"A mind, once stretched, can never return to its old dimensions"

CP CHEMISTRY VOORHEES, 2017-2018ROOM 317

Course Objectives:

to apply scientific methods of inquiry, math, computer tools, and interdisciplinary connections in your study of chemistry

to gain an in-depth 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

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

Materials: 3-ring binder (1 inch-for chemistry only), 3-hole punch paper, dividers or folders, blue or black pens, pencilsCalculator (must have log and exponent, graphing a plus)Activated account on school computer network

Assignments/ You are responsible for what is covered in class. To succeed, you must Homework: 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 approximately 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 advanced, 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 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.

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: An approximate distribution of your grade follows. Some special assignments/projects will be counted as a laboratory or quiz grade. Grades are calculated on a points system and these percentages are approximate.Tests/Quizzes 45%Laboratory 35%Do Now 10%Homework 10% Total- 100%

Conduct: Arrive to class on time. 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:1. My expectations are that we will treat each other with respect and courtesy. 2. Enter the room quietly and be ready to work each day.3. Avoid language that insults, hurts, or offends others. 4. Remain seated until the bell rings.5. No cell phones should be visible during instruction.6. Leave the room neat. This is a shared space as well as our “home” for the

year. Keep it clean.

Consequences:1. verbal warning2. teacher detention3. parent phone call 4. immediate removal from the classroom at discretion of the teacher5. administrative referral

CP CHEMISTRY – SYLLABUS 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 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. Recognize general shape of s, p, d, f atomic orbitals.h. Identify the number of electrons in the outermost energy level.i. State the importance of a noble gas configuration and explain and use the

octet rule.j. Draw electron-dot diagrams for the elements, monatomic ions, and excited

state atoms.2. Laboratory/Assignments

a. Flame Testsb. Gas tubes and spectroscopes

3. Homework

D. Unit 4: 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/Assignments

a. Patterns puzzleb. Periodic table puzzlesc. Periodic Properties (Group II and IV)

3. Homework

E. Unit 5: 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

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/Assignments

a. Flash cardsb. Percent of sugar in gumc. Percent KClO3

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

G. Unit 7: 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/Assignments

a. Five Types of Chemical Reactionsb. Precipitation Reactions

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)..

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

g. 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.

h. 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

I. Unit 9: States of Matter 1. 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.2. Laboratory/Assignments

a. Melting and Cooling Curveb. Boiling point demo

3. HomeworkJ. Unit 10: 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/Assignments

a. 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

K. Unit 11: Thermochemistry 1. Objectives:

a. Define internal heat(q), work(w), enthalpy(H)).b. Investigate calorimetry as a method for measuring energy changes.c. Perform calculations involving specific heat.d. Associate the enthalpy of a reaction with an exothermic or endothermic

process.e. Write thermochemical equations and perform quantitative calculations on heat

loss or gain.2. Laboratory/Assignments

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

3. Homework

L. Unit 12: 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 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/Assignments

a. Solutions of Sodium Acetateb. Molarity of NaCl Solutionc. Molarity and Density

3. HomeworkM. Unit 13: 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/Assignmentsa. Iodine Clock reaction

3. Homework

N. Unit 14: 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 17: Nuclear Chemistry 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….

Prepare a PowerPoint presentation for the class.