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Types of Reactions: Decomposition and Single Replacement
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Types of Reactions: Decomposition and Single Replacement

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Created for a student who had a planned absence from class. Use it if it helps you!

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Types of Reactions: Decomposition and Single Replacement Types of Reactions: Decomposition and Single Replacement Presentation Transcript

  • Classifying Equations The Five Types of Chemical Equations Chapter 11.2
  • Objectives
    • Describe the five types of chemical equations.
    • Predict the products of the five types of chemical equations.
  • Preview of the Five Reaction Types
    • using the terminology of your Chemistry Reference Tables/EOC (it may not match with the book)
    • 1) Synthesis
    • 2) Decomposition
    • 3) Single Replacement
    • 4) Double Replacement
    • 5) Combustion
    • Found on p. 6 of your Chemistry Reference Tables
  • Decomposition Reactions
    • Opposite of synthesis: one substance to multiple substances
  • Decomposition Reactions
    • Opposite of synthesis: one substance to multiple substances
    • 2HgO --> 2Hg (l) + O 2 (g)
  • Decomposition Reactions
    • Opposite of synthesis: one substance to multiple substances
    • 2HgO --> 2Hg (l) + O 2 (g)
    • IDENTITY BADGE : Only one substance to begin with.
  • Decomposition Reactions
    • Opposite of synthesis: one substance to multiple substances
    • 2HgO --> 2Hg (l) + O 2 (g)
    • IDENTITY BADGE : Only one substance to begin with.
    • Try it: Complete and balance this decomposition reaction -- HI --->
  • Decomposition Try It
    • HI ---> H 2 (g) + I 2 (g)
  • Decomposition Try It
    • HI ---> H 2 (g) + I 2 (g)
    • Why H 2 and I 2 ? Hint: I bring clay for our new h ouse.
  • Decomposition Try It
    • HI ---> H 2 (g) + I 2 (g)
    • Why H 2 and I 2 ? Hint: I bring clay for our new h ouse.
    • ? HI ---> ? H 2 (g) + ? I 2 (g)
  • Decomposition Try It
    • HI ---> H 2 (g) + I 2 (g)
    • Why H 2 and I 2 ? Hint: I bring clay for our new h ouse.
    • ? HI ---> ? H 2 (g) + ? I 2 (g)
    • Balanced: 2 HI ---> H 2 (g) + I 2 (g)
  • Decomposition Try It 2
    • Write the decomposition equation from the binary formula that produces H 2 and Br 2 .
  • Decomposition Try It 2
    • Write the decomposition equation from the binary formula that produces H 2 and Br 2 .
    • H 2 = H; Br 2 = Br
  • Decomposition Try It 2
    • Write the decomposition equation from the binary formula that produces H 2 and Br 2 .
    • H 2 = H; Br 2 = Br
    • Add their oxidation numbers: H + and Br -
  • Decomposition Try It 2
    • Write the decomposition equation from the binary formula that produces H 2 and Br 2 .
    • H 2 = H; Br 2 = Br
    • Add their oxidation numbers: H + and Br -
    • Cross down the charges: HBr
  • Decomposition Try It 2
    • Write the decomposition equation from the binary formula that produces H 2 and Br 2 .
    • H 2 = H; Br 2 = Br
    • Add their oxidation numbers: H + and Br -
    • Cross down the charges: HBr
    • Write equation: HBr ---> H 2 (g) + Br 2 (g)
  • Decomposition Try It 2
    • Balance: 2HBr ---> H 2 (g) + Br 2 (g)
  • Decomposition Try It 2
    • Balance: 2HBr ---> H 2 (g) + Br 2 (g)
  • Single Replacement Reactions
    • Substituting one element for another in a compound.
  • Single Replacement Reactions
    • Substituting one element for another in a compound.
    • 2 K (s) + 2 H(OH) (l) --->2 K(OH) (aq) + H 2 (g)
    • [HINT: H 2 O = H(OH)]
  • Single Replacement Reactions
    • Substituting one element for another in a compound.
    • 2 K (s) + 2 H(OH) (l) --->2 K(OH) (aq) + H 2 (g)
    • [HINT: H 2 O = H(OH)]
    • IDENTITY BADGE : One pure substance on each side of the --->.
  • Replacement?
    • Will the pure substance kick the other element out of the compound?
  • Replacement?
    • Will the pure substance kick the other element out of the compound?
    • Use the activity series (p. 9 in your reference tables)
  • Replacement?
    • Will the pure substance kick the other element out of the compound?
    • Use the activity series (p. 9 in your reference tables)
    • A pure substance will replace any pure substance located below it in the activity series.
  • Single Replacement Try It
    • Write the balanced equation for the reaction between Zinc (II) metal ( = Zn (s)) and hydrogen sulfide (H 2 ( SO 4 )).
  • Single Replacement Try It
    • Write the balanced equation for the reaction between Zinc (II) metal ( = Zn (s)) and hydrogen sulfide (H 2 ( SO 4 )).
    • Zn (s) + H 2 (SO 4 ) (aq) --->
  • Single Replacement Try It
    • Write the balanced equation for the reaction between Zinc (II) metal ( = Zn (s)) and hydrogen sulfide (H 2 ( SO 4 )).
    • Zn (s) + H 2 (SO 4 ) (aq) --->
    • Is Zn above H in the activity series?
  • Single Replacement Try It
    • Write the balanced equation for the reaction between Zinc (II) metal ( = Zn (s)) and hydrogen sulfide (H 2 ( SO 4 )).
    • Zn (s) + H 2 (SO 4 ) (aq) --->
    • Is Zn above H in the activity series?
    • Yes
  • Single Replacement Try It
    • Write the balanced equation for the reaction between Zinc (II) metal ( = Zn (s)) and hydrogen sulfide (H 2 ( SO 4 )).
    • Zn (s) + H 2 (SO 4 ) (aq) --->
    • Is Zn above H in the activity series?
    • Yes
    • Zn (s) + H 2 (SO 4 ) (aq) ---> Zn(SO 4 ) (aq) + H 2 (g)
  • Single Replacement Try It
    • Write the balanced equation for the reaction between Zinc (II) metal ( = Zn (s)) and hydrogen sulfide (H 2 ( SO 4 )).
    • Zn (s) + H 2 (SO 4 ) (aq) --->
    • Is Zn above H in the activity series?
    • Yes
    • Zn (s) + H 2 (SO 4 ) (aq) ---> Zn(SO 4 ) (aq) + H 2 (g)
  • Single Replacement Try It
    • Write the balanced equation for the reaction between Zinc (II) metal ( = Zn (s)) and hydrogen sulfide (H 2 ( SO 4 )).
    • Zn (s) + H 2 (SO 4 ) (aq) --->
    • Is Zn above H in the activity series?
    • Yes
    • Zn (s) + H 2 (SO 4 ) (aq) ---> Zn(SO 4 ) (aq) + H 2 (g)
  • Single Replacement Try It 2
    • Write the balanced equation for the reaction between Chlorine gas and Sodium iodide.
  • Single Replacement Try It 2
    • Write the balanced equation for the reaction between Chlorine gas and Sodium iodide.
    • Cl 2 (g) + NaI (aq) --->
  • Single Replacement Try It 2
    • Write the balanced equation for the reaction between Chlorine gas and Sodium iodide.
    • Cl 2 (g) + NaI (aq) --->
    • Is Cl above I in the activity series?
    • Yes
  • Single Replacement Try It 2
    • Write the balanced equation for the reaction between Chlorine gas and Sodium iodide.
    • Cl 2 (g) + NaI (aq) --->
    • Is Cl above I in the activity series?
    • Yes
    • Cl 2 (g) + NaI (aq) ---> NaCl (aq) + I 2 (g)
  • Single Replacement Try It 2
    • Write the balanced equation for the reaction between Chlorine gas and Sodium iodide.
    • Cl 2 (g) + NaI (aq) --->
    • Is Cl above I in the activity series?
    • Yes
    • Cl 2 (g) + NaI (aq) ---> NaCl (aq) + I 2 (g)
  • Single Replacement Try It 2
    • Cl 2 (g) + 2 NaI (aq) ---> 2 NaCl (aq) + I 2 (g)