Chem - Units 6-10: reactions

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!