CCHEMISTRYHEMISTRY VOORHEES HIGH SCHOOL, 2016-2017

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

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 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 10% 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. Reminder – Labs must be made up immediately! After 2 late bus days labs will be taken down.

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.

QUIZZES:Quizzes are usually announced, although they may be unannounced. Questions for quizzes may come from

notes, video, worksheets, lab activities, and class discussions. Be prepared to take a quiz the day it is scheduled, even if you were absent any day before. If you are absent the day of a quiz, you must take it the day you return. (Exceptions will be made for extended absences, at the instructor’s discretion). You are responsible for scheduling a make-up for a quiz with the teacher immediately upon return. In general, a make-up quiz 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. 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.

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: quizzes will account for approximately 35% of your grade,

laboratory assignments 30%, homework 25%, and participation 10%. Depending on how the marking period progresses, these percentages may change.

Alternative assessments include:o Chemistry at Home ~ poster and demonstration.

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.

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.

CONSEQUENCES

CCHEMISTRYHEMISTRY VOORHEES HIGH SCHOOL, 2016-2017

1.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: We are available for extra help on Monday, Wednesday and Thursday after school. Please come if you

need assistance or if you have any concerns.CCHEMISTRYHEMISTRY ~ S ~ SYLLABUSYLLABUS

A. Unit 1: Introduction To Chemistry (Matter, Change, and Energy) 1. Objectives:

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

heterogeneous substances, elements and compounds.h. Differentiate between physical and chemical properties of matter.i. Distinguish physical and chemical changes in matter.j. Review lab techniques, equipment, and safety. k. List and use the SI base/or derived units for mass, length, volume, time, and temperature.l. Express and convert quantities using the common SI prefixes..m. Use the factor-label (dimensional analysis), to obtain the desired unit in solving problems.n. Use significant figures to express the exactness of measurements.o. Express any number in scientific notation.p. Compare and contrast the accuracy and precision of a measurement.q. Determine the densities of different substances.r. Perform calculations using density measurements.s. Learn and apply the rules of good graphing.

2. Laboratory/Assignments a. Candle Observations

b. UV beads and scientific method.c. Evidence of Interaction (Copper Chloride)d. Product Labelse. Why do I have to study chemistry?f. Laboratory Techniques, Equipment, and Safetyg. Physical and Chemical Change h. Density of Metalsi. Density using Pennies.

3. Homework

B. Unit 2: Atomic Structure 1. Objectives:

a. Discuss the Dalton’s atomic theory.b. Identify and describe the three fundamental particles of the atom and how they are arranged in or

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

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

whole numbers.e. Learn the names and symbols for ~40 elements.

2. Laboratory/Assignmentsa. Flame Testsb. Felt-tip electron distributions

c. Element bingod. Element flash cards

3. HomeworkC. Unit 3: Periodic Table Trends

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 (periods and groups or

families).d. Be able to classify an element as a metal, non-metal, metalloid, halogen, or noble gas.e. Summarize some general characteristics for families of elements. f. Explain the periodic trends (atomic radius, ionization energy, electronegativity)g. Using the periodic table, identify the number of electrons in the outermost energy level and write

their Lewis structures.h. State the importance of a noble gas configuration and explain and use the octet rule.i. Describe the formation of a cation from an atom of a metallic element.j. Describe the formation of an anion from an atom of a nonmetallic element.

2. Laboratory/Assignmentsa. Chemical Comic Projectb. Patterns puzzlec. Periodic table posterd. Periodic table puzzlese. Periodic Properties (Group II and

IV)3. Homework

D. Unit 4: Formula Writing1. Objectives:

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

2. Laboratory/Assignmentsa. Flash cards (Ions)b. Formula writing activity

3. Homework

E. Unit 5: Gram Formula Weights and Percent Mass 1. Objectives:

a. Calculate formula weight b. Distinguish between empirical and molecular formulas.c. Calculate the % composition of a substance in a mixture.d. Calculate the % composition of an element in a pure substance given the formula.

2. Laboratory/Assignmentsa. Percent Sugar in Gumb. Percent with M&M’sc. Percent of water in a hydrate (Copper sulfate)

d. Percent Composition of KClO3

e. Percent of water in popcorn3. Homework

F. Unit 6: 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.2. Laboratory/Assignments

a. Five Types of Chemical Reactions b. Precipitation Reactions and Naming Compounds

3. Homework

G. Unit 7: Bonding1. Objectives:

a. Differentiate between covalent and ionic bonding.b. Explain how electronegativity changes when looking at the periodic table.

2. Laboratory/Assignmentsa. Bonding Lab

3. Homework

H. Unit 8: Factor Labeling1. Objectives:

a. Convert between unitsb. Mole conversions

2. Laboratory/Assignmentsa. Mole boxesb. “The Jole” Bean Labc. Various Worksheets

3. Homework

I. Unit 9. 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. Convert from moles to volume to particles.

2. Laboratory/Assignmentsa. Smores Activityb. Intro to Stoichiometry Activityc. Mass of Magnesium

3. Homework

J. Unit 10: Phase Changes1. Objectives:

a. Explain the nature of liquids, KE and intermolecular forces.b. Define vapor pressure and boiling point.c. Explain the nature of solids, KE and intermolecular forces.d. Characterize a heating curve in terms of changes in energy and physical state (melting, boiling,

sublimation).e. Analyze a phase diagram for changes in state, the triple point, and critical point.

2. Laboratory/Assignmentsa. Phase Change Lab

3. Homework

K. Unit 11: Thermochemistry (Heat)1. Objectives:

a. Define heat (q) and enthalpy (H).b. Perform calculations involving specific heat (Cp).c. Investigate calorimetry for the measurement of heat changes and

identification of a substance.d. Perform calculations involving enthalpy of phase changes.e. Associate the enthalpy of a reaction with an exothermic or endothermic

process.2. Laboratory/Assignments

a. Specific heat of metalsb. Enthalpy of fusion of icec. Enthalpy of solution

3. Homework

L. Unit 12: Gas Laws 1. Objectives:

a. Explain the concept of an Ideal gas.b. List and explain the postulates of the Kinetic Molecular Theory.c. Describe pressure and temperature in terms of molecular motiond. Describe the conditions of standard temperature and pressure. e. Explain the significance of absolute zero. Know its value in both °C and K and be able to convert

between the two temperature scales.f. Convert between units of pressure (kPa, atm, mm Hg).g. Relate the laws of Boyle, Charles, Gay-Lussac, and combined gas law and perform calculations

using these laws.h. Explain and use the ideal gas equation. Solve problems involving change of more than one

condition.2. Laboratory/Assignments

a. Introduction to the Gas Lawsb. Gay-Lussac’s Law: Pressure-Temperature Relationship in Gasesc. Boyle’s Law: Pressure-Volume Relationship in Gases (CBL)d. Charles’ Law: Temperature-Volumee. Crushing soda cansf. Sucking eggs into flasks

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. Explain factors that affect solubility.d. Describe the process of solvation and sue the “like dissolves like” rule to predict solubility.e. Explain the factors that define how fast a substance will dissolve.f. Use solubility curves.g. 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. 2. Laboratory/Assignments

a. Solutions of Sodium Acetateb. Temperature vs solubilityc. Molarity of NaCl Solution-Layer different densities

3. Homework

N. Unit 14: Acids and Bases1. Objectives:

a. Identify the properties of acidic and basic solutions.b. Distinguish between acids and bases.c. Use different indicators to distinguish acids and basesd. Name and write the formula for common acids and bases.e. Explain how the pH scale is used for measuring solution acidity.f. Review reactions of acids with metals, carbonates and bases.g. Explain the concept of neutralization, the process of titration and perform calculations using the

data from titrations.2. Laboratory/Assignments

a. Indicators and household chemicalsb. Reacting acids and metalsc. Reacting acids with carbonatesd. The Acetic Acid Content of Vinegar by Titratione. Measuring pH

3. Homework

O. Unit 15: Reaction Rates1. Objectives:

a. Investigate how temperature, concentration, stirring and surface area affect the rate of reaction. 2. Laboratory/Assignments

a. Reaction Rate Lab3. Homework

P. Unit 16: Chemistry At Home (Poster and Demonstration)This assignment requires you to illustrate a basic concept in chemistry using a common household product. We will brainstorm ideas together and you will choose a product to investigate. You will design a poster that describes the product and devise a demonstration that describes the chemistry.