Chem 20 Alberta

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1) Chemistry Review
Key Terms:
empirical knowledge
theoretical knowledge
law of conservation of mass
coefficient
chemical amount
mole

Key Concepts:
Write chemical equations when given reactants and products (1.5, 1.6) Write balanced chemical equations (2.2, 2.3)
Interpret balanced chemical equations in terms of chemical amount (in moles) (2.3) Convert between chemical amount and mass (2.4)
Classify chemical reactions (2.5, 2.6)
Predict the solubility of elements and ionic and molecular compounds in water (2.6) Predict products for chemical reactions (2.5, 2.6)
Memorized molecular compounds pg. 34

Sample Questions:
Chapter One Review pg. 40 #11-19, 25 Chapter Two Review pg. 66 #5-7, 9 Unit Review pg. 68 #1-8, 11-25 Are You Ready pg. 74 #2-8

2) Chemical Bonding
Key Terms:

structural formula
valence electron
orbital
valence orbital
bonding electron
lone pair
octet rule
Lewis formula
electronegativity
covalent bond
ionic bond
bonding capacity
empirical formula
molecular formula
structural formula
VSEPR theory
polar molecule
nonpolar molecule
nonpolar covalent bond
polar covalent bond
bond dipole
dipole–dipole force
hydrogen bond
crystal lattice
covalent network
intermolecular force
London force

Key Concepts:
Define valence electron, electronegativity, and ionic bond (3.1, 3.3) Use the periodic table and Lewis structures to support and explain ionic bonding theory (3.1) Explain how an ionic bond results from the simultaneous attraction of oppositely charged ions (3.1) Relate electron pairing to covalent bonds (3.1, 3.2)

Draw electron-dot diagrams (Lewis symbols/formulas) of atoms, molecules and ions, writing structural formulas for molecular substances & using Lewis structures to predict bonding in molecules (3.2) Apply VSEPR theory to predict molecular shapes (3.3)

Illustrate, by drawing, the structure of simple molecular substances (3.2) Explain intermolecular forces, London forces, dipole–dipole attractions, and hydrogen bonding (3.4) Relate properties of substances to the predicted intermolecular bonding in the substance (3.4, 3.5) Determine the polarity of a molecule based on structural shapes and unequal charge distribution (3.3) describe bonding as a continuum ranging from electron transfer to equal sharing of electrons. (3.3, 3.4)

Sample Questions:
Unit Review pg. 137 #3,4,6-17, 25,26,28, 32,39,41,43,47-51
3) Gases
Key Terms:

pressure
atmospheric pressure
STP
SATP
Boyle’s law
absolute zero
absolute temperature scale
Charles’ law
combined gas law
law of combining volumes
Avogadro’s theory
molar volume
ideal gas
ideal gas law
universal gas constant (R)

Key Concepts:
Convert between the Celsius and absolute (kelvin) temperature scales (4.1, 4.4) Describe the behaviour of real and ideal gases in terms of kinetic molecular theory (4.2, 4.4) Explain the law of combining volumes (4.2)

Illustrate how Boyle’s, Charles’, and combined gas laws are related to the ideal gas law (4.4) Perform calculations using Boyle’s, Charles’ and the Combined Gas Law (4.4) Perform calculations based on the ideal gas law under STP, SATP, and other conditions (4.4)

Sample Questions: Pg. 159 #20-23, Pg. 166 #7, Pg. 171 #5-7, Pg. 176 #5, 9 Unit Review pg. 181 #1-10, 12-18, 20, 21, 26-29

4) Solutions, Acids and Bases
Key Terms:

solute
solvent
electrolyte
non-electrolyte
dissociation
ionization
amount concentration
standard solution
stock solution
saturated solution
solubility
dynamic equilibrium
hydronium ion
pH/pOH
acid−base indicator
neutralization
strong and weak acid
strong and weak base
monoprotic acid or base
polyprotic acid or base

Key Concepts:
Explain the difference between dissociation and ionization (5.2) Differentiate between electrolytes and non-electrolytes (5.1, 5.2) Understand the major entities present when any substance is in a water environment (5.2: Tables 2,3)...
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