CP CCP CHEMISTRYHEMISTRY VOORHEES HIGH SCHOOL, 2014-2015

INSTRUCTORS: Miss Jessica Clark and Mr. Ben PerlowskiPHONE: 908-638-2199 ext. 2240 and 2082EMAIL: jclark@nhvweb.net and bperlowski@nhvweb.net WEBSITE: http://missclarkswebsite.weebly.com/

COURSE OBJECTIVES: to appreciate the ubiquity of chemistry in our everyday world to apply scientific methods of inquiry, math, computer tools, and interdisciplinary connections in your study

of chemistry to gain an introductory knowledge of basic chemical and physical principles to become experienced with standard safety and operating procedures in a chemical laboratory to develop interpersonal, study, writing, and presentation skills

TEXTBOOK: Chemistry (© 2002) by Addison-Wesley

REQUIRED MATERIALS: (ORGANIZATION IS KEY!) 3-ring binder (for chemistry only) with 3-hole punch paper dividers or folders blue or black pens and pencils Laboratory Notebook (you will be given 1 at the beginning of the year – don’t lose it!!!) activated account on school computer network

ASSIGNMENTS/HOMEWORK:You are responsible for what is covered in class. To succeed, you must come to class prepared and keep up with

the assigned homework, assignments (including, but not limited, to research papers and projects), and labs. I will check for the completion of homework at the beginning of class and may occasionally collect and grade it. Homework will account for approximately 15% of your grade.

Absences: If you are absent, you must take the initiative to make up any work missed, such as class notes, worksheets, homework, etc. In accordance with school policy, you have the same number of days absent to make up missed work. If you are absent the day an assignment is due, it is to be turned in the day you return.

Late Policy: All assignments are to be submitted on the specified due dates. You are responsible for knowing your assignments and their due dates. Assignments will not be collected late. Instead, homework will be assessed for completion on the due date with partial credit given. This is at the instructor’s discretion.

Don’t procrastinate in getting help if you need it.

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 (which must be written in your lab notebook), 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. Late labs will follow the same late policy previously noted.

Although data may be shared with a lab partner, the body of the lab is individual work and copying will NOT be tolerated. Copying will result in a zero for the assignment. Remember, if you lose notebook, you are responsible for replacing the lab notebook and all the labs that have been completed to date.

GRADING:Your grade will be calculated on a total point basis:

Your grade = # of points earned ÷ total number of points possible x 100% An approximate distribution of your grade follows: tests/quizzes will account for approximately 30% of your

grade, laboratory assignments 30%, do nows/notebook check/participation 20%, and homework 20%. Depending on how the marking period progresses, these percentages may change.

CLASS RULES Always do your best. Your best is going to change from moment to moment; it will be different when you are

healthy as opposed to sick. Under any circumstance, simply do your best, and you will avoid self-judgment, self-abuse and regret.

Be impeccable with your word. Speak with integrity and respect. Say only what you mean. Avoid using the word to speak against yourself or to gossip about others. Use the power of your word in the direction of truth and love.

Don’t take anything personally. Nothing others do is because of you. What others say and do is a projection of their own reality, their own dream. When you are immune to the opinions and actions of others, you won’t be the victim of needless suffering.

Don’t make assumptions. Find the courage to ask questions and to express what you really want. Communicate with others as clearly as you can to avoid misunderstandings, sadness, and drama.

There is a no-tolerance policy for lab safety. No exceptions! Cutting class is not acceptable. Don’t even go there. Action taken will be to notify your parents and Assistant

Principal. You will receive no credit nor have an opportunity to make up work that was due or done on that day.o Come to class on time. Remember 3 lates = 1 unexcused absence.

Do your own work. Cheating or plagiarizing will result in a zero for that assignment with no opportunity to make up the work. This includes copying homework, lab work, or allowing your work to be copied.

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.

We will rarely be absent, but on such an occasion, make sure you follow the directions of the substitute teacher to complete the assigned work.

CONSEQUENCES1.Verbal warning2.Teacher detention3.Parent phone call 4.Administrative referral5. Immediate removal from the classroom at discretion of the teacher

CLASS PROCEDURES/ROUTINES: Arrive to class on time. Three lates equals one unexcused absence. Be prepared and on time~ Enter the room quietly and be ready to work each day. This includes having your

materials (notebook, writing instrument, and assignments) and your minds ready to work when the bell rings. Clean up after yourselves and make sure the room is neat. I am not your mom. We will review other classroom activity procedures at the time of the activity. Get into the course, give it your best effort, and enjoy it.

EXTRA HELP: I will be available for extra help on Monday, Wednesday and Thursday after school usually in room 337. On

occasion, you may also find me in 316 or 144. Please come if you need assistance or if you have any concerns.

CCHEMISTRYHEMISTRY ~ S ~ SYLLABUSYLLABUS**Instructor reserves the right to change or alter the syllabus at any time.**

Text: Chemistry (© 2002) by Addison-Wesley.

A. Unit 1: Introduction to Chemistry and Matter 1. Objectives:

a. Define chemistry and matter.b. Define observation, hypothesis, experiment, theory, and law in scientific process.c. Apply the scientific method of investigation.d. Define energy and distinguish between kinetic and potential energy.e. Explain the law of conservation of mass-energy.f. Describe and distinguish between mixtures and pure substances, homogeneous and heterogeneous

substances, elements and compounds.g. Differentiate between physical and chemical properties of matter.h. Distinguish physical and chemical changes in matter.i. Explain the relationship between chemical change and energy.j. Review lab techniques, equipment, and safety.

2. Laboratory/Assignmentsa. Laboratory Techniques, Equipment, and Safetyb. Candle observationsc. Evidence of Interaction-Copper II Chlorided. Physical and Chemical Change

3. Homework

B. Unit 2: The Measurement of Matter and Problem Solving 1. Objectives:

a. List and use the SI base/or derived units for mass, length, volume, time, and temperature.b. Express and convert quantities using the common SI prefixes.c. Use the factor-label (dimensional analysis) to obtain the desired unit in solving problems.d. Use significant figures to express the exactness of measurements.e. Express any number in scientific notation.f. Make use of scientific notation in addition, subtraction, multiplication, and division.g. Compare and contrast the accuracy and precision of a measurement.h. Determine the densities of different substances.i. Perform calculations using density measurements.

2. Laboratory/Assignmentsa. Density of metalsb. Density and Pennies.c. Coke Density and Accuracy and Precision of Lab Glassware.

3. Homework

C. Unit 3: Atomic Structure and Theory 1. Objectives:

a. Discuss the Dalton’s atomic theory.b. Discuss the historical development of the atomic theory and contributions from Thompson,

Rutherford, Bohr, and Schrodinger.c. Identify and describe the three fundamental particles of the atom and how they are arranged in or

about the nucleus.d. Define atomic number and atomic mass and use them to fine the number of protons, neutrons, and

electrons in an atom.e. Describe how atoms of isotopes of an element differ and explain why atomic masses are not whole

numbers.f. Calculate the average atomic mass given the isotope distribution of an element.g. Draw electron-dot diagrams for the elements, monatomic ions, and excited state atoms.

2. Laboratory/Assignmentsa. Periodic Table Postersb. Beanium Lab

3. Homework

D. Unit 4: Electron Configuration1. Objectives:

a. Differentiate between frequency and wavelengtha. Recognize general shape of s, p, d, f atomic orbitals.b. Identify the number of electrons in the outermost energy level.c. State the importance of a noble gas configuration and explain and use the octet rule.

2. Laboratory/Assignmentsa. Spectroscopy and Flame Testb. Electron Hotel

3. Homework

E. Unit 5: Periodic Table 1. Objectives:

a. Describe the early attempts at classifying elements.b. State the Periodic Law.c. Explain the basis for the arrangement of the modern periodic table.d. Recognize the organization of the periodic table into s, p, d, and f blocks.e. Use the periodic table to predict the electron configurations of elements.f. Identify metals (alkali, alkaline earth, transition, inner transition), nonmetals, metalloids, halogens,

and noble gases on the periodic table.g. Summarize the characteristics for families of elements. h. Explain the periodic trends (atomic radii, ionic radii, ionization energy, electronegativity, oxidation #)i. Explain how the shielding effect and increased nuclear charge influences periodic trends.

2. Laboratory/Assignmentsa. Patterns puzzleb. Periodic table puzzlesc. Periodic Properties (Group II and IV)

3. Homework

F. Unit 6: Chemical Names and Formulas 1. Objectives:

a. Write the symbol and charge for monatomic and polyatomic ions.b. Demonstrate proficiency in naming an ionic or molecular compound when given the formula.c. Demonstrate proficiency writing the formula of an ionic or molecular compound when given the

name.d. Calculate formula weight (ionic compound) or molecular weight (covalent compound).e. Using sample problems, show how different samples of the same compound obey the law of definite

proportions.f. Show that two different compounds composed of the same tow elements obey the law of multiple

proportions.g. Calculate the % composition of a substance in a mixture.h. Calculate the % composition of an element in a pure substance given the formula.

2. Laboratory/Assignmentsa. Flash cardsb. Percent of sugar in gumc. Percent KClO3

d. Percent water in hydrate (copper sulfate pentahydrate)3. Homework

G. Unit 7: Chemical Bonding 1. Objectives:

a. Define ionic, covalent, metallic bonds.b. Identify the type of bonding between two elements given their electronegativities.c. Given a list of properties, match the type of bonding with the correct properties.d. Describe the formation of a cation from an atom of a metallic element.e. Describe the formation of an anion from an atom of a nonmetallic element.f. Recognize an ionic bond as the electrostatic attraction between a cation and an anion.g. Recognize a covalent bond (between two non-metallic elements) as the sharing of electrons. h. Use electronegativity values to determine whether a bond is polar or non-polar covalent bonds. i. Use the theory of metallic bonds to explain the physical properties of metals.j. Distinguish between polar and nonpolar covalent bonds.

2. Laboratory/Assignmentsa. Classification of Chemical Compoundsb. Molecular Models

3. Homework

H. Unit 8: Mole Concept and Stoichiometry 1. Objectives:

a. Use Avogadro’s constant to define the mole.b. Identify the representative particle of elements and compounds.c. Calculate the number of representative particles of any substance given

the number of moles (and visa-versa).d. Calculate the mass of any substance given the number of moles (and visa-

versa).e. Calculate the volume of a gas (@STP) of any substance given the number of moles (and visa-versa).

2. Laboratory/Assignmentsa. Aluminum Foil Thicknessb. Determination of an Empirical Formula.c. Calculate mass of magnesium

3. Homework

I. Unit 9: Chemical Reactions 1. Objectives:

a. Define reactants and products and interpret symbols used in writing equations.b. Write a word equation and a formula equation given a description of a chemical reaction. c. Balance a chemical reaction using coefficients.d. Classify reactions as synthesis, decomposition, single replacement, double replacement, or

combustion.e. Use the activity series of metals to predict the products of single-replacement reactions.

2. Laboratory/Assignmentsa. Five Types of Chemical Reactionsb. Precipitation Reactions

3. Homework

J. Unit 10: Stoichiometry 1. Objectives:

a. Construct mole ratios from balanced chemical equations for use as conversion factors in stoichiometric problems.

b. 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.

c. Calculate actual yield and theoretical yield.2. Laboratory/Assignments

a. Aluminum Foil Thicknessb. Determination of an Empirical Formula.c. Calculate mass of magnesium

3. Homework

K. Unit 11: States of Matter and Heat1. Objectives:

a. Differentiate among the four states of matter.b. Explain the nature of liquids, KE and intermolecular forces.c. Define vapor pressure and boiling point.d. Explain the nature of solids, KE and intermolecular forces.e. Characterize a heating curve in terms of changes in energy and physical state f. Analyze a phase diagram for changes in state, the triple point, and critical point.g. Define internal heat(q), work(w), enthalpy(H)).h. Investigate calorimetry as a method for measuring energy changes.i. Perform calculations involving specific heat.j. Associate the enthalpy of a reaction with an exothermic or endothermic process.k. Write thermochemical equations and perform quantitative calculations on heat loss or gain.

2. Laboratory/Assignmentsa. Melting and Cooling Curveb. Boiling point democ. Specific heat of metalsd. Enthalpy of fusion for icee. Enthalpy of solution

3. Homework

L. Unit 12: Gas Laws 1. Objectives:

a. Explain the concept of an Ideal gas.b. Describe the conditions of standard temperature and pressure.c. Relate the laws of Boyle, Charles, Gay-Lussac, and Dalton and perform calculations using these laws.d. Explain the significance of absolute zero. Know its value in both °C and K and be able to convert

between the two temperature scales.e. Convert between units of pressure (kPa, atm, mm Hg).

2. Laboratory/Assignmentsa. Boyle’s Law: Pressure-Volume Relationship in Gases (CBL).b. Gay-Lussac’s Law: Pressure-Temperature Relationship in Gases c. Charles Law: Temperature-Volume

3. Homework

M. Unit 13: Solutions 1. Objectives:

a. Define the terms solution, solute, solvent.b. Explain the differences between a saturated, supersaturated, unsaturated, solution.c. Distinguish among electrolytic and non-electrolytic solutions.d. Distinguish between solutions, colloids, and suspensions.e. Explain factors that affect solubility.f. Use Henry’s Law to explain gas solubility.g. Describe the process of solvation and use the “like dissolves like” rule to predict solubility.h. Explain the factors that define how fast a substance will dissolve.i. Use solubility curves.j. 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. k. Solve problems involving molarity.

2. Laboratory/Assignmentsa. Solutions of Sodium Acetate b. Molarity of NaCl Solutionc. Molarity and Density

3. Homework

N. Unit 14: Reaction Rate and Chemical Equilibrium 1. Objectives:

a. List and describe the factors that influence the rate of reaction.b. Define activation complex and activation energy.c. Use LeChatelier’s principle to explain the effects of changes in concentration, pressure, and

temperature on the equilibrium system.2. Laboratory/Assignments

a. Iodine Clock reaction3. Homework

O. Unit 15: Acids, Bases, and Salts 1. Objectives:

a. Identify the properties of acidic and basic solutions.b. Discuss Arrhenius acids and bases.c. Name and write the formula for common acids and bases.d. Given hydrogen ion or hydroxide ion concentration, classify a

solution as neutral, acidic, or basic.e. Explain how the pH scale is used for measuring solution acidity.f. Calculate pH/pOH given molar concentrations of

hydronium/hydroxide ions and vice-versa.g. Explain the concept of neutralization, the process of titration and perform calculations using the data

from titrations.2. Laboratory/Assignments

a. The Acetic Acid Content of Vinegar by Titration3. Homework

O. Unit 16: Nuclear Chemistry 1. 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….

2. Prepare a PowerPoint presentation for the class.