Reaction Types Flashcards
(25 cards)
Synthesis
A chemical reaction in which two or more reactants (elements and/or compounds) combine to produce a single product
Example: 2Mg(s) + O2(g) → 2MgO(s)
Note: synthesis reaction is also a combustion reaction.
Combustion
Rapid reaction of a substance with oxygen, resulting in the formation of oxides and release of energy as heat and light.
Decomposition
A chemical reaction in which a compound breaks down into two or more elements and/or simpler compounds
Example: CaCO3(s) → CaO(s) + CO2(g)
Single Displacement
A chemical reaction in which one element in a compound is replaced (displaced) by another element
Example: 2AgNO3(aq) + Cu(s) → 2Ag(s) + Cu(NO3)2(aq)
Double Displacement
A chemical reaction in which the cations of two ionic compounds exchange places, resulting in the formation of two new compounds
DD Precipitate
A double displacement reaction that results in the formation of a solid (an insoluble ionic compound)
Example: 2KI(aq) + Pb(NO3)2 (aq) → 2KNO3(aq) + PbI2(s)
DD Gas
A double displacement reaction in which one of the compounds produced decomposes into water and a gas.
Example: HC2H3O2(aq) + NaHCO3(s)→ NaC2H3O2(aq) + H2O(l) + CO2(g)
H2CO3(aq) → H2O(l) + CO2(g)
H2SO3(aq) → H2O(l) + SO2(g)
NH4OH(aq) → H2O(l) + NH3(g)
Neutralization
A double displacement reaction in which an acid and a base react to form water and a salt
Example: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
Salt
An ionic compound that is neither an acid nor a base nor a metal oxide
Combustion of hydrocarbons and their oxygen derivatives
Complete: Hydrocarbons are burned with sufficient quantities of oxygen.
Ex: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
Incomplete: w/o sufficient quantities of oxygen.
Ex. 2CH4(g) + 3O2(g) → 2CO + 4H2O
univalent metal + non-metal
ionic compound
multivalent metal + non-metal
ionic compound
Can’t predict what charge of the multivalent metal,
so write all possibilities.
Two non-metals combine
molecular compound
An element reacts with a compound
new compound
Two compounds combining
new compounds
metal oxide + water
metal hydroxide (a base)
non-metal oxide + water
acid
binary compound decomposing
elements
metal nitrate decomposing
metal nitrite and oxygen gas
metal carbonate decomposing
metal oxide and carbon dioxide
metal hydroxide decomposing
metal oxide and water
SD: A metal (or hydrogen) displacing
another metal (or H+) in an ionic solution.
SD: A non-metal displacing
another non-metal in an ionic solution.
when a metal reacts with water
the products are metal hydroxide (base) and hydrogen gas
