Download Chemistry 11 Review Checklist

Chemistry 11 Final Exam Review Checklist
Unit 1 – Skills and Processes
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Safety equipment in classroom
Protocol if a fire occurs
Lighting bunsen burners
Creating conversion factors
SI units
Multi-step unit conversions
Metric conversions
Derived quantities
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Significant figures
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Accuracy and precision
Reading scales (to the correct
number of significant figures)
Uncertainty in scales
Scientific notation
Carrying out calculations with
significant figures
(multiplication/division and
addition/subtraction)
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Experimental definitions
Valence electron counting
Naming simple ionic
(metal/non-metal)
compounds
Writing chemical formulae
of simple ionic (metal/nonmetal) compounds
Lewis structures of ionic
compounds
Naming polyatomic ionic
compounds
Writing chemical formulae
of polyatomic ionic
compounds
Naming hydrates
Writing chemical formulae
of hydrates
Common acids
Naming covalent
compounds
Writing chemical formulae
of covalent compounds
Classifying compounds as
ionic or covalent
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Classification of substances
(element, compound, solution,
mechanical mixture)
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Physical separation methods (hand
separation, filtration, evaporation,
distillation, solvent extraction,
recrystallization, gravity separation,
chromatography)
Unit 4 – The Mole
Design of experiments for separation
of mixtures
Heating and cooling curves
Physical and chemical changes
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Kinetic energy
Kinetic Molecular Theory
Chemical symbols on periodic table
of elements
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Lewis structures of atoms
Physical and chemical properties
Unit 3 – Chemical Bonding, Structures
and Nomenclature
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Density
Unit 2 – Nature of Matter
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Lewis structures of covalent
compounds
Molecular geometry
(VSEPR)
Avogadro’s number
Atomic mass units
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Calculating molar mass of
elements and compounds
Calculations involving
molar mass
Avogadro’s hypothesis
STP
Molar volume of gas at STP
Multiple conversions using density,
molar mass, molar volume, atom
count
Calculating percent composition
from chemical formulae
Calculating empirical and molecular
formulae from percent composition
Calculating empirical and molecular
formulae from mass distribution of
compound
Calculating concentration of
solutions in units mol/L (M)
Calculating mass of solute required
to produce solution of set molarity
Calculating resulting concentrations
after dilution with water
Calculating resulting concentrations
after mixing two solutions
Unit 5 – Chemical Reactions
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Understanding the idea of
“1 mole of a substance”
Particles (atom, molecule or
formula unit)
Calculations between moles and
particles (atom, molecule or formula
unit)
Conservation Laws
Open/closed systems
Balancing chemical reactions
Writing chemical word equations
from chemical (symbol) equations
Writing chemical (symbol) equations
from chemical word equations
Writing phase designations in
chemical equations
Types of chemical reactions
(synthesis, decomposition, single
replacement, double replacement,
neutralization, combustion)
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Energy changes in reactions
(endothermic, exothermic)
Unit 6 – Stoichiometry
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Creating mole bridges/ratios from
balanced equation
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Perform stoichiometric calculations
involving moles, mass, gas volume
and molecules
Titration-based stoichiometric
calculations
Stoichiometry of excess quantities
Determining limiting reactant
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Calculations involving percentage
yield
Calculations involving percentage
purity
Unit 7 – Atomic Theory
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Unit 8 – Solution Chemistry
Law of Definite Proportions
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Law of Multiple Proportions
Law of Conservation of Mass
Atomic theory contributions by John
Dalton, J.J. Thomson, Henri
Becquerel, Marie and Pierre Curie,
Ernest Rutherford, James Chadwick,
Niels Bohr, J. Robert Oppenheimer
Bohr model of atom
Bright-line emission spectra
Explanation of electron excitation
and relaxation
Flaws of the Bohr model of atom
Atomic number, atomic mass
number, atomic mass
Isotopes and isotopic distribution
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Electron configuration (including
core notation) for atoms or ions
Energy Rule, Hund’s Rule and Pauli
Exclusion Principle
Different groups in the periodic table
Trends in atomic properties (atomic
radius, ionic radius, ionization
energy, electronegativity and
conductivity)
Trends in atomic properties, as
explained by electron configuration
or nuclear charge)
Common ion charges for main group
elements
Saturated, unsaturated and
supersaturated solutions
Conductivity of solutions
Van der Waals forces
(London forces, dipoledipole forces, hydrogen
bonding)
Polar versus non-polar
molecules
Relative strength of bonds
Explanation of
melting/boiling, with
regards to intermolecular
forces
“Like dissolves like”
Solubility of polar and ionic
solutes
Solubility of non-polar
solutes
Dissociation reactions
Calculating individual ion
concentrations in solution
Calculating individual ion
concentrations when mixing
solutions
Unit 9 – Organic Chemistry
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Quantum mechanical model of atom
Orbitals, shells and subshells
Solute, solvent, aqueous
solutions and solubility
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Definition of organic
chemistry
Allotropes
Alkanes, substituted
alkanes, and cycloalkanes
(naming, recognition,
geometry)
Structural isomers
Alkyl halides (naming,
recognition)
Alkenes (naming,
recognition, geometric
isomerism)
Alkynes (naming,
recognition)
Aromatic rings (naming,
recognition, resonance)
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Alcohols (naming, recognition,
properties)
Ethers (recognition, properties)
Aldehydes (recognition)
Ketones (recognition)
Carboxylic acids (recognition)
Esters (recognition)