Syllabus - Milwaukie High School

Chemistry : Milwaukie High SchoolSyllabusCourse DescriptionChemistry I Grades: 10, 11, 12 YearCredit: .5 each semesterPre: Biology/Algebra, ~ C GradesCRLEHS, IE, NRIn this one year long class, you will learn about the chemical elements, their structures, theirproperties and the commercial and technological applications of chemicals in the real world as well.You will gain a hands-on, working knowledge of chemistry in the world through a variety of laboratoryexperiments designed to provide contextual applications of chemical concepts. You will use scientificinquiry in the laboratory, the classroom and in real life activities to improve critical thinking skills.Topics studied will include nomenclature, measurement, writing and balancing chemical reactions,properties of gases, thermodynamics, atomic, solutions, and properties of acids and bases. This classdevelops readiness for any other science classes at MHS as well as promoting high level collegepreparedness. Expect to have one hour of homework for every period attended per week. Each Unitwill have a packet of homework assignments, computer assignments and hands-on laboratoryprojects. At the conclusion of each unit, students will have a Unit assessment.Instructors Contact InformationName: Jeff LinmanRoom # 303/307/309Voice Mail/Phone 503 353 5840 ext38388 (cell: 503.515.3590)Email Address linmanj@nclack.k12.or.usHours/Days of Availability 7:15 am to 8:35 am Monday, Tuesday, Thursday, FridayAlso available after school every dayName: Sara SchipperRoom # 303Email Address schippers@nclack.k12.or.usVoice Mail/Phone 503 353 5840 ext 38598During Periods 3 and 4 ext. 38388Clackamas Phone: 503.353.5000 ext. 38050Hours/Days of Availability Day 1 (after school)Required Texts: Holt Chemistry Visualizing Matter, 2000 Edition.Course ObjectivesChemistry 1Topics, Goals and ObjectivesUnit One: Naming Compounds/Writing FormulasHow are ions different from atoms?-Identify ions that are isoelectronic with the noble gases.-Explain why the properties of ions differ from the properties of their parent atoms.-Relate an atom's tendency to form an ion to the element's position in the periodic table and to the octet-Describe the consequences of the electroneutrality principle.-Name cations, anions, and salts.-Write formulas for binary compounds.

The MoleHow are atoms counted and measured?-Explain the relationship between atomic mass and atomic mass units.-Use a periodic table to determine the relative atomic masses of elements.-Solve problems involving moles, atoms, and molar mass.-Calculate the mass of individual atoms. How is the mole concept related to chemical formulas?-List the information you can derive about a compound from its chemical formula.-Determine the molar mass and percentage composition of a compound from its formula.-Derive a compound's empirical formula from its percentage composition.-Calculate the molecular formula of a compound from its empirical formula and its formula mass.What is the Nature of Matter?-Use chemical tables to determine the names and symbols for various elements.-Distinguish between atoms, elements, and molecules.-Describe different forms of elements.How is Matter Classified?-Distinguish between pure substances and mixtures.-Interpret chemical formulas.-Classify mixtures as homogeneous or heterogeneous.-Classify compounds as inorganic or organic.What is Chemistry?-Describe the characteristics of the three most common physical states.-Draw models to represent solids, liquids, and gases.-Write a word equation for a chemical reaction.-Identify the reactants and products in a chemical reaction.What holds a salt together?-Describe the nature of ionic bonding.-Explain what is meant by a crystal structure, and distinguish between the structures of NaCl and CsCl.-Explain the energy changes that occur in the formation of a salt.-Summarize the properties of binary ionic compounds.What are polyatomic ions?-Explain how polyatomic ions and their salts are named and how their formulas relate to their names.-Describe the pattern used in naming oxyanions.-Assign oxidation numbers to atoms in polyatomic ions and their compounds.-Discuss differences between silicate minerals, hydrates, and conventional saltsUnit Two: Balancing Chemical ReactionsWhat is a chemical reaction?-List evidence that suggests a chemical reaction might have occurred and evidence that proves achemical reaction has occurred.-Describe a chemical reaction using a word equation.-Describe endothermic and exothermic reactions in terms of bond energies.-Relate conservation of mass to the rearrangement of atoms in a chemical reaction.-Explain how a nonspontaneous reaction can occur.-Explain why reactants must be brought into contact for a reaction to occur.

How are chemical equations for reactions written?-Translate word equations into formula equations.-Relate conservation of mass to a balanced equation.-Write a balanced chemical equation for a reaction.-Distinguish between coefficients in a chemical formula.What does a chemical equation tell you?-Describe how the conditions for a chemical reaction can be specified in the chemical equation.-Include information about the states of reactants and products in a chemical equation.-Interpret a chemical equation in terms of the relative numbers of molecules involved.-Determine whether a reaction is endothermic or exothermic using information from a chemicalequation.-Derive mole ratios from a balanced chemical equation.-Calculate energy changes in reactions using mole ratios and change in heat values.How are chemical reactions classified?-Classify a given reaction as a combustion, decomposition, double-displacement, displacement, orsynthesis reaction.-Write chemical equations representing each type of chemical reaction.-Use the activity series to predict whether a given reaction will occur and what its products will be.-write total and net ionic equations for double-displacement reactions.Unit Three: Significant Digits & MeasurementsHow do Chemists Measure Quantities?-Distinguish between accuracy and precision in measurements.-Determine the number of significant figures in a measurement.-Perform calculations using measurements, and round the results to the correct number ofsignificant figures.-Write very large and very small numbers in scientific notation.What is Matter?-Relate mass, volume, and density.-Distinguish between qualitative and quantitative properties.-Describe the difference between a quantity and a unit.-Convert measurements between SI units.-Distinguish between physical and chemical properties.-List four ways to determine if a chemical change has occurred.Unit Four: StoichiometryHow much can a reaction produce?-Distinguish between composition stoichiometry and reaction stoichiometry.-Apply a three-step method to solve stoichiometry problems.-Use mole ratios and molar masses to create conversion factors for solving stoichiometry problems.How much does a reaction really produce-Distinguish between a limiting reactant and an excess reactant.-Identify the limiting reactant in a problem, and calculate the theoretical yield.-Distinguish between theoretical yield and actual yield.

-Calculate the percentage yield, given the actual yield and the quantity of the limiting reactant.-Use percentage yield to calculate actual yield.How can Stoichiometry be used?-Relate volume calculations in stoichiometry to the inflation of automobile safety air bags.-Use the concept of limiting reactants to explain why fuel-air ratios affect engine performance.-Compare the efficiency of pollution-control mechanisms in cars using percentage yield.How are atoms counted and measured?-Explain the relationship between atomic mass and atomic mass units.-Use a periodic table to determine the relative atomic masses of elements.-Solve problems involving moles, atoms, and molar mass.-Calculate the mass of individual atoms.How is the mole concept related to chemical formulas?-List the information you can derive about a compound from its chemical formula.-Determine the molar mass and percentage composition of a compound from its formula.Unit Five: Gas LawsWhat are the characteristics of gases?-Describe the general properties of gases.-Relate the kinetic-molecular theory to the properties of an ideal gas.-Define pressure, and give the SI unit for pressure.-Describe the events that are believed to be responsible for global warming.What behaviors are described by the gas law?-Relate the ideal gas model to the observed behavior of real gases.-State the following laws describing the behavior of gases: Boyle's law, Dalton's law, Charles's law,Avogadro's law, Gay-Lussac's law, and Graham's law.-Use these laws to solve problems.-Describe the relationship between gas behavior and chemical formulas.How do the gas laws fit together?-Use the ideal gas law and combined gas law to solve mathematical problems.-Apply your knowledge of reaction stoichiometry to solve gas stoichiometry problems.What conditions will cause a gas to condense?-List the conditions under which gases deviate from ideal behavior.-Relate attractive forces to boiling points.-Interpret a phase diagram.-Relate vapor pressure to temperature.-Define boiling point in terms of vapor pressure.Unit Six: Oxidation/Reduction & Electrochemistry-Assign oxidation numbers to atoms-Balance Chemical Reactions by looking at changes in oxidation numbers-Distinguish between: metallic conduction and electrolytic (ionic) conduction; oxidation and reduction;

electrolytic cells and voltaic cells; anode and cathode.-Understand the general concepts of electrolysis.-Given the components of the electrodes and observations of what happens at the electrodes when anelectrolytic cell is in operation, be able to do the following: Describe the operation of the cell;write balanced oxidation and reduction half-reactions; write balanced chemical equations for theoverall reaction; construct a simplified diagram of the cell, including designation of anode andcathode, positive and negative electrode, direction of electron flow in the external circuit,and direction of migration of ions within the cell.-Understand Faraday's Law of Electrolysis; perform calculations to relate the amount ofelectricity passing through an electrolytic cell to the amount of a specified reactantconsumed or product formed in the cell.Unit Seven: Solutions-Distinguish between solutions, suspensions, and colloids.-Explain the role of a solute and a solvent in a solution.-Describe some techniques chemist use to separate mixtures.-Relate various ways that concentrations may be expressed.-Use units of molarity in stoichiometry calculations.-Describe the procedure for making a solution of prescribed molarity.What causes conductivity in solutions?-Identify substances that are good, intermediate, and poor conductors of electricity.-Discuss nonelectrolytes, weak electrolytes, and strong electrolytes.How are a liquid's properties changed by solutes?-Explain why a liquid's boiling point is elevated but its freezing point is depressed when a solutedissolves.-Describe how the magnitude of a colligative property depends on the amount of solute and onthe chemistry of the dissolution process.Unit Eight: Atomic TheoryHow Do We Know Atoms Exist?-State the three laws that support the existence of atoms.-List the five principles of Dalton's atomic theory.-Calculate the masses of atoms in amu and gram units.-Describe how the atomic mass unit was chosen.What is the Internal Structure of Atoms?-Describe the evidence for the existence of electrons and their presence in atoms.-Explain how Rutherford's experiments led to the discovery of the nucleus.-Discuss atoms of different elements in terms of the numbers of electrons, protons, andneutrons they contain.-Define the terms atomic number, mass number, and isotope.How are an Atom's electrons Configured?-Describe the nature of light and how it is produced.-Explain how the wavelengths of light emitted by an atom provide information about electronenergy levels.

-Compare the atomic models of Rutherford and Bohr.-Describe the quantum mechanical interpretation of electrons in atoms.-State Pauli's exclusion Principle, the aufbau principle, and Hund's rule, and describe their roles indetermining the electron configuration of atoms.Unit Nine: Periodic TableWhat Makes a Group of Elements?-Describe the organization of the modern periodic table.-State the periodic law.-Describe characteristic properties of groups of elements.-Relate the properties of the main-group elements to their electron configuration.What Gives Metals Their Distinctive Properties?-Identify the defining property of metals.-Describe the varied properties of metals.-Explain why metals are good conductors of electricity and heat.-Describe how atoms in most metals pack.What Trends are Found in the Periodic Table?-Describe periodic trends in atomic radius, ionization energy, election affinity, melting points,and boiling points.-Relate trends in the periodic table to the atomic structures of the elements.Where Did the Elements Come From?-Distinguish between naturally occurring and synthetic elements.-Describe how the naturally occurring elements are formed.-Describe how particle accelerators are used to create synthetic elements.Unit Ten: Chemical BondingWhy do some atoms form covalent bonds?-Explain how a covalent bond forms between two atoms.-Describe the change in energy and stability as a covalent bond forms.-Describe the differences between covalent and ionic bonds and between polar and nonpolarcovalent bonds.-Describe the influence of electronegativity difference on bonding.-Classify the types of bonds between atoms using electronegativity values.How are molecules depicted?-Draw Lewis structures to show the arrangement of valence electrons among atoms in moleculesand polyatomic ions.-Explain the differences between single, double, and triple covalent bonds.-Draw resonance structures for simple molecules and polyatomic ions, and recognize whenresonance structures are required.-Name binary inorganic compounds using prefixes, roots, and suffixes.How are molecular shapes determined?-Predict the shape of a molecule from its Lewis structure using VSEPR theory.-Associate the polarity of molecules with their shapes.-Relate the boiling point of a molecular substance to the shape and plarity of its molecules.

What forces exist between molecules?-Contrast ionic solids and covalent solids.-Describe the types of forces that exist between molecules._Explain how a hydrogen bond differs from other polar-polar forces.Unit Eleven: EquilibriumWhat is an equilibrium system?-Distinguish between reactions that go to completion and those that do not.-Determine whether the forward or reverse reaction is favored when a stress is applied to anequilibrium system using Le Chartelier's principle.-Describe complex-ion behavior in aqueous equilibrium.-Discuss examples of equilibrium systems.How is equilibrium measured?-Write Keq expressions for reactions in equilibrium.-Calculate concentrations of reactants or products in an equilibrium system using Keq values.-Write Keq expressions for the solubility of slightly soluble salts.-Determine concentrations using Keq expressions.Unit Twelve: Acids & BasesWhat are acids and bases?-Describe the distinctive properties of acids and bases.-Distinguish between the terms strong and weak as they apply to acids and bases.-Explain the unusually high electrical conductivities of acidic solutions.-Use Kw to calculate a solution's hydronium ion or hydroxide ion concentration.-Name and describe the functional groups that characterize organic acids and bases.How are acidity and pH related?-State the definition of pH, and explain the relationship between pH and H30+ ion concentration.-Perform calculations using pH, [H30+],[OH-], and quantitative descriptions of aqueous solutions.-Describe two methods of measuring pH.-Describe how a buffer solution is able to resist changes in pH.

Chemistry GRADING POLICY1. Your letter grade will be based upon the percentage of the total possible points you earnduring the grading period. The percentage scale is as follows:GRADING SCALE90.0000 - 100.0000 A80.0000 - 89.9999 B70.0000 - 79.9999 C60.0000 - 69.9999 D0.00000 - 59.9999 F2. Points will be earned from the following:• Homework & Laboratory assignments (about 40%)• Quizzes & Exams(both announced and unannounced) (about 50%)• You may use a cheat sheet of notes on a test. They MUST be written in your hand.• Classroom participation (about 10%)3. We will usually set the high score on any given piece of work at 100 % and then curve therest of the scores to their respective percentages.4. All assignments MUST be completed on time, or you will suffer the penalty of loss of points atthe rate of 10% per class day. Our assignments are handed out. Make it a point of getting themaximum value for the work that you accomplish in this course. Our assignments will comeout in Unit packets with all the assignments, labs and computer assignments contained in onedocument (also available online at www.milwaukiehigh.org/chemistry). You will hang on tothat packet all the way through the unit and we will assess that packet in class. Makecorrections per your teacher’s instructions during the unit. If you get behind you can still makeup the homework and get partial credit. At the end of a unit, on a test day, you will hand inthe packet and we will enter it into the gradebook and hand it back when you are finished withthe unit exam. You can still make up missing work in the packet afterwards to receive partialcredit. Prior to the exam we will hand out an exam review. It is not an assignment (worthpoints) but it will definitely help prepare you for the unit exam. We will post answers to thereview on the Chemistry Website and we will post them in Room 303 as well, so you cancheck your work prior to the Exam. We will not be giving retakes on exams this year with theexception of the Unit 1 Exam (since you need to experience a Chemistry Exam). If you aregoing to opt to retake the Unit 1 exam, you will need to demonstrate you have preparedsufficiently, but doing a second Review along with having all your assigned work completedbefore we will allow you to take it. Preparing for Unit Exams is a very important process andwe ask you to focus on that. You will be allowed to use a cheat sheet on the exams, it must bewritten in your handwriting (not word processed, or copied). You will also be allowed to use allresource documents we provide to you.5. Students with excused absences will have one day per day excused absence to make up workbefore the penalty applies. It is the students' responsibility to find out what they have missed

on the first day back. Students will need to schedule a time to make up the work with theirinstructor ASAP. Make sure you get your late work in quickly, so you do not get behind, wemove at a fast pace in this course. If you miss a lab, you will need to schedule a time to comein and make that lab up. We will make every attempt not to give you busy work, we believe allof our assignments have value in doing them !!!!!!! Let’s work together to make sure thatevery student in this course achieves success in their learning and completes their work in atimely fashion.6. No course credit can be earned unless the required work is turned in, 60 % of the totalpossible points accumulated, and the minimum competencies achieved.7. It is your responsibility to be in class when the tardy bell rings. If you are tardy, please informme as to why you were tardy, I view being tardy as a “cup half full” and focus on the fact thatyou DID come to class. There is a school wide policy for tardies, in which after three tardies inthe semester, the fourth tardy (and every tardy after that) will result in serving detentionbefore school, or after school. Please make every attempt to get to class in a timely fashion.If you arrive after 10 minutes, it is school policy to record this as an absence, please excusethe absence downstairs in the Attendance Office.8. We highly recommend you get to know others in the class since we are confident you will bespending a sizeable amount of time with each other. We will all need to collaborate toaccomplish many of the tasks in front of us this year.9. Whenever you get stuck, please do not hesitate to call Mr. Linman at 503.515.3590 (cell)(Please leave a message with a phone number and I will call you back if I am not there). I donot want you to stare at the problem, that is a waste of your time. I can usually get you ontrack in a couple of minutes, so give me a call and let me help you. You may call me up to10:00 PM on school nights and I am also available on weekends. Sundays, I am out on thesoccer pitch, but just leave a message on voicemail and I will return your phone call. You canalso e-mail me at jlinman@techcadre.com . I arrive at school each day by 7:15 AM in the TechCadre(Room 309) and that is where you can usually find me (or in the Chem Lab Room 303). Iam also there after school daily and would be more than happy to assist you in any waypossible. Mrs. Schipper will be here after school in Room 303 on Day 1’s to assist you as well.Since we are sharing curriculum and lessons this year, either one of us can help you. If youare Mrs. Schipper’s student and need to come in before or after school on a Day 2, Mr. Linmancan help you and vice versa.10. Always doing your work in a timely manner will pay great dividends this semester. There willbe a lot of individualized learning where you will decide how much work you do. That couldbe a very positive situation for you OR it could ruin the whole semester. Do yourself a favorand go for broke, We guarantee it will be worth your while. This course is for motivatedstudents who want to learn about the world around them. Make this year a great experiencefor all of us !!!!!!!!!!!!!!!11. This year, we will be trying to streamline notes, lectures and accessing assignments. You canaccess almost all information for Chemistry this year on the high school Web site(http://www.milwaukiehigh.org/science/chemistry). You will also be able to see whathomework is due for each day as well (Calendar). If you do not have Acrobat Reader on yourComputer system, go to http://www.adobe.com and download a copy (it is free!). We would

appreciate feedback from all of you letting meus know what else we can do to improveefficiency of our learning organization. We will have all our PowerPoint notes, assignmentpackets and links to helpful resources available on the site.Let’s all work together to make this learning organization work for ALL OF US!!!Where to find Mr. Linman. ?????Before School (7:15 and on…. )Tech Cadre Room 309 or 303 (Except Wednesdays…staff meetings)Day 1Period 1: Chemistry Room 303Period 2: Chemistry Room 303Period 3: Tech Cadre (1 st Lunch) Room 309Period 4: Physics Room 307Day 2Period 1: Physics Room 307Period 2: Chemistry Room 303Period 3: Prep Room 303/309Period 4: Chemistry Room 303After School (3:45 to ?????) 303/307/309If you are going to call and leave a message for me: my cell phone is best…………….I always have it.Cell Phone: 503.515.3590School Phone: 503.353.5840 ext. 38388Cadre Phone: 503.353.5840 ext. 38420Where to find Mrs. Schipper. ?????Day 1Period 1: At ClackamasPeriod 2: Traveling to MHSPeriod 3: Chemistry(1 st Lunch) Room 303Period 4: Chemistry Room 303After School (3:45 to ?????) Room 303

Milwaukie High School : Chemistry Grading Policy Review ConfirmationPlease take this grading policy home, review it with your parents/guardians and have them signthis……………Student Name:Parent/Guardian(Print):I have reviewed this grading policy with my son/daughter and understand that if myson/daughter falls behind academically, after school tutoring will be suggested by Mr.Linman/Mrs. Schipper. After school tutoring takes place every Tuesday and Thursday from 3:30 –4:50 PM in the MHS Library. Activity busses will be available at 5:00 PM to take the studentshome. It is the goal of our learning organization to make sure every student has access to thesupport they need in order to be successful in Chemistry.Parent/Guardian Signature:Please provide an email address where Mr. Linman/Mrs. Schipper can contact you regarding theacademic performance of your student.EMAIL(Please print clearly):We look forward to continuing to work with your son/daughter as we look at the world ofChemistry throughout the rest of the year.Mr. Linman and Mrs. Schipper. ☺

SAFETY IN THE LABORATORYThe chemistry laboratory is a safe place to experiment if you are careful. You must assumeresponsibility for the safety of yourself and your neighbors. Following are some safety rules tohelp guide you in protecting yourself and others from injury in the laboratory.1. The chemistry laboratory is to be used for serious work.2. Do not perform experiments that are unauthorized. Always obtain your teacher's permission.3. Study your lab assignment before you come to the lab. If you are in doubt about anyprocedure, ask your teacher for help.4. Safety goggles and a laboratory apron should be worn whenever you work in the lab.5. Gloves should be worn whenever you use chemicals that cause skin irritations or can beabsorbed through the skin.6. Use the safety equipment provided for you. Know the location of the fire extinguisher, safetyshower, eye wash, fire blanket, and the first aid kit.7. Report any accident, injury, or incorrect procedure to your teacher at once (NO MATTER HOWSMALL).8. If you spill acid or other corrosive chemical, wash it off immediately with a large amount ofwater.9. Never taste any chemical substance unless you are directed specifically by your teacher to doso. Never draw materials into a pipette with your mouth.10. Smother fires with a towel. If clothing should catch fire, smother it with a blanket or coat orquench it under a safety shower.11. Handle chemicals carefully. Check the label of all bottles before removing the contents. Do notreturn unused chemicals to reagent bottles.12. Keep combustible materials away from open flames. (Some combustible materials are alcohol,carbon disulfide, and acetone.)13. Handle toxic or combustible gases only under the direction of your teacher. Use the fume hoodwhen handling such materials.14. When heating a substance in a test tube, be careful not to point the mouth of the test tube atanother person or yourself.15. Never stopper a test tube that is being heated or one in which a reaction is occurring.16. Use caution and the proper equipment to handle hot glassware. Cool glass looks the same ashot glass.17. Place broken glass and solid substances in designated containers. Keep insoluble wastematerialout of the sink.18. Know the correct procedure for mixing acid solutions. Always add the acid slowly to the water.Never add water to a large amount of acid.19. Long hair should be tied back. Avoid wearing clothing with loose sleeves as it may catch fire.

CLASSROOM PROCEDURE1. You are expected to be courteous to the teacher and fellow students.2. You are expected to be seated quietly at your desk when the tardy bell rings.3. You are expected to follow all classroom and school rules.4. You are expected to attend class regularly and follow the school attendance policy.5. Any student coming to class after the tardy bell will be marked tardy.6. You are expected to bring a pen or pencil, notebook, and a calculator to class each day.7. You are expected to participate in all classroom activities.8. You are expected to follow all classroom and laboratory safety procedures.9. You are expected to work quietly at your assigned desk during the class period.10. You are expected to stay out of the science store rooms.11. Profane language will not be accepted in the classroom.12. Seating assignments will be made when necessary.12. Cell phones are to be turned off at all times, except if we are texting homework reminders orcontacting a community member for a chemistry project.13. Please keep backpacks and personal items out of the aisles and under your desk.