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Metal Oxide + H2O →
Base
Nonmetal Oxide + H2O →
Acid
Metal Oxide + Nonmetal Oxide →
Salt and Water
Element + Element →
Binary Compound
Metallic Carbonate →
Metal Oxide and Carbon Dioxide
Ammonium Carbonate →
Ammonia, Water, and Carbon Dioxide
Metallic Sulfite →
Metal Oxide and Sulfur dioxide
Metallic Chlorate →
Chloride salt and Oxygen
Binary Compound →
Element and element
Combustion of Organic Compound (Oxygen excess)→
Carbon Dioxide and Water
Combustion of Organic Compound (Oxygen limited)→
Carbon Monoxide and Water
Combustion of Metal→
Metal Oxide
Combustion of Metal Sulfide→
Metal Oxide and Sulfur dioxide
Group 1 Solubility
Soluble
Ammonium Solubility
Soluble
Nitrate Solubility
Soluble
Acetate Solubility
Soluble
Chlorate and Perchlorate Solubility
Soluble
Hydrogen Carbonate Solubility
Soluble
Halide Solubility
Soluble except with Ag, Pb, and Hg.
Sulfate Solubility
Soluble except with Ca, Ba, Sr, Pb, and Ag.
Carbonate Solubility (Exceptions Group 1 and Ammonium)
Insoluble
Chromate Solubility (Exceptions Group 1 and Ammonium)
Insoluble
Hydroxide Solubility (Exceptions Group 1 and Ammonium)
Insoluble, partially with Ca, Ba, and Sr.
Phosphate Solubility (Exceptions Group 1 and Ammonium)
Insoluble
Sulfide Solubility (Exceptions Group 1 and Ammonium)
Insoluble, except for group 2
Formation of Precipitate
Double Replacement
Neutralization
Double Replacement, creates water from ions
Acetate Salt + Strong Acid →
Acetic Acid and Salt
Phosphate Salt + Strong Acid →
Phosphoric Acid and salt
Fluoride + Strong Acid →
Hydrofluoric Acid and salt.
Sulfide salt + acid →
Hydrogen Sulfide and salt
Carbonate/Bicarbonate salts + acid →
Carbon Dioxide, water, and salt
Ammonium + base →
Ammonia, water and salt
Sulfite salt + acid →
Sulfur dioxide, water, and salt
Oxidizing agent
Gets reduced, gains an electron
Reducing agent
Gets oxidized, loses an electron
Redox: MnO4 (-1) in acid →
Reduced, Mn+2
Redox: MnO4 (-1) in base →
Reduced, MnO2
Redox: Cr2O7 (-2) in acid →
Reduced, Cr (+3)
Redox: Cr2O7 (-2) in base →
not Redox, CrO4 (-2)
Redox: H2O2 in base →
Reduced, H2O
Redox: MnO2 in acid →
Reduced, Mn (+2)
Redox: HNO3 (Concentrated) →
Reduced, NO2
Redox: HNO3 (Dilute) →
Reduced, NO
Redox: H2SO2 (Hot and concentrated) →
Reduced, SO2
Redox: Metal-ic ions →
Reduced, Metal-ous ions
Redox: Halate ions →
Reduced, halide ions
Redox: Free halogens →
Reduced, halide ions.
Redox: Halide ions →
Oxidized, free halogen
Redox: Metal-ous ions →
Oxidized, Metal-ic ions
Redox: Sulfite or SO2 ions →
Oxidized, Sulfate ions
Redox: Nitrite ions →
Oxidized, Nitrate ions
Redox: H2O2 →
Oxidized, O2 + H+
Redox: Free metals →
Oxidized, Metal ions
Redox: Oxalic Acid (H2C2O4) →
Oxidized, CO2
Redox Titrations
Balance the equation, then use stoichiometry
Your score on the test
100!
Note 
Flashcard (43)