Reactions and Balancing Equations
Balancing Equations
to balance an equation you have to make sure that every part of the equation is equal
ex: MgF2 + Li2CO3 -> MgCO3 + LiF
__MgF2 + __Li2CO3 -> __MgCO3 + 2LiF
There are 4 types of common "driving forces" for a reaction
Solubility Rules
to balance an equation you have to make sure that every part of the equation is equal
ex: MgF2 + Li2CO3 -> MgCO3 + LiF
__MgF2 + __Li2CO3 -> __MgCO3 + 2LiF
There are 4 types of common "driving forces" for a reaction
- the formation of a solid- ex: precipitation
- the formation of water- ex: combustion
- the transfer of an electron- ex: oxidation-reduction
- the formation of a gas- ex: combustion
- the products and reactants of an equation are labeled as either a solid (s), a liquid (l), a gas (g), or aqueous (aq)
- aqueous means it is soluble and can dissolve in water
Solubility Rules
ex: Find the product
AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)
Three ways to write a chemical equations
1. Molecular Equation
2. Complete Ionic Equation
The spectator ion- find the aqueous product(s) and find the the ions that make up the compound and those are the spectator ions
Types of Reactions
1. Combustion
2. Synthesis
3. Decomposition
4. Single Displacement
5. Double Displacement
6. Acid Base Reaction
7. Precipitation
AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)
Three ways to write a chemical equations
1. Molecular Equation
- there are no charges shown; only the symbols of the compounds
- ex: AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)
2. Complete Ionic Equation
- All aqueous compounds will "break" into their ions
- ex: Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) -> AgCl(s) + Na+(aq) + NO3-(aq)
- Find the solid and write the ions in the reactants that make up the product
- ex: Ag+(aq) + Cl-(aq) -> AgCl(s)
The spectator ion- find the aqueous product(s) and find the the ions that make up the compound and those are the spectator ions
Types of Reactions
1. Combustion
- look for a carbon source and an oxygen gas in the reactant and CO or CO2 in the product
- ex: CH4 + O2 -> CO2 + H2O
2. Synthesis
- adding elements and/or compounds to form one new compound as a product.
- ex: H2 + O2 -> H2O
3. Decomposition
- breaking a compound into small, simpler parts
- ex: H2O -> H2 + O2
4. Single Displacement
- when one element or compound replaces another
- ex: Zn + FeCl2 -> Fe + ZnCl2
5. Double Displacement
- when elements or compounds switch partners to form two new compounds
- ex: AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)
6. Acid Base Reaction
- both an acid(H) and a base(OH) are in the reactant
- ex: HNO3 + NaOH -> H2O + NaNO3
7. Precipitation
- the formation of a solid when two or more aqueous solutions are formed
- ex: AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)
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