Reactions. Chapter 3 Combustion Decomposition Combination. Chapter 4 Reactions. Exchange reactions (Metathesis) Formation of a precipitate

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1 Reactions Chapter 3 Combustion Decomposition Combination Chapter 4 Reactions Exchange reactions (Metathesis) Formation of a precipitate Formation of a gas Formation of a week or nonelectrolyte Single Displacement Reactions Redox reactions Oxidation numbers Mary J. Bojan Chem 110 1

2 Balancing Equations Law of conservation of mass: matter cannot be lost in any chemical reaction Mary J. Bojan Chem 110 2

3 Patterns of reactivity Know how to balance a chemical reaction (Complete) Combustion reactions (Chapter 3) C 3 H 8 (g) + 5O 2 (g) 3CO 2 (g) + 4H 2 O(g) Combination reactions (Chapter 3) 2Mg(s) + O 2 ( ) 2MgO(s) Decomposition reactions (Chapter 3) PbCO 3 (s) PbO(s) + CO 2 (g) Mary J. Bojan Chem 110 3

4 Write balanced reactions for The combustion of ethanol CH 3 CH 2 OH The decomposition of lead carbonate PbCO 3 The combination of nitrogen and hydrogen to form ammonia (NH 3 ) Mary J. Bojan Chem 110 4

5 Patterns of reactivity Know how to balance a chemical reaction Exchange reactions (Chapter 4) Precipitation it ti Pb(NO 3 ) 2 (aq) + 2KI(aq) PbI(s) + 2KNO 3 (aq) Neutralization NaOH(aq) + HCl(aq) NaCl(aq) + H 2 O( ) Gas formation 2HCl(aq) + Na 2 S(aq) H 2 S(g) + 2NaCl(aq) Single displacement reactions (Chapter 4) 2Ca(s) + O 2 2(g) 2CaO(s) Mary J. Bojan Chem 110 5

6 Example: Exchange reaction (Double Displacement) Exchange positive ions to get products AD + XZ AZ + XD Reactants: t Pb(NO 3 ) 2 + KI Balance the reaction. Does anything happen? TRY! Do you have to do the reaction to know? Mary J. Bojan Chem 110 6

7 Metathesis Reactions (Double Displacement) Given reactants: exchange positive ions to get products Requires a driving force (otherwise nothing happens) Di Driving i Forces 1. Precipitate forms 2. Weak or nonelectrolyte forms 3. Gas forms How do you know what is happening? Net Ionic Equation Mary J. Bojan Chem 110 7

8 Precipitation Reaction Mix silver nitrate and sodium chloride. What happens? Molecular Equation Ionic Equation Spectator ions: Net Ionic Equation Mary J. Bojan Chem 110 8

9 SOLUBILITY RULES FOR COMMON IONIC COMPOUNDS IN WATER 1. Almost all ammonium and alkali metal salts are soluble. 2. Most nitrates, acetates, chlorides, bromides, and sulfates are soluble. Exceptions: silver halides sulfates of Ca,Ba,Pb,Ag 3. Most sulfides, carbonates, phosphates and hydroxides are insoluble. Exceptions: alkali salts ammonium salts. (See #1 above.) See Table 4.1 of Brown, LeMay, and Bursten for a more comprehensive listing. Mary J. Bojan Chem 110 9

10 Formation of Weak or Nonelectrolyte (neutralization reaction) Acid + base salt + water Molecular Equation Ionic Equation Spectator ions: Net Ionic Equation Mary J. Bojan Chem

11 Practice What is the net ionic equation for the reaction between sodium hydroxide and acetic acid? What is the net ionic equation for the reaction between sodium chloride and potassium iodide? Mary J. Bojan Chem

12 GAS FORMATION Direct production of a gas CO 2, H 2 S, NO 2, SO 2 Production of weak acid which decomposes. Example: Molecular Equation NaHCO 3 (aq) + HCl(aq) H 2 CO 3 (aq) + NaCl(aq) CO 2 (g) + H 2 O(l) Ionic Equation Na + (aq) + HCO (aq)+ + + (aq) H (aq) Cl (aq) H 2 CO 3 Na (aq) Cl (aq) Na + (aq) + Cl (aq) + CO 2 (g) + H 2 O(l) Net Ionic Equation H + (aq) + HCO 3 (aq) CO 2 (g)+ H 2 O(l) Mary J. Bojan Chem

13 Single Displacement reactions (Oxidation-Reduction) Zn(s) + CuSO 4 (aq) ZnSO 4 (aq) +Cu(s) What is oxidized? What is reduced? What is the oxidizing agent? What is the reducing agent? Ionic equation: Net ionic equation Mary J. Bojan Chem

14 Rules for determining Oxidation States 1. Oxidation state of atom in elemental form is zero. e.g. Cl 2 O 2 P 4 C(s) S 8 2. The oxidation number of a monatomic ion equals its charge. 3. Some elements have common oxidation numbers that can be used as reference in determining the oxidation numbers of other atoms in the compound. Alkali metals +1 Alkaline earth metals +2 Fluorine 1 H usually +1 Hydrides: metal-h compounds ( 1) O usually 2 peroxides ( 1) & superoxides possible Cl, Br, I almost always 1 4. Sum of oxidation numbers is equal to overall charge of molecule or ion: For a neutral compound the sum of oxidation numbers equals zero. For a polyatomic ion, the sum of the oxidation numbers is equal to the charge on the ion. 5. Shared electrons are assigned to the more electronegative atom of the pair: more electronegative atom will have a negative oxidation number. Mary J. Bojan Chem

15 ActivitySeries Table 4.5 Will the metal element displace the atom from its compound in a reaction? Na(s) + H 2 O(l) Au(s) + H 2 O(g) Zn(s) + AgNO 3 (aq) Active metals (groups IA, IIA, Al) very reactive! Inactive (inert metals): jewelry metals Do not react readily Other metals in between Mary J. Bojan Chem

16 Reactions: Stoichiometry Solving problems involving Chemical reactions Limiting Reactants Solution reactions Gas phase reactions Mary J. Bojan Chem

17 Basics: before you start! Assume you know: Avogadro s number memorize it! definition of mole Formula weight (molar mass) the following connections (or conversions) gram mole gram molecules what is meant by: Use these along with the empirical ii lformula balanced chemical molecular formula reaction to solve problems in chemistry Mary J. Bojan Chem

18 How to solve problems write the balanced chemical reaction (or process). make connections between experimentally measured properties and the balanced equation. In other words: Given information such as mass, volume, pressure and temperature, how can one determine quantities of moles/molecules? Mary J. Bojan Chem

19 IMPORTANT CONNECTIONS Avogadro s number Connects molecules l (or atoms) )to moles Connects microscopic properties to macroscopic properties. Conservation of Mass Mass of Products = Mass of reactants Balance the reaction Balanced Chemical Equation Connects moles (molecules) of reactants with moles (molecules) of products Related to conservation of Mass Formula weight Connects mass to moles Connects a property that can be measured (determined) experimentally to moles (or molecules) of substance given in the balanced reaction. Empirical Formula Tells relative number of atoms in a molecule Obtained from %mass or molecular formula Mary J. Bojan Chem

20 Problem Solving 1. Write balanced chemical equation 2. Make a table: Fill in given information 3. Note connections between measured quantities and moles Mass Volume (solutions) P, V, T (gases) M.W. concentration ideal gas law moles moles moles 4. Fill in table until you are able to solve the problem 5. Make sure your answer is REASONABLE 6. TRY things Mary J. Bojan Chem

21 Sample Problems Methane reacts with water to produce hydrogen gas and carbon monoxide. If 8.0g of methane reacts with 9.0 g of water, how many grams of hydrogen gas will be produced? Mary J. Bojan Chem

22 If a clean burning engine e burns 1 gallon of gasoline (assume this is 2600 g of octane), how many kg of CO 2 will it produce? Octane is C 8 H 18 Assume: Gasoline is all octane Density of octane = 0.692g/ml 1 gal = 3.79 l = 3790 ml 3790ml x 0.692g/ml = g 2600 g of octane Mary J. Bojan Chem

23 You try! If 36.6 g of C 2 H 5 OH reacts with 63.8 g of O 2, how many grams of CO 2 will be produced? g g g g g Mary J. Bojan Chem

24 Limiting reagent Reactant that is used up first Determines the amount of product Must start with a balanced reaction BE SURE TO TEST BOTH REACTANTS Mary J. Bojan Chem

25 Problem Solving with solutions: Titration Molarity is the connection between moles and volume in solutions. If 46.0ml of 0.100M NaOH is needed to neutralize 20.0 ml of a H 2 SO 4 solution what is the concentration of H 2 SO 4? Mary J. Bojan Chem

26 Problem Solving with gases For a gas, PV=nRT is the link between the # of moles (n) and the experimental quantities P,V, and T of gas. Example: How many L of N 2 at 735 mm Hg and 26 C are produced from 126g of NaN 3 (sodium azide)? sodium azide gas in an airbag 2NaN 3 (s) 2Na(s) + 3 N 2 (g) mass P,V,T MW moles ideal gas law moles Mary J. Bojan Chem

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