UConn ECE Chemistry 1127Q/1128Q Christian Heritage School Fall 2014/Spring 2015

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1 The heavens declare the glory of God; the skies proclaim the work of his hands. Day after day they pour forth speech; night after night they display knowledge. Psalm 19: 1-2 For since the creation of the world God s invisible qualities his eternal power and divine nature have been clearly seen, being understood from what has been made, so that men are without excuse Romans 1:20 Mrs. Roessler lroessler@kingsmen.org Phone: (203) x 576 Extra help is available during my free periods, when I am available, and from 2:30-3:00 on most school days. UConn ECE Chemistry 1127Q/1128Q Christian Heritage School Fall 2014/Spring 2015 Chemistry 1127Q Four credits. Recommended preparation for CHEM 1127Q; Basic Algebra with applications, or equivalent. Designed to provide a foundation for more advanced courses in chemistry. Atomic theory; laws and theories concerning the physical and chemical behavior of gases, liquids, solids, and solutions. Properties of some of the more familiar elements and their compounds. Quantitative measurements illustrating the laws of chemical combination in the first semester lab. Equilibrium in solutions and qualitative reactions of the common cations and anions in the second semester lab. Chemistry 1128Q Four credits. A continuation of CHEM 1127Q. MATERIALS: 1. Required text: Chemistry: Principles and Reactions, 7th Edition Masterton, Hurley, Neth ISBN-13: Scientific calculator GRADING: Your UConn course grade will calculated using the point system. Points Percent Distribution Exams I, II, III (150 points 450 points 45% each) Final Exam 250 points 25% Laboratory 150 points 15% Quiz/Homework 150 points 15% Total 1000 points 100%

2 Your CHS quarter grade will be based on a percentage system. Percent Exams 60% Homework/Quizzes 20% Laboratory 20% HOMEWORK: Problems from the text will be assigned based on UConn s problem sets. EXAMS: Each exam will be created by the professor(s) at UConn and need to be administered at least a week after it is given in Storrs. Exams are created to be completed in 90 minutes and they will be administered over the course of two days. QUIZZES: Quizzes for each problem set will be created by the professor(s) at UConn. Quizzes will be given approximately every other week. LABORATORY: Laboratory experiments will be conducted almost every week. Information from the laboratory experiments will be on each test as well as on the final. MAKE-UP WORK: If you have an excused absence, you are responsible for determining what took place during your absence. You will be given as many days as you were absent to make up any missed work. ACADEMIC DISHONESTY: Academic dishonesty on any assignment will result in a grade of zero. This includes plagiarism and cheating on exams, quizzes, homework, projects, and laboratories. Plagiarism includes not only presenting someone else s work from any source as your own, but also giving your work to someone else so that it can be presented as his/her own work. I encourage students to study together, exchange notes (which each have taken on their own during class) and discuss ideas presented in the lectures and texts. However, the final work you submit must be your own interpretation of the material based on your own work. Taking credit for someone else s work or submitting essays on material that you did not read, study, or think about is academically dishonest and constitutes plagiarism.

3 Course Outline Introduction: Matter and Measurement classification of matter properties of matter units of measurement uncertainty in measurement dimensional analysis Atoms, Molecules, and Ions atomic theory of matter discovery of atomic structure modern view of atomic structure atomic weights nomenclature of inorganic substances molecular and empirical formulas Stoichiometry: Calculations with Chemical Formulas and Equations balancing equations classifying reactions percent composition mole conversions quantitative information from balanced equations limiting and excess reactants and percent yield Aqueous Reactions and Solution Stoichiometry properties of aqueous solutions precipitation reactions acid-base reactions oxidation-reduction reactions solution concentration solution stoichiometry Gases kinetic molecular theory characteristics of gases the gas laws the ideal-gas law gas mixtures and partial pressure effusion and diffusion deviations from ideal behavior Electronic Structure of Atoms wave nature of light line spectra and the Bohr model wave behavior of matter quantum mechanics and atomic orbitals many-electron atoms electron configurations electron configurations and the periodic table

4 Periodic Properties of the Elements development of the periodic table effective nuclear charge periodic trends o atomic and ionic radii o ionization energy o electronegativity Basic Concepts of Chemical Bonding chemical bonds, Lewis structures, and the Octet Rule ionic Bonding covalent Bonding bond polarity and electronegativity resonance structures exceptions to the octet rule strengths of covalent bonds Molecular Geometry and Bonding Theories molecular shapes VSEPR theory molecular shape and molecular polarity hybrid orbitals multiple bonds Thermochemistry the nature of energy the First Law of Thermodynamics enthalpy and enthalpies of reaction Calorimetry Hess s law enthalpies of formation Intermolecular Forces, Liquids, and Solids intermolecular forces in solids, liquids, and gases properties of liquids phase changes vapor pressure phase diagrams structures of solids bonding in solids Properties of Solutions solution process solubility factors affecting solubility ways of expressing concentration colligative properties colloids

5 Chemical Kinetics reaction rate concentration and rate change of concentration with time temperature and rate reaction mechanisms catalysis Chemical Equilibrium equilibrium constant heterogeneous equilibria calculating equilibrium constants applications of equilibrium constants Le Chatelier s Principle Acid-Base Equilibria Bronsted-Lowry Acids and Bases autoionization of water the ph scale strong and weak acids and bases Ka and Kb Lewis acids and bases Additional Aspects of Aqueous Equilibria common-ion effect buffers acid-base titrations Ksp Precipitation and separation of ions Chemical Thermodynamics spontaneous processes entropy and the Second Law of Thermodynamics Gibbs Free Energy free energy and temperature and the equilibrium constant Electrochemistry oxidation states balancing redox reactions voltaic cells cell EMF under standard and nonstandard conditions Nuclear Chemistry radioactivity rates of radioactive decay fission and fusion