Coefficient- In a chemical equation, the number written in front of a reactant or product; gives the smallest number of particles of the substance involved in the reaction.
Reactants- starting substances.
Products- substances formed during the reaction.
Synthesis Reactions- chemical reaction in which two or more substances react to produce a single product.
Combustion Reaction- oxygen combines with a substance and release energy in the form of heat and light.
Decomposition Reaction- a single compound breaks down into two or more elements or new compounds.
Single Replacement- A reaction in which the atoms of one element replace the atoms of another element in a compound.
Double Replacement- Involves an exchange of ions between two compounds.
When two elements react, the reaction is always a synthesis reaction.
Example:
2 Na (s) + Cl2 → 2 NaCl
Example:
C (s) + O2 → CO2
In a combustion a substance is always combined with a oxygen. Note: Oxygen is on the reactants side.
Example 2:
2 H2 (g) + O2 (g) → 2 H2O (l)
Single compound breaks down into two or more substances.
Example:
2NaN3(s) → 2 Na (s) + 3 N2
Atoms of one element replace the atoms of another element in a compound.
Example:
Cu (s) + 2 AgNO3 (aq) → 2 Ag (s) + Cu(NO3)2 (aq)
Exchange of ions between two compounds
Example:
KCN(aq) + HBr (aq) → KBr(aq) + HCN (g)
1.) Zn + Cu(NO3)2 → Cu + Zn(NO3)2 Double- Replacement Rxn
Answer: Single- Replacement Rxn
2.) Magnesium Chloride + Silver Nitrate → Combustion Rxn
Answer: Double Replacement Rxn: Magnesium Chloride + Silver Nitrate → Magnesium Nitrate + Silver Chloride
MgCl2 + AgNO3 → Mg(NO3)2 + AgCl
4.) 4 Fe (s) + 3 O2 (g) → 2 Fe2O3(s) Synthesis Rxn
Answer: Synthesis Rxn/Combustion Rxn – These are the only type of reactions that can go together.
5.) 2Al (s) + 3S (s) → Al2S3(s) Combustion Rxn
Answer: Synthesis Rxn
3.) NaClO3 → NaCl + O2 Synthesis Rxn
Answer: Decomposition Rxn
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