SCH3U0-D
Quantities of Chemical Reactions
Gases and Atmospheric Pressure
Solutions and Stoichemetry
Solution
Components
Solvent
Golden Rule "Like Dissolves Like"
Solute
Concentration
Solution Concentrations
Percentage by Volume(L) (%V/V)
% C (m/V) = msolute/Vsolution
Percentage Mass(g) by Volume(L) (%m/V)
% C (m/V) = msolute/Vsolution
Percentage Mass(g) (%m/m)
% C (m/V) = msolute/Vsolution
Very Small Concentrations
Parts Per Million
ppm = solute/solution * 10^6
Parts Per Billion
ppb = solute/solution * 10^9
Parts Per Trillion
ppt = solute/solution * 10^12
Molar Concentrations
M = n/V
C₁V₁ = C₂V₂
Solubility
Solubility Factors
Temperature
Pressure
Subtopic
Solubility Curves
On the line, any dissolved solute
Above the line, any dissolved solute
Below the line, any dissolved solute
Saturated
Supersaturated
Unsaturated
Amount of solute per amount of solvent: e.g. 36.0 NaCl/100g of H20 at 20°C
Suspension +(precipitate)
Colloid
Chemical Reactions
Observations
Chemical Changes
Heat/Light
New Substance
Bubbles/Gas
Color
Odor
Temperature
Irreversible
Physical Changes
Temperature
Shape
Change in States of Matter
Boiling Point
Melting Point
exothermic
endothermic
Texture
Color
Chemical Composition
An indicator may not necessarily be a chemical change, but physical.
Painting a car (change in color) is a physical change. While a solution changing color is a chemical change
Types of Reactions
Reactants and Products
Synthesis
A + B -> AB
Decomposition
AB -> A + B
Neutralization
A salt and water
Combustion
Complete Combustion
Carbon Dioxide, Water Vapor, and Energy
extra oxygen gas
"Connect the extra and limited to the concept of excess reagent and limited reagent"
Incomplete Combustion
Carbon Dioxide, Water Vapor, and Energy + Carbon Monoxide and/or Soot (Carbon)
limited oxygen
Fuel
Subtopic
Subtopic
Subtopic
Displacements
Double Displacement
Precipitate
ionic formed
insouluble (connect to solutions unit)
AB + CD -> AD + CB
Single Displacement
A(metal) + B(metal)C -> AC + B
A(non-metal) + B(metal)C -> AB + C
Activity Series
Compound's element if it's below
Displacment occurs quicker
Element's reactivity relative to each other
Oxidations
Metal Oxide
Non-metal Oxide
Equations
Word Equation
Sodium + Chloride -> Sodium Chloride
Chemical Equations
Balanced (Equal number of atoms on reactant and product side)
2KI(aq) + Pb(NO₃)₂(aq) → 2KNO₃(aq) + PbI₂(s)
Stoichiometry
Complete Ionic Equations
Net Ionic Equations
Matter, Chemical Trends and Chemical Bonding
Nomenclature
Criss Cross
Simplify Formula
Acid
Oxyacid
Binary Acid
Base
Hydrate
*H₂O
Bonds
Metallic
M + M
Covalent
Molecular Compound
Diatomic
HOFBRNCl
Ionic
Polyatomic Ion
Multivalent Compound
Metal has more than one charge
roman numerals (e.g. I, II, IV, V)
Ionic Compound
All Metals (M) have + charge
Cation
All Non-metals (NM) have - charge
Anion
Hydronium/Hydrogen Ion Concentration [H30+/H+]
Hydroxide Ion Concentration [OH-]
pH Scale
Acidic
Neutral
Basic/Alkaline
Picture of ph Scale
Ionization/Dissociation
Equations
HCl(aq) + H₂O(l) -> H₃O⁺(aq) + Cl⁻(aq)
CH₃COOH(aq) + H₂O(l) -> CH₃COOH⁻(aq) + H(aq)
NaOH(aq) + H₂O(l) -> Na⁺(aq) + OH⁻(aq)
NH₃(aq) + H₂O(l) -> NH₄⁺(aq) + OH⁻(aq)
such as
Logarithmic Equations
pH + pOH = 14
pH = -log[H₃O⁺/H⁺]
pOH = -log[OH⁻]
[H₃O⁺/H⁺] = 10⁻^pH
Subtopic
[OH⁻] = 10⁻^pOH
if
are
Symbols
Gas (g)
Solid (s)
Liquid (l)
Aqueous (aq)
represented as
(WIP) NET IONIC AND PERCIPITATION
represented as
artificially made
include
Periodic Table
Metalloids
Metal (M)
Non-metal (NM)
Periods
Groups
100% ionized in water
Less than 100% ionized in water
Less than 100% dissociated in water
100% dissociated in water
Matter
States of Matter
Solid
Liquid
Gas
Plasma
Bose-Einstien Condensate
NOTE: Connect back to Gase unit
Types of Matter
Mixtures
Homogenous
Heterogenous
Pure Substances
Elements
Atoms
Properties
Atomic Number
Atomic Mass
Mass Number
Isotopes
Parts
Nucleus
Protons (+ charge)
Neutrons (no charge)
Shells
Electrons (- charge)
Valence Electrons
Stability
Octet Rule
Boron and Beryllium
Molecules
Compounds
Physical Properties
Chemical Properties
M + NM
NM + NM
Example of Criss Cross
Strength
Strong Acid
Weak Acid
Strong Base
Weak Base
Intramolecular Forces
can be
Transfer of Electrons
Shared Electrons
contain
contain
Electronegativity (EN)
Intermolecular Forces
London Dispersion Force
Hydrogen Bonding
Induced dipole-dipole
Ion Dipole
Molecular Polairty
Polar
Asymmetrical
lone pairs
one negative end
one positive end
Non-polar
Symmetrical
Bond Polarity
Non-polar covalent bond
Equal sharing
Polar covalent bond
Unequal Sharing
dipole
Partially positive end (electron deficient)
δ-
Partially negative end (electron rich)
δ+
picture