HOLIDAY 1/2 Tu Lab Safety Expt. 1 Exploding Particles 1/3 W Lab Safety Expt. 3 (I) Density 1/4 Th Expt. 4. Characteristics of Hydrates 1/8 M Expt. 5 Determination of the Formula of a Compound 1/9 Tu Expt. 7 Stoichiometry 1/10 W Expt. 37 The Eight Solution Problem 1/11 Th Expt. 13 Acid Content in Foods 1/15 M HOLIDAY, 1/16 Tu Expt. 8 Molar Volume of Nitrogen 1/17 W Expt. 10 Antacid Analysis with HCl 1/18 Th Expt. 18 Chemistry of Aluminum 1/22 M Expt. 3 part II Specific Heat 1/23 Tu Expt. 11 Calorimetry 1/24 W Expt. 12 Emission Spectra and Atomic Structure 1/25 Th Expt. 14 Beer s Law, electron dot structures, resonance structures 1/29 M Expt. 15 VSEPR Theory, 1/30 Tu Valence Bond Theory handout, Expt. 2 TLC of analgesics 1/31 W Molecular Orbital theory handout. 2/1 Th Expt. 9 Flame tests 2/5 M Expt. 21 Determination of Molar Mass by Freezing Point Depression 2/6 Tu Partial Thermal Degradation of Mixed Disaccharides 2/7 W Checkout, Handout solid state 2/8 Th Course Final Exam