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Types of Chemical Reactions

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Presentation on theme: "Types of Chemical Reactions"— Presentation transcript:

1 Types of Chemical Reactions
(See Chapter 10.3)

2 Types of Chemical Reactions
How many songs exist? Let’s say I want to sort my music. How could I do that?

3 Types of Chemical Reactions
There are too many chemical equations to count. However, we can sort them into five general categories.

4 Type 1: Synthesis Reaction
Two compounds combine to make one compound A A + B B A + B AB

5 Type 1: Synthesis Reaction
Example H O H H O + H O O H H 2H2 + O2 2H2O

6 Type 2: Decomposition Reaction
One compound breaks apart into two or more compounds or elements A B A B + B AB A +

7 Type 2: Decomposition Reaction
Example O C O Ca O O Ca C + O CaCO3(s) CaO(s) CO2(g) +

8 Type 3: Single Replacement Reaction
Two compounds swap a single element or polyatomic ion A B C A C + + B A + BC AC + B

9 Type 3: Single Replacement Reaction
Example Na K Cl Na Cl + + K Na(s) + KCl(s) NaCl(s) + K(s)

10 Type 4: Double Replacement Reaction
Two ions “trade partners” + + A B C D A D C B AB + CD AD + CB

11 Type 4: Double Replacement Reaction
Example K I K O H H O I + + Ca Ca K I I O H K O H 2KI(s) + Ca(OH)2(s) 2KOH(s) CaI2(s) +

12 Type 5: Combustion Reaction
A molecule reacts with O2 to make CO2, H2O, and lots of heat O C O C H H O + + CxHy + O2 CO2 + H2O

13 Type 5: Combustion Reaction
Example H O O C O C H O + + H O CH4 + 2H2O 2O2 CO2 +

14 Practice N2(g) + 3H2(g)  2NH3(g) What type of reaction is:
1) Synthesis 2) Decomposition 3) Single Replacement 4) Double Replacement 5) Combustion

15 NaNO3(s) + K(s)  Na(s) + KNO3(s)
Practice What type of reaction is: NaNO3(s) + K(s)  Na(s) + KNO3(s) 1) Synthesis 2) Decomposition 3) Single Replacement 4) Double Replacement 5) Combustion

16 2C4H10(g) + 13O2(g) 8CO2(g) + 10H2O(g)
Practice What type of reaction is: 2C4H10(g) + 13O2(g) 8CO2(g) + 10H2O(g) 1) Synthesis 2) Decomposition 3) Single Replacement 4) Double Replacement 5) Combustion

17 Practice 2H2O(g)  2H2(g) + O2(g) What type of reaction is:
1) Synthesis 2) Decomposition 3) Single Replacement 4) Double Replacement 5) Combustion

18 PbCl2(s) + 2HBr(g)  PbBr2(s) + 2HCl(g)
Practice What type of reaction is: PbCl2(s) + 2HBr(g)  PbBr2(s) + 2HCl(g) 1) Synthesis 2) Decomposition 3) Single Replacement 4) Double Replacement 5) Combustion

19 Demonstration 1 Reactants: Products: Chemical Equation (unbalanced)
Chemical Equation (balanced) Type of Reaction C C12H22O11 H2O C12H22O11(s)  C(s) + H2O(g) C12H22O11(s)  12C(s) +11 H2O(g) Decomposition

20 Demonstration 2 Reactants: Products: Chemical Equation (unbalanced)
Chemical Equation (balanced) Type of Reaction Mg O2 MgO Mg(s) + O2(g)  MgO(s) 2Mg(s) + O2(g)  2MgO(s) Synthesis

21 Demonstration 3 Reactants: Products: Chemical Equation (unbalanced)
Chemical Equation (balanced) Type of Reaction Pb(NO3)2 NaOH Pb(OH)2 NaNO3 Pb(NO3)2(aq) + NaOH(aq)  Pb(OH)2(s) + NaNO3(aq) Pb(NO3)2(aq) + 2NaOH(aq)  Pb(OH)2(s) + 2NaNO3(aq) Double Replacement

22 Demonstration 4 Reactants: Products: Chemical Equation (unbalanced)
Chemical Equation (balanced) Type of Reaction Mg HCl MgCl2 H2 Mg(s) + HCl(aq)  MgCl2(aq) +H2(g) Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g) Single Replacement

23 Demonstration 5 Reactants: Products: Chemical Equation (unbalanced)
Chemical Equation (balanced) Type of Reaction CH4 O2 CO2 H2O CH4(g) + O2(g)  CO2(g) + H2O(g) CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) Combustion


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