Download Chemistry COS 2011-2012

Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Acid, Base, and Salt Solutions
CONTENT STATEMENT
 Acids and bases are frequently encountered in our daily lives in the
environment, in the foods we eat, but most importantly, in our bodies.
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Acids, in general, are proton donors while bases are proton acceptors.
Acids and bases react in a neutralization reaction to form a salt and water.
Unknown solutions can be titrated with a standard using an acid-base indicator.
Weak acids and bases reach equilibria in aqueous solutions. These can be
calculated using pH and pOH equations.
Buffers protect living organisms by resisting changes in pH when limited amounts
of acids or bases are added from physiologic processes or diet.
CONCEPTS
VOCABULARY
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Acids and bases
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Salts and solutions
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Water equilibria
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Titration
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Electrolyte
Hydronium ion
Conjugate acid and base
Binary and ternary acid
Amphoteric,
Anhydrides
Spectator ions
Neutralization
Salt
Ionization constant
pH
pOH
Titration
Indicator
Buffers
Ion product constant
Grade 10-12: Chemistry
2011-2012
Science Course of Study
PERFORMANCE SKILLS:
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Distinguish the definitions of acids and bases as outlined in the theories of Arrhenius,
Bronsted-Lowry and Lewis
Name acids and bases
Define acidic and basic anhydrides and write their formulas
Define and give examples of strong and weak acids and bases
Explain the concepts of neutralization and the composition of a salt and be able to
name salts
Write net ionic equations
Derive and use ionization constants
Compute the percent ionization of a weak electrolyte
Explain the concepts of solubility product and solve problems using the solubility
product constant
Solve problems using the ion product constant of water
Explain how the pH scale is used for measuring solution acidity
Describe the process of hydrolysis and buffering
State the principles and uses of indicators
Explain the process of titration and perform calculations using the data from titrations
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Energy
CONTENT STATEMENT
 The transfer of energy and how energy interacts with matter is the driving force
behind human processes, geologic systems and atmospheric conditions.
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Energy can be released (exothermic) or gained (endothermic) during both
chemical and physical reactions.
Energy of a reaction can be measured with a colorimeter using Joules.
Chemical reactions require activation energy to proceed from reactants to
products.
Heat and temperature are not the same thing. Specific heat is the amount of
energy required to heat 1 g of a substance 1 degree Celsius.
CONCEPTS
VOCABULARY
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Energy transfer
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Energy and Chemical Change
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Measuring energy changes
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Calorimeter
Activation energy
Endothermic
Exothermic
Heat
Joule
PERFORMANCE SKILLS:
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Describe conditions under which heat is transferred
Convert between units
Describe exothermic and endothermic processes
State the function of activation energy
Perform calculations involving specific heat
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Thermodynamics
CONTENT STATEMENT
 Heat released or absorbed in chemical reactions is proportional to the amounts
of reactants consumed. When a reversible process occurs, the same amount of
energy is involved no matter which way the reaction proceeds. The difference
will be if the energy is released or absorbed.
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Potential energy is stored whenever work must be done to change the distance
between two objects. Chemical potential energy is the result of electrostatic
attractions between atoms.
Energy transferred in a reaction will be the same regardless of the chemical
pathway. This relationship is called Hess’s Law.
In an exothermic reaction, the products have less energy than the reactants. In an
endothermic reaction, the products have more energy than the reactants.
Changes of state require a transfer of energy. Water has unusually high-energy
changes associated with its changes of state.
CONCEPTS
VOCABULARY
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Introduction to thermodynamics
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Driving forces of chemical reactions
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Isothermal
Isobaric
Thermodynamics
Internal energy
Enthalpy
Hess’s law
Gibbs free energy
Exergonic
Endergonic
PERFORMANCE SKILLS:
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State reasons why reactions occur
Calculate changes in internal energy
Explain why energy changes occur in chemical reactions and perform calculations
Relate Gibbs free energy to the spontaneity of reactions and to equilibrium
Perform calculations involving Gibbs free energy and entropy, equilibrium constants
or cell voltage
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Kinetic Theory: Solids, Liquids and Gases
CONTENT STATEMENT
 Atoms and molecules are constantly in motion, as a substance changes phase, the
movement of the atoms or molecules that make up that substance also changes.
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Gas molecules undergo random motions in a container. This causes them to
collide into each other as well as the surface of the container.
Spaces between molecules in a gas are larger than spaces in liquids, which are
larger than spaces in solids.
The properties of gasses can be determined through a combination of equations
derived from the ideal gas law.
Diffusion is the gradual mixing of two substances due to the spontaneous random
motion of their particles. Effusion is the process of a molecule randomly passing
through a tiny opening in a container.
Grade 10-12: Chemistry
2011-2012
Science Course of Study
CONCEPTS
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Pressure
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Motion and physical states
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Variable conditions of the gas laws
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Avogadro’s Principle
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Gas Stoichiometry
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Crystal structure
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Changes of State
VOCABULARY
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Kinetic theory
Pressure
Manometer
Barometer
Absolute zero
Mean free path
Point mass
Ideal gas
STP
Boyle’s Law
Dalton’s Law
Charles’ Law
Graham’s Law
Diffusion
Effusion
Molar volume
Ideal gas equation
Limiting and excess reagents
Unit cells
Macromolecule
Doped
Network crystals
Isomorphous
Polymorphous
Hygroscopic
Deliquescent
Anhydrous
Liquid crystal
Vapor
Equilibrium
Sublimation
Triple point
Enthalpy
Grade 10-12: Chemistry
2011-2012
Science Course of Study
PERFORMANCE SKILLS:
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List and explain the basic assumptions of the kinetic theory
Relate pressure to molecular motion
Describe characteristics of solid substances
Explain relationship of melting point to bonding type and crystal type
Distinguish isomorphous and polymorphous crystals
Identify and explain crystal defects
Describe semiconductors
Distinguish between hydrated ions and anhydrous substances
Describe the structure and properties of crystals, liquid crystals and amorphous solids
Describe the properties of liquids and changes of state in terms of kinetic theory
Use LeChatelier’s principle to explain reversible changes
Determine the relationship between energy and change of state and perform related
calculations
Differentiate among open and closed arm manometers
Calculate the pressure of gases using manometers
Relate temperature and energy transfer to molecular motion
Determine the relative velocities of gas molecules at the same temperature
Differentiate among the four states of matter
Explain the concepts of an ideal gas
Describe the conditions of STP
Relate and perform calculations using gas laws
Differentiate between an ideal gas and a real gas
State Avogadro’s principle
Define molar volume
Explain, use and manipulate the ideal gas equation
Solve gas stoichiometry problems
Identify the limiting reactant and solve problems based upon it
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Organic Chemistry
CONTENT STATEMENT
 Carbon is found in nature both as an element and in combined form. It is
exceedingly important because it is found in all living matter.
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Different variations of carbon-carbon bonding allows for different carbon
allotropes: Diamond, graphite and fullerenes.
Carbon atoms can form single double and triple bonds, as well as ringed
structures with itself or with other atoms, leading to a large diversity of organic
compounds.
Hydrocarbons are long chains that contain a carbon backbone. They have many
uses and are of significant importance in today’s world. They can be saturated –
containing only single bonds – or unsaturated – containing double or triple bonds.
CONCEPTS
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Hydrocarbons
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Organic reactions and products
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Biochemistry
VOCABULARY
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Alkanes
Alkenes
Alkynes
Single, double and triple bonds
Benzene
Aromatic
Radicals
Branches
Functional groups
Saponification
Polymer
Octane rating
Enzyme
Protein
Amino acid
Carbohydrate
Fat
Grade 10-12: Chemistry
2011-2012
Science Course of Study
PERFORMANCE SKILLS:
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Differentiate between different types of hydrocarbons
Identify, name and write structural formulas for hydrocarbons
Differentiate between functional groups
Describe esterification, polymerization and condensation reactions
Describe the processing of petroleum and the octane rating of gasoline
Explain how synthetic fibers, plastics and elastomers are produced industrially
State the structure and function of the four main biomolecules
Describe the progress in and problems associated with the biomaterials industry
TOPIC: Periodic Table
CONTENT STATEMENT
 Diversity of species occurs through gradual processes over many generations.
Fossil records provide evidence that changes have occurred in number and types
of species.
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Fossils provide important evidence of how life and environmental conditions have
changed.
Changes in environmental conditions can affect how beneficial a trait will be for
the survival and reproductive success of an organism or an entire species.
Throughout Earth’s history, extinction of a species has occurred when the
environment changes and the individual organisms of that species do not have the
traits necessary to survive and reproduce in the changed environment. Most
species (approximately 99 percent) that have lived on Earth are now extinct.
Grade 10-12: Chemistry
2011-2012
Science Course of Study
CONCEPTS
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Developing the periodic table
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Using the periodic table
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Periodic trends
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Reaction Tendencies
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Hydrogen and the main group metals
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Nonmetals
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Transition metals
VOCABULARY
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Groups
Periods
Families
Metals
Nonmetals
Metalloids
Transition metals
Triads
Mendeleev
Moseley
Atomic radii
Noble gas configurations
Stable configurations
First ionization energy
Shielding effect
Electron affinity
Ionic radius
Hydrogen ion
Hydride ion
Catalyst
Allotrope
Amphoteric
Galvanizing
Grade 10-12: Chemistry
2011-2012
Science Course of Study
PERFORMANCE SKILLS:
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Describe the early attempts at classifying elements
Use the periodic table to predict the electron configurations of elements
Explain the basis for the arrangement for the modern periodic table
Identify, characterize and give uses for metals, nonmetals and metalloids using the
periodic table
Relate chemical reactivity of the families due to similar electron configurations
Predict the chemical stability of the atoms using the octet rule and Hund’s rule
Use examples to explain the periodic properties of elements
State how atomic and ionic sizes change in groups and periods
Predict oxidation numbers of elements
Define ionization energy, electron affinity and shielding effect and its importance to
reactivity
Describe the factors that affect ionization energy and electron affinity
Use multiple ionization energies to predict oxidation numbers of elements
List ways in which hydrogen can bond and give examples
Relates importance of elements to everyday life
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Atomic Structure and Quantum Theory
CONTENT STATEMENT
 Atoms are the base unit of all matter in the universe. They are the structural
make-up for all substances that we know of.
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Atoms are made up of a nucleus of protons and neutrons which are surrounded by
a cloud of charged electrons.
Inside of an atom, neutrons have no charge, while protons are positively charges
and electrons are negatively charged. Protons and electrons exist in equal
quantities in all atoms, so the overall charge of all atoms is zero.
Atoms are organized and categorized by there properties as well as the number of
protons they contain in their nucleus.
The wave properties of electrons can be mathematically described through the
quantum theory developed by Heisenberg and Schrodinger.
Light is a form of electromagnetic radiation and exhibits properties of both a
particle and a wave, giving it many unique attributes and characteristics.
Grade 10-12: Chemistry
2011-2012
Science Course of Study
CONCEPTS
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Early atomic models
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Parts of the atom
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Modern atomic structure
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Quantum theory
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Electron configurations
VOCABULARY
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Rutherford
Bohr
Dalton
Nucleus
Protons
Neutrons
Electrons
Quarks
Leptons
cathode ray tubes
Isotopes
Atomic number
Average atomic mass
Mass spectrums
Spectroscopy
Electromagnetic spectrum
Emission spectra
Absorption spectra
Planck’s constant
Quantum theory
Photons
Wave-particle duality of nature
Heisenberg uncertainty principle
Sublevels
Orbitals
Pauli exclusion principle
Lewis dot structures
Schrodinger’s equation
Grade 10-12: Chemistry
2011-2012
Science Course of Study
PERFORMANCE SKILLS:
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Discuss early developments in atomic theory
Explain the laws of definite and multiple proportions and give examples
Determine the atomic number (Z) and mass number (A) of given isotopes of elements
Differentiate among the major subatomic particles
Discuss the development of modern atomic theory
Calculate the average atomic mass
Calculate problems using E=h
Compare and contrast relative sizes and masses of subatomic particles
Describe the wave-mechanical view of the hydrogen atom
Characterize the position and velocity of an electron in an atom
Describe an electron cloud
Characterize the four quantum numbers
Use the Pauli exclusion principle and quantum numbers to describe an electron in an
atom
Determine the electron configurations of the elements
Write Lewis dot structures
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Reaction Rate and Chemical Equilibrium
CONTENT STATEMENT
 Knowledge of the rate of a reaction and its equilibrium gives important
information about chemical processes.
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Reaction rate can be fast or slow. The lower the activation energy, the faster the
reaction
Reaction rates and equilibrium can be controlled by changing concentration,
pressure and temperature of the reactants and products.
Catalysts speed up reactions by providing an alternative pathway with a lower
activation energy.
When a reaction is at equilibrium, the rates do not change.
Le Chatelier’s principle explains what happens when a stress is put on a system
already at equilibrium.
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CONCEPTS
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Reaction Rates
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Chemical equilibrium
VOCABULARY
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Thermodynamically stable
Kinetically stable
Reversible reactions
Reaction rate
Catalysts
Inhibitor
Rate determining step
Reaction mechanism
PERFORMANCE SKILLS:
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Distinguish between thermodynamic and kinetic stability
List and describe factors that influence the rate of reaction
Distinguish among heterogeneous and homogeneous catalysts and inhibitors
Describe and determine reaction mechanisms for simple reactions
Determine an equilibrium expression
Use Le Chatelier’s principle to explain the effects of changes on equilibrium
Calculate equilibrium constants and concentrations of reactants or products
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Solutions and Colloids
CONTENT STATEMENT
 Systems containing more than one component are mixtures. Mixtures can be
either homogeneous or heterogeneous.
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A solution is when a solute is mixed with a solvent. Different concentrations of
solutions can be measured using molarity, molality, and percent concentration.
All substances have different solubilities which are directly affected by
temperature.
Solubility depends on the chemical make up of both the solute and the solvent.
Colligative properties depend only on the number of solute particles present.
Colligative properties include freezing point depression, boiling point elevation
and osmotic pressure.
CONCEPTS
VOCABULARY
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Solutions
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Colloids
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Vapor Pressure Changes
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Solvents
Solute
Dissociation
Salvation
Solution equilibrium
Saturated solutions
Unsaturated solutions
Supersaturated solutions
Suspension
Tyndall effect
Colligative property
Raoult’s law
Ideal solution
Semi-permeable membrane
Osmostic pressure
Grade 10-12: Chemistry
2011-2012
Science Course of Study
PERFORMANCE SKILLS:
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Describe and explain the process of solution formation
Discuss factors that effect solubility
Relate enthalpy of solution to endothermic and exothermic dissolving processes
Solve problems involving molarity, molality, mole fraction and mass percent
Distinguish, describe and characterize solutions, colloids and suspensions
State Roult’s law and use to calculate the vapor pressure of solutions
Explain how the process of fractional distillation can be used to separate components
of a solution
Identify the effects of solute particles on boiling point and freezing point of a solvent
Explain the concept of osmotic pressure
Calculate the effect of a solute on the boiling point, freezing point and osmotic
pressure of a solution
Determine the molecular mass of a solute from freezing point, boiling point or
osmotic pressure data
Relate the concept of ion activity to non-ideal solutions
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: The Mole
CONTENT STATEMENT
 The mole is the amount of substance that contains as many atoms, molecules or
ions as there are atoms in 12 g of Carbon-12.
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Avogadro’s number is equal to one mole.
Molar mass is the formula mass of a substance expressed as grams.
Percent composition of elements allows the empirical formula of a compound be
determined.
Hydrates contain a specific mole ratio of water attached to one mole of an ionic
compound.
Molarity of solutions is the number of moles of solute dissolved in 1 liter of
solution. Specific molarities of solutions are necessary for most chemical
reactions to take place.
CONCEPTS
VOCABULARY
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The mole and Avogadro’s Number
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Moles in solution
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Percent composition
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Hydrates
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Molecular and formula mass
Avogadro’s constant
Molar mass
Molarity
PERFORMANCE SKILLS:
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Use the Avogadro constant to define the mole and to calculate molecular and molar
mass
Use the molar mass to calculate the molarity of solutions, percentage composition and
empirical formulas
Determine the formulas of hydrates
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Oxidation and Reduction
CONTENT STATEMENT
 Oxidizing and reducing (redox) reactions must take place simultaneously as the
electrons involved move from one chemical species to another.
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Oxidizing agents accepts electrons while reducing agents donate electrons.
All combustion reactions are redox reactions where the compounds burned are
oxidized by oxygen.
All humans and animals get their energy from respiration, where the oxygen in
the air oxidizes carbon-containing compounds in cells.
Metals oxidize to form either protective metallic oxides or destructive metallic
oxides.
Batteries store and release electrical energy utilizing redox reactions.
CONCEPTS
VOCABULARY
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Oxidation and reduction processes
Balancing redox reactions
Oxidation
Reduction
Reducing agent
Oxidizing agent
PERFORMANCE SKILLS:
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Compare the process of oxidation with the process of reduction
Explain an oxidizing agent and a reducing agent
Describe how to assign oxidation numbers to atoms in compounds
State how to identify oxidation-reduction reactions
Explain the concept of half-reactions
Determine how to balance redox equations by the half-reaction method
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Nuclear Chemistry
CONTENT STATEMENT
 Radioactivity energy emanating from the nucleus has major uses in the health
and biological sciences. Nuclear energy is a major source of power in our
modern world.
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Radioactive nuclides are capable of producing alpha particles, beta particles and
gamma rays.
Half-life is the time it takes for one half of any sample to decay. Half-life is
important for dating historical and archeological artifacts.
Nuclear medicine is the use of radionuclei for diagnostic imaging and therapy.
Nuclear fusion releases massive amounts of energy and creates heavier elements.
Nuclear fission is the combining of two nuclei to create heavier elements. This
process takes place within stars and particle accelerators.
CONCEPTS
VOCABULARY
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Nuclear structure and stability
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Nuclear applications
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Isotopes
Accelerator
Fission
Fusion
Half-life
Nuclear reactor
PERFORMANCE SKILLS:
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Describe the operation of particle accelerators and fission reactors
Describe the probing of the nucleus through the use of accelerators and reactors
Apply three tests for relative stability of nuclides
Explain the concept of half-life and write nuclear equations
Explain how synthetic elements are produced
List the biological effects of radiation and the units used to measure them
Describe the uses of radioactive nuclides
Describe fusion reactions and the ongoing research being devoted to controlling the
fusion process
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Intermolecular Forces
CONTENT STATEMENT
 The forces of attraction between molecules are intermolecular forces (IMFs).
The strength of IMFs determine physical phases as well as solubilities.
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Dipole-dipole interactions are the strongest IMFs and exist between polar
molecules.
Hydrogen bonds are a specialized form of dipole-dipole interactions that
contribute unique qualities to substances.
London dispersion forces account for attractions between nonpolar molecules.
CONCEPTS
VOCABULARY
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Molecular attraction
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Chromatography
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Hydrogen bonding
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Polar covalent
Dipole
Intramolecular force
Intermolecular force
Chromatography
Mobile phase
Stationary phase
Hydrogen bond
Surface tension
Capillary rise
PERFORMANCE SKILLS:
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Distinguish between polar and non-polar covalent bonds
Use electronegativities to predict polarities of bonds
Compare the strengths of intermolecular forces based on dipole moments
Define and describe the types of van der Waals forces and list the three factors
contributing to them
Define chromatography, mobile phase, and stationary phase
Describe the uses for the different types of chromatography
Use polarity to explain hydrogen bonding
Explain the unique properties of water in terms of its molecular structure
Explain surface tension and capillary rise on the basis of unbalanced surface forces
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Electrochemistry
CONTENT STATEMENT
 Electrochemistry involves electricity-related applications of oxidation reduction
reactions. Redox reactions that occur naturally can be sources of electrical
energy. Electricity can drive redox reactions which do not occur naturally.
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An electrode and its electrolyte in an electrochemical cell make up half-cells.
The potential difference between an electrode and its solution is the electrode
potential.
Standard electrode potentials are measured relative toa standard hydrogen
electrode and indicate the relative strengths of substances as oxidizing and
reducing agents.
CONCEPTS
VOCABULARY
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Cells
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Quantitative electrochemistry
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Salt bridge
anode
cathode
electrochemical cell
Volt
Ampere
electrode potential
standard electrode potential
reduction potenetial
half-cell
electrolytic cell
electrolysis
Voltaic cell
PERFORMANCE SKILLS:
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Describe the construction and functioning of electrolytic and voltaic cells
Compare electrolytic and electronic conduction
Describe and use reaction cells
Use the tables of standard reduction potentials
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Classification and Properties of Matter
CONTENT STATEMENT
 Chemistry is the study of the composition, structure and properties of matter
and its changes. All matter can be classified according its chemical and physical
properties.
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Matter can be classified into elements, compounds, solutions and heterogeneous
mixtures.
Chemical changes involve a rearrangement of atoms whereas physical changes do
not.
The periodic table organizes the elements based on reoccurring properties and
increasing atomic number.
Energy changes accompany physical and chemical changes.
CONCEPTS
VOCABULARY
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Physical and chemical changes
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Physical and chemical properties
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Homogeneous and heterogeneous
materials
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Elements and compounds
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Material
Mixture
Solution
Solute
Solvent
Phase
Interface
Extensive physical properties
Intensive physical properties
Precipitate
PERFORMANCE SKILLS:
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Describe and distinguish heterogeneous and homogeneous materials
Describe and give examples of elements and compounds
Classify examples of matter
Classify changes in matter as chemical or physical
Obtain information from a graph
Distinguish among extensive and intensive physical and chemical properties
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Chemical Reactions
CONTENT STATEMENT
 When atoms rearrange to form something new, a chemical reaction has taken
place.
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Chemical reactions can be classified into five basic types where products are able
to be predicted.
Chemical reactions must be balanced so that the law of conservation of mass is
observed.
Chemical reactions can either consume or produce energy and this can be
calculated using a balanced chemical reaction.
CONCEPTS
VOCABULARY
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Chemical Equations
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Stoichiometry
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Synthesis
Decomposition
Single and double displacement
Combustion
Reactants
Products
Percentage yield
Mass-mass problems
Mass-energy problems
PERFORMANCE SKILLS:
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Write chemical equations to represent chemical reactions
Balance chemical equations
Differentiate among different types of chemical reactions
Determine the mass of a reactant or product in a mass-mass problem
Calculate the actual yield of product as a percentage of the theoretical yield
Determine the heat of reaction for a chemical reaction using mass-energy problems
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Chemical Nomenclature
CONTENT STATEMENT
 Naming and writing correct chemical formulas of atoms, compounds and
molecules are important for the efficient communication of a chemical reaction.
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Ionic compounds are held together via electrostatic attraction and named by
naming the cation first, followed by the anion.
Binary molecules are held together by covalent bonds and named using
multiplying prefixes.
Oxidation numbers are the resulting charge on an element after electrons are lost
or gained.
Metallic ions with multiple oxidation states require Roman numerals in their
name.
Polyatomic ions are held together via covalent bonds and carry a charge that is the
net sum of the oxidation numbers of the elements involved.
CONCEPTS
VOCABULARY
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Symbols and formulas
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Naming compounds
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Symbols
Polyatomic ions
Oxidation numbers
Binary compounds
Molecular formulas
Empirical formulas
Formula units
PERFORMANCE SKILLS:
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Demonstrate proficiency in writing chemical formulas
Define oxidation number and state oxidation numbers for common monatomic ions
and charges for polyatomic ions
Demonstrate proficiency for naming chemical formulas
Distinguish between molecular and empirical formulas
Demonstrate the use of coefficients
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Bonding Theory and Molecular Structure
CONTENT STATEMENT
 Bonding occurs between atoms because it is an energetically favored physical
state. The combination of bond types and atom order determine the overall
shape of a compound.
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Atoms combine with each other in order to gain an octet of electrons in their
valence shell.
Valence-shell electron-pair repulsion (VSEPR) predicts bond angles and
molecular shapes.
An asymmetrical distribution of charge on a molecule contributes a degree of
polarity.
Metallic bonding is a result of delocalized electrons and this give metals
characteristic properties, such as malleability and luster.
CONCEPTS
VOCABULARY
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Bond formation
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Particle sizes
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Molecular arrangements
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Ionic bonds
Covalent bonds
Metallic bonds
Bond angle
Bond length\
Bond axis
Internuclear distance
Van der Waals radius
Shared and unshared pairs of electrons
Delocalization
VSEPR
PERFORMANCE SKILLS:
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Identify the type of bonding between two elements
Differentiate among properties of ionic, covalent and metallic bonds
Use covalent radii to calculate bond length
Use models to demonstrate the structure of molecules
Grade 10-12: Chemistry
2011-2012
Science Course of Study
TOPIC: Chemistry and the Chemistry Lab
CONTENT STATEMENT
 The lab is an integral part of learning chemistry. Experimentation allows the
students to see first-hand how manipulating variables directly affects the
outcome.
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All equipment in the lab has a specific purpose and proper handling technique.
Each piece of measuring equipment has its own precision which directly
contributes to significant digits, accuracy and calculations.
Safety rules must be followed at all times to ensure accidents are avoided.
CONCEPTS
VOCABULARY
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Lab Safety
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Measurements
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Equipment
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Scientific method
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The chemist
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Scientific processes
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PERFORMANCE SKILLS:
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Locate safety equipment and be able to use it.
Read and follow directions.
Listens and follows safety instructions
Goggles
Aprons
Close-toed shoes
Horse-play
Metric system
Significant digits
Accuracy
Precision
Beakers
Graduated cylinders
Pipets
Inquiry
Theory
Law
Conclusions
Experiment
Research