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Synthesis Reactions
Two compounds or elements form a compound:
A + B → AB
Decomposition Reactions
A compound decomposes into two or more elements or compounds:
AB → A + B
Decomposition of Binary Compounds
AB → A + B (Elemental products)
Decomposition of Metal Carbonates
Metal Oxide + CO2
Decomposition of Metal Hydroxides
Metal Oxide + H2O
Decomposition of Metal Chlorates
Metal Chloride + Oxygen
Decomposition of Acids
Non-metal oxide + H2O
Single Replacement
A cation in an equation replaces a cation bonded to an anion in a compound.
A + BC → B + AC
Double Replacement
The cations in each compound switch in the equation.
AB + CD → AD + CB
Combustion
A hydrocarbon burns in oxygen to produce CO2 + H2O
Ex: C8H8 + O2 → CO2 + H2O
Precipitation Reaction
In double replacement, a nonsoluble, solid product forms.
Net Ionic Equations
The removal of spectator ions from a precipitation reaction.
Redox Reactions
The transfer of electrons from chemicals
Oxidation
The loss of electrons in a redox reaction
EX: CL- → Cl
Reduction
The gain of electrons in a redox reaction
Ex: Na+ → Na
Limiting Reactant
A reactant that determines the amount of product produced.
Excess Reactant
The reactant left over after the limiting reactant has finished reacting.
Percent Yield
Actual Yield/Theoretical Yield x 100 = Percent Yield
Energy
The ability to do work or produce heat.
Potential Energy
Energy of chemical composition or position.
Kinetic Energy
Energy of Motion
Heat
Process of energy moving from cold to warm environments.
System
Area containing a thermochemistry reaction.
Surroundings
Everything other than the system.
Exothermic
Heat leaves from the system into the surroundings.
Endothermic
Heat is absorbed by the system from its surroundings.
calorie
One gram of water raised one degree celsius.
1 calorie
4.184 Joules
Joules
SI unit of heat
Specific Heat
The energy required to raise one gram of any substance 1 degree celsius.
Q
mCp Delta T
Delta T
Final temperature - initial temperature in degrees celsius.
Gas Properties
Gases take the shape and volume of their containers, have lighter and faster molecules, are easily compressed, and are less dense than solids and liquids.
Volume
Liters, mL
Pressure
Pascals, Torr, Atm, mmHg
mmHg/torr to atm
1 atm = 760 mmHg or 760 torr
Pascals to atm
1 atm = 1.01 × 10^5 Pascals or 101 KPa
Temperature
Celsius, Kelvin
Kelvin to Celsius
K = Celsius + 273
Dalton’s Law
P1 + P2 + P3 = Ptotal
Boyle’s Law
P1V1 = P2V2; Pressure is inversely related to volume.
Charles’ Law
V1T2 = V2T1; Volume is directly related to temperature.
Gay-Lussac’s Law
P1T2 = P2T1; Pressure is directly related to temperature.
Combined Gas Law
P1V1T2=P2V2T1
Ideal Gas Law
PV = nRT; Used when the number of moles is in a gas problem. Atm must be the pressure, Liters must be the volume, and T must be in Kelvin
Gas Constant R
0.0821 L atm/moles K
Graham’s Law
Rate 1/Rate 2 = SQRT(Molar mass 2/Molar mass 1);
Gases of lower molar mass diffuse and effuse faster than gases of higher molar mass.
1 mole
22.4 Liters
STP Values
T— 273 K
P— 1.0 atm
Solution
Homogeneous mixture of a solute in a solvent with tiny particles.
Colloid
Homogeneous mixture with medium-sized particles.
Suspension
Heterogeneous mixture with large particles; temporary
Electrolyte
A solution that conducts electricity.
Saturated
There is the maximum amount of solute to solvent in a solution; no more will dissolve.
Supersaturated
There is more solute than solvent; will not dissolve.
Unsaturated
There is less solute than solvent; appears dilute.
Miscible
A solution that will successfully mix
Immiscible
A solution that will not successfully mix.
Emulsion
Colloidal size droplets of one substance suspended inside another.
Emulsifying Agent
An agent that allows an emulsion to fully mix together or become miscible.
Molarity
The amount of moles of solute per Liter of solution.
Stock Solution Formula
M1V1=M2V2
Solubility
The ability of a solute to dissolve in a solvent; usually measured in grams solute per 100 grams water.
Solubility increases for solids
when temperature increases
When temperature increases in a gas
solubility decreases
Triple Point
The point at which all phases of a substance exist.
Acids Properties
Taste sour
Burn skin
pH is less than 7
Turns blue litmus paper red
Reacts with metals
Has more H+ than OH-
Bases Properties
Taste bitter
Slippery on skin
pH is greater than 7
Turns red litmus paper blue
Do NOT react with metals
Have more OH- than H+
Both Acids and Bases
Conduct electricity
Neutralize each other
Bronsted-Lowry Law
Acids donate hydrogen ions
Bases accept hydrogen ions
Conjugate acid
Substance that forms when a base receives a hydrogen ion, the reaction can be reversed by the donation of a hydrogen ion.
Conjugate base
Substance that forms when an acid donates a hydrogen ion, the reaction can be reversed by the acceptance of a hydrogen ion.
pH formula
pH = -log[H+]
pOH formula
pOH= -log[OH-]
[H+] formula
[H+] = 10^-pH
[OH-] formula
[OH-] = 10^-pOH
pH+pOH
=14.0
When does the concentration of hydrogen or hydroxide change?
When the multiplier of hydrogen or hydroxide ions is raised, the multiplier of the concentration is raised as well.
Note 
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