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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!

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

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  • This was total utter bullshit. I can't believe you call this CHEMISTRY!!!

    lol just kidding, it was helpful, thanks for the slide + audio :D
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  • you know the day destroys the night
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  • Thank you so much. I'm glad that it was of use to you.
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  • Transcript

    • 1. Classifying Equations The Five Types of Chemical Equations Chapter 11.2
    • 2. Objectives
      • Describe the five types of chemical equations.
      • Predict the products of the five types of chemical equations.
    • 3. 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
    • 4. Decomposition Reactions
      • Opposite of synthesis: one substance to multiple substances
    • 5. Decomposition Reactions
      • Opposite of synthesis: one substance to multiple substances
      • 2HgO --> 2Hg (l) + O 2 (g)
    • 6. Decomposition Reactions
      • Opposite of synthesis: one substance to multiple substances
      • 2HgO --> 2Hg (l) + O 2 (g)
      • IDENTITY BADGE : Only one substance to begin with.
    • 7. 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 --->
    • 8. Decomposition Try It
      • HI ---> H 2 (g) + I 2 (g)
    • 9. 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.
    • 10. 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)
    • 11. 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)
    • 12. Decomposition Try It 2
      • Write the decomposition equation from the binary formula that produces H 2 and Br 2 .
    • 13. 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
    • 14. 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 -
    • 15. 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
    • 16. 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)
    • 17. Decomposition Try It 2
      • Balance: 2HBr ---> H 2 (g) + Br 2 (g)
    • 18. Decomposition Try It 2
      • Balance: 2HBr ---> H 2 (g) + Br 2 (g)
    • 19. Single Replacement Reactions
      • Substituting one element for another in a compound.
    • 20. 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)]
    • 21. 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 --->.
    • 22. Replacement?
      • Will the pure substance kick the other element out of the compound?
    • 23. Replacement?
      • Will the pure substance kick the other element out of the compound?
      • Use the activity series (p. 9 in your reference tables)
    • 24. 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.
    • 25. Single Replacement Try It
      • Write the balanced equation for the reaction between Zinc (II) metal ( = Zn (s)) and hydrogen sulfide (H 2 ( SO 4 )).
    • 26. 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) --->
    • 27. 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?
    • 28. 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
    • 29. 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)
    • 30. 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)
    • 31. 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)
    • 32. Single Replacement Try It 2
      • Write the balanced equation for the reaction between Chlorine gas and Sodium iodide.
    • 33. Single Replacement Try It 2
      • Write the balanced equation for the reaction between Chlorine gas and Sodium iodide.
      • Cl 2 (g) + NaI (aq) --->
    • 34. 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
    • 35. 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)
    • 36. 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)
    • 37. Single Replacement Try It 2
      • Cl 2 (g) + 2 NaI (aq) ---> 2 NaCl (aq) + I 2 (g)