2014-2015 Chemistry Syllabus 2014-2015 Regents Chemistry - SCN11 2014-2015 Chemistry Laboratory - SCN11QL Angela Sterling, Instructor Email Contact: asterling@erhsnyc.net Dear Students and Families, Welcome to our Chemistry curriculum. Chemistry is an opportunity to probe a world that is both unseen and mysterious. The atoms which join together in infinite combinations, the energy which journeys 92 million miles from the sun, and basically everything you will eat, touch or breathe in today is a part of chemistry. This year even the simplest things like water will never be viewed as simple again. You will understand both the beauty and terror of an atom split apart and why nature favors disorder! Our curriculum is enriched and thus goes beyond the textbook. There are worlds between what we call a solid and liquid, as there are subatomic particles composed of sub-sub atomic particles! Where it all began or ends is the eternal question, but you will enjoy exploring the possibilities! You will learn to observe, inquire, and perform experiments to reinforce your understanding. Extra help will always be available. I look forward to a wonderful year together. Angela Sterling
A. Essential Questions for Chemistry/Physical Environment How are energy and matter related? How does matter interact to form different phases? Why do systems trend towards lower energy and increased randomness? How can our knowledge of atomic structure help us predict chemical reactions? B. Chemistry Course Objectives To use scientific inquiry, mathematical analysis, and deductive and inductive reasoning to ask questions, seek answers, and develop solutions. To develop an understanding of the components of matter and how the interaction of these components forms everything in our universe. To explain how matter and energy are interrelated and interact through forces that result in motion. To comprehend the changes that can occur in the nucleus of an atom and the implications of this phenomenon. C. Resources and Materials Notebook 2 or 3 ring binder with section tabs in the following sequence: o Section 1 = Class notes o Section 2 = Class handouts o Section 3 = Homework o Section 4 = Vocabulary A TI-83 (or higher) calculator should be with you each day Chemistry Reference Table Hi-lighter marker and ruler Textbook: LeMay, Eugene. Chemistry - Connections to Our Changing World. Prentice Hall : New Jersey 2002 Review Book: Kavanah, Patrick. Chemistry: The Physical Setting. Prentice Hall : New Jersey 2011 D. Grading Policy Examinations 55% Laboratory Reports 25% Homework 10% Class Participation 5% Lab Participation 5% Page 2 of 13
E. Academic Integrity All students are expected to arrive to class on time and be prepared to discuss and answer questions based upon the prior day's material. In addition, students must complete their work in compliance with ELRO's policy of academic integrity. All written work must be in the student's own words. Plagiarism is a serious offense and will be reported. F. Class Schedule Section 4 Day of the Week Period Room Number Monday 3 and 4 417 Lab Tuesday 3 403 Wednesday 3 403 Thursday 3 403 Friday 3 403 Class Schedule Section 5 Day of the Week Period Room Number Monday 8 and 9 417 Lab Tuesday 9 403 Wednesday 9 403 Thursday 9 403 Friday 9 403 G. Extra Help Schedule Extra help is available on Monday and Tuesday at 7:45 in 403. H. Laboratory A double period laboratory is given each week. An in depth lab report is required to be handed in one week later at the next lab session. Late labs will be deducted one grade level per day they are late. A minimum of 13 labs are mandatory for the New York State Regents. Page 3 of 13
Chemistry Lab Report Format All laboratory reports must adhere to the following format: 1. Heading Your full name Lab # and name of lab Date Ms. Sterling 2. Introduction Clearly state the topic/question/problem that the lab is addressing. Explain why we did the lab. Include the name of the lab and its number. Make sure you are clearly explaining the main idea of this lab! Our labs are designed to reinforce concepts from class lectures. You must summarize (in your own words) what you have learned in class that applies to the lab. 3. Hypothesis State a hypothesis and identify the independent variable, dependent variable, and control. 4. Materials List all of the chemicals used in the lab, name and formula. List all of the equipment used in the lab. 5. Procedure Explain basically what you did during the lab. Do not copy the procedure. Identify any safety procedures used. Discuss any problems you encountered and how the outcome of your results may have been affected. 6. Data Collection Show all data collected in a labeled data table. Make certain that you use proper units. 7. Data Analysis This shows any calculations the lab required. If a graph is required be certain that the independent and dependent variables are represented on the proper axes. In addition, explain what your data says! You must show your math when appropriate!! All graphs must be hand drawn (very neatly) and not computer generated. Page 4 of 13
8. Conclusion Does the data support or refute your hypothesis? State a final conclusion from the data. Include any sources of error. Explain how you could have improved your experiment. 9. Cover Page Provide a neat and appropriate cover page. The cover page should have the title of the lab and a picture that reflects the theme of the lab. 10. Laboratory Safety You will perform a safety lab to advise you about safe laboratory practices. You and your parent/guardian will sign a laboratory safety contract. Any behavior that proves to be a safety issue will be reported to the principal. Page 5 of 13
I. Chemistry Course Outline Term 1 Unit 1 Nature of Science - Dimensional analysis [1 week] What are the units of measurement used in chemistry? How do we define SI base units for time, length, mass and temperature? How do we express numbers in scientific notation? How do we define and compare accuracy and precision? How do we use significant figures and rounding to reflect the certainty of our data? How can percent error describe the accuracy of experimental data? Unit 2 Matter, Chemical and Physical Changes [2 weeks] How do we compare/contrast elements, compounds, substances, and mixtures? How do we distinguish between physical and chemical properties? How do we differentiate the physical states of matter? How do we apply the law of conservation of mass to chemical reactions? How do we classify mixtures as homogeneous or heterogeneous? Explain how all compounds obey the laws of definite and multiple proportions. Unit 3 Gases, Liquids and Solids [2 weeks] How do we distinguish the different states of matter: solid, liquid and gases? What does standard temperature and pressure (STP) mean? What are melting, boiling, and freezing points? What phase changes occur in a heating curve? What phase changes occur in a cooling curve? How do we determine the heat of fusion and vaporization? What is happening at the molecular level when a substance is at its heat of fusion/vaporization? What is sublimation? How does the kinetic molecular theory describe the behavior of gases? Page 6 of 13
Unit 4 Atomic Structure [2 weeks] How do we compare the Dalton, Thomson, and Rutherford models of the atom? Describe the placement of protons, neutrons, and electrons according to the nuclear model of the atom. How do we describe and apply the terms atomic number, mass number and isotope? How do we calculate the atomic mass of an element? What is an isotope? How do we define and apply the terms molecule, ion, monoatomic and polyatomic? Describe the Bohr model and its relationship to atomic spectra. How do we describe the modern wave-mechanical model and its relationship to electron configuration? How do we apply the terms principal energy level, sublevel, orbital, ground state, excited state, spin state and valence electron? How do we create Lewis Structures? Unit 5 Chemical Bonding [2 weeks] Explain how energy/stability is related to chemical bonds. How do we compare/contrast ionic and covalent bonding? How do we draw Lewis structures for simple ions and covalently bonded molecules? What is the difference between polar and nonpolar covalent bonding? How can we predict whether a bond will be ionic or covalent? What is a dipole? What is a hydrogen bond? How do we compare/contrast metallic, ionic, and covalent bonds? How is the polarity of a molecule related to its symmetry? What are intermolecular forces and what are the different types? Page 7 of 13
Unit 6 Nomenclature [2 weeks] How do we distinguish between a structural, molecular, and empirical formula? How do we write formulas using the IUPAC system? What is an oxidation number? How do we assign oxidation numbers to elements, simple ions and elements in compounds? How do we write chemical equations using names and chemical formulas? How do we balance equations? When do we classify a chemical reaction as a synthesis, decomposition, single replacement or double replacement? Unit 7 Periodic trends [2 weeks] What is the periodic law of Moseley? Describe the arrangement of elements in the Periodic table in terms of electron configuration. How do properties of metallic elements differ from non-metallic elements? What is a metalloid? What is the difference between an ionic radius and an atomic radius? How do the following behave in terms of groups and periods: metallic character, atomic radius, ionization energy, electron affinity, ionic radius and electronegativity? How do the properties of the transition elements compare with those of the representative elements? What is ionization energy? What is electronegativity? Page 8 of 13
Unit 8 Chemical Reactions [2 weeks] Define the terms systems and surroundings as they relate to chemical processes. What is internal energy? What is heat? Distinguish between endothermic and exothermic reactions. How do we define specific heat? How does the first law of thermodynamics relate to the law of conservation of energy? How do we use heat of reaction to solve problems related to standard heat of formation? How do we interpret a potential energy diagram? What is activation energy? Name and describe the factors involved in spontaneous reactions. Define entropy and predict whether a given reaction leads to an increase or decrease in entropy. Page 9 of 13
Term 2 Unit 9 Chemical Mathematics [2 weeks] How do we differentiate between atomic mass unit, isotopic mass and atomic mass? How do we calculate the formula mass of a substance? How do we define the term mole in relation to the number of particles and the mass of the substance? What is molar mass? How do we calculate molar mass? How do we calculate the molecular formula of a substance given its empirical formula and molar mass? How do we calculate the empirical formula of a substance from its percent composition by mass? How do we solve mole and mass problems involving chemical equations? Unit 10 Thermodynamics [2 weeks] How do we distinguish between potential and kinetic energy? How do we calculate the amount of heat absorbed or released by a substance as its temperature changes? Describe how a calorimeter is used to measure energy released or absorbed. What is enthalpy and how does it relate to chemical processes? Describe how energy is lost or gained during changes of state. How do we calculate the heat gained/released in a reaction? How does one calculate enthalpy changes during a reaction? Differentiate between spontaneous and non-spontaneous processes. Unit 11 Kinetics/Equilibrium [2 weeks] Define the term chemical kinetics. What factors affect the rate of a reaction? What is dynamic equilibrium? Provide examples of phase and solution equilibria. What is chemical equilibrium? What is Le Chatelier s principle? How do we use Le Chatelier s principle to determine the effects of changes in concentration, volume, temperature, catalysts, and the addition of an inert gas? How do we write equilibrium-constant expressions for a homogeneous/heterogeneous reaction? How do we describe the effect of temperature on the equilibrium constant? Page 10 of 13
Unit 12 Solutions [2 weeks] How do we define solution, solute and solvent? What is a miscible, saturated, unsaturated or supersaturated solution? What factors affect the solubility of a solution? What are the solubility rules? How do we use the solubility rules to predict solubility? How do we interpret a solubility curve? Define the term electrolyte. How does the solute affect the freezing/boiling point of a solution? Unit 13 Oxidation-Reduction [2 weeks] How do we compare/contrast oxidation and reduction? What is a redox reaction? How do you write oxidation/reduction reactions for redox equations? When will a redox reaction occur spontaneously? What is a voltaic cell? What is a salt bridge? Describe electron movement in a voltaic cell. Define the term standard electrode potential. How do we calculate the potential difference of a voltaic cell? What is electrolysis and how do you draw a simple electrolytic cell? What is the basic concept behind electroplating? How can you describe the electrolysis of fused salts? Unit 14 Nuclear Chemistry [2 weeks] What are the common nuclear particles and their symbols? What is a nuclide? What is the process of transmutation? Describe the process of radioactive decay. What are the various types of radioactive decay? Define the term half-life. How are radioactive isotopes used? What happens during nuclear fission? Describe the four fundamental forces in the universe. Page 11 of 13
Unit 15 Acids and Bases [2 weeks] What is an acid/base? What is the Arrhenius definition of an acid/base? How do we solve acid-base titration problems? What is the Bronsted-Lowry definition of an acid/base? What is a conjugate acid-base pair? Define the terms PH and POH. What are the properties of acid/base indicators? What is a Lewis acid/base? Unit 16 Organic Chemistry [2 weeks] What is the difference between an organic and inorganic substance? Describe the bonding of carbon in simple organic compounds. What is a hydrocarbon? What is the difference between an alkene, alkane and alkyne? What is a functional group? What is a polymer? What are the following organic reactions: fermentation, esterification, saponification, combustion, addition, and substitution? Page 12 of 13
J. New York State Regents examination All students are required to take the New York State Living Environment Regents examination in June. The minimum passing grade is a 65%, but students are expected to strive for a mastery grade of 85% or higher. In January, the students are asked to purchase the Barrons Regents Review Book. In addition, the New York State Regents provides several online study aids such as: www.nysedregents.org www.nysl.nysed.gov/regentsexams www.regentsprep.org www.amazon.com/newyorkstateregents-exam www.chemthink.org www.dbchem.net/resource/review www.chemistry.about.com/ www.acs.org/portal/chemistry The following books can be purchased for extra help: Henrickson, Charles. Cliffs Study Solver. Wiley Publishing: New Jersey 2005. < www.cliffnotes.com > Moore, John T. Chemistry for Dummies. Wiley Publishing: New Jersey 2003. < www.dummies.com > Williams, Linda. Chemistry Demystified. McGraw Hill: New York 2003. < www.books.mcgraw-hill.com > Goldberg, David E. Schaum s Beginning Chemistry. McGraw Hill: New York 2005. < www.books.mcgraw-hill.com > Welcher, Sharon H. High Marks: Regents Chemistry. McGraw Hill : New York 2005. < www.highmarksinschool.com > Page 13 of 13