Types of Reaction
Synthesis
Decomposition
Double Displacement
Combustion
Single Displacement
Combustion is a chemical reaction in which a fuel "burns" or react quickly with oxygen. These reactions are used to generate energy that can be used in various ways.
In a Synthesis Reaction, two or more substances are coming together to form a single compound
AB --> A + B
A complex compound breaks down into several simpler substances
Combustion with Hydrocarbon
Types of decomposition
Can only have a single compound product
Decomposition of Metal Carbonates
Binary decomposition
A+B=AB
If oxygen is plentiful, hydrocarbons burn completely to release the energy they contain.Besides, the only products of complete combustions are carbon dioxide and water.
Decomposition of Metal Hydroxide
Decomposition of Metal Nitrates
Equation: Hydrocarbon + Oxygen = Carbon Dioxide + Water + Energy
Combustion with Hydrogen
Binary compounds tend to break down into their substituent elements e.g H2O --> H2 + O2
Hydrogen reacts or burns with oxygen to form water.
Breaks down into Metal Nitrite and Oxygen
Equation: 2H2 + O2 = 2H2O
Double displacement reaction occurs when one element displaces another element in a chemical compound. They folllow the general equation; AB + CD = AD + CB
Breaks down into Metal oxide and water
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Two compounds forming a new compound.
Two compounds reacting to form a new compound involving the reaction of metal or non-metal oxides and water
An element and a compound forming a new compound.
2SO2 + 3O2 → 2SO3
Can be difficult to predict the product for as they often involve covalent compounds, which can form in many ratios
Two elements forming a compound
Breaks down into Metal Oxide and CO2
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Metal Oxide: a compound with a metal and oxygen.
When a metal oxide reacts with water, it forms a metal hydroxide which produces a base
E.g. Na2O(s) + H2O(l) → NaOH(aq).
Non-metal Oxide: a compound with a non-metal and oxygen.
When a non-metal oxide reacts with water, it forms an acid.
E.g. CO2 (g) + H2O(l) → H2CO2 (aq)
Reaction that forms solid
In double displacement reaction, precipitates can form which is an insoluble solids that are produced during the double displacement reaction.
An element takes another element's place in a compound
A + BC → AC + B
Types
Reaction that forms gas
A metal displaces another metal in an ionic compound
If Carbonic Acid is included in the double displacement reaction, it will produce Carbon Dioxide gas.
A non - metal displaces another non - metal in a covalent compound
A metal displaces Hydrogen in water/acid
Al(s) + FeCl2 → Fe(s) + AlCl3
CH3COOH(aq) + NaHCO3(aq) ⟶ NaCH3COO(aq) + H2O(ℓ) + CO2(g)
Mg + HCl --> MgCl2 + H2
Cl2 + 2NaBr(aq) → 2NaCl(aq) + Br2 (l)
If Ammonium Hydroxide is included in the double displacement reaction, it will produce Ammonia gas.
e.g Ca(OH)2 --> CaO + H2O
e.g CaCO3 --> CaO + CO2
e.g 2NaNO3 --> Na + NO3
NH4Cl(aq) + NaOH(aq) ⟶ NaCl(aq) + H2O(ℓ) + NH3(g)
Reaction that forms water
Neutralization Reaction (H+(aq) + OH-(aq) ⟶ H2O(aq)
Acid + Base = Water & Salt
Displacement involving metals can only occur if said metal is more reactive than the one it replaces (Activity Series)
Some metals may not be reactive enough to displace Hydrogen in water and/or Acids (Activity Series)