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
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 |
|
Back to Top |
|
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 |
|
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 |
|
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 |
|
Back to Top |
|
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 |
|
Back to Top |
|
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 |
|
Back to Top |
|
Unit
5 |
Stoichiometry (2nd
semester continuation) |
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 |
|
Back to Top |
|
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 |
|
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 |
|
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 |
|
Back to Top |
|
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 |
|
Back to Top |
|
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 |
|
Back to Top |
|
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 |
|
Back to Top |
|
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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Science curriculum e-mail contact:
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