HONORS CHEMISTRYCOURSE OF STUDY

Revised September 2003

HONORS CHEMISTRY

TABLE OF CONTENTS

PAGE #PREREQUISITES 3

POPULATION 3

RATIONALE 3

GOALS 4

OBJECTIVES 5

COURSE OUTLINE 11

COURSE OUTLINE – LABORATORY ACTIVITIES 14

BIBLIOGRAPHY 15

PORTFOLIO AND PERFORMANCE ASSESMENT 16

PROFICENCY STATEMENTS 17

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HONORS CHEMISTRY

The Honors Chemistry, a whole year course, is usually given to 10th and 11th grade students in the honors science track. Students earn 7 science credits at the successful completion of this course.

PREREQUISTITES

The prerequisites for honors Chemistry are:Successful completion of Algebra I course with at least of 85% average. Successful completion/or concurrent enrollment in Geometry.It is advised that the student has had or is taking Algebra-Trigonometry .

POPULATIONThe course is intended primarily for 10th and 11th grade students that never took chemistry before. There are two target populations for the Honors Chemistry class. The first group are students that wish to pursue a careers in the sciences and related areas. The second population is comprised of those students who do not wish to pursue a science career, but want to experience the challenge of a high level science class.

RATIONALE

The Honors Chemistry is a frst year accelerated chemistry course taught to highly motivated students interested to continue their education in the sciences and medical professions. It involves highly technical concepts, integration of mathematical analysis in chemical theories and practical applications to laboratory problems. Principles and concepts are mainly developed through an inquiry approach. Greater emphasis is placed on chemical calculations, problem solving and laboratory experiences. Investigations will include the use of instrumentation such as electronic balances, and Computer Based Laboratories (Texas Instruments). The patterns and regularities to be found in experimental observations are then correlated to reveal models or theories which are used in chemistry.

In the course an awareness of the significance of scientific activities in past as well as in shaping the future of man and his world will be conveyed. Students will understand and wisely judge the growing impact of technology on their physical and social environment.

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HONORS CHEMISTRY

GOALS

1. To make the student aware of the interaction of matter and energy as viewed by the chemist.

2. To extend the students ability to accurately collect, sort, and interpret data in scientific manner.

3. To increase the students quantitative skills in applying appropriate mathematical tools to problem solving.

4. To increase student awareness that they live in a technical world with technical problems and that they must understand the basic laws of nature in order to be responsible citizens in their adult life.

5. To increase the students ability to question, probe, and think critically and to logically apply chemical principles to practical problems.

6. To understand that all science is a study of nature and that chemistry is an integral part of that investigation.

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HONORS CHEMSITRYCOURSE OBJECTIVES

Unit I. Introduction1. Identify problems that can be solved using the Scientific method.2. Differentiate between elements, compounds, and mixtures.3. Identify the physical and chemical properties of substances and differentiate between

physical and chemical changes.4. Use the SI system of measurements, scientific notation, and significant figures in problem

solving and laboratory data collection.

Unit II. Atomic Theory1. Describe and explain evidence for the Atomic Theory.2. Summarize the experiments of Thomson, Rutherford, and Milliken3. Describe the components of the atom.4. Differentiate among the electron, proton, and neutron, and indicate the electrical charge

and relative mass associated with each particle.5. Define isotope, nucleon, and nuclide.6. Define atomic number and mass number and their relationship to isotopes.7. Differentiate between molecule, ion, and atom.8. Differentiate between chemical symbols and chemical formulas.9. Given a formula, state the number of atoms of each element present.10. Name ionic and molecular compounds.11. Write formulas for ionic and molecular chemical compounds.12. Name the common acids.13. Use the Periodic Table as a reference

Unit III. Mass relationships in Chemistry; Stoichiometry1. Given a formula, state the number of atoms of each element present.2. Differentiate between molecular, structural, and empirical (simplest) formulas and derive

empirical formulas from experimentally determined percent composition of an unknown compound.

3. Calculate the molecular or formula mass of any substance.4. Given the masses and abundance of the isotopes of an element, calculate the average

atomic mass. 5. Define the mole (Avogadro’s constants) and relate it to gram atomic mass.6. Define percentage composition and calculate the percentage composition for any given

compound (including hydrates).7. Determine the empirical formula of a substance from experimental percentage composition

data, or from a given number of grams.8. Given the molecular mass and the empirical formula, calculate the molecular formula.

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Unit IV. Chemical Reactions1. Define chemical reaction, and list the reactants and products in a given reaction.2. Distinguish between synthesis, decomposition, single replacement, double replacement,

and combustion reactions.3. Write and balance equations to represent reactions.4. Use a balanced equation to relate the numbers of moles or grams of reactants and products.5. Given the numbers of moles or grams of each reactant, determine the limiting reactant and

calculate the theoretical yield of product.6. Relate the actual yield of product to the theoretical yield and percent yield.7. Describe oxidation-reduction in terms of oxidation numbers, electron loss and gain.8. Determine experimentally the stoichiometric relationship between reactants and products

using a single replacement reaction such as Fe(s) + Cu+2(aq) → Fe+3(aq) + Cu(s).

Unit V. Gas Laws1. Explain the concept of an ideal gas.2. Use the Combined Gas Law (Boyle’s, Charles’, and Gay-Lussac’s) to solve problems

involving the change of more than one condition of gases.3. Derive the ideal gas equation and use it to solve gas law problems in solving problems.4. Using the ideal gas equation calculate the density or molar mass of a gas.5. Use Dalton’s Law to find partial pressure of a gas in a mixture; relate partial pressure to

mole fraction.6. Relate the volumes of reacting gases (measured at the same temperature and pressure) in a

reaction.7. List and explain the basic assumptions of the Kinetic Theory of Gases.8. List properties of real gases that are responsible for the deviations of gases from ideal gas

behavior.9. Define diffusion and effusion; use Graham's Law to determine the relative rates of

diffusion of various gases.10. Determine the molar volume of a gas in the laboratory.

Unit VI. Electronic Structure and the Periodic Table1. Differentiate between a continuous and line spectra.2. Use the Bohr Theory to calculate the energy of an electron in a given principal energy level

of the hydrogen atom.3. Explain the wave-particle duality of the electron.4. List the four quantum numbers and describe their significance.5. Given the atomic number of an element, or its position in the periodic table, write its

electron configuration using orbital notation, electron configuration, or electron dot notation (Lewis structure).

6. Relate the electron configuration of the elements to the trends in the properties of the elements.

7. Describe the historical background that led to the development of the Periodic Table. 8. Predict trends in the Periodic Table with respect to atomic radius, ionization energy,

electronegativity, electronaffinity, and metallic character.

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9. Use a simulation experiment to demonstrate the nature of the electron in the hydrogen atom.

Unit VII. Chemical Bonding1. Describe and distinguish between ionic, covalent, and metallic bond.2. Differentiate between the properties of ionic and covalent bonds.3. Use Lewis dot structures to show molecular structures.4. Use electronegativities to predict the polarity and bonding of substances.5. Illustrate, using examples, the concept of resonance.6. Predict the shapes and bond angles of simple molecules based on the VSEPR theory.7. Explain the process of hybridization and relate it to sp, sp2, sp3, sp3d, and sp3d2 bonds. 8. Differentiate between sigma and pi bonding.9. Use the bonding theory to explain unsaturated bonds.

Unit VII. Liquids and Solids1. Describe the properties of liquids and solids using the Kinetic Theory of matter.2. Identify all inter- and intermolecular bonds in substances.3. Distinguish among ionic, molecular, network covalent, and metallic solids with regard to

both particle structure and physical properties ( m.p., b.p., conductivity, solubility, etc).4. Explain the causes of vapor pressure for a solid and a liquid and relate vapor pressure to

intermolecular forces.5. Define melting point and boiling point in terms of vapor pressure.6. Define and give examples of critical temperature and critical pressure. 7. Using a phase diagram, determine melting point, boiling point, critical temperature, critical

pressure, and triple point for a substance.8. Define and give examples of sublimation and deposition

Unit VIII. Solutions1. Describe the types and nature of various types of solutions.2. Discuss the factors affecting the solubility of a solute in a given solvent and its rate of

solution.3. Understand the terms saturated , unsaturated, supersaturated, dilute, and concentrated as

they pertain to solutions.4. Compute the concentrations of solutions in percent, molarity and molality.5. Using colligative properties of solutions (Raoult’s Law) explain and solve problems related

to boiling point elevation, freezing point depression, and determination of molecular mass.6. Compare the colligative properties of electrolytes to those of nonelectrolytes.7. Determine experimentally the solubility of an ionic compound in water.8. Determine the freezing point depression of a known solution.

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Unit IX. Chemical Kinetics and Equilibrium1. Define and give examples of reversible reactions.2. List and describe the factors that influence the rate of a chemical reaction.3. Define activation energy and activated complex.4. Describe the effect of reaction mechanism and rate-defining step on the rate of chemical

reaction..5. Given the rate law for a reaction, predict the effect of changes in concentration,

pressure/volume, and temperature on the rate of the reaction.6. Define catalysis.7. Given an equation for a reaction, write the expression for the equilibrium, Keq.8. State the relationship between the relative amounts of products and reactants in a given

reaction using the values of Keq.9. Calculate the equilibrium constant for a reaction, given final concentrations of reactants

and products.10. Calculate the final concentration of a reactant or product using Keq.11. State Le Chatellier’s principle and use it to explain the effects of stress on a reaction.12. Use the solubility product constant, Ksp, to evaluate the solubility of compounds.13. Determine experimentally the rate of a chemical reaction.

Unit X. Calorimetry and Thermochemistry.1. Distinguish between system and surroundings.2. Distinguish between heat energy and temperature. Name the SI units of temperature and

thermal energy.3. Calculate the heat content (thermal energy) of a substance using its specific heat,

temperature and mass.4. Solve calorimetry problems.5. Name the energy associated with a change of state and calculate the energy required to

change a given mass of substance from solid to liquid or liquid to gas.6. Explain the properties of gases, liquids, and solids in terms of the kinetic theory of matter.7. Distinguish between endothermic and exothermic reactions.8. Use thermo chemical equations to describe energy changes in a chemical reaction.9. Explain how energy and entropy both influence the spontaneity of a reaction.10. Determine experimentally the heat absorbed or released in a chemical reaction (burning

of a candle) and during a phase change (heat of fusion of ice).

Unit XI. Acid-Base theory1. Define acids and bases according to the Arhenius, Brönsted, and Lewis theories.2. Given and acid-base reaction identify the acid, base, conjugate acid, and conjugate base.3. Define a strong and weak acid; strong and weak base and give examples for each.4. Given a reaction-taking place in water, write a net ionic equation for the reaction.5. Calculate the ionization constant for acid, Ka, and the percent ionization for a weak acid

and weak base.6. Define ion product constant for water, Kw, and use it to find the ion product constant for

water.

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7. Explain the concept of pH by solving problems.8. Define buffer system, and give examples of buffered solutions.9. Define and describe the use of indicators.

Time Permitting:

Unit XII. Nuclear Chemistry1. Write complete nuclear equations representing nuclear charge.2. Use the half-life concept to solve related problems.3. Differentiate between fission and fusion.

Unit XIII. Electrochemistry1. Differentiate between a galvanic and a voltaic cell.

Calculate the cell potential of a chemical cell2. Make measurements using electrochemical cells.

Unit XIV. Organic Chemistry1. Distinguish between alkanes, alkenes, and alkynes.2. Use functional groups to identify common organic molecules.

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HONORS CHEMISTRYCOURSE OUTLINE

I. IntroductionA. Measurement

1. Metric System (SI), basic algebra, scientific notation2. Significant digits3. Fundamental and derived units4. Factor label method for solving problems

B. Scientific methodC. Matter

1. elements2. compounds3. mixtures4. states of matter

D. Physical and chemical properties and changes

II. Atomic TheoryA. Historical overview

1. Democritus and the atomos2. Thomson’s experiments with cathode ray tubes(the plum pudding model of the

atom)3. Rutherford experiments and the planetary model of the atom4. Bohr atom5. modern model of the atom

B. Components of the atom1. nucleus and energy levels2. protons, electrons, and neutrons3. atomic mass number, atomic number, and isotopes

C. Formulas1. molecular2. empirical

D. Mass relationships1. molar mass determination2. percentage composition

III. Chemical ReactionsA. Reaction types

1. synthesis (Haber industrial process for the production of ammonia)2. decomposition3. single replacement4. double replacement5. combustion (greenhouse gases)6. oxidation-reduction

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B. Writing and balancing chemical equationsC. Formula and equation stoichiometryD. Limiting reactant

IV. Gas lawsA. pressure, volume, and temperatureB. general gas laws(Boyle’s, Gay-Lussacs’, and Charles’ laws)C. mole concept and Avogadro’s HypothesisD. ideal gas law, gas density, gas mole weightE. Graham’s Law of DiffusionE. Kinetic Molecular Theory of gasesF. real gases

V. Quantum Theory/Electron Structure and Periodic TableA. Electron Configuration and Energy Levels

1. spectra; excited and ground state2. quantum numbers3. orbitals

B. Periodic Table1. Historical development2. Periodic variation in properties3. Families and periods; metal, nonmetal, and metalloids4. predicting chemical reactivity

VI. Chemical BondingA. Types of Intermolecular Chemical Bonding

1. ionic2. nonpolar and polar covalent3. metallic

B. Types of Intramolecular Chemical binding1. hydrogen bonding2. van der Waals forces and London dispersion forces3. polar covalent forces

C. Lewis StructuresD. Polarity and electronegativityE. Covalent structures

1. molecular geometry2. hybridization3. resonance4. VSEPR5. geometrical isomers

VII. Solids and LiquidsA. Amorphous and crystalline solidsB. HydratesC. Kinetic model of liquids and solids D. Effect of temperature and pressure on phase changes; triple pointE. Ionic, molecular, metallic, and network covalent compounds

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VIII. SolutionsA. Solution process and energy changesB. Selectivity of solvents; solubility curvesC. Effect of temperature and pressure changes on solubilityD. Calculate concentrations

1. percent2. molarity3. molality

E. Colligative properties

IX. Chemical Kinetics and EquilibriumA. Chemical kinetics

1. factors that influence the rate of chemical equation2. activation energy and activated complex3. collision theory4. catalysts5. simple reaction mechanisms: rate determining step

B. Chemical equilibrium1. equilibrium constant2. LeChatellier’s principle3. effect of temperature, pressure, and concentration changes on equilibrium 4. application of equilibrium concepts to processes for industrial preparation of key

chemicals X. Calorimetry and Thermochemistry

A. Potential and kinetic energyB. Spontaneous changes and stabilityC. Calorimetric determination of heat of reactionsD. Enthalpy, free energy, and entropy and spontaneity

XI. Acid-Base TheoryA. Acid-base theory

1. Arhenius2. Brönsted-Lowry 3. Lewis

B. Strength of acids and basesC. Neutralization reactionD. Ionic equilibriaE. Titrations

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XII. Nuclear ChemistryA. Nuclear structureB. Radioactivity and nuclear stability

1. alpha radiation2. beta radiation3. gamma radiation

C. Nuclear equationsD. Fission and fusionE. Nuclear power: pro and conF. Half-life and nuclide dating

XIII. ElectrochemistryA. Oxidation-reduction reactions B. Balancing redox reactionsC. Voltaic cells: standard electron potentialsD. Application: corrosion, batteries, electroplating

XIV. Organic ChemistryA. Alkanes, alkenes, and alkynesB Functional groupsC. Identify common organic compounds

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HONORS CHEMISTRYBIBLIOGRAPHY

Student Text:Masterton, William L., and Hurley Cecile N. Chemistry: Principles and Reactions, Fourth Edition. Orlando, Florida: Harcourt College Publications, 2001

Additional Resources:Brother Carmen Ciardullo. Micro Action Chemistry, Volumes I and II. Batavia, Illinois: Flynn Scientific Inc. 1999.

Ehrenkrantz, David, and Mauch, John J. Chemistry in Microscale, Book I. Dubuque, Iowa: Kendall/Hunt Publishing Company, 1993.

Eubanks I. Dwaine, and Eubanks, Lucy Pride. ACS Test-Item Bank for High School Chemistry. Clemson University, South Carolina: ACS DivCHED, Examination Institute, 1993.

Russo, Tom. Microchemistry, Volumes 1,2 and 3. Batavia, Illinois: Flynn Scientific Inc. 1999.

Slowinski Emil, and Wolsey Wayne. Chemical Principles in the Laboratory, Seventh Edition. Orlando, Florida: Harcourt College Publications, 2001.

PeriodicalsJournal of Chemical educationScientific AmericanScienceDiscoverNational GeographicChemMatters

NewspapersNew York Times/Science TuesdaysBergen Record

Mass mediaSelected documentaries taped from television Nova, Cosmos, Accent of Man, etc.The Internet

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PORTFOLIO AND PERFORMANCE ASSESMENTHONORS CHEMISTRY

All major units of science work should be followed by appropriate testing of student performance. While the accumulation of factual knowledge is expected of each student, more emphasis is placed on evaluation of his/hers developments of an understanding and appreciation of the important conceptual themes of chemistry. Students are also evaluated on their progress toward the following outcomes:

1. laboratory skills2. facility of communicating scientific ideas3. ability to analyze problems4. ability to utilize new concepts.

Laboratory work will be based on the following experiences and skills:1. making observations of chemical reactions and substances2. recording data3. calculating and interpreting results based on the quantitative data obtained4. communicating effectively the results of experimental work

Because every experimental experience necessitates keeping detailed records, students in Honors Chemistry will keep reports of their laboratory work in such a fashion (permanent lab notebook) that the reports can be easily reviewed and evaluated. These notebooks will become a major part of students’ portfolios.

The laboratory program should have the following characteristics which challenge the student’s ability to:

1. think analytically and to reduce problems of identifiable, answerable questions;2. understand problems expressed as experimental questions;3. design and carry out experiments that answer questions;4. manipulate data acquired during an experiment;5. make conclusions and evaluate the quality and validity of such conclusions;6. communicate accurately and meaningfully about observations and conclusions.

Students should gain experience with traditional experiments but opportunities must be

provided to carry out novel investigations. Writing in response to open-ended questions will be evaluated by providing open-ended laboratory experiments in which students write to describe their method, results, and conclusions. In addition students will be challenged to search the literature for current topics and report the results of their investigation to class in form of a written and/or oral report.

OBJECTIVE EVALUATIONDuring the course of study teacher-made tests for each of the completed units will be used

for objective evaluation of students’ performance. Most of the questions will be drawn from standardized testing instruments (American Chemical Society, and public domain SAT II like questions). The Final Exam for the year is a standardized test available from the American

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Chemical Society. In addition, frequent quizzes will be administered to gauge students’ daily performance and homework mastery.

PROFICIENCIES – HONORS CHEMISTRY (FULL YEAR)Grades 10, 11

1. Make a measurement in the laboratory using the proper metric units and use these units in problem solving. (CCCS 5.1A:2, 3, 4; 5.1B: 1, 2, 3; 5.1C: 1, 2; 5.3A: 1, 2, 3; 5.3B: 1, 2:; 5.3C: 1; 5.3D: 1 - 4) [CCW 4.3.10; 5.2.4]

2. Collect, graph, analyze data and report results in writing in a student-designed and/or teacher prescribed laboratory experiment using appropriate chemical terminology. (CCCS 5.1A: 1, 3, 4; 5.1B:1. 2; 5.3D: 1-4; 5.4B:1) [CCW 5.2.3; 5.2.7]

3. Explain how the behavior of matter under various conditions is dependent on its properties; relate the three states of matter to the Kinetic Theory of Matter. (CCCS 5.1A: 1, 3, 4; 5.1B:1. 2; 5.3D: 1-4; 5.4B:1) [CCW 5.2.3; 5.2.7]

4. State the gas laws and predict the effect of changes in temperature, pressure, and number of molecules on the volume of a gas. (CCCS 5.6A: 2; 5.6B: 1, 2, 3)

5. Determine how energy and matter are related in many ways through their transportation, transformation, and conservation. (CCCS 5.6A: 2; 5.7B: 1, 2, 3)

6. Understand the historic developments that lead to the understanding of the structure of the atom and to the development of the modern periodic table. (CCCS 5.2A: 1, 2; 5.2B: 1, 2,3)

7. Identify the components and structure of the atom and describe the atom in terms of the modern quantum mechanical theory. (CCCS 5.6A: 1, 2, 3, 8)

8. Use the periodic table to extract information concerning properties of the elements in chemical reactions and for applying this to chemical bonding. (CCCS 5.6A: 1, 2, 3, 5, 8; 5.6B: 2, 3, 4)

9. Demonstrate the effect of molecular structure and geometry on chemical properties.(CCCS 5.6A: 6, 7)

10. Apply the mole concept to explain the behavior of matter and calculate quantitative relationships such as calculating the molar mass of a compound, the percentage composition of a compound, and develop empirical formulas from percentage data.(CCCS 5.6B: 1; 5.4B: 1)

11. Write chemical formulas, explain the significance of the formula, balance equations, and solve stoichiometric problems based on chemical equations. (CCCS 5.6B: 1, 4, 3)

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12. Comprehend the dynamics of the solution process and apply this process to solution concentration ionization, solubility, and acid-base theory.(CCCS 5.6A: 4)

13. Understand Kinetic Theory and solve chemical kinetics problems as applied through calorimetry. (CCCS 5.6B: 1, 2; 5.7A: 1)

14. Denote the conditions that establish an equilibrium system, recognize the existence of equilibrium systems in the laboratory and the real world, and understand the factors which affect equilibrium. And interpret the meaning of the equilibrium constant. (CCCS 5.4C: 1; 5.4A: 1)

15. Apply LeChatelier’s Principle to the effects of pressure, temperature, and concentration on shifting equilibrium. (CCCS 5.4C: 1, 2)

16. Calculate the Free Energy changes for chemical reactions, given the enthalpy and entropy, and use the result to determine the conditions for spontaneous reactions. (5.6B: 2, 3)

17. Describe radioactivity and its effect on nuclear stability. (CCCS 5.7A: 5)

18. Compare and contrast physical, chemical, and nuclear changes. (CCCS 5.7A: 5)

19. Balance nuclear reactions. (CCCS 5.7A: 5)

20. Describe fission and fusion and some applications. (CCCS 5.4A: 1; 5.4B: 1; 5.4C: 1, 2, 3) [CCW 5.4.9]

21. Describe oxidation-reduction process and use it to explain how electrochemical cells produce electricity. (CCCS 5.4A: 1; 5.4C: 1)

22. Illustrate how chemical systems control nature and the man-made world. (CCCS 5.4: 1; 5.4B: 1; 5.4C: 1, 2, 3) [CCW 6.5.4]

23. Cite examples of how technologies have been influenced by changes in understanding of atomic theory from early Greeks through Dalton to the modern theories. (CCCS 5.2B: 1, 2, 3) (CCW 5.3.6]

NOTE: The number(s) in parenthesis at the end of each proficiency corresponds to the appropriate NJ State Core Proficiency.

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