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Questions and Answers
Match the following chemical reaction types with their descriptions:
Match the following chemical reaction types with their descriptions:
Synthesis = Two or more reactants combine to form a single product Decomposition = A single compound breaks down into two or more simpler substances Single Replacement = An element replaces another element in a compound Double Replacement = Ions from two compounds exchange places in an aqueous solution
Match the following examples with their corresponding reaction types:
Match the following examples with their corresponding reaction types:
2H2 + O2 → 2H2O = Synthesis 2NaCl → 2Na + Cl2 = Decomposition Zn + CuSO4 → ZnSO4 + Cu = Single Replacement AgNO3 + NaCl → AgCl + NaNO3 = Double Replacement
Match the following reaction types with their common characteristics:
Match the following reaction types with their common characteristics:
Synthesis = Energy is usually absorbed or released Decomposition = Often requires heat or light to initiate Combustion = Involves oxygen and produces heat and light Double Replacement = Typically occurs in solutions
Match the following criteria with the reaction types:
Match the following criteria with the reaction types:
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Match the following reaction characteristics with the corresponding reaction type:
Match the following reaction characteristics with the corresponding reaction type:
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Study Notes
Synthesis Reactions
- Synthesis reactions, also known as combination reactions, involve two or more reactants combining to form a single product.
- The general form of a synthesis reaction is: A + B → AB
- Examples include the reaction of hydrogen gas with oxygen gas to form water (2H₂ + O₂ → 2H₂O) and the reaction of magnesium with oxygen to form magnesium oxide (2Mg + O₂ → 2MgO).
- Often, energy (heat, light, or electricity) is required to initiate the reaction.
Decomposition Reactions
- Decomposition reactions involve a single reactant breaking down into two or more simpler products.
- The general form of a decomposition reaction is: AB → A + B
- Examples include the decomposition of water into hydrogen and oxygen (2H₂O → 2H₂ + O₂) and the decomposition of calcium carbonate into calcium oxide and carbon dioxide (CaCO₃ → CaO + CO₂).
- Heat is often necessary to drive the decomposition.
Single Replacement Reactions
- Single replacement reactions, also known as single displacement reactions, involve one element replacing another element in a compound.
- The general form of a single replacement reaction is: A + BC → AC + B (where 'A' is a more reactive metal)
- Examples include the reaction of zinc metal with hydrochloric acid to produce zinc chloride and hydrogen gas (Zn + 2HCl → ZnCl₂ + H₂), and the reaction of copper sulfate solution with zinc metal producing copper metal and zinc sulfate (CuSO₄ + Zn → Cu + ZnSO₄).
- The element being replaced is typically a metal in the compound being reacted with, but there can be non-metals as well. Reactivity series determines which element will replace the other.
Double Replacement Reactions
- Double replacement reactions, also known as double displacement reactions, involve the exchange of ions between two compounds.
- The general form of a double displacement reaction is: AB + CD → AD + CB
- Examples include the reaction of sodium chloride and silver nitrate to produce sodium nitrate and silver chloride (NaCl + AgNO₃ → NaNO₃ + AgCl), and the reaction of sodium hydroxide and hydrochloric acid to produce sodium chloride and water (NaOH + HCl → NaCl + H₂O).
- Precipitation, formation of a gas, and formation of a molecular compound (like water) are common results of this reaction type.
Combustion Reactions
- Combustion reactions are rapid reactions that produce a flame. They typically involve a fuel reacting with oxygen from the air.
- The general form of a combustion reaction is: Fuel + O₂ → Products (often CO₂, H₂O and heat).
- Examples include the burning of methane gas (CH₄ + 2O₂ → CO₂ + 2H₂O) and the burning of gasoline (C₈H₁₈ + 25/2 O₂ → 8CO₂ + 9H₂O).
- Complete combustion, producing solely carbon dioxide and water, is favoured when there is ample oxygen. Incomplete combustion, producing carbon monoxide (CO) is possible when insufficient oxygen is present.
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Description
Test your knowledge on synthesis, decomposition, and single replacement reactions in chemistry. This quiz covers the definitions, general forms, and examples of these fundamental chemical reactions. Perfect for students looking to solidify their understanding of reaction types.
