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Exam 3 • Objectives: o o o o o o o o o o Nomenclature m-nm, m(VOS)-nm, nm-nm Evidence for Chemical Reactions Writing Chemical Equations Balancing Chemical Equations Classifying Chemical Reactions Combination Reactions Decomposition Reactions Single-Replacement Reactions The Activity Series Double-Replacement Reactions Solubility Rules Neutralization Reactions H+ + OH- H2O(l) Nomenclature 1 Evidence for a chemical Reactions • There are four ways to tell if a chemical reaction has occurred: 1. A gas is produced. 2. An insoluble solid is produced. 3. A permanent color change is observed. 4. An energy change is observed. • An exothermic reaction gives off heat and an endothermic reaction absorbs heat. 2 Diatomic Molecules • Seven nonmetals occur naturally as diatomic molecules: 1. 2. 3. 4. 5. 6. 7. Hydrogen (H2) Nitrogen (N2) Oxygen (O2) Halogen (F2) Halogen (Cl2) Halogen (Br2) Halogen (I2) • These elements are written as diatomic molecules when they appear in chemical reactions. H2(g) N2 (g) F2(g) O2(g) I2(s) Cl2(g) Br2(l) Have No Fear Of Ice Cold Beer‖ Solid – (s) Fe(s) Liquid – (l) H2O(l) Gas – (g) CO2(g) Aqueous – (aq) NaCl(aq) Aqueous means “dissolved in water” 3 A Chemical Reaction reacts with, added to produces, yields, gives A(s) + B (aq) C (l) + D(g) + E(aq) solid aqueous liquid gas Balancing Chemical Eqs • When we balance a chemical equation, the number of each type of atom must be the same on both the product and reactant sides of the equation. • We use coefficients in front of compounds to balance chemical reactions. Never change the subscripts P + I2 PI3 P + 3/2 I2 PI3 x2 2P + 3 I2 2 PI3 2P 6I 2P 6I 4 Practice: Balancing Chemical Eqs Classifying Chemical Reactions • We can place chemical reactions into five categories: Synthesis rxs Decomposition rxs Oxidation–Reduction rxs A + BC B + AC Precipitation rxs Acid-base rxs 5 Combination Reactions • A combination reaction is a reaction in which simpler substances are combined into a more complex compound. • Combination reactions are also called synthesis reactions. • We will look at two combination reactions: 1. The reaction of a metal with nonmetal 2. The reaction of a nonmetal with nonmetal Reactions of Metals with Oxygen • When a metal is heated with oxygen gas, a metal oxide is produced. metal + oxygen gas → metal oxide • For example, magnesium metal produces magnesium oxide. 6 Reactions of Nonmetals with Oxygen • Oxygen and a nonmetal react to produce a nonmetal oxide. nonmetal + oxygen gas → nonmetal oxide • Sulfur reacts with oxygen to produce sulfur dioxide gas. ∆ S(s) + O2(g) → SO2(g) Metal and Nonmetal Reactions • A metal and a nonmetal react in a combination reaction to give an ionic compound. metal + nonmetal → ionic compound • Lithium reacts with bromine gas to produce lithium bromide. ∆ 2 Li(s) + Br2(g) → 2 LiBr(s) • When a main group (group I & II) metal reacts with a nonmetal, the formula of the ionic compound is predictable. If the compound contains a transition metal, the formula is not predictable. 7 Decomposition Reactions • Occurs when a compound is broken down into simpler substances. • Ex: Electrolysis of water 2H2O(l) 2H2(g) + O2(g) E=+1.23v Ex: Carbonates will decompose when heated Combination/decomposition summary • In combination reactions, two or more smaller molecules are combined into a more complex molecule. • In a decomposition reaction, a molecule breaks apart into two or more simpler molecules. 8 Single-Replacement Reactions • A single-replacement reaction is a reaction in which a more active metal displaces another less active metal in a compound. • If a metal precedes another in the activity series, it will undergo a single-replacement reaction. A + BC B + AC Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) Double-Replacement Reactions • In a double-replacement reaction, two ionic compounds in aqueous solution switch anions and produce an insoluble substance. AX + BZ → AZ + BX • If either AZ or BX is an insoluble compound, a precipitate will appear and there is a chemical reaction. • If no precipitate is formed, there is no reaction. 9 Neutralization Reactions • A neutralization reaction is the reaction of an acid and a base. HX + BOH → BX + HOH • A neutralization reaction produces a salt and water. H2SO4(aq) + 2 KOH(aq) → K2SO4(aq) + 2 H2O(l) Classify the following Reactions 10 Predicting whether a reaction will occur In a single-replacement reaction, a more active metal displaces a less active metal according to the activity series. • In a double-replacement reaction, two aqueous solutions produce a precipitate of an insoluble compound. • The insoluble compound can be predicted based on the solubility rules. Single-Replacement: Activity Series More active will react! Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au Mg > Cd so it WILL react! Mg(s) + CdCl2(aq) MgCl2(aq) + Cd (s) The MORE active metal wants to be in a compound!! 11 Double-Replacement Reactions, Continued • Aqueous barium chloride reacts with aqueous potassium chromate as follows: BaCl2(aq) + K2CrO4(aq) → BaCrO4(s) + 2 KCl(aq) From the solubility rules, BaCrO4 is insoluble, so there is a double-replacement reaction. • Aqueous sodium chloride reacts with aqueous lithium nitrate as follows: NaCl(aq) + LiNO3(aq) → NaNO3(aq) + LiCl(aq) Both NaNO3 and LiCl are soluble, so there is no reaction. Practice problems • Write M.E., C.I.E., and N.I.E. for each of the following reactions. • 1) potassium phosphate with copper (II) acetate • • 2) sodium sulfide with iron (III) nitrate • • 3) cesium hydroxide and oxalic acid • • 4) nickel (III) chloride and lead (II) nitrate • • 5) chromium (II) bromide with lithium oxalate • • 6) sulfuric acid with rubidium hydroxide 12 Practice problems • Write M.E., C.I.E., and N.I.E. for each of the following reactions. • 7) barium hydroxide with perchloric acid • • 8) cesium chromate with rubidium oxide • • 9) sodium fluoride with nickel (III) sulfate • • 10) antimony (V) carbonate reacts with sulfuric acid to form antimony (V) sulfate, carbon dioxide, and water • • 11) acetic acid with zinc hydroxide 13