Eleanor Roosevelt High School
Dimitri Saliani, Principal
Angela Sterling, Instructor
2009 - 2010
Dear Parents and Students,
Welcome to our Chemistry curriculum. Chemistry is an opportunity to
probe a world that is both unseen and mysterious. The atoms which
join together in infinite combinations, the energy which journeys 92
million miles from the sun, and basically everything you will eat,
touch or breathe in today is a part of chemistry.
This year even the simplest things like water will never be viewed as
simple again. You will understand both the beauty and terror of an
atom split apart and why nature favors disorder! Our curriculum is
enriched and thus goes beyond the textbook. There are worlds
between what we call a solid and liquid, as there are subatomic
particles composed of sub-sub atomic particles! Where it all began or
ends is the eternal question, but you will enjoy exploring the
possibilities!
You will learn to observe, inquire, and perform experiments to
reinforce your understanding. Extra help will always be available. I
look forward to a wonderful year together.
A. Essential Questions for Chemistry/Physical Environment
 What is the structure of matter and how do we explain its
properties?
 What are the different forms of energy and how is energy
conserved and converted into matter?
 How do we explain the behavior of radioactive isotopes and
how can they beneficial in medicine, dating of materials,
nuclear power, and industry?
 How do the Laws of Thermodynamics and the concept of
entropy explain whether a given chemical reaction will occur?
B. Chemistry Course Objectives
 Students will use scientific inquiry, mathematical analysis, and
deductive and inductive reasoning to ask questions, seek
answers, and develop solutions.
 To develop an understanding of the components of matter and
how the interaction of these components forms everything in
our universe.
 Students will be able to explain how matter and energy are
interrelated and interact through forces that result in motion.
 Students will comprehend what changes that can occur in the
nucleus of an atom and the implications of this phenomenon.
C. Resources and Materials
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Notebook
= 2 or 3 ring binder with section tabs
In the following sequence:
 Section 1 = Class notes
 Section 2 = Class handouts
 Section 3 = Reference table
 Section 4 = Homework
 Section 5 = Vocabulary
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A TI-83 (or higher) calculator should be with you each day
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Chemistry Reference Table
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Hi-lighter marker and ruler
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Textbook
= Chemistry by LeMay/Beall by Prentice Hall
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Review Book = Brief Review for Chemistry/Prentice Hall
D. Grading Policy
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Examinations
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Laboratory
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Homework
55%
20%
25%
E. Chemistry Course Outline
Term 1
Unit 1 Nature of Science - Dimensional analysis
 What are the units of measurement used in chemistry?
 How do we define SI base units for time, length
mass and temperature?
 How do we express numbers in scientific notation?
 How do we define and compare accuracy and precision?
 How do we use significant figures and rounding to reflect
the certainty of our data?
 How can percent error describe the accuracy of experimental
data?
Unit 2 Matter Chemical and Physical Changes
 How do we compare/contrast elements, compounds,
substances, and mixtures?
 How do we distinguish between physical and chemical
properties?
 How do we differentiate the physical states of matter?
 How do we apply the law of conservation of mass to chemical
reactions?
 How do we classify mixtures as homogeneous or
heterogeneous?
 Explain how all compounds obey the laws of definite and
multiple proportions?
Unit 3 Gases, liquids and solids
 How do we distinguish the different states of matter, solid,
liquid and gases?
 What does standard temperature and pressure (STP) mean?
 What is melting, boiling, and freezing point?
 What phase changes occur in a heating curve?
 What phase changes occur in a cooling curve?
 How do we determine the heat of fusion and vaporization?
 What is happening at the molecular level when a substance is
at its heat of fusion/vaporization?
 What is sublimation?
 How does the kinetic molecular theory describe the behavior of
gases?
Unit 4 Atomic Structure
 How do we compare the Dalton, Thomson, and Rutherford
models of the atom?
 Describe the placement of protons, neutrons, and electrons
according to the nuclear model of the atom.
 How do we describe and apply the terms atomic number, mass
number, and isotope?
 How do we calculate the atomic mass of an element?
 What is an isotope?
 How do we define and apply the terms molecule, ion,
monoatomic and polyatomic?
 Describe the Bohr model and its relationship to atomic spectra.
 How do we describe the modern wave-mechanical model
and its relationship to electron configuration?
 How do we apply the terms principal energy level, sublevel,
orbital, ground state, excited state, spin state, valence
electron and create Lewis structures?
Unit 5 Chemical Bonding
 Explain how energy/stability are related to chemical bonds.
 How do we compare/contrast ionic and covalent bonding?
 How do we draw a Lewis structure for simple ions and
covalently bonded molecules?
 What is the difference between polar and nonpolar covalent
bonding?
 How can we predict whether a bond will be ionic or covalent?
 What is a dipole?
 What is a hydrogen bond?
 How do we compare/contrast metallic, ionic, and covalent
bonds?
 How is the polarity of a molecule related to its symmetry?
 What are intermolecular forces and what are the different types?
Unit 6 Nomenclature
 How do we distinguish between a structural, molecular, and
empirical formula?
 How do we write formulas using the IUPAC system?
 What is an oxidation number?
 How do we assign oxidation numbers to elements, simple ions,
and elements in compounds?
 How do we write chemical equations using names and chemical
formulas?
 How do we balance equations?
 When do we classify a chemical reaction as a synthesis,
decomposition, single or double replacement?
Unit 7 Periodic trends
 What is the periodic law of Moseley?
 Describe the arrangement of elements in the Periodic table
in terms of electron configuration.
 How do the properties of metallic elements differ from the non
metallic elements?
 What is a metalloid?
 What is the difference between an ionic radius and an atomic
radius?
 How do the following behave in terms of groups and periods:
metallic character, atomic radius, ionization energy, electron
affinity, ionic radius and electronegativity?
 How do the properties of the transition elements compare with
those of the representative elements?
 What is ionization energy?
 What is electronegativity?
Unit 8 Chemical Reactions
 Define the terms systems and surroundings as they relate to
chemical processes.
 What is internal energy?
 What is heat?
 Distinguish between endothermic and exothermic reactions.
 How do we define specific heat?
 How does the first law of thermodynamics relate to the law of
conservation of energy?
 How do we use heat of reaction to solve problems related to
standard heat of formation?
 How do we interpret a potential energy diagram?
 What is activation energy?
 Name and describe the factors involved in spontaneous
reactions.
 Define entropy and predict whether a given reaction leads to an
increase or decrease in entropy.
Term 2
Unit 9 Chemical Mathematics
 How do we differentiate between atomic mass unit, isotopic
mass and atomic mass?
 How do we calculate the formula mass of a substance?
 How do we define the term mole in relation to the number of
particles and the mass of the substance?
 What is molar mass?
 How do we calculate molar mass?
 How do we calculate the molecular formula of a substance
given its empirical formula and molar mass?
 How do we calculate the empirical formula of a substance from
its percent composition by mass?
 How do we solve mole and mass problems involving chemical
equations?
Unit 10 Thermodynamics
 How do we distinguish between potential and kinetic energy?
 How do we calculate the amount of heat absorbed or released
by a substance as its temperature changes?
 Describe how a calorimeter is used to measure energy released
or absorbed.
 What is enthalpy and how does it relate to chemical processes?
 Describe how energy is lost or gained during changes of state.
 How do we calculate the heat gained/released in a reaction?
 How does one calculate enthalpy changes during a reaction?
 Differentiate between spontaneous and non spontaneous
processes.
Unit 11 Kinetics/Equilibrium
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Define the term chemical kinetics.
What factors affect the rate of a reaction?
What is dynamic equilibrium?
Provide examples of phase and solution equilibria.
What is chemical equilibrium?
What is Le Chatelier’s principle?
How do we use Le Chatelier’s principle to determine the effects
of changes in concentration, volume, temperature, catalysts,
and the addition of an inert gas?
 How do we write equilibrium-constant expressions for a
homogeneous/heterogeneous reaction?
 How do we describe the effect of temperature on the
equilibrium constant?
Unit 12 Solutions
 How do we define solution, solute and solvent?
 What is a miscible, saturated, unsaturated or supersaturated
solution?
 What factors affect the solubility of a solution?
 What are the solubility rules?
 How do we use the solubility rules to predict solubility?
 How do we interpret a solubility curve?
 Define the term electrolyte.
 How does the solute affect the freezing/boiling point of a
solution?
Unit 13 Oxidation-Reduction
 How do we compare/contrast oxidation and reduction?
 What is a redox reaction?
 How do you write oxidation/reduction reactions for redox
equations?
 When will a redox reaction occur spontaneously?
 What is a voltaic cell?
 What is a salt bridge?
 Describe electron movement in a voltaic cell.
 Define the term standard electrode potential.
 How do we calculate the potential difference of a voltaic cell?
 What is electrolysis and how do you draw a simple
electrolytic cell?
 What is the basic concept behind electroplating?
 How can you describe the electrolysis of fused salts?
Unit 14 Nuclear Chemistry
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What are the common nuclear particles and their symbols?
What is a nuclide?
What is the process of transmutation?
Describe the process of radioactive decay.
What are the various types of radioactive decay?
Define the term half-life.
How are radioactive isotopes used?
What happens during nuclear fission?
Describe the four fundamental forces in the universe.
Unit 15 Acids and Bases
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What is an acid/base?
What is the Arrhenius definition of an acid/base?
How do we solve acid-base titration problems?
What is the Bronsted-Lowry definition of an acid/base?
What is a conjugate acid-base pair?
Define the terms PH and POH.
 What are the properties of acid/base indicators?
 What is a Lewis acid/base?
Unit 16 Organic Chemistry
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What is the difference between an organic/inorganic substance?
Describe the bonding of carbon in simple organic compounds.
What is a hydrocarbon?
What is the difference between an alkene, alkane and alkyne?
What is a functional group?
What is a polymer?
What are the following organic reactions:
fermentation, esterification, saponification, combustion,
addition, and substitution?
F. Review for the New York State Regents examination
In January the students are asked to purchase the Barrons
Regents Review Book. In addition, the New York State
Regents provides several online study aids such as:
 www.nysedregents.org
 www.nysl.nysed.gov/regentsexams
 www.regentsprep.org
 www.amazon.com/NewYorkStateRegents-exam
 www.chemthink.org
 www.dbchem.net/resource/review
The following
extra help:
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books can be purchased at Barnes and Noble for
Chemistry Demystified by Linda Williams
Chemistry for Dummies by John T. Moore
Cliffs Study Solver
by Charles Henrickson