Platte Canyon High School

Mathematics and Science

Chemistry Syllabus

Platte Canyon High School

January 29, 2001 – June 8, 2001

General Information

This class meets every school day for 90 minutes from 7:25 – 8:55.

Instructor Information

Debbi Marks

Platte Canyon High School, Room 215

303-838-4642 Ext 219  All homework and class information will be on my voicemail each night.

email:  debbimarks@uswest.net

Website for the class:  http://plattecanyonms.tripod.com

            Class information for chemistry is located on this website under my name.

I am available before school, after school and during 3^rd period for questions or extra help.  You may drop in or make an appointment to see me.

Course Prerequisites

Algebra 2

Textbook

Chemistry.  Wilbraham, Staley, Matta, Waterman. Prentice Hall. 2000.

Classroom Procedures and Grades

Instruction in chemistry will include a variety of activities.  Lecture and discussion, demonstrations, lab activities, homework, computer activities, quizzes and tests will all be used regularly.  Students are expected to actively participate in all of these activities.  Class discussion is important to assist understanding and to build on the ideas presented.  Questions are encouraged to promote understanding and interest.

Frequent tests and quizzes will be used to monitor the progress of students.  “Pop” quizzes will be given to ensure that students keep up with their work and understanding.

Grades will be based on the accumulation of points.  All assignments, activities and assessments will be worth points.  In addition, students will be asked to self-evaluate many assignments as well as their learning dynamics (see attached).

Late work is discouraged.  Homework is due at the beginning of the period, completed.  If work is one day late there will be a 25% - 50% penalty.  Work will not be accepted after one day late.  Major projects are due on the due date regardless of absence or other circumstances.

Students are to submit only their own work for evaluation and to acknowledge the work and conclusions of others and to do nothing that would provide an unfair advantage in their academic efforts.  Cheating is unacceptable.  All work for this class is to be unique.  Any copied work, including homework is cheating.  Those students who give as well as receive for the purposes of cheating are both guilty and will receive the same penalty.  This applies to all work for this class. Working together as a team to discuss chemistry is acceptable but each person should write answers and solve calculations on their own.  Comparing answers on homework or classwork is acceptable.  If you have any questions about what is acceptable, please ask!

Materials

Each student will need their book, notebook with paper, calculator, pencils, pens and a grading pen of a different color to grade homework.

Expectations

●          You are expected to assume responsibility for your own learning as this is an honors class.  You are expected to ask questions to clarify your understanding and to enhance your learning experience.

●          You are expected to attend class and be on time.

●          All assignments must be turned in.

●            Homework should be done in one color and graded in another color.  You are encouraged, after the homework is returned, to correct mistakes.  If you have any questions, please ask in class or at another time.  It is important for you to understand what we are doing and I am happy to help in any way I can.

●          You are expected to actively participate in classroom discussions and activities.

●          Each student must bring their materials each day.

●          Each student is expected to keep an organized notebook with all of their chemistry materials.  This should be brought to class every day.

●          Any test grade lower than a C must schedule a conference with Mrs. Marks within the next 24 hours to correct mistakes and relearn the material.

●          Group work should be turned in with all names of the group.

●          All books are to be covered for the entire year.

Course Objectives

I.                    Introduction to Chemistry

A.                 Define chemistry and differentiate among its traditional divisions.

B.                 Describe the steps involved in the scientific method.

C.                 Distinguish between a theory and scientific law.

II.                 Matter and Change

A.                 Identify the characteristics of matter and substances.

B.                 Differentiate among the three states of matter.

C.                 Define physical property and list several common physical properties of   substances.

D.                 Categorize a sample of matter as a substance or a mixture.

E.                  Distinguish between homogeneous and heterogeneous samples of matter.

F.                  Explain the difference between an element and a compound.

G.                 Identify the chemical symbols of common elements and name common elements given their symbols.

H.                 Differentiate between physical and chemical changes in matter.

I.                   Apply the law of conservation of mass.

III.               Scientific Measurement

A.                 Distinguish between quantitative and qualitative measures.

B.                 Convert measurements to scientific notation.

C.                 Distinguish among the accuracy, precision and error of a measurement.

D.                 Identify the number of significant figures in a measurement and in the result of a calculation.           

E.                  List SI units of measurement and common SI prefixes.

F.                  Distinguish between the mass and weight of an object.

G.                 Calculate the density of an object from experimental data.

H.                 List some useful applications of the measurement of specific gravity

I.            Convert between the Celsius and Kelvin temperature scales.           

IV.               Problem Solving in Chemistry

A.                 Construct conversion factors from equivalent measurements.

B.                 Apply the techniques of dimensional analysis to a variety of conversion problems.

C.                 Convert complex units using dimensional analysis.

V.                   Atomic Structure and the Periodic Table

A.            Summarize Dalton’s atomic theory.

B.            Describe the size of an atom.

C.            Distinguish among protons, electrons, and neutrons in terms of relative mass and charge.

D.            Describe the structure of an atom, including the location of the protons, electrons, and neutrons with respect to the nucleus.

E.            Explain how the atomic number identifies an element.

F.            Use the atomic number and mass number of an element to find the numbers of protons, electrons, and neutrons.

G.            Explain how isotopes differ and why the atomic masses of elements are not who numbers.

H.            Calculate the average atomic mass of an element from isotope data.

I.            Describe the origin of the periodic table.

J.            Identify the position of groups, periods and the transition metals in the periodic table.

VI.            Chemical Names and Formulas

A.                 Distinguish between ionic and molecular compounds.

B.                 Define cation and anion and relate them to metal and nonmetal.

C.                 Distinguish among chemical formulas, molecular formulas and formula units.

D.                 Use experimental data to show that a compound obeys the law of definite proportions.

E.                  Use the periodic table to determine the charge on an ion.

F.                  Define a polyatomic ion and give the names and formulas of the most common polyatonic ions.

G.                 Apply the rules for naming and writing formulas for binary and ternary ionic compounds.

H.                 Apply the rules for naming and writing formulas for binary molecular compounds.

I.                   Name and write the formulas for common acids.

J.                  Write the name of a compound given its chemical formula.

K.                   Write a chemical formula given the compound name.

VII.            Chemical Quantities

A.                 Describe how Avogadro’s number is related to a mole of any substance.

B.                 Calculate the mass of a mole of any substance.

C.                 Use the molar mass to convert between mass and moles of a substance.

D.                 Use the mole to convert among measurements of mass, volume and number of particles.

E.                  Calculate the percent composition of a substance from its chemical formula or experimental data.

F.                  Derive the empirical formula and the molecular formula of a compound from experimental data.

G.                 *Solve problems involving the molarity of a solution.

H.                 *Describe how to prepare dilute solutions from more concentrated solutions of known molarity.

VIII.          Chemical Reactions

A.            Write equations describing chemical reactions using appropriate symbols.

B.                 Write balanced chemical equations when given the names of formulas of the reactants and products in a chemical reaction.

C.                 Identify a reaction as combinations, decomposition, single-replacement, double replacement or combustion.

D.                 Predict the products of combination, decomposition, single-replacement, double replacement or combustion.

E.                  Write and balance net ionic equations.

F.                  Use solubility rules to predict the precipitate formed in double-replacement reactions.

IX.               Stoichiometry

A.                 Calculate the amount of reactants required or product formed in a non-chemical process.

B.                 Interpret balanced chemical equations in terms of interacting moles, representative particles, masses and gas volume at STP.

C.                 Construct mole ratios from balanced chemical equations, and apply these ratios in mole-mole stoichiometric calculations.

D.                 Calculate stoichiometric quantities from balanced chemical equations using units of moles, mass, representative particles and volumes of gases at STP.

E.                  Identify and use the limiting reagent in a reaction to calculate the maximum amount of product(s) produced and the amount of excess reagent.

F.                  Calculate theoretical yield, actual yield, or percent yield given appropriate information.

X.         State of Matter

A.                 Describe the motion of gas particles according to the kinetic theory.

B.                 Interpret gas pressure in terms of kinetic theory.

C.                 Describe the nature of a liquid in terms of the attractive forces between the particles.

D.                 Differentiate between evaporation and boiling of a liquid, using the kinetic theory.

E.                  Describe how the degree of organization of particles distinguishes solids from gases and liquids.

F.                  Distinguish between a crystal lattice and a unit cell.

G.                 Explain how allotropes of an element differ.

H.                 Interpret the phase diagram of water at any give temperature and pressure.

I.                   Describe the behavior of solids that change directly to the vapor state and recondense to solids without passing through the liquid state.

XI.               Thermochemistry – Heat and Chemical Change

A.                 Explain the relationship between energy and heat.

B.                 Distinguish between heat capacity and specific heat.

C.                 Construct equations that show the heat changes for chemical and physical processes.

D.                 Calculate heat changes in chemical and physical processes.

E.                  Classify, by type, the heat changes that occur during melting, freezing, boiling, and condensing.

F.                  Apply Hess’s law of heat summation to find the heat changes for chemical and physical processes.

G.                 Calculate heat changes using standard heats of formation.

XII.             The Behavior of Gases

A.                 Describe the properties of gas particles.

B.                 Explain how the kinetic energy of gas particles relates to Kelvin temperature.

C.                 Explain how the amount of gas and the volume of the container affect gas pressure.

D.                 Infer the effect of temperature changes on the pressure exerted by a contained gas.

E.                  State Boyle’s Law, Charles’s Law, Gay-Lussac’s Law and the combined gas law.

F.                  Apply the gas laws to problems involving the temperature, volume, and pressure of a contained gas.

G.                 Calculate the amount of gas at any specified conditions of pressure, volume, and temperature.

H.                 Distinguish between ideal and real gases.

I.                   State Avogadro’s hypothesis, Dalton’s Law and Graham’s Law.

J.                  Calculate moles, masses and volumes of gases at STP.

K.                 Calculate partial pressures and rates of effusion.

XIII.          Electrons in Atoms

A.                 Summarize the development of atomic theory.

B.                 Explain the significance of quantized energies of electrons as they relate to the quantum mechanical model of the atom.

C.                 Apply the aufbau principle, the Pauli exclusion principle, and Hund’s rule in writing the electron configurations of elements.

D.                 Explain why the electron configurations for some elements differ from those assigned using the aufbau principle.

E.                  Calculate the wavelength, frequency, or energy of light, given two of these values.

F.                  Explain the origin of the atomic emission spectrum of an element.

XIV.           Chemical Periodicity

A.                 Explain why you can infer the properties of an element based on those of other elements in the periodic table.

B.                 Use electron configurations to classify elements as noble gases, representative elements, transition metals, or inner transition metals.

C.                 Interpret group trends in atomic radii, ionic radii, ionization energies, and electronegativities.

D.                 Interpret periodic trends in atomic radii, ionic radii, ionization energies and electronegativities.

XV.             Ionic Bonding and Ionic Compounds

A.                 Use the periodic table to infer the number of valence electrons in an atom and draw its electron dot structure.

B.                 Describe the formation of cations from metals and of anions from nonmetals.

C.                 List the characteristics of an ionic bond.

D.                 Use the characteristics of ionic compounds to explain the electrical conductivity of ionic compounds when melted and when in aqueous solutions.

E.                  Use the theory of metallic bonds to explain the physical properties of metals.

F.                  Describe the arrangements of atoms in some common metallic crystal structures.

XVI.            Covalent Bonding

A.                 Use electron dot structures to show the formation of single, double and triple covalent bonds.

B.                 Use electronegativity to classify a bond as nonpolar covalent, polar covalent or ionic.

C.         Name and describe the weak attractive forces that hold groups of molecules together.

Last Updated February 17, 2001             visits to this site!

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