'A mind, once stretched by trying something new, can



Honors Chemistry Voorhees, 2015-2016Mrs. KerrRoom 317Course Objectives:to appreciate the ubiquity of chemistry in our everyday worldto apply scientific methods of inquiry, math, computer tools, and interdisciplinary connections in your study of chemistryto gain an in-depth knowledge of basic chemical and physical principles to become experienced with standard safety and operating procedures in a chemical laboratoryto develop interpersonal, study, writing, and presentation skillsText:World of Chemistry (? 2002) by Zumdahl.Other assigned readings from literature. Please leave your text at home. Materials:3-ring binder (for chemistry only), 3-hole punch paper or notebooks, dividers or folders, blue or black pens, pencils, highlighters, (Organization is key!)Calculator (must have log and exponent)Activated account on school computer network Assignments:You are responsible for what is covered in class. To succeed, you must study, come to class prepared and keep up with the assigned readings, homework, special assignments, and labs. (Don’t procrastinate in getting help if you need it.)I will check for the completion of homework at the beginning of class and may occasionally collect it. Homework will account for 10% of your grade.All assignments are to be submitted on the specified due dates. If you are absent the day the assignment is due, it is to be turned in the day you return. No assignments will be accepted after the indicated due date except for legitimate reasons. You are responsible for knowing your assignments and their due dates.Tests/Quizzes:Tests and quizzes will be based on notes, reading, labs, and classroom discussions. Tests are always announced in advance, quizzes may not be. Be prepared to take a test the day it is scheduled, even if you were absent any day before. If you are absent the day of a test you must take it the day you return. (Exceptions will be made for extended absences). Make-up tests are generally more challenging. You are responsible for scheduling a make-up for a test with the teacher. In general, a make-up test will only be delayed for the same number of days you were absent. Laboratory:Your laboratory grade will be based upon how you conduct yourself in lab, on the written lab reports, and on pre-lab quizzes or assignments. Reports are due at the beginning of a class period. Labs handed in any time after the beginning of class will be considered late. There will be a reduction of 10% of the lab grade for each day late.Although data may be shared with a lab partner, the body of the lab is individual work and copying will not be tolerated. Missed labs must be made up within 1 week of due to chemical degradation. Lab make ups should be scheduled the first day the student returns after missing a lab. Extra Help:I will be available for extra help Monday, Wednesday and Thursday after school. Forming a study group with classmates is helpful. But remember, you are responsible for turning in work that is your own.Grading:Grading will be total points earned. An approximate distribution of your grade follows.Unit Tests/quizzes60%Laboratory20%Do Now/Classwork/Participation10%Homework10%Total-100%In Aspen, a 0 is a 0 and will not be replaced. The code EX means that the student was excused from that particular assignment.The code MU means that the student needs to make that assignment up. A MU is averaged in as a 0 until it is turned in and graded by the teacher. THERE IS NO EXTRA CREDIT IN CHEMISTRY CLASS. Conduct: Arrive to class on time. A teacher detention will be assigned for the third tardy. Visits to the restroom and lockers should take place before the class period is scheduled to begin. If there is an urgent need to leave the classroom, you are required to get permission and sign out. Only one person is allowed to be out of the classroom at any given time.Classroom Rules:My expectations are that we will treat each other with respect and courtesy. Enter the room quietly and be ready to work each day.Avoid language that insults, hurts, or offends others. Remain seated until the bell rings.No food, ipod, cell phones, smartphones in class. Leave the room neat. This is a shared space as well as our “home” for the year. Keep it clean. Consequences:verbal warningteacher detentionparent phone call immediate removal from the classroom at discretion of the teacheradministrative referralHonors Chemistry – Syllabus Text: World of Chemistry (? 2002) by Zumdahl.Unit 1: Introduction To Chemistry and Matter (Chapter 1 and 2)Objectives:Discover the ubiquity of chemistry in our world.Define chemistry and matter.Define observation, hypothesis, experiment, theory, and law in scientific process.Apply the scientific method of investigation.Define energy and distinguish between kinetic and potential energy.Explain the law of conservation of mass-energy.Describe and distinguish between mixtures and pure substances, homogeneous and heterogeneous substances, elements and compounds.Differentiate between physical and chemical properties of matter.Distinguish physical and chemical changes in matter.Explain the relationship between chemical change and energy.Review lab techniques, equipment, and safety.Research, summarize, and present the safety and handling precautions for a chemical. Learn the names and symbols for 40 elements.Laboratory/AssignmentsWhy do I have to study chemistry?Laboratory Techniques, Equipment, and SafetyCandle observationsEvidence of Interaction-Copper chlorideElement flash cardsPhysical and Chemical ChangeHomeworkUnit 2: The Measurement of Matter and Problem Solving (Chapter 5)Objectives:List and use the SI base/or derived units for mass, length, volume, time, and temperature.Express and convert quantities using the common SI prefixes.Use the factor-label (dimensional analysis) to obtain the desired unit in solving problems.Use significant figures to express the exactness of measurements.Express any number in scientific notation.Make use of scientific notation in addition, subtraction, multiplication, and pare and contrast the accuracy and precision of a measurement.Determine the densities of different substances.Perform calculations using density measurements.Laboratory/AssignmentsDensity of metalsDensity and Pennies.Coke Density and Accuracy and Precision of Lab Glassware.HomeworkUnit 5: Atomic Theory (Chapter 3 and 11)Objectives:Discuss the Dalton’s atomic theory.Discuss the historical development of the atomic theory and contributions from Thompson, Rutherford, Bohr, and Schrodinger.Identify and describe the three fundamental particles of the atom and how they are arranged in or about the nucleus.Define atomic number and atomic mass and use them to fine the number of protons, neutrons, and electrons in an atom.Describe how atoms of isotopes of an element differ and explain why atomic masses are not whole numbers.Calculate the average atomic mass given the isotope distribution of an element.Characterize the four quantum numbers.Recognize general shape of s, p, d, f atomic orbitals.Use the Aufbau principle, the Pauli exclusion principle, and Hund’s rule to write electron configurations.Identify the number of electrons in the outermost energy level.State the importance of a noble gas configuration and explain and use the octet rule.Draw electron-dot diagrams for the elements, monatomic ions, and excited state atoms.Discuss the dual wave-particle nature of light and its connection to atomic structure.Explain the mathematical relationship among the variables (, , c) relating to electromagnetic radiation.Laboratory/AssignmentsFlame TestsGas tubes and spectroscopesFelt-tip electron distributionsHomeworkUnit 6: Periodic Table (Chapter 3 and 11)Objectives:Describe the early attempts at classifying elements.State the Periodic Law.Explain the basis for the arrangement of the modern periodic table.Recognize the organization of the periodic table into s, p, d, and f blocks.Use the periodic table to predict the electron configurations of elements.Identify metals (alkali, alkaline earth, transition, inner transition), nonmetals, metalloids, halogens, and noble gases on the periodic table.Summarize the characteristics for families of elements. Explain the periodic trends (atomic radii, ionic radii, ionization energy, electronegativity, oxidation #)Explain how the shielding effect and increased nuclear charge influences periodic trends.Laboratory/AssignmentsPatterns puzzlePeriodic table puzzlesPeriodic Properties (Group II and IV)HomeworkUnit 7: Chemical Bonding (Chapter 12)Objectives:Define ionic, covalent, metallic bonds.Identify the type of bonding between two elements given their electronegativities.Given a list of properties, match the type of bonding with the correct properties.Describe the formation of a cation from an atom of a metallic element.Describe the formation of an anion from an atom of a nonmetallic element.Recognize an ionic bond as the electrostatic attraction between a cation and an anion.Recognize a covalent bond (between two non-metallic elements) as the sharing of electrons. Use electronegativity values to determine whether a bond is polar or non-polar covalent bonds. Use the theory of metallic bonds to explain the physical properties of metals.Given simple molecules, identify or write their Lewis structures.Describe the VSEPR theory and use it to predict bond angles and the shape of molecules.Distinguish between polar and nonpolar covalent bonds. Define dipole and compare the strengths of intermolecular forces bases on dipole moments.Define hydrogen bonding, van der Waals, dipole-dipole interactions.Laboratory/AssignmentsClassification of Chemical CompoundsMolecular ModelsHomeworkUnit 8: Chemical Names and Formulas (Chapter 4 and 6)Objectives:Write the symbol and charge for monatomic and polyatomic ions.Demonstrate proficiency in naming an ionic or molecular compound when given the formula.Demonstrate proficiency writing the formula of a ionic or molecular compound when given the name.Calculate formula weight (ionic compound) or molecular weight (covalent compound).Distinguish between empirical and molecular formulas.Using sample problems, show how different samples of the same compound obey the law of definite proportions.Show that two different compounds composed of the same tow elements obey the law of multiple proportions.Calculate the % composition of a substance in a mixture.Calculate the % composition of an element in a pure substance given the formula.Derive empirical and molecular formulas from appropriate experimental data.Laboratory/AssignmentsFlash cardsEmpirical formula of copper sulfidePercent of sugar in gumPercent KClO3Percent water in hydrate (copper sulfate)HomeworkUnit 9: Chemical Reactions (Chapter 7 and 8)Objectives:Define reactants and products and interpret symbols used in writing equations.Write a word equation and a formula equation given a description of a chemical reaction. Balance a chemical reaction using coefficients.Classify reactions as synthesis, decomposition, single replacement, double replacement, or combustion.Use the activity series of metals to predict the products of single-replacement reactions.Define oxidation and reduction in terms of the loss, gain, or shift of electrons.Identify the oxidizing and reducing agents in a redox reaction.Determine the oxidation number of an atom of any element in a pure substance.Define oxidation and reduction in terms of a change in oxidation number.Use the oxidation number change method to identify atoms being oxidized or reduced in redox reactions.Given a combination of aqueous ionic compounds, write the net ionic equation.Laboratory/AssignmentsSix Types of Chemical ReactionsPrecipitation ReactionsHomeworkUnit 10: Mole Concept and Stoichiometry (Chapter 9)Objectives:Use Avogadro’s constant to define the mole.Identify the representative particle of elements and compounds.Calculate the number of representative particles of any substance given the number of moles (and visa-versa).Calculate the mass of any substance given the number of moles (and visa-versa).Calculate the volume of a gas (@STP) of any substance given the number of moles (and visa-versa).Use molar mass to calculate % composition of an element or water in a formula. Construct mole ratios from balanced chemical equations for use as conversion factors in stoichiometric problems.Given a fixed number of moles, mass, or volume of a reactant or product and a balanced equation, calculate the moles, mass, or volume of either a product or a reactant.Identify the limiting reactant and be able to solve problems based upon it.Calculate actual yield and theoretical yield.Laboratory/AssignmentsAluminum Foil ThicknessDetermination of an Empirical Formula.Calculate mass of magnesium HomeworkUnit 3: States of Matter (Chapter 14)Objectives:Differentiate among the four states of matter.Explain the nature of liquids, KE and intermolecular forces.Define vapor pressure and boiling point.Explain the nature of solids, KE and intermolecular forces.Characterize a heating curve in terms of changes in energy and physical state Analyze a phase diagram for changes in state, the triple point, and critical point.Laboratory/AssignmentsMelting Curve of naphthalene/paradichlorobenzeneBoiling point demoHomeworkUnit 4: Thermochemistry (Chapter 10)Objectives:Define internal energy(U), heat(q), work(w), enthalpy(H), and entropy(S).Investigate calorimetry as a method for measuring energy changes.Perform calculations involving specific heat.Explain heat of reaction, heat of formation, and enthalpy.Associate the enthalpy of a reaction with an exothermic or endothermic process.Write thermochemical equations and perform quantitative calculations on heat loss or gain.Solve problems involving Hess’ Law.Laboratory/AssignmentsSpecific heat of metalsEnthalpy of fusion for iceEnthalpy of solutionHeat of reactionHomeworkUnit 11: Gas Laws (Chapter 13)Objectives:Explain the concept of an Ideal gas.Describe the conditions of standard temperature and pressure.Relate the laws of Boyle, Charles, Gay-Lussac, and Dalton and perform calculations using these laws.Explain the significance of absolute zero. Know its value in both °C and K and be able to convert between the two temperature scales.Convert between units of pressure (kPa, atm, mm Hg).Explain and use the ideal gas equation. Solve problems involving change of more than on condition.Explain Graham’s law and solve problems using pute the molar mass of a gas or density using the ideal gas law.Account for deviations from ideal behavior.Laboratory/AssignmentsBoyle’s Law: Pressure-Volume Relationship in Gases (CBL).Gay-Lussac’s Law: Pressure-Temperature Relationship in Gases Charles Law: Temperature-VolumeMolar Mass of butaneHomeworkUnit 12: Solutions (Chapter 15)Objectives:Define the terms solution, solute, solvent.Explain the differences between a saturated, supersaturated, unsaturated, solution.Distinguish among electrolytic and non-electrolytic solutions.Distinguish between solutions, colloids, and suspensions.Explain factors that affect solubility.Use Henry’s Law to explain gas solubility.Describe the process of solvation and sue the “like dissolves like” rule to predict solubility.Explain the factors that define how fast a substance will dissolve.Use solubility curves.Define molarity (M). Instruct how to prepare solutions of given molarity. Calculate the mass or number of moles in a given volume of solution with known molarity. Differentiate among and solve problems involving molarity, molality, mole fraction, and mass percent.Describe why a solution has a lower vapor pressure than the pure solvent of that solution.Explain how the addition of a solute to a pure solvent causes an elevation of the boiling point and a depression of the freezing point of the resultant solution.Solubility product constantsLaboratory/AssignmentsSolutions of Sodium AcetateMolarity of NaCl SolutionFreezing Point Depression to Find MWSolubility product constantsHomeworkUnit 13: Reaction Rate and Chemical Equilibrium (Chapter 17)Objectives:Distinguish between thermodynamic stability and kinetic stability.List and describe the factors that influence the rate of reaction.Differentiate between the rate of a reaction and the rate constant.Write a rate expression for a reaction given concentration of a reactant or product and initial rate data.Define activation complex and activation energy.Define chemical equilibrium and explain the nature of the equilibrium constant.Determine an equilibrium constant expression for a system at equilibrium. Calculate the equilibrium constant or predict the concentrations of products and reactions.Use LeChatelier’s principle to explain the effects of changes in concentration, pressure, and temperature on the equilibrium system.Explain the concept of solubility product and solve problems using the solubility product constant.Laboratory/AssignmentsDetermination of an Equilibrium Constant. (CBLs)Crystal Violet Rate Equation (CBLs)Iodine Clock reactionHomeworkUnit 14: Acids, Bases, and Salts (Chapter 16)Objectives:Identify the properties of acidic and basic solutions.Distinguish between Arrhenius, Bronsted-Lowry, and Lewis acids and bases.Name and write the formula for common acids and bases.Discuss the auto-ionization of water and solve problems using the ion product constant for water.Given hydrogen ion or hydroxide ion concentration, classify a solution as neutral, acidic, or basic.Explain how the pH scale is used for measuring solution acidity.Calculate pH/pOH given molar concentrations of hydronium/hydroxide ions and vice-versa.Derive and use acid/base dissociation constants.Explain the concept of neutralization, the process of titration and perform calculations using the data from titrations.Describe the composition and function of buffers.Ionization constants (Ka)Laboratory/AssignmentsThe Acetic Acid Content of Vinegar by TitrationMeasuring pH and Making a BufferHomeworkUnit 15: Redox Reactions and Electrochemistry (Chapter 18)Objectives:a. Assign oxidation numbersb. Identify redox reactionsc. Balance redox reactionsDescribe the construction and functioning of electrolytic and voltaic pare electrolytic and electronic conduction.Describe the movement of anions and cations and their reactions in cells.Laboratory/AssignmentsA Redox TitrationElectrolysis3. HomeworkUnit 16: Organic Chemistry (Chapter 20)Objectives:Differentiate between aromatic and aliphatic, saturated and unsaturated, chain and cyclic hydrocarbons.Identify, name, and write structural formulas for the main classes of organic compounds.Investigate structural and optical isomers.Discover the unique properties of polymers.Laboratory/AssignmentsSynthesis of SoapSynthesis of an ester3. HomeworkUnit 17: Nuclear Chemistry (Chapter 19)Literature readings and topics will by provided as a springboard to some independent study of nuclear chemistry topics including Chernobyl, Marie Curie, the Manhattan Project, Robert Oppenheimer, Nuclear Power Plants….. ................
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