Boise Schools Curriculum

Accelerated Chemistry

District Course #1235

Course Description

Open to: Grade 11, 12 One Year Course
Prerequisite: "C" or better in Algebra 1
Content: Recommended for the college-bound student. Students will study matter and the changes it undergoes, learning the structure of atoms and molecules, elements, compounds, and mixtures. Also included will be why chemical reactions occur and how to control them. Strongly recommended for the college-bound student.

Adopted Materials

Title: Modern Chemistry
Authors: Davis et.al.
Publisher: Holt, Reinehart, and Winston

Grades

The grade that a student receives in this course will be a reflection of how the student has performed in three main areas; the assimilation of content, the acquisition of performance skills, and the knowledge gained from homework. The course grade will be calculated from scores obtained on unit tests, projects and activities (labs, model building, reports, etc.), homework, and a semester final. Progress reports should provide the student and parents with information (average grades or percentages) in three main areas: unit tests, projects/activities, and homework completed.

The Final is also the End of Course Exam (EOC), which will count as 10% of the student’s final grade and determine whether or not the student has met the State Standards in Science for this particular course. The science curriculum supervisor discourages the use of notes, note cards, or books when taking a unit test. Students will not be allowed to use these items on the Final Exam.

Copyright Resources

Course Scope and Sequence for Semester I

Unit 1	Properties of Matter and Measurement	3 Weeks
Unit 2	Atomic Theory	3 Weeks
Unit 3	Periodic Law	3 Weeks
Unit 4	Chemical Bonding and Compounds	3 Weeks
Unit 5	Chemical Equations, Reactions and Stoichiometry	5 Weeks

Course Scope and Sequence for Semester II

Unit 5	Stoichiometry	3 Weeks
Unit 6	Gases	3 Weeks
Unit 7	Solids, Liquids and Solutions	4 Weeks
Unit 8	Acids, Bases and Salts	4 Weeks
Unit 9	Equilibrium (Optional)	2 Weeks
Unit 10	Reaction Kinetics and Mechanisms	2 Weeks
Unit 11	Oxidation-Reduction Reactions (Optional)	2 Weeks
Unit 12	Nuclear Chemistry (Optional)	1 Week
Unit 13	Organic Chemistry (Optional)	1 Week
Appendix: Laboratory Activities

Assessment Correlation acronyms key

Download this curriculum as a "Printer Friendly" pdf file

Accelerated Chemistry Curriculum

The following objectives will be covered in our laboratory exercises, conducted throughout the year. Individual labs for specific units can be found in the Resource Reference section. Additional lab resources can be found at each school within Accelerated Chemistry curriculum notebook.

Instructional Objective 1235.01 Know laboratory equipment, techniques and safety			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Understand scientific inquiry	Modern Chemistry from Laboratory Resources, A & B		TMA
02	Develop critical thinking skills	Vernier: Chemistry Using Computers		TMA
03	Work efficiently and safely in a laboratory			TMA
04	Correctly measure and carry out calculations using significant digits			TMA

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Unit 1	Properties of Matter and Measurement	3 weeks

Instructional Objective 1235.02 Understand equipment, procedures and safety in the chemistry laboratory			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Identify and know the use of common laboratory equipment Conduct required laboratory procedures safely and competently	Ch. 1 Lab: Accuracy and Precision		EOC, TMA
Instructional Objective 1235.03 Identify, compare and contrast physical and chemical properties and changes			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Compare and contrast phases of matter	Ch. 1		EOC, TMA
02	Describe and distinguish between physical and chemical properties	Ch. 1 Lab: Separation of a Mixture		EOC, TMA
03	Describe and identify physical and chemical changes	Ch. 1 Lab: Evidence of Chemical Change		EOC, TMA
Instructional Objective 1235.04 Understand energy changes in chemical reactions and the conservation of matter and energies			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Distinguish between endo and exothermic reactions and the types of energy changes involved in chemical reactions	Ch. 1		EOC, TMA
02	Distinguish potential and kinetic energy and restate the Laws of Conservation of Mass and Energy	Ch. 1		EOC, TMA
Instructional Objective 1235.05 Understand scientific inquiry and method			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Apply scientific method in the laboratory Compare and contrast basic research, applied research and technological development	Ch. 2		EOC, TMA
Instructional Objective 1235.06 Develop math skills using scientific method, scientific notation, the metric system and dimensional analysis (factor label)			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Solve chemistry problems requiring answers in significant digits and scientific notation	Ch. 2		EOC, TMA
02	Measure using metric system and calculate derived units from measurements	Ch. 2 Lab: Determination of Density		EOC, TMA
03	Use dimensional analysis for solving problems	Ch. 2		EOC, TMA
04	Compare accuracy and precision	Ch. 2		EOC, TMA

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Unit 2	Atomic Theory	3 weeks

Instructional Objective 1235.07 Interpret the classic historical experiments that determine the structure of the atom			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	State and explain the atomic theory	Ch. 3		EOC, TMA
02	Discuss the contributions of scientists in describing atomic structure	Ch. 3		EOC, TMA
Instructional Objective 1235.08 Determine the atomic mass of elements and relate this information to arrangement of subatomic particles in atoms			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Determine the atomic number, mass number, numbers of protons, neutrons, electrons and diagram the arrangement of these particles in any atom	Ch. 3,4		EOC, TMA
Instructional Objective 1235.09 Understand the Law of Conservation of Mass, the Law of Definite Proportions, and the Law of Multiple Proportions			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain the relationship between Dalton�s atomic theory and the law of conservation of mass, law of definite proportion, and law of multiple proportion	Ch. 3		EOC, TMA
02	Mathematically relate the mass of substance to amount of amu., number of atoms or molecules, moles, and grams	Ch. 3 Lab: The Mole		EOC, TMA
Instructional Objective 1235.10 Understand the relationship between the structure of atoms, and light energy			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain the mathematical relationship between speed, wavelength, and frequency of electromagnetic radiation	Ch. 4		TMA
02	Discuss the significance of the photoelectric effect and line emission spectrum in the development of the atomic model	Ch. 4 Lab: The Flame Test		EOC, TMA
Instructional Objective 1235.11 Understand and illustrate electron arrangements within atoms			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Describe the arrangement of electrons in energy levels and sublevels of the atom using electron configurations, orbital notations, and Lewis dot structures for elements	Ch. 4		EOC, TMA

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Unit 3	Periodic Law	3 weeks

Instructional Objective 1235.12 Understand the historical development of the periodic table			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain the roles of Mendelev and Mosely in the development of the periodic table	Ch. 5 Lab: The Periodic Table		EOC, TMA
02	Recognize how and why elements are arranged in specific groupings on the periodic table	Ch. 5 Lab: Mendeleev for a Day		EOC, TMA
Instructional Objective 1235.13 Describe the arrangement of elements on the periodic table and to use the periodic table to predict physical and chemical properties			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Restate the periodic law and explain how the periodic law can be used to predict physical and chemical properties of elements	Ch. 5 Lab: The Halogen Lab		EOC, TMA
02	Understand the interrelationships of atomic numbers, position on the periodic table, electron configurations, and properties of elements	Ch. 5		EOC, TMA
Instructional Objective 1235.14 Correctly write names and symbols for common elements			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Correctly write names and symbols of common elements	Ch. 5		EOC, TMA
02	Construct Lewis structures, and predict the number of valence electrons for elements using the periodic chart	Ch. 5		EOC, TMA

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Unit 4	Chemical Bonding and Compounds	3 weeks

Instructional Objective 1235.15 Explain and understand how electrons are involved in the formation of chemical bonds			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Know the importance of valence electrons and explain the octet rule	Ch. 6		EOC, TMA
02	Define ionic, covalent and metallic bonds in terms of a)electronegativity differences b)metals and nonmetals c)mobility of electrons(electron sea)	Ch. 6 Lab: Types of Chemical Bonds		EOC, TMA
03	Differentiate polar and nonpolar covalent bonds and recognize multiple bonds	Ch. 6 Lab: Molecular Models		EOC, TMA
04	Utilize the periodic table to predict bond type	Ch. 6		EOC, TMA
05	Construct ionic and covalent compound Lewis diagrams and polyatomic ion Lewis structures	Ch. 6		TMA
06	Explain VSEPR and Hybridization theories about molecular geometry. Study intermolecular bonding	Ch. 6		TMA
07	Name binary and ternary compounds including acids and bases using the stock system and existing monatomic and polyatomic ion names	Ch. 7		EOC, TMA
08	Calculate and/or use quantitative data give by chemical formulas including percent composition, empirical formulas and interconversion of grams moles and molecules	Ch. 7		EOC, TMA

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Unit 5	Chemical Equations, Reactions and Stoichiometry	8 weeks

Instructional Objective 1235.16 Classify, write and balance chemical equations for common types of chemical reactions			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Know the observations that indicate a chemical reaction has taken place	Ch. 8 Lab: Evidence for Chemical Change		EOC, TMA
02	Predict products for five types of chemical reactions studied and balance by inspection	Ch. 8 Lab: Types of Chemical Reactions		EOC, TMA
03	Use the activity series to predict the occurrence of single replacement reactions	Ch. 8 Lab: Decomposition of Sodium Bicarbonate		EOC, TMA
Instructional Objective 1235.17 Use critical thinking skills to analyze and solve reaction stoichiometry problems. Perform stoichiometry calculations from balanced chemical equations.			Standard Reference District/National
No.	Performance Objectives	Resource Reference		Assessment Correlation
01	In a balanced chemical equation, use dimensional analysis (factor label) to convert numerical data about one constituent of the equation to numerical data about another member of the equation	Ch. 9		EOC, TMA
02	Calculate quantitative data in chemical reactions using the limiting reactant concept	Ch. 9		EOC, TMA
03	Distinguish between theoretical yield, actual or lab yield and use these to determine percent yield	Ch. 9		EOC, TMA

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Unit 5	Stoichiometry (2nd semester continuation)	3 weeks

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Unit 6	Gases	3 weeks

Instructional Objective 1235.18 Understand the unique physical properties of gases through the use of kinetic molecular theory			Standard Reference District/National
No	Performance Objectives	Resource Reference		Assessment Correlation
01	Learn the principles behind the kinetic molecular theory of gases	Ch. 10, 11 Lab: Boyle�s Law		EOC, TMA
02	Describe characteristic properties of gases compared to liquids and solids	Ch. 10, 11		EOC, TMA
03	Study the inverse nature of Graham�s Law of Effusion	Ch. 10, 11		TMA
04	State and use the standard temperature and pressure (STP) conversion factors.	Ch. 10, 11		EOC, TMA
05	Use the following laws; Boyles, Charles, Gay-Lussacs, Daltons, Combined Gas and Ideal gas law to study the variations of volume, pressure, temperature and amount (moles) of gas.	Ch. 10, 11 Lab: Molar Volume of Gas		EOC, TMA

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Unit 7	Solids, Liquids and Solutions	4 weeks

Instructional Objective 1235.19 Understand the relationship of the properties of liquids and solids to the kinetic molecular theory			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Describe the motion of particles in liquids and the properties of liquids according to the kinetic molecular theory	Ch. 12		EOC, TMA
Instructional Objective 1235.20 Describe the attractive forces holding particles together in a crystal and predict how these affect the physical properties of the substance			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Distinguish between crystalline and amorphous solids and describe various crystal structures	Ch. 12		TMA
Instructional Objective 1235.21 Understand both kinetic and potential energy changes involved in phase changes and will predict how heating or cooling will affect these changes			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain the relationship between equilibrium and change of state	Ch.12		EOC, TMA
02	Predict changes in equilibrium using LeChatelier�s principle	Ch.12		EOC, TMA
03	Describe the processes of boiling, freezing, melting and sublimation and be able to calculate energy	Ch. 12 Lab: Heat of Fusion		EOC, TMA
04	Interpret a phase diagram	Ch. 12 Lab: Phase Change		EOC, TMA
Instructional Objective 1235.22 Understand the structure of water and be able to explain the relationship of its structure to the properties and physical behavior of water			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Describe the structure of water and discuss it physical properties	Ch. 12		EOC, TMA
02	Calculate the energy changes that occur when water changes state	Ch. 12		TMA
Instructional Objective 1235.23 Develop an understanding of properties and behavior of various types of solutions and will recognize common solutions and their use			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Give a definition of a solution, list the general properties of solutions, name the types of solutions possible, and give examples of each type of solution	Ch. 13 Lab: Heats of Solution		EOC, TMA
Instructional Objective 1235.24 Understand the solution process			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain the steps in the solution process for both ionic and covalent solids in liquids and explain the "like dissolves like" rule relative to this mechanism	Ch. 13		EOC, TMA
02	Predict the effect of temperature and pressure on solubility of gases and solids in liquids	Ch. 13		EOC, TMA
03	State and apply solubility rules for common salts and hydroxides	Ch. 13		EOC, TMA
Instructional Objective 1235.25 Express concentrations of solutions in terms of molarity, normality and molality			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Use the definitions for molarity, normality and molality to do calculations with appropriate data	Ch. 13 Lab: Beer�s Law		EOC, TMA
Instructional Objective 1235.26 Understand and distinguish between dissociation and ionization of compounds in aqueous solutions			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Write equations for the dissolution of soluble ionic compounds in water	Ch. 14		EOC, TMA
02	Predict whether a precipitate will form when solutions of ionic compounds are combined and write net ionic equations for precipitation reactions	Ch. 14		EOC, TMA
03	Compare dissociation of ionic compounds to ionization of molecular compounds	Ch. 14 Lab: Electrolyte		EOC, TMA
Instructional Objective 1235.27 Understand how the presence of solute particle affects the properties of a solution and be able to do calculations involving these colligative properties			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	List the four colligative properties and explain why they are classified as colligative properties	Ch. 14 Lab: Ice Cream Lab		TMA
02	Calculate freezing point depression and boiling point elevation of a solution	Ch.14		TMA
03	Discuss the causes of differences between experimentally observed colligative properties and calculations involving these colligative properties	Ch. 14		TMA

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Unit 8	Acids, Bases and Salts	4 weeks

Instructional Objective 1235.28 Understand classification of substances into acids, bases, and salts and will be familiar with properties and uses of these groups and common reactions involving them			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Classify substances as acids, bases, or salts	Ch. 15 Lab: pH of Household items		EOC, TMA
02	State general properties of acids and bases and name common acids and bases given their chemical formulas	Ch. 15		EOC, TMA
03	Describe some uses of common acids and based used in the laboratory and in industry	Ch.15		EOC, TMA
04	Recognize a neutralization reaction	Ch. 15		EOC, TMA
Instructional Objective 1235.29 Distinguish between the three common theories defining acids and bases			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Define acids and bases in terms of Arrhenius, Bronsted-Lowry, and Lewis theories using appropriate terminology	Ch. 15		EOC, TMA
02	Identify acids, bases, and their conjugates in an acid base equation and predict their relative strengths	Ch. 15 &16		EOC, TMA
03	Identify amphoteric substances and explain the conditions under which it acts as an acid or a base	Ch. 15		TMA
Instructional Objective 1235.30 Understand the role of dissociation and ionization in producing strong, weak, and nonelectrolytes			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain the differences between strong and weak acids and bases and relate their strength to their ionization equation	Ch. 15		EOC, TMA
02	Predict the electrolytic nature of salts based on their relative solubility	Ch. 15		TMA
Instructional Objective 1235.31 Use quantitative relationships involved in acid/base chemistry and titrations			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Describe the self-ionization of water	Ch. 16		EOC, TMA
02	Define [H₃O⁺], [OH^-], pH, and pOH and use their relationship to calculate any three if given the fourth.	Ch. 16		EOC, TMA
03	Use molarity to calculate [H₃O⁺],[OH^-], pH, and pOH	Ch. 16		EOC, TMA
04	Understand the concept of acid-base neutralization and be able to do molarity titration calculations given appropriate data	Ch. 16 Lab: Titration		EOC, TMA

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Unit 9	*Equilibrium (Optional)*	2 weeks

Instructional Objective 1235.32 Explain the concept of chemical equilibrium as a dynamic state			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Define chemical equilibrium and the conditions under which chemical equilibrium occurs	Ch. 18		TMA
02	Explain the nature of the equilibrium constant	Ch. 18		TMA
03	Write chemical equilibrium expressions and carry out calculations involving them	Ch. 18		TMA
Instructional Objective 1235.33 Recognize and explain factors that influence whether a chemical system will reach equilibrium and factors that will disturb a chemical equilibrium			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Discuss factors that disturb equilibrium and predict direction of equilibrium shifts	Ch. 18 Lab: Le Chatelier�s		TMA
02	Identify and discuss conditions where reactions go to completion	Ch. 18		TMA
Instructional Objective 1235.34 Discuss acid ionization equilibrium and carry out calculations associated with this type of equilibrium			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain the concept of acid ionization constants and write acid ionization equilibrium expressions	Ch. 18		TMA
02	Relate the ionization constant of water to acid ionization constants and base ionization constants	Ch. 18		TMA
03	Explain the common ion effect and how it relates to buffer systems	Ch. 18 Lab: Common Ion		TMA
04	Calculate pH of acid and bases using acid ionization constants	Ch. 18		TMA
Instructional Objective 1235.35 Discuss solubility equilibrium and carry out calculations associated with this type of equilibrium			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain what is meant by solubility product constants and calculate their values	Ch. 18		TMA
02	Calculate solubilities using solubility product constants	Ch. 18		TMA
03	Predict whether a precipitate will form when solutions are combined based of calculations using solubility product constants	Ch. 18		TMA

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Unit 10	Reaction Kinetics and Mechanisms	2 weeks

Instructional Objective 1235.36 Explain the changes in heat energy that occur during chemical reactions			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Define temperature and heat and state the units of both	Ch. 17		EOC, TMA
02	Explain heat of reaction, heat of formation, heat of combustion and enthalpy	Ch. 17		EOC, TMA
Instructional Objective 1235.37 Demonstrate ability to solve thermochemical problems			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Perform specific heat calculations	Ch. 17		EOC, TMA
02	Solve problems involving heats of reactions, heats of formation, and heats of combustion	Ch. 17		EOC, TMA
Instructional Objective 1235.38 Identify and explain the forces that drive a chemical reaction			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain the relationship between enthalpy changes and the tendency of a reaction to occur	Ch. 17		EOC, TMA
02	Explain the relationship between entropy changes and the tendency of a reaction to occur	Ch. 17		EOC, TMA
03	Discuss the concept of free energy as how it can be used to predict reaction spontaneity	Ch. 17		TMA
Instructional Objective 1235.39 Summarize reaction mechanisms			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain the concept of reaction mechanism	Ch. 17		TMA
02	Restate key concepts of the collision theory and use these to interpret chemical reactions	Ch. 17		TMA
03	Relate activation energy to heat of reaction	Ch. 17		TMA
Instructional Objective 1235.40 Describe the factors that influence the rates of chemical reactions			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Define chemical kinetics and explain two conditions necessary for chemical reactions to occur	Ch. 17		EOC, TMA
02	Discuss factors that influence reaction rate	Ch. 17		EOC, TMA
03	Identify and explain catalysts and how they influence reaction rate	Ch. 17		EOC, TMA
04	Explain and write rate laws for chemical reactions	Ch. 17 Lab: Rate Law		TMA

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Unit 11	*Oxidation Reduction Reactions* (Optional)	2 weeks

Instructional Objective 1235.41 Understand the concept of oxidation-reduction and be able to identify these reactions and their essential parts			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Assign oxidation numbers to elements in a compound or ion	Ch. 19		TMA
02	Identify a substance being oxidized or reduced; identify oxidizing agents and reduce agents	Ch. 19		TMA
03	Explain and use the activity series of metals	Ch. 19		TMA
Instructional Objective 1235.42 Apply appropriate rules to balance oxidation-reduction reactions			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Balance oxidation-reduction reactions	Ch. 19 Lab: Redox Titration		TMA
Instructional Objective 1235.43 Apply oxidation-reduction concept to electrolytic and voltaic cells			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Define a voltaic cell and write the equations for the oxidation-reductions reaction involved	Ch. 19		TMA
02	Calculate cell potentials using a table of standard electrode potentials	Ch. 19 Lab: Making Batteries		TMA
03	Define an electrolytic cell and identify the oxidation-reduction reaction involved	Ch. 19		TMA

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Unit 12	*Nuclear Chemistry* (Optional)	1 week

Instructional Objective 1235.44 Explain unique structure of carbon and its importance to inorganic chemistry			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Explain how the structure and bonding of carbon leads to the diversity and number of organic compounds	Ch. 20		TMA
02	Explain the importance and limitations of molecular and structural formulas	Ch. 20		TMA
Instructional Objective 1235.45 Recognize homologous series and functional groups and use the IUPAC nomenclature system			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Distinguish between structure of saturated and unsaturated hydrocarbons	Ch. 20		TMA
02	Explain how hydrocarbon structure relate to their properties and uses	Ch. 20		TMA
03	Classify and name organic compounds according to their functional groups	Ch. 20		TMA
Instructional Objective 1235.46 Recognize simple reactions involving organic molecules and understand basic concepts of polymerization			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Describe and distinguish between types of organic reactions	Ch. 20		EOC, TMA
02	Describe how differences in general structures in polymers contribute to their properties and uses	Ch. 20 Lab: Polymer�s		EOC, TMA

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Unit 13	*Organic Chemistry (Optional)*	1 week

Instructional Objective 1235.47 Understand natural radioactive decay			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Recognize notable scientists in the development of nuclear chemistry	Ch. 22		TMA
02	Name and describe properties of particles given off in a natural radioactive decay	Ch. 22		TMA
03	Describe a radioactive decay series and predict nuclides formed by the loss of specific particles	Ch. 22		TMA
04	Write equations representing nuclear changes using isotopic notation	Ch. 22		TMA
Instructional Objective 1235.48 Be aware of the dangers and benefits of present and potential applications of nuclear chemistry in fields such as energy production, defense, and medicine			Standard Reference District/National
No.	Performance Objective	Resource Reference		Assessment Correlation
01	Define and explain nuclear fission reactions and relate them to their use in nuclear power plants and atom bombs	Ch. 22		TMA
02	Define and explain the importance of nuclear fusion	Ch. 22		TMA
03	Discuss mass-energy relationships in nuclear reactions	Ch. 22		TMA
04	List several uses of nuclear chemistry and explain the benefits and dangers related to each	Ch. 22		TMA

Appendix: Laboratory Exercises

Accuracy and Precision
Separation of a Mixture
Evidence of Chemical Change
Determination of Density
The Mole
The Flame Test
The Periodic Table
Mendeleev for a Day
Halogen Lab
Types of Chemical Bonds
Molecular Models
Evidence for Chemical Change
Types of Chemical Reactions
Decomposition of Sodium Bicarbonate
Boyles Law Lab
Molar Volume of a Gas
Heat of Fusion
Phase Change
Heats of Solution
Beer�s Law
Electrolytes
Ice Cream Lab
pH of Household Items
Titration

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