Unit 4: Chemical Reactions Flashcards
Synthesis Reaction
When elements or simple compounds are combined to form a single, more complex compound
Decomposition
A reaction in which a single compound is split into two or more elements or simple compounds, usually in the presence of heat
Acid-Base Reaction
A reaction when an acid reacts with a base to form water and a salt
Oxidation-Reduction (Redox) Reaction
A reaction that results in the change of the oxidation states of some participating species
Hydrocarbon Combustion
When a covalent substance containing carbon and hydrogen (and sometimes oxygen) is ignited, it reacts with the oxygen in the atmosphere. The products are always CO2 and H2O
Precipitation
When two aqueous solutions mix and an insoluble salt is created
Spectator Ions
Free ions that start and end as free ions
Hydroxide
OH (-)
Nitrate
NO3 (-)
Acetate
C2H3O2 (-)
Cyanide
CN-
Permanganate
MnO4 (-)
Carbonate
Co3 (2-)
Sulfate
SO4 (2-)
Dichromate
Cr2O7 (2-)
Phosphate
Po4 (3-)
Ammonium
NH4 (+)
Chromate
CRO4 (2-)
Peroxide
O2 (2-)
Oxalate
C2O4 (2-)
Thiosulfate
S2O3 (2-)
Limiting Reactant
The reactant that runs out first
LEO says GER
Lose electrons = oxidation
Gain electrons = reduction
Conjugate Pair
The species with the H+ ion (acid) and the same species without the H+ ion (conjugate base)
7 Diatomic Elements
H2, N2, O2, F2, Cl2, Br2, I2
Charge of Silver
1+
Charge of Zinc
2+
Ammonium Formula
NH4 1+
Acetate Formula
CH3COO 1-
Hydronium Formula
H3O 1+
Carbonate Formula
Hydrogen Carbonate Formula
P
Perchlorate Formula
Chlorate Formula
Chlorite Formula
Dichromate Formula
Cyanate Formula
Thiocyanate Formula
Hydroxide Formula
Peroxide Formula
Iodate Formula
Nitrate Formula
Nitrite Formula
Permanganate Formula
Sulfate Formula
Sulfite Formula
Thiosulfate Formula
Phosphate Formula
7 Strong Acids
7 Strong Bases
