Types of Chemical Reactions

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Presentation transcript:

Types of Chemical Reactions (See Chapter 10.3)

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

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

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

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

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

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

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

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

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

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) +

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

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

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

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

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

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

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

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

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

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

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

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