A. Major Points and Concepts
Predicting Reaction
4 common "driving forces" for reaction:
-Formation of solid (ex. precipitation)
-Formation of water (ex. combustion)
-Transfer of electron (ex. oxidation-reduction)
-Formation of gas (ex. combustion)
Remember Chemical Equations
Reactants -> Products
-(s)-solid
-(l)-liquid
-(g)-gas
-(aq)-aqueous solution
Solubility Rules
-1. Most nitrate (NO3-) are soluble.
-2. Most salts of Na+, K+, and NH4+ are soluble.
-3. Most chloride salts are soluble. Exceptions: AgCl, PbCl2, and Hg2Cl2
-4. Most sulfates are soluble. Exceptions:BaSO4, PbSO4, and CaSO4
-5. Most hydroxide (OH-) compounds are insoluble. Exceptions: ions in rule number 2/ Ba(OH)2 and Ca(OH)2
-6. Most sulfides, carbonate, and phosphate are insoluble. Exceptions: ions in rule number 2
Writing Equations
There are 3 ways to write chemical equations:
-1. Molecular equation-no charges are showing, only compounds
-2. Complete ionic equation-all (aq) compounds will disassociate "break" into their ions
-3. Net ionic equation-find the solid and then write the ions in the reactants that make up the product-Spectator ions= look for the (aq) in the product and those are your spectator ions
Types of Reactions
-Combustion-always look for in the reactant a carbon source and oxygen gas and in the product CO2
-Synthesis-adding elements and/or compounds to form a new single compound
-Decomposition-breaking a compound into simpler parts
-Single Displacement-one element/compound replaces another one (only a cation can replace a cation and an anion can only replace an anion)
-Double Displacement-elements/compounds switches partners to form 2 new compounds
-Precipitation-formation of a solid when two or more aqueous solutions are combined
-Acid Base Reaction-in the reactant, there must be both an acid (H) and a base (OH)
4 common "driving forces" for reaction:
-Formation of solid (ex. precipitation)
-Formation of water (ex. combustion)
-Transfer of electron (ex. oxidation-reduction)
-Formation of gas (ex. combustion)
Remember Chemical Equations
Reactants -> Products
-(s)-solid
-(l)-liquid
-(g)-gas
-(aq)-aqueous solution
Solubility Rules
-1. Most nitrate (NO3-) are soluble.
-2. Most salts of Na+, K+, and NH4+ are soluble.
-3. Most chloride salts are soluble. Exceptions: AgCl, PbCl2, and Hg2Cl2
-4. Most sulfates are soluble. Exceptions:BaSO4, PbSO4, and CaSO4
-5. Most hydroxide (OH-) compounds are insoluble. Exceptions: ions in rule number 2/ Ba(OH)2 and Ca(OH)2
-6. Most sulfides, carbonate, and phosphate are insoluble. Exceptions: ions in rule number 2
Writing Equations
There are 3 ways to write chemical equations:
-1. Molecular equation-no charges are showing, only compounds
-2. Complete ionic equation-all (aq) compounds will disassociate "break" into their ions
-3. Net ionic equation-find the solid and then write the ions in the reactants that make up the product-Spectator ions= look for the (aq) in the product and those are your spectator ions
Types of Reactions
-Combustion-always look for in the reactant a carbon source and oxygen gas and in the product CO2
-Synthesis-adding elements and/or compounds to form a new single compound
-Decomposition-breaking a compound into simpler parts
-Single Displacement-one element/compound replaces another one (only a cation can replace a cation and an anion can only replace an anion)
-Double Displacement-elements/compounds switches partners to form 2 new compounds
-Precipitation-formation of a solid when two or more aqueous solutions are combined
-Acid Base Reaction-in the reactant, there must be both an acid (H) and a base (OH)