AP Chemistry Mrs. Hopkins Rm A200 Conference Period: 9:15am-10:11am Tutorials: Wed. 3:10-4:10pm Room A200

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1 AP Chemistry Mrs. Hopkins Rm A200 Conference Period: 9:15am-10:11am Tutorials: Wed. 3:10-4:10pm Room A200 Course Description Welcome to our AP Chemistry Class! I hope you will find this class rewarding, interesting, and fun. Please familiarize yourself with the class layout and expectations so you may have a successful experience in this class. Chemistry is the study of the world around you. In AP Chemistry, We will be studying matter, energy, atoms, chemical reactions, solutions, and more. In addition, we will spend time in the laboratory with emphasis on safety, scientific processes and developing critical thinking skills. Everything in the AP Chemistry class is geared to prepare the student for success on the AP Chemistry exam and for University level Chemistry. *Please note that there is a great deal of math involved. You will need a binder with dividers and writing utensils every day. Please come prepared. Be prepared to turn in assignments at the end of class each day. Grading Policy** **Please refer to the district AP/PAP contract for all Grading and Homework policies Grade Categories 40% - Major Exams/Major Projects 40 % - Labs/Lab Writeups 20 % - Daily Work/Class Work/Quizzes Cheating will never be tolerated on ANY assignment. Your parents will be contacted, both parties involved in cheating will receive a zero and the grade will not be allowed to be made up. If you need help on an assignment, ask for help. It is the job of the teacher to make sure that all students understand the lesson. SPEAK UP if you need help!!! Homework Any and all homework given will be meaningful to the work done in class. All students will be required to do their homework in Google Classroom. Their access will be set up on day 1. It will also be required that all students have access to remind.com either through a computer or on their phone via the remind app. **Late work will be per District Grading Policy. Textbooks will not be passed out by the teacher, but it is HIGHLY RECOMMENDED if you do NOT have access to a computer or device that you check out a book from the textbook office. There will be a classroom set of books to use during class, but these books may not leave the classroom! The textbook is an excellent resource for students that may struggle or need extra reinforcement. Instructions will also be passed out that will allow you to access the textbook online. Tests Regular formative assessments will be given to check for student understanding. I anticipate that the assessments will be at least weekly, if not 2-3 times per week. These formative

2 assessments will allow me to more accurately determine where the student is academically in my class. These smaller assessments will lead up to Unit, Semester, and Final exams; Exams will be at least every unit. Each unit will therefore have a minimum of 2 exam grades each: the multiple choice exam and the free response exam (FRQ). Make-Up Policy If you are absent, I have an area at the front of the room (organized by period) that has work from the week that you may pick up. This is YOUR responsibility. It is also your responsibility to turn the make-up work in to me by the deadline in accordance with the student handbook. Cell Phone/Device Policy There are no cell phones/devices allowed in class. They are a distraction and student grades go down because of them. During class time, you may connect your phone to your own charger and charge your phone/device if you would like to charge your phone. Please understand that if I see you on your phone, I will take the phone up immediately. We do not have much time to cover the amount of material in class that we need to cover. Classroom Discipline Students are to adhere to the Social Contract that we will develop on Days 1 and 2. Any deviation from the contract will result in: Warning #1: Name written on the board Warning #2: Mark after the name on the board Warning #3: Mark after the name and a Teacher Detention/Call home (30 min detention on a scheduled date) Warning #4: Another mark after the name and Office referral/call home SCOPE OF THE AP CHEMISTRY CLASS I. Structure of Matter (20%) A. Atomic theory and atomic structure 1. Evidence for the atomic theory 2. Atomic masses; determination by chemical and physical means 3. Atomic number and mass number; isotopes 4. Electron energy levels: atomic spectra, quantum numbers, atomic orbitals 5. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states B. Chemical bonding 1. Binding forces a. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces) b. Relationships to states, structure, and properties of matter c. Polarity of bonds, electronegativities 2. Molecular models a. Lewis structures

3 b. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds c. VSEPR 3. Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes; dipole moments of molecules; relation of properties to structure II. States of Matter (20%) A. Gases 1. Laws of ideal gases a. Equation of state for an ideal gas b. Partial pressures 2. Kinetic molecular theory a. Interpretation of ideal gas laws on the basis of this theory b. Avogadro s hypothesis and the mole concept c. Dependence of kinetic energy of molecules on temperature d. Deviations from ideal gas laws B. Liquids and solids 1. Liquids and solids from the kinetic-molecular viewpoint 2. Phase diagrams of one-component systems 3. Changes of state, including critical points and triple points 4. Structure of solids; lattice energies C. Solutions 1. Types of solutions and factors affecting solubility 2. Methods of expressing concentration (use of normalities is not tested) 3. Raoult s law and colligative properties (nonvolatile solutes); osmosis 4. Nonideal behavior (qualitative aspects) 2008 The College Board. All rights reserved. Visit the College Board on the Web: III. Reactions (35 40%) A. Reaction types 1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism 2. Precipitation reactions 3. Oxidation-reduction reactions a. Oxidation number b. The role of the electron in oxidation-reduction c. Electrochemistry: electrolytic and galvanic cells; Faraday s laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions B. Stoichiometry 1. Ionic and molecular species present in chemical systems: net ionic equations 2. Balancing of equations, including those for redox reactions 3. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants C. Equilibrium 1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier s principle; equilibrium constants 2. Quantitative treatment a. Equilibrium constants for gaseous reactions: Kp, Kc b. Equilibrium constants for reactions in solution (1) Constants for acids and bases; pk; ph (2) Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds (3) Common ion effect; buffers; hydrolysis

4 D. Kinetics 1. Concept of rate of reaction 2. Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws 3. Effect of temperature change on rates 4. Energy of activation; the role of catalysts 5. The relationship between the rate-determining step and a mechanism E. Thermodynamics 1. State functions 2. First law: change in enthalpy; heat of formation; heat of reaction; Hess s law; heats of vaporization and fusion; calorimetry 3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes 4. Relationship of change in free energy to equilibrium constants and electrode potentials 2008 The College Board. All rights reserved. Visit the College Board on the Web: IV. Descriptive Chemistry (10 15%) Knowledge of specific facts of chemistry is essential for an understanding of principles and concepts. These descriptive facts, including the chemistry involved in environmental and societal issues, should not be isolated from the principles being studied but should be taught throughout the course to illustrate and illuminate the principles. The following areas should be covered: 1. Chemical reactivity and products of chemical reactions 2. Relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements 3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties) V. Laboratory (5 10%) The differences between college chemistry and the usual secondary school chemistry course are especially evident in the laboratory work. The AP Chemistry Exam includes some questions based on experiences and skills students acquire in the laboratory: making observations of chemical reactions and substances recording data calculating and interpreting results based on the quantitative data obtained communicating effectively the results of experimental work Colleges have reported that some AP students, while doing well on the exam, have been at a serious disadvantage because of inadequate laboratory experience. Meaningful laboratory work is important in fulfilling the requirements of a collegelevel course of a laboratory scienceand in preparing a student for sophomore-level chemistry courses in college. Because chemistry professors at some institutions ask to see a record of the laboratory work done by an AP student before making a decision about granting credit, placement, or both, in the chemistry program, students should keep a laboratory notebook that includes reports of their laboratory work in such a fashion that the reports can be readily reviewed.

5 2 1 Week 2 2 Year at a Glance AP Chemistry Learning Objectives 1 st Quarter 2 nd Quarter MATTER, ATOMS AND STOICHOMETRY Classifying matter and separating different types of mixtures (LO 1.19, 2.10) Properties of matter (LO 2.1) Physical and chemical changes (LO 3.10) Dimensional analysis (LO 1.4) Atomic theory/structure(lo 1.1, 1.12, 1.13 Average atomic mass and isotopes (LO 1.14) Empirical and molecular formula (LO 1.3) Naming compounds Balancing chemical equations (LO 1.17, 3.2, 3.5, 3.6) Percent composition (LO 1.2, 1.3) Combustion analysis (LO 3.3) Stoichiometry (LO 1.4, 3.3, 3.4) Limiting Reagent (LO 1.4, 3.4) Percent yield (LO 1.4) REACTIONS IN AQUEOUS SOLUTIONS o (Chapter 4 is important) Properties of solutions (LO 1.18) Precipitation reactions (LO 1.18) Redox reactions (LO 1.18, 3.8) Neutralization reactions (LO1.18) Titrations, Stoichometry of titrations ( LO 1.20) Redox titration (LO 3.9) Particle view (LO 3.1) THERMOCHEMISTRY Energy (LO 311) Kinetic Energy (LO 5.2) Maxwell- Boltzman distribution (LO 5.2) Heat (LO 5.3) Work (LO 5.4) Skip state functions and ship 5.8 Enthalpy (LO 3.11) Calorimetry (LO 3.11, 5.5, 5.6, 5.7) Specific Heat Capacity(LO 5.6) Hess s Law Enthalpy of formation (LO 5.6) Heat of solution (LO 6.24) KINETICS Rate Law (LO 4.2, 4.4) Factors that affect the rate of a reaction (LO 4.1) 1.5 weeks 1 week weeks 1.5 EQUILIBRIUM Concept of Equilibrium (LO 5.18, 6.7) Reversible reactions (LO 6.1) Equilibrium constant (LO 5.17, 6.5, 6.6, 6.7) Heterogeneous Equilibrium (LO 6.5) Le-Chatelier principle (LO 5.16, 6.3, 6.8, 6.9, 6.10) Q vs K (LO 6.4, 6.6) SOLUTION (Only sections 13.1 to 13.4) Solvation process (LO 2.8) Solubility (LO 2.14, 2.15) Factors affecting Solubility (LO ) Saturated, unsaturated and super saturated Molarity and mass percent (LO 2.9) Skip mole fraction and molality ACID BASE EQUILIBRIUM Strong and weak acids and bases (LO 6.11, 6.12,6.17) Bronsted acid and bases/conjugate acid and base pair (LO 3.7, 6.18) ph scale (LO 6.12, 6.15, 6.19) Auto-ionization of water (LO 6.14) Kw, Ka and Kb (LO 2.2, 6.14) Acid strength (LO 6.12) Factors that affect acid strength (LO 2.2) Percent ionization of acids (LO 6.12) Titration (LO 6.13) pka and pkb (LO 6.13,6.19) RICE/ICE table (LO 6.16) Skip Section AQUEOUS EQUILIBRIUM Buffers (LO 6.18, 6.20) Common ion effect Titrations, Section 17.3 Ksp, section 17.4 and 17.5 (LO 6.21, 6.22) Common ion effect (LO 6.23) Skip 17.7 Q vs K (LO 6.2, 6.6) THERMODYNAMICS Entropy (LO 5.12) Thermodynamically favorable (LO 5.13, 5.14)

6 Zero, first and second order reactions (LO 4.2) Half-life for first order reactions only (LO 4.3) Integrated Rate Law Collision theory (LO 4.1, 4.4, 4.5) Reaction mechanism (LO 4.7) Identification of catalyst and intermediates (LO 4.8, 4.9) Energy profile (LO 4.6, 4.8) Skip Arrehenius equation and enzymes. Free Energy/ Equilibrium Constant (LO 6.25) Coupled reactions (LO 5.15) Vibrational and rotational motion (LO 1.15) Skip Boltzman s equation Start EQUILIBRIUM 3 1 Week 1 Week 2 3 rd Quarter 4 th Quarter ELECTROCHEMISTRY Redox reactions (LO 3.8) Half-reactions (LO 3.12) Galvanic and Electrolytic cells (LO 3.12, 3.13) Cell Potential (3.12) Free energy (FC) Batteries (LO )) Electrolysis (LO ) Skip Nernst equation Skip oxidizing and reducing agents Reduction Potential (LO 3.12) ELECTRONIC STRUCTURE OF ATOMS Skip quantum numbers Skip De Broglie and Heisenberg Wavelength, frequency, Energy calculations (FC) Beers law (LO 1.16) Electromagnetic spectrum (FC) Electronic configuration (LO )) Photons and quanta of energy (FC) Ground state and excited state (LO 1.5) PES (LO 1.5, 1.6 and 1.7) Coulomb s law(lo 1.7 and 1.8) PERIODIC PROPERTIES Effective nuclear charge (LO 1.9 and 1.10) Atomic Radii, Ionization energy and electron affinity (LO 1.7, 1.8, 1.9 and 1.11) Skip 7.7 and 7.8 BONDING Lewis dot structures (LO 2.21, 2.29) Covalent vs Ionic (LO 2.17, 2.22) Crystal Lattice (LO 2.23, 2.24) Bond energy(important) (5.1) Polarity (LO 2.18, 2.21) Electronegativity (LO 2.17) Resonance structures GASES Gas laws (LO 2.5, 2.6) Barometer (LO 2.6) Density and molar mass (LO 3.3) Partial pressure and Mole fraction (3.3) Gases over water (LO 2.6) Kinetic molecular theory (LO 2.4, 2.5) Effusion and diffusion Real gases (LO 2.4) Why does a gas deviate from ideal gas behavior (LO 2.4, 2.12, 2.12) Skip Graham s Law and Vander Waal s equation INTERMOLECULAR FORCES (important) All intermolecular forces (LO 2.3, 2.11, 2.29, 2.32, 5.9, 5.11) Dipole-dipole attraction and Hydrogen bonding (LO 2.13) Particulate models (LO 2.3, 2.25) Intermolecular versus Intramolecular interactions (LO 5.10) Phase changes (LO ) Heating curves (LO ) Vapor pressure (2.16) Intermolecular forces on micro and macro level (LO 2.16) Skip Section 11.7, liquid crystals Chromatography (LO 2.7) End of year Review End of year lab Review After AP exam Additional labs Project Lab Inventory

7 2 Exceptions to octet rule (LO 2.21) Bond strength (LO 5.1) Bond enthalpy (LO 5.8) Boiling point, Solubility, hardness, brittleness, low volatility, malleability, ductility, conductivity in terms of ionic and covalent bonding. (LO 2.19, 2.22, 2.30, 2..31) Metallic bonding (LO 2.20 and 2.26, 2.25, 2.27) MOLECULAR GEOMETRY VSEPR (LO 2.21) Hybridization, sp, sp2, sp3 only (LO 2.21) Delocalized electrons (LO 2.28) HOFBrINCl Skip 9.7 and 9.8 (molecular orbitals and diatomic molecules)

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9 Acknowledgement of Receipt of Syllabus *Please print this page off and complete the information Return to Hopkins ASAP The student and parent(s) have reviewed the PreAP Chemistry syllabus and contract and understand that it is the responsibility of the student to follow all rules and to complete and return all work within the time specified by the teacher. The student and parent(s) understand that it is best to contact the teacher in order to address concerns about assignments, safety requirements, and/or policies. PARENTS- PLEASE VISIT THE ALVIN ISD WEBSITE AND SET UP ACCESS TO SKYWARD, OUR NEW GRADING AND ATTENDANCE PROGRAM, TO BE ABLE TO CHECK YOUR CHILD S GRADES/ATTENDANCE ON A DAILY BASIS!!! Parent Access to remind.com - Parents, please sign up for remind.com reminders regarding student work, labs, and tests. This is a very important method of communication for me. The Code to access remind.com reminders for Hopkins AP Chemistry or to Student Name: Student Signature: Parent Name: Parent Signature: Parent (VERY Important): Parent Phone # (Cell phone preferred): Date: