1. Chemical Reactions Ch 11

2. Chemical Reactions Reactions involve chemical changes in matter resulting in new substances Reactions involve rearrangement and exchange of atoms to produce new substances Reactants  Products

3. Chemical reaction = the process by which one or more substances are changed into one or more different substances. Elements are not changed during a reaction

4. Evidence of a chemical reaction/change: 1. Release of a gas 2. Unexpected color change 3. Changes in heat or light 4. Formation of a precipitate 5. Production of an odor (Sometimes there isn’t any evidence!)

5. Chemical Equations Chemical changes are classified and represented by balanced chemical equations These are a shorthand way to describe the changes that substances undergo.

6. Chemical Equations Provide information about the reaction: ◦Formulas of reactants and products ◦States of reactants and products ◦Relative numbers of reactant and product molecules that are involved ◦Can be used to determine mass of reactants used and of products that can be made

7. Writing equations Use proper formulas for each reactant and product Proper equation should be balanced - obey the Law of Conservation of Mass ◦all elements on reactants side also on product side ◦equal numbers of atoms of each element on reactant side as on product side

8. Symbols used in equations Symbols used after chemical formula to indicate state ◦(g) = gas; (l) = liquid; (s) = solid ◦(aq) = aqueous, dissolved in water

9. Writing Balanced Equations Steps: 1.Determine the reactants and products. 2.Write the reactants on the left side, and the products on the right. 3.Balance the equation by placing coefficients where needed (NEVER change subscripts in a formula in order to balance an equation). 4.Use the lowest whole number coefficients possible.

10. Example ___H 2 (g) + ___O 2 (g)  ___H 2 O(l)

11. 2 H 2 (g) + O 2 (g)  2 H 2 O(l)

12. Practice __SnS 2 (s) + __O 2 (g)  __SnO 2 (s) + __SO 2 (g)

13. __Mg(s) + __HCl(aq)  __MgCl 2 (aq) + __H 2 (g) PRACTICE

14. __C 2 H 6 (g) + __ O 2 (g)  __ CO 2 (g) + __ H 2 O(g) PRACTICE

15. Example – Recognizing Reactants and Products When iron metal (steel wool) burns in air it produces a red compound iron (III) oxide ◦Burning in air means reacting with O 2 ◦Metals are solids, except for Hg which is liquid ◦Ionic compounds are solid unless they are dissolved in water (aq)

16. ¬write the equation in words ◦identify the state of each chemical iron(s) + oxygen(g)  iron(III) oxide(s) ­write the equation in formulas ◦identify diatomic elements ◦identify polyatomic ions – count as 1 “unit” when balancing IF it does not change ◦determine formulas 4 Fe(s) + 3 O 2 (g)  2 Fe 2 O 3 (s)

17. Practice For each of the following, write (including states) and balance the chemical equation: 1.Aqueous aluminum nitrate reacts with aqueous sodium hydroxide to produce aluminum hydroxide as a precipitate and aqueous sodium nitrate. 2.Iron reacts with sulfuric acid (H 2 SO 4 ) to produce aqueous iron(III) sulfate and hydrogen.

18. Practice 3. Ethyne (C 2 H 2 ) gas reacts with oxygen to produce carbon dioxide and water. 4. Magnesium reacts with nitrogen to produce magnesium nitride.

19. Classifying Chemical Reactions - Reactions can be classified into 5 types. - Recognizing these types can be used to predict the products or reactants of a reaction. - Some reactions fit into more than 1 class

20. 1. Single Replacement One element or ion replaces another element in a compound. 2 Al (s) + 3 CuCl 2 (aq)  2 AlCl 3 (aq) + 3 Cu (s)

21. Single replacement reactions start with an element and a compound and produce an element and a compound. Often a metal as an element replaces a metal in a compound.

22. 2. Double Replacement Positive (cation) and negative (anion) portions of two compounds interchange. Pb(NO 3 ) 2 (aq) + 2 KI(aq)  PbI 2 (s) + 2 KNO 3 (aq)

23. This reaction type always involved 2 ionic compounds and the cations (or the anions) are exchanged. They generally take place in water.

24. 3. Decomposition Substance breaks down into simpler substances; starts with 1 compound and giving 2 (or more) compounds. 2 H 2 O 2 (l)  2 H 2 O(l) + O 2 (g)

25. 4. Combination (synthesis) Two (or more) substances (usually elements) combine to form one new compound. 2 Mg(s) + O 2 (g)  2 MgO(s)

26. 5. Combustion Oxidation (reaction with oxygen) of an organic compound (containing C, H, and sometimes O) forming carbon dioxide and water. C 2 H 5 OH(l) + 3 O 2 (g)  2 CO 2 (g) + 3 H 2 O(l)

27. Practice For each of the following, write (including states) and balance the chemical equation and give the reaction type: Nitrogen reacts with oxygen to produce dinitrogen pentoxide gas Mercury(II) oxide reacts when heated. Zinc metal reacts with aqueous copper(II) sulfate. Aqueous silver nitrate reacts with aqueous potassium chloride.

28. Practice Ethane (C 2 H 6 ) gas burns in the presence of oxygen. Aluminum metal reacts with (aqueous) hydrochloric acid (HCl). Water reacts when subjected to electricity. Aqueous sodium carbonate reacts with (aqueous) nitric acid (HNO 3 ). Potassium metal reacts with chlorine.