Grade 11 
Matter, Trends, and Bonding
Gases
Chemical Reactions
Quantities in Chemical Rxns
Solutions
Periodic Table Trends
Isotopes
Nomenclature
Ionic vs Covalent
Polarity
Synthesis
Molecular Shape
Single Displacement
Double Displacement
Combustion
Proportions In Chemical Rxns
Decomposition
The Mole
Molar Mass
Percent Composition
Mole Ratios
Mass-Mass Ratios
Limiting Reactant & theoretical Yield
Percent Yield
Concentration
Titration
Net Ionic Eqn
Stoichiometry
Laws
Ideal Gas
Valence Shell Electron Pair Repulsion
A+B=AB
AB=A+B
AB+C=AC+B
AB+CD=AD+CB
Boyles law P1V1=P2V2
Charles Law V/T=V/T
Gay-Lussucs Law P/T=P/T
Combined Law PV/T=PV/T
Complete
Incomplete
(Mass of element/ Mass of compound)x100
The Amount of a substance that contains as many atoms/molecules/formula units as exactly 12g of carbon-12
Symbol-mol
Avogadro's constant- 6.02x10^23
1 mol= elements average atomic mass
Conversion factor (CF )
1 mol/g or g/1mol
6.02x10^23/1 mol or 1 mol/6.02x10^23
Ionic Compound (metal+non-metal)
Oxide (metal or nonmetal bonds with O2)
Base (Metal oxide+ OHr)
Acid (non-metal oxide+H2)
Binary Compound form its elements
Metal Nitrates (NO3-N)2+O2)
Metal carbonate (metal Oxide + C)2)
Metal Hydroxide-Metal Oxide+H2O
Reactants are CO2+H2O
C+H20 or CO+H2O or CO+H2) or CO+C+H2O or CO2+CO+C+H2O
Metal replaces metal and Non-metal replaces Non-Metal based on their solubility (use chart given)
Neutralization- Acid+Base= Salt+Water
Formation of Precipitate
Gas Formation
One Product aq other s
both aq then NR
formation of an unstable product
H2CO3, NH4OH, or H2SO3 (break down with decomposition)
Quantitatively determine the concentration of unknown solution called titrand/analyte
A=central atom X=# of ligands E=# of lone pairs
Linear AX2
Trigonal AX3 AX2E
Tetrahedral AX4 AX3E AX2E2
Ionization: increases up and to the left
Atomic Radius: Increases down and to the right
Ion Radius: Increases up and to the left
Electron affinity: increases up and to the left
Electronegativity: increases up and to the left
Review grade 10 material
Binary Compound
Stoichiometry
Always use a balanced equations
Concentration (C) is in mol/L
Volume (V) is in litres (L)
Eqn: C=n/V
use coefficients from balanced equation for mole ratio
kinetic molecular theory
Gas particles are in constant motion
indivduel gas molecules are considered point masses
Gas particles DO NOT ATTRACT OR REPEL each other
Gas particles interact through elastic collisions
Kinetic NRG is directly proportional to temperature
PV=nRT
Avogadro's Law n/V=n/V
Concentration: quantity of solute per unit quantity of solvent
Concentrated: having a high ratio of solute to solvent
Dilute: Having a low ratio of solute to solvent
Precent: m/v, m/m, or v/v
molar: C=n/v
Very small: ppm=(Solute m/ Solution)x10^6 m ppb=(solute m/solution m)x10^9
LR: reactant that limits product
ER: Reactant left over
Use mol ratio to find mol of product (the lowest value of product is the LR)
Required= Given x CF
Balanced equations coefficients indicates the number of moles of each chemical
[actual yield/theoretical yield]x100
Method of finding the efficiency of a reactant can be converted into a product in a given chemical rxn
Actual yeild: determined in lab
theoretical yield= determined with stoichiometry
1) write balanced eqn
2) m of G compound- mol of G compound
3) mol of G compound- mol of Req compound
4) mol of Req compound- mass of Required
1) complete chemical eqn
2) write soluble ionic compounds as ions
3) leave insoluble ionic compounds as formula units
4) Write acids as formula units
5) Cancel out Spectator ions
6) Balance charges
HCl to H+ Cl-
HBr to H+ Br-
HI to H+ I-
H2SO4 to 2H+ SO4 2-
HClO4 to H+ ClO4 -
HNO3 to H+ NO3-
STP= 101.325kPa= 0 C= 273.15K= 22.4 L/mol
SATP= 100.0kPa= 25 C= 298.15K= 24.8L/mol
R=8.314x(kPa x L / mol x K)
1) Balanced eqn
2) Convert all amounts to mol (solve for n)
3) Compare molar amounts using mol ratio (solve for unknown Ma)
4) Convert Ma to unit req using set conditions with Ideal Gas Law
Polyatomic ions
Salts
Acids
Ionic= 2.0 up
Polar= 0.4-1.9
non polar= 0.0-0.4
Metal (roman numeral of valence e of metal) non-metalide
cross over to know amount or charge of each element