6Parts of a Chemical Equation CO2 + H2O C6H12O6 + O2To the Left of the Arrow are the REACTANTS (what goes in)The Arrow is called a YIELD SIGNTo the Right of the yield sign are the PRODUCTS (what comes out)
7Rearranging the Atoms CO2 + H2O C6H12O6 + O2 Notice that no new atoms appear when the products are made. The atoms just rearrange themselves to form new compounds!
8How does this happen?Energy must be added to break the bonds of the reactants.When new bonds form the products, energy is then released.
92 Major Types of Reactions Exothermic: more energy is released then was absorbed. This produces HEAT!Endothermic: More energy is abosrbed the released. Results in COLD
10Classifying Chemical Reactions There are 5 general types of chemical reactions.SynthesisDecompositionCombustionSingle DisplacementDouble Displacement
11Synthesis ReactionA reaction of at least 2 substances that forms a new, more complex compound.(Synthesis means to make)Example: Hydrogen + oxygen waterGeneral Form: A+ B AB2Na + Cl NaCl
122. Decomposition Reaction A reaction in which one compound breaks into at least 2 products.Example: digestion (breaking down your food molecules)General Form: AB A + BEx.) 2H2O H2 + O2The Decomposition of Water
133. Combustion A reaction in which a compound and oxygen burn. Oxygen is a reactant in every combustion reaction.Example) the burning of methane2CH4 + 4O CO2 + 4H2O
144. Single-Displacement Reaction A reaction in which atoms of one element take the place of atoms of another element in a compound.General Form: XA + B AB + XExample: CuCl2 + Al AlCl3 + Cu
155. Double-displacement reaction A reaction where a compound is formed from the exchange of ions between 2 compounds.General form: AX + BY AY + BXExample:Pb(NO3)2 + K2CrO PbCrO4 + 2KNO3
17Review…. What is a chemical Equation? The use of chemical formulas and symbols to show the reactants and products in a chemical reaction.Write an equation and label the reactants, products, and yield sign.
18Why do we need to balance equations? Equations must be balanced to account for the Conservation of Mass!
19For Example….. CH4 + O2 CO2 + H2O This equation is not balanced. It appears that we have lost Hydrogens and gained Oxygens…..does this agree with the Law of Conservation of Energy?
20How to Balance Equations CH4 + O CO2 + H2OCount the # of atoms on each side of the yield sign.C = 1 C = 1H = 4 H = 2O = 2 O = 3
21You can NOT change the subscripts! Now what?You can NOT change the subscripts!2. Place Coefficients to balance the equation.Coefficient = a # in front of atoms or compounds.
22Using Coefficients CH4 + O2 CO2 + H2O There are 4 Hydrogens on the left side, how many more do you need to get 4 on the right side?Answer = 2
23Using Coefficients Place a 2 in front of H2O. CH4 + O2 CO2 + 2H2O 3. Now Re-count atoms for both sides!C = 1 C = 1H = 4 H = 4O = 2 O = 4
24How to Balance the Oxygen We need to add another Coefficient.CH4 + O CO2 + 2H2OOxygen needs 2 more on the left side.Place a 2 in front of the O2.
254. Re-count atoms for both sides. CH4 + 2O CO2 + 2H2OC = C = 1H = H = 4O = O = 4All is balanced!
26Try this! Mg + O2 MgO KI + Br2 KBr + I2 3. What types of reactions are these?4. P.168 # 1, 2a. , 3