CURRICULUM GUIDE Chemistry 11-21 (Honors) SC3C05 Length: 2 semesters Credit: 2 credits Open to Grades: 10-11 Grade Weight: V Prerequisite: Completion of Biology 11-21 with a grade of "B" or better, OR Biology 12-22 with a grade of "A". Completion of Algebra 3A-4A or Algebra 31-41. Teacher recommendation is also required. AP Environmental Science may be taken concurrently

Chemistry 11-21 is the second course in the honors science sequence. It is a general introductory course on the nature and composition of matter, the laws which describe its behavior, and the theories which explain and account for the properties and behavior of matter. Topics are covered in great depth with high achievement standards. Laboratory work constitutes an integral and important part of the course objectives. A graphing calculator is recommended.

District 219 Niles Township High Schools Skokie, Illinois

Ami LeFevre, Director of Science, Niles West Joan Gallagher-Bolos, Director of Science, Niles North

Table of Contents

I.

Department Structure…………………………………………………… p. 3

II.

Instructional Materials………………………………………………...... p. 4

III.

Agreed upon elements……………………………………...……………..p. 5

IV.

Learning Targets……………………………………………………….…p. 7

Instructional Materials

Textbook Chemistry – The Central Science 11th Edition Brown, LeMay, and Bursten, AP Edition Prentice Hall 2009 Workbook Workbook for General Chemistry Shakhashiri & Schreiner Stipes Publishing, 2004 Laboratory Manuals Labs are used from several sources. Below is a list of suggested lab manuals you may choose to use: 1.

Chemistry Connections to Our Changing World Bette Bridges and John Hugo, et. al. Prentice Hall, 2000

2.

Chemistry With Computers Vernier Software www.vernier.com

3.

Microscale Experiments for General Chemistry Williamson and Little Houghton Miffilin Co., 1997

4.

Laboratory Manual for Chemistry Maxine Wagner Allyn and Bacon, Inc., 1983

Demonstration Manuals 1. 2. 3.

Demo A Day, by Bob Becker Chemical Demonstrations volume 1 and 2, by Summerlin and Ealy, ACS, 1985 Chemical Demonstrations volume 1-4, by B. Shakashari, University of Wisconsin Press, 1985

Agreed- Upon Elements Course expectations: Teachers will follow the Course Outline. The list includes the minimum amount of topics to be covered in each 9 week period. Timeline per chapter is only a suggestion. Teachers should determine the length of time based on student performance and skill level. Time is allotted at the end of each semester to cover optional topics. Number and type of labs: Students will complete at least one lab and/or activity per chapter. Incorporating inquiry based labs are encouraged. Types of Homework Assignments: Workbook problems, textbook problems, and online questions are suggested.

Chemistry 11-21 Curriculum Guide Course Outline

First Semester Topics First 9 Weeks Chapter 1 Matter and Measurement (3 weeks) Chapter 2 Atoms, Molecules, and Ions – remove 2.9 organic nomenclature, add 21.1 and 21.3 (3 weeks) Chapter 3 Stoichiometry (3 weeks) Second 9 Weeks Chapter 4 Aqueous Solutions- add 20.1 & 20.2 (3 weeks) Chapter 5 Thermochemistry- remove 5.8 foods & fuels (2 weeks) Chapter 6 Electron Structure (1 week) Chapter 7 Periodic Trends (1 week)

Second Semester Topics Third 9 Weeks Chapter 8 Bonding (1 week) Chapter 9.1- 9.3 Molecular Geometry (1 week) Chapter 10 Gas Laws (2 weeks) Chapter 11 Intermolecular Forces- Liquids and Solids (2 weeks) Chapter 13 Properties of Solutions (2 weeks) Chapter 14 Kinetics (1 week) Fourth 9 Weeks Chapter 15 Chemical Equilibrium (2 weeks) Chapter 16 Acids and Bases (2 weeks) Chapter 17 Equilibria Acids and Bases (Buffer and Titration) (2 weeks) Suggested Elective Topics- Time Allowed Chapter 12 Modern Materials Chapter 18 Chemistry of Environment Chapter 20 Electrochemistry Chapter 21 Nuclear Chemistry Chapter 23 Metals & Metallurgy Chapter 25 Organic Chemistry

Learning Targets SEMESTER 1 Matter & Measurement A. I can classify matter and its changes based on its properties. 1. I can define the states of matter and compare and contrast their properties. 2. I can classify materials as elements, compounds, or mixtures, stating the

evidence for the classification. I can describe several techniques for the separation of mixtures. I can distinguish between physical and chemical properties; extensive and intensive properties. 5. I can define melting point, boiling point, and solubility. B. I can solve measurement problems using the metric system. 1. I can identify and define fundamental and derived SI Units. 2. I can convert any number from decimal to scientific notation, and vice versa. 3. I can use metric prefixes to define different sized metric units. 4. I can convert units in the SI and English systems. 5. I can define accuracy and precision. 6. I can determine the number of significant figures in a measurement. 7. I can perform calculations rounding answers to the correct number of significant figures. 8. I can define and calculate density. 3. 4.

2. Atoms, Molecules, and Ions A. I can discuss atomic structure (both historically and currently) and how it relates to

atomic properties. 1. I can describe the basic postulates of Dalton’s Atomic Theory. 2. I can describe the key historical discoveries of J.J. Thomson, Millikan, Curie, Rutherford, and Chadwick that led to the discovery of the structure of the atom. 3. I can describe the structure of the atom in terms of protons, neutrons, and electrons. 4. I can list the relative charge, mass, and location of protons, neutrons, and electrons. 5. I can use isotope notation to express the subatomic composition of atoms. 6. I can calculate average atomic mass from natural abundance of isotopes and masses of individual atoms. 7. I can explain how ions are formed and determine the number of electrons gained or lost based on ionic charge. B. I can use the periodic table as a reference tool. 1. I can describe how elements are organized in the periodic table leading to periods and groups. 2. I can identify the location of metals, nonmetals, and metalloids. 3. I can use the periodic table to predict charges of ions. C. I can write names and formulas for simple, inorganic compounds. 1. I can identify, name , write formulas for ionic compounds. 2. I can identify, name, and write formulas for molecular compounds. 3. I can identify, name, and write formulas for acids.

3. Stoichiometry A. I can use chemical formulas to create balanced equations and calculate values from those

chemical formulas. 1. I can balance chemical equations and interpret their meaning. 2. I can classify and write equations for combination, decomposition, & combustion 3. I can calculate formula weight, molecular weight, and molar mass 4. I can calculate percent composition given a chemical formula 5. I can calculate empirical and molecular formulas. B. I can perform stoichiometric calculations. 1. I can convert between the mass, moles, and number of particles of a substance. 2. I can use a balanced equation to calculate amounts of reactants and products for a reaction. 3. I can identify a limiting reactant and determine the theoretical yield of the reaction. 4. I can calculate the percent yield of a reaction.

4. Aqueous Reactions and Solution Stoichiometry A. I can identify the general properties of aqueous solutions. 1. I can identify strong, weak and nonelectrolytes. 2. I can list the ions present in a dissolved ionic compound. 3. I can write reactions showing how strong and weak electrolytes differ. B. I can categorize chemical reactions and use them to write complete, balanced equations

representing those equations. 1. I can classify and write equations for single replacement, and double replacement reactions. 2. I can identify a precipitation reaction and determine the products of a precipitation reaction. 3. I can use basic solubility rules to determine the states of products. 4. I can write complete and net ionic equations for precipitation reactions by way of identifying spectator ions. 5. I can identify and determine the products of an acid-base reaction. 6. I can identify an acid or a base as strong or weak and relate that to electrolytic properties. 7. I can write complete and net ionic equations for acid-base reactions by way of identifying spectator ions. 8. I can identify the reduction and oxidation components of a REDOX reaction. 9. I can assign oxidation numbers to elements. 10. I can write half reactions. 11. I can balance REDOX reactions. C. I can perform solution stoichiometry. 1. I can define Molarity (M). 2. I can calculate moles, volume, or grams of a substance using molarity. 3. I can prepare a solution with a known concentration. 4. I can carry out a dilution to achieve a desired solution concentration.

5. Thermochemistry A. I can define work and heat and apply it to internal energy.

1. 2. 3. 4. B.

I can explain the difference between kinetic and potential energy I can define heat and explain the sign of ‘q’ with respect to the system. I can state and interpret the First Law of Thermodynamics. I can calculate the heat of a reaction using thermochemical equations and stoichiometry.

I can determine the enthalpy change (∆H) of a reaction using calorimetry, Hess’s Law and Enthalpies of Formation 1. I can distinguish between endothermic and exothermic reactions. 2. I can define enthalpy. 3. I can calculate ‘q’ for a reaction from calorimetric data. i. I can explain why + energy in = - energy out. ii. I can perform calculations based on quantitative data. 4. I can calculate ‘q’ for a reaction from Hess’s Law. i.

I can modify reactions (flip, multiple, divide) and change their

∆H values accordingly. ii. I can explain and apply Hess’s Law to calculate enthalpy of a reaction. 5. I can calculate ‘q’ for a reaction from enthalpies of formation. i. I can write the equation that expresses the standard enthalpy of formation of a compound. ii. I can define standard enthalpy of formation and use those values to calculate enthalpy of a reaction. 6. Electrons Structure of the Atom A. I can describe the wave/particle nature of light and matter and explain how this led to the

Bohr model of the atom. 1. I can define electromagnetic radiation and describe the electromagnetic spectrum. 2. I can perform calculations relating the wavelength, frequency, and photon energy of light based on the equations c=wavelength x frequency and E=hv. 3. I can explain the photoelectric effect and describe its importance in the development of modern atomic theory. 4. I can explain the existence of discrete spectral lines and attribute those to quantized jumps of electrons between energy levels. 5. I can explain and perform calculations with deBroglie’s equation: λ=h/mν 6. I can describe the Heisenberg Uncertainty Principle and its implications for atomic structure. B. I can describe electrons within an atom based on the Quantum Mechanical model of the atom. 1. I can identify the four quantum numbers and their relationship to energy levels, sublevels, and orbitals. 2. I can write complete and condensed electron configurations of atoms and ions. 3. I can explain the electron configuration of atoms and ions using the Periodic Table. 4. I can write electron orbital diagrams of atoms by correctly applying, Aufbau’s principle, Hund’s rule, and the Pauli Exclusion Principle.

SEMESTER 2 7. Bonding A. I can identify and apply periodic trends. 1. I can provide a brief history of the development of the periodic table. 2. I can define the following quantities, describe their periodic trends, and use

them to predict relative magnitudes when comparing elements. i. Effective Nuclear Charge ii. Atomic radii iii. Ionic radii iv. Ionization energy v. Electron Affinity B. I can analyze ionic and covalent compounds. 1. I can compare and contrast ionic, covalent and metallic bonds. 2. I can define and apply the octet rule. 3. I can draw Lewis Symbols for elements. 4. I can define and explain the periodic and group trend for electronegativity. 5. I can determine if a compound is ionic or covalent based on electronegativity differences. 6. I can illustrate ionic bond formation through electron transfer using Lewis Dot Structures. 7. I can predict charges of ions based on electron configuration. 8. I can discuss transition metal ions and their formation, understanding that they are exceptions to the octet rule. 9. I can illustrate covalent bond formation through electron sharing using Lewis Dot Structures 10. I can explain the formation of multiple bonds in covalent bonding. 11. I can identify polar and nonpolar bonds using electrongativity differences. 12. I can calculate formal charge and use those values to determine plausible Lewis Dot Structures. 13. I can explain resonance and draw valid resonance structures using Lewis Dot Structures. 14. I know and can explain the exceptions to the Octet Rule 15. I can relate bond type to bond strength and bond length. 16. I can calculate ∆Hrxn using bond enthalpies. C. I can discuss molecular geometry as it relates to covalent bonding. 1. I can define dipole moments and indicate dipole moment on a Lewis Dot 2. 3. 4. 5.

Structure. I can explain the differences between strengths in single and multiple bonds. I can explain the valence-shell-electron-pair repulsion model (VSEPR). I can predict the molecular geometry of molecules. I can predict polarity of the molecule based on molecular geometry.

8. Gases A. I can perform calculations based on the pressure, volume, temperature and/or amount of a

gas. 1.

I can define, list the units for its measurement, and perform calculations related

to gas pressure. I know the definition and values of Standard Temperature and Pressure. I can convert between different units of pressure, volume, temperature, and amount of gas 4. I can state and apply the following gas laws: i. Boyle’s law: P1V1=P2V2 ii. Charles Law: V1/T1=V2/T2 iii. Lussac’s Law: P1/T1=P2/T2 iv. Combined Gas Law: P1V1/T1=P2V2/T2 v. Avogadro’s law: V1/n1=V2/n2 vi. Ideal Gas law: PV=nRT a. Rearranged to solve for density: d=PM/RT 5. I can solve stoichiometric problems that involve gas volumes 6. I can use Dalton’s law to relate partial pressure and mole fractions i. Pt=P1 + P2 + P3 + …. ii. Pt= iii. P1==X1Pt B. I can discuss Kinetic Molecular Theory and how it relates to the behavior of gases. 1. I can interpret the five postulates of the Kinetic Molecular Theory 2. I can calculate the average speed of gas molecules i. Root mean square velocity: u= 3. I can explain the principles of diffusion and effusion. 4. I can apply Graham’s law of effusion to determine the molar mass of a gas i. Relative rates of effusion: 5. I can differentiate between an ideal and a real gas 2. 3.

9. Intermolecular Forces, Liquids and Solids A. I can relate intermolecular forces to the properties of a substance. 1. I can identify the different types of intermolecular forces in a substance based

on its structure. i. London dispersion forces ii. ion-dipole iii. dipole-dipole iv. hydrogen bonding. 2. I can evaluate the effects of I.M.F. on properties of a substance. 3. I can define viscosity and relate it to IMF 4. I can define surface tension and relate it to IMF B. I can evaluate the characteristics of liquids and solids. 1. I can create and use heating curves 2. I can calculate heat changes using a heating curve 3. I can define critical temperature and critical pressure 4. I can relate vapor pressure, volatility of a liquid, and the process of dynamic equilibrium. 5. I can define boiling point normal boiling point, freezing point, and melting point. 6. I can use a phase diagram to determine the phase(s) present at a given temperature and pressure. 7. I can identify types of solids as molecular, network covalent, ionic, or metallic. 8. I can discuss the crystal structures and the unit cell in metals and ionic crystals. i. Simple cubic: 2r=s

ii. Face centered cubic: 4r=s iii. Body centered cubic cell: 4r=s

10. Properties of Solutions A. I can describe the process of solution formation. 1. I can explain the energy changes in the solution process (endothermic and

exothermic portions of the process) I can distinguish between unsaturated, saturated and supersaturated solutions I can interpret a solubility graph. I can explain the factors that affect solubility I can define a colloid. B. I can perform calculations related to solutions. 1. I can apply Henry’s Law to relate gas solubility to partial pressure. 2. I can calculate the concentration of a solution. i. molarity (M=mol solute/L solution) ii. molality (m=mol solute/kg solvent) iii. mole fraction (mol component/total mol) iv. mass percent ((mass component/total mass solution)x100) 3. I can convert one concentration unit to another. 4. I can perform dilution calculations using the equation M1V1 = M2V2 5. I can describe how colligative properties affect vapor pressure, boiling point and freezing point. 6. I can perform calculations related to colligative properties: i. Vapor Pressure depression (PA=XAPA°) ii. Boiling point elevation (∆Tb=iKbm) 2. 3. 4. 5.

iii. Freezing point depression (∆Tf=iKfm) 7.

I can calculate molar mass of a non-electrolyte solute from freezing point depression data.

11. Chemical Kinetics A. I can perform calculations to determine the speed of a reaction based on experimental

data. 1. 2. 3.

I can explain the factors that affect the rate of chemical reactions. I can determine the rate of a reaction given time and concentrations. I can relate the rate of formation of products and the rate of disappearance of reactants given the balanced chemical equation for the reactions. i.

I can understand the form and meaning of a rate law including the ideas of reaction order and rate constant. 5. I can determine the rate law and rate constant for a reaction from a series of experiments given the measured rates for various concentrations of reactants. m n i. Rate = k[A] [B] 4.

12. Chemical Equilibrium A. I can describe the quantitative relationship between the concentrations of the reactants

and products in a system which exists in a state of equilibrium. 1. I can define Keq and write expressions for Keq for both homogeneous and heterogeneous reactions.

i.

I can relate the magnitude of Keq to relative amounts of product and reactant. I can calculate the reaction quotient, Q, and use the value to predict the direction of a reaction when compared to the equilibrium constant, Keq. i. QK the reaction moves to produce more reactant 4. I can calculate the equilibrium constant when given the equilibrium concentrations. 5. I can calculate equilibrium concentrations using the value of the equilibrium constant, Keq. 6. I can define Le Chatelier’s principle and apply it to predict the shift in a reaction when conditions are changed. i. Concentration ii. Pressure iii. Temperature 2. 3.

13. Acid and Base Equilibirium A. I can analyze acids and bases. 1. I can define acids and bases according to the Arrhenius, Bronsted-Lowry, and

Lewis theories and give examples of each. I can identify the Bronsted-Lowry conjugate acid-base pairs and conjugate base-acid pairs in a given reaction. 3. I can identify strengths of acids and bases. 4. I can analyze the pH and pOH scale. 5. I can explain the water ionization constant + 6. I know the value of the equilibrium constant for water, Kw, and relate it to [H ] & [OH-]. 7. I can predict whether an aqueous solution of a salt is acidic, basic, or neutral. B. I can perform calculations with weak and strong acids and bases. + 1. I can calculate pH and pOH given [H ] & [OH ]. 2. I can calculate the pH & pOH of a strong acid & base given its concentration. 3. I can calculate the pH and percent ionization of a weak acid or a weak base. 4. I can determine Ka or Kb when given the molarity and the pH of a weak acid, or weak base. 5. I can calculate the pH of a salt solution. 2.

14. Additional Aspects of Aqueous Equilibria A. I can analyze systems in which acids and bases react. 1. I can describe the common-ion effect. 2. I can describe the composition of a buffer and explain how it works to maintain 3. 4.

a constant pH I can explain how to prepare a buffer with a specific pH. Calculate the pH of a buffer system. i.

I can calculate the pH of a buffer system after adding small amounts of strong acid or base . 6. I can choose the proper indicator for an acid-base titration 7. I can calculate the pH at any point during the titration of: 5.

i. strong acid with a strong base ii. weak acid with a strong base iii. strong acid with a weak base. 8.

I can interpret the titration curves for the above solutions

B. I can analyze systems in which solids are involved. 1. I can calculate the solubility of an ionic solid in a solution containing a

common ion. 2. I can write the Ksp expression for any ionic solid. 3. I can calculate the solubility of an ionic solid in water 4. I can determine whether a precipitate will form when two solutions are mixed. i. Q>Ksp

15. Reaction Mechanisms A. I can determine which ion will precipitate first from a mixture. B. I can apply the concept of selective precipitation to explain the groups of cations of

qualitative analysis. C. Write balanced net ionic equations to explain why a precipitate dissolves in strong acid,

strong base, or ammonia.

16. Additional Topics A. I can apply the van der Waals equation to real gases 1. B. I can apply the Clausius-Clapeyron Equation to determine the ∆Hvap of a

substance 1.

C. I can interpret a graph made from the Clausius-Clapeyron equation.

List of General Labs for Chemistry 11-21 The labs and activities in the Honors Chemistry curriculum range from simple verification activities to inquiry based lab experiments, to large scale projects. Each type of activity involves some type of data collection, analysis, and conclusions to varying degrees of difficulty and depth with some form of formal report to be written. In some cases, class data are combined and/presented to the class as a whole by the instructor or the students using various media and technologies. While each lab activity is linked to specific content objectives for the class, the State Learning Goals related to scientific content and process that correlate are listed below: Chapter Lab Activity 1

Classification of Matter Lab

1

Scientific Method: Blue Bottle Lab

1

Density and Significant Figures Lab

2

Atomic Mass Activity

3

Counting by Weighing Activity

3

Percent of Water in Hydrate Lab

3

Empirical Formula of Ionic Compound Lab

3

Stoichiometry Lab 1: Production of NaCl

3

Stoichiometry Lab 2: Copper from Ore

4

Predicting Reaction Products Lab

4

Redox Titration Lab

5

Specific Heat Lab

5

Hess's Law Lab

6

Flame Tests Lab

9

Molecular Modeling Lab

10

Gas Law Labs

10

Molar Volume of a Gas Lab

10

Weight of Air Lab Activity

11

Vapor Pressure and Temperature Lab

13

Preparation of Solutions

13

Supersaturated Solutions

13

Ice Cream Lab

14

Crystal Violet Kinetics Lab

14

Effect of Concentration on Reaction Rate

15

Equilibrium and Le Chatelier's Principle

16

pH Lab

17

Acid Base Titration Lab

17

Ksp Lab