Chemical Reactions. Writing chemical reactions Types of chemical reactions Reactions in aqueous solutions. (ionic equations and solubility rules)
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1 Chemical Reactions Writing chemical reactions Types of chemical reactions Reactions in aqueous solutions (ionic equations and solubility rules)
2 Writing Equations REACTANTS PRODUCTS gold (III) sulfide is mixed with hydrogen gas to produce gold and hydrogen sulfide gas
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4 Balancing Equations Use coefficients to make the equation follow the law of conservation of mass.
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6 Copper metal reacts with an aqueous solution of silver nitrate to produce copper (II) nitrate and silver. Gold (III) sulfide is mixed with hydrogen gas to produce gold and hydrogen sulfide gas. Hydrogen peroxide is heated to form water vapor and oxygen gas.
7 Types of Reactions There are 5 major types of reactions. Knowing these will help you predict the products of reactions. There five types are: Synthesis, Decomposition, Single Replacement, Double Replacement, and Combustion.
8 Synthesis (Combination) General form: A + B --> AB Two reactants combine to form one product. A and B can be elements or compounds The product AB is always a single compound 1. Metal + oxygen --> metal oxide 2. Nonmetal + oxygen --> nonmetal oxide 3. Metal + nonmetal --> salt 4. Metal oxide + water --> base 5. Nonmental oxide + water --> acid
9 Decomposition General form: AB --> A + B A single compound breaks down into two or more simpler products Usually require energy or catalyst Can be difficult to predict products
10 Single Replacement General forms: A + BC --> B + AC A + BC --> C + BA One element replaces a second element in a compound. To identify, notice both the reactants and products consist of one element and one compound. Produces a new element and a new compound.
11 Single Replacement 1. Metal + acid --> hydrogen + salt 2. Metal + water --> hydrogen + metal hydroxide or metal oxide 3. Metal + salt --> metal + salt (look at activity series) 4. Halogen + halogen salt --> halogen + halogen (halogens higher will replace lower) salt
12 Whether one metal will displace another metal from a compound depends on the reactivities of the two metals. We use an activity series, which lists metals in order or reactivity, to make the prediction. A metal will replace any metal listen below it in the series.
13 Mg(s) + Zn(NO 3 ) 2 (aq) --> Mg(s) + 2AgNO 3 (aq) --> Mg(s) + LiNO 3 (aq) -->
14 Double Replacement General form: AB + CD --> AD + CB Two compounds trade positive ions. Usually produce a precipitate, a gas, or a molecular compound. For double replacement to occur, one of the following is true: 1. one product is slightly soluble and precipitates from solution 2. one product is a gas that bubbles out of the mixture 3. one product is a molecular compound like water
15 Combustion An element or compound reacts with oxygen, producing energy (heat & light) Reactants: combustion requires oxygen; usually involves a hydrocarbon Products: metals and carbon compounds combust. The complete combustion of carbon produces carbon dioxide and water Ionic compounds do not combust; as well as carbon molecules that already contain too much oxygen (like carbon dioxide)
16 Predicting Precipitate Formation Precipitate: an insoluble salt; a solid Forms in some reactions, but not others. Use solubility rules to determine if a precipitate will form.
17 Will a precipitate form when aqueous solutions of Na 2 CO 3 (aq) and Ba(NO 3 ) 2 (aq) are mixed?
18 Stoichiometry
19 N 2 (g) + H 2 (g) NH 3 (g) nitrogen gas reacts with hydrogen to produce ammonia Law of Conservation of Mass: matter is not created or destroyed; it is rearranged Balancing chemical reactions
20 N 2 (g) + 3H 2 (g) 2NH 3 (g) one molecule of nitrogen gas reacts with three molecules of hydrogen to produce two molecules of ammonia. one mole of nitrogen molecules reacts with three moles of hydrogen molecules to form two moles of ammonia molecules. Coefficients = # of moles
21 Mole-Mole Calculations *** MUST HAVE A BALANCED EQUATION FOR THIS TO WORK! Example#6: How many moles of ammonia are produced when 0.60 mol of N reacts with H? N 2 (g) + 3H 2 (g) 2NH 3 (g)
22 Mass-Mass Calculations g A --> moles A g A --> moles of A --> moles of B --> grams of B Example#7: Calculate the number of grams of NH 3 produced by the reaction of 5.40g of hydrogen with an excess of nitrogen. N 2 (g) + 3H 2 (g) 2NH 3 (g)
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