Types of Reactions
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Transcript of Types of Reactions
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Types of Reactions
Chapter 7
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Synthesis(Combination) Reaction
• Na (l) + Cl2(g) --> NaCl(s)– Balance the reaction.
• You know you have a synthesis reaction when…
• 2 Reactants, 1 Product• Reactants are elements or simpler compound• Product is a compound
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Decomposition Reaction
• Cu(NO3)2 (aq) --> NO2 (g) + O2 (g)+ CuO (s)
• Balance the reaction
• You know you have a decomposition reaction when…
• 1 Reactant, 2+ products
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Single Replacement
• Al (s) + Fe2O3 (s) --> Al2O3 (s) + Fe(l)– Balance the equation
• You know you have a single replacement reaction when…
• Element + compound element + compound
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Combustion
• CH4(g) + 2O2(g) CO2 (g) +2H2O(g)
• You know you have a combustion reaction when…
• Oxygen is a reactant and carbon dioxide + water are the products.
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Double Replacement
• NaOH (aq) + AgNO3 (aq) --> AgOH (s) + NaNO3(aq)
• You know you have a double replacement reaction when…
• Compound + Compound Compound + Compound
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Back to ions…
• What is an ionic compound?• What happens when an ionic compound
dissolves in water?– The compound dissociates, or separates into the
individual ions.
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So…
• When mixing two dissolved ionic compounds, you are really mixing the ions together.
• A chemical reaction can occur!• A precipitation reaction: reaction in which a
solid forms and separates from the solution.
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How do precipitation reactions work?
• Example: Let’s mix potassium chromate solution and barium nitrate solution together
• What is the chemical equation (reactants only) for this reaction?
• K2CrO4 (aq) + Ba(NO3)2 (aq)
• But these are ionic compounds, so it’s really the ions dissolved in water
• 2K+ (aq) + CrO42- (aq) + Ba2+ (aq) + 2NO3
- (aq)
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The reaction
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But what are the products?
• Experimental evidence tells us that one product is a solid. A solid must be electrically neutral, a cation with an anion– What are the options?
• K2CrO4 ; Ba(NO3)2
• KNO3 ; BaCrO4
• But which one is the solid?
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Use solubility rules!
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What does it all mean?
• Nitrate and potassium salts are soluble, so potassium nitrate cannot be a precipitate.
• Therefore, barium chromate is the solid.
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How do you write all of this
• Molecular (undissociated) equation• K2CrO4 (aq) + Ba(NO3)2 (aq) KNO3(aq) + BaCrO4 (s)
• Complete ionic equation (any ionic “aq” broken up into ions.
• 2K+(aq) + CrO42-(aq) + Ba2+(aq) + 2NO3
- (aq) 2K+(aq) + 2NO3-
(aq)+BaCrO4 (s)
• Net ionic equation(eliminate spectator ions)• CrO4
2-(aq) + Ba2+(aq) BaCrO4 (s)
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