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BALANCING EQUATIONS & CHEMICAL REACTIONS Evidence of Chemical Change Changes in Energy (E) Release of E as heat Release of E as light Production of sound Reduction or increase of temperature Absorption or release of electrical Energy Formation of new substances Formation of a gas Formation of a precipitate Change in color Change in odor Conservation of Mass Law of Conservation of Mass In any physical or chemical reaction, mass is neither created nor destroyed; it is conserved! Reactants Products Same number of atoms on both sides of the equation! Balancing Equations In every balanced equation each side of the equation has the same number of atoms of each element Important stuff! Four abbreviations are used to indicate physical states of chemicals: shown as subscripts in the chemical equation (s) = solid (l) = liquid (g) = gas (aq)= aqueous solution (dissolved in water) Symbols over the arrow indicate the conditions of the reaction Heat Pressure Temperature Catalyst Reversible reaction Balance this equation… NaNO3 + CrCl3 NaCl + Cr(NO3)3 How would you “write” it? Combination Reaction or Synthesis Reaction Two or more simple substances react to form a more complicated one A + B AB Fe + S FeS Combination Reactions We can predict the products of ionic compounds by thinking about the charge! Al (s) + O2 (g) Cu (s) + S(s) Are there 2 possible products to this reactions How would we “say” these equations? Decomposition Reaction A decomposition reaction is the opposite of a composition reaction - a complex molecule breaks down to make simpler ones. AB A + B 2 H2O 2 H2 + O2 Decomposition Reactions Harder to predict the products…always remember your diatomics. Water is often a product! HgO(s) NH4NO3 Decomposition Reactions HgO(s) 2HgO(s) 2Hg(l) + O2 (g) NH4NO3 NH4NO3 N2O + 2H2O The only way to really know is to do the reaction!! Single Replacement This is when one element trades places with another element in a compound. A + BC AC + B Mg + 2H2O Mg(OH)2 + H2 Single Replacement Reactions Easy to predict the products. Look at the ions… remember that a cation has to bond to an anion!! Don’t forget about diatomics! Zn(s) + H2SO4(aq) Na(s) + H2O OOPS! Did we balance them? Single Replacement Reactions ZnSO4(aq) Zn(s) + Zn(s) + H2SO4(aq) H2SO4(aq) Na(s) + Na(s) + 2Na(s)+ H2O H+OH-(l) 2H+OH-(l) 2NaOH + H2(g) + H2(g) Single Replacement Reactions Reactivity of a metal makes a difference! If a metal is more reactive than the metal it is displacing a rxn will occur. If the metal is less reactive than the metal it is displacing, a rxn will not occur. Metal Reactivity Increases down a group Decreases across a period Brainiacs-- Metal Reactivity Reactivity in Single Displacement + KMnO4 CsMnO4 Will this occur?? Cs Na + KMnO4 NaMnO4 + K Will this occur? Double Replacement Reaction This is when the anions and cations of two different molecules switch places, forming two entirely different compounds AB + CD AD + CB Pb(NO3)2 + 2KI PbI2 + 2KNO3 Double Replacement Reactions Generally take place between two ionic compounds in aqueous solution Pb(NO3)2 + 2KI PbI2 + 2KNO3 Double Replacement Reactions 2NaCl + H2SO4 Double Replacement Reactions Ca(OH)2(aq) + 2HCl(aq) ) Combustion Reactions A combustion reaction is when oxygen combines with another compound or element producing energy. When hydrocarbons (C?H?) combust, water, carbon dioxide and energy are produced. C10H8 + 12 O2 10 CO2 + 4 H2O + Energy Combustion of Naphthalene Combustion Reactions Combustion of propane: C3H8 + O2 Combustion of methane: CH4 + O2 Combustion of butene (this one is tricky!) C4H6 + O2 Teacher Demo Extraordinaire! What is a flame video- Science Friday http://www.sciencefriday.com/video/06/08/2012/ what-is-a-flame.html Recap: 5 Types of Reactions 1. 2. 3. 4. 5. Combination Decomposition Single Replacement Double Replacement Combustion Warm Up: Predict the products, balance and classify the following reactions. Li + MgCl2 C6H12 + O2 Ca(NO3)2 + NaOH Types of Rxns Lab Take about 10 minutes to do the prelab questions on the lab. Most of the answers should be in your CB notes. Warm UpBalance the following combustion equations: C4H4 + O2 CO2 + H2O C3H6 + O2 CO2 + H2O C7H14 + O2 CO2 + H2O Types of Reaction Lab a. Synthesis: Mg + O2 b. Decomposition CuCO3 c. Single Replacement Zn + HCl d. Double Replacement PbNO3 + KI Finish the lab You have 20 minutes to get it done! Be sure that all your questions are answered! Debrief Types of Rxns Lab Types of Reaction Lab Synthesis: Mg + O2 Did the mass of the system change after the reaction took place? Did you detect the presence of ammonia gas? Endothermic or exothermic? Types of Reaction Lab Decomposition CaCO3 What evidence indicates a chemical reaction. How do you know that carbon dioxide was formed? Endothermic or exothermic? Types of Reaction Lab Single Replacement Zn + HCl What evidence did you see? What was in the little tube– how do you know? Endothermic or exothermic? Types of Reaction Lab Double Replacement PbNO3 + KI What evidence did you see? Endothermic or exothermic? Work on classifying the types of reactions on your balancing WS. When you finish, you can start working on the back side of the Current Mole WS…. The front side should be complete! Warm Up Balance and classify the following reactions: 1. Zn + H2SO4 2. CaCl2 + 3. C3H8 + → NaNO3 → O2 → H2 + Zn(SO4)2 Ca(NO3)2 CO2 + + H2O NaCl You should have most of these WS done! 1. Balancing equations WS– classified rxn type 2. Mole Practice WS… Finish both of these… turn them in! Work on the Review! Due the beginning of class on Monday! Test after we go over the review!! Warm Up Balance and classify the following reactions: → 1. Na + H2CO3 2. NaF + Ca(NO3)2 → 3. C5H12 + O2 → H2 + Na2CO3 NaNO3 CO2 + + H2O CaF2 Warm Up- part 2 Determine the molar mass of MgF2 Convert 5.7 g of magnesium fluoride to moles. Convert 6.3 g of magnesium fluoride to molecules. Warm Up Quiz 1. Determine the molar mass of Na3PO4 2. How many moles in 10.6g of Na3PO4 3. How many atoms in 0.50 mol Al? 4. How many atoms in 3.6 g of carbon? Warm Up Balance and classify the following reactions: 1. K 3. CH12 + H3PO4 + O2 → → H2 CO2 + K3PO4 + H2O