1. Chemical Reactions

2. 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 required ◦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. Ions in solution (aq) Ionic compounds dissolved in water are often written with (aq); Example: NaCl (s)  NaCl(aq) When dissolved, ionic compounds are split in ions: NaCl (s)  Na + (aq) + Cl - (aq)

10. 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.

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

12. 2 H 2 (g) + O 2 (g)  2 H 2 O(l)

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

14. __Al(s) + __HCl(aq)  __AlCl 3 (aq) + __H 2 (g) PRACTICE

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

16. 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)

17. ¬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)

18. 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.

19. 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.

20. 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

21. 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) The Activity Series of Metals

23. Activity series I: Fe(s) + CuCl 2 (aq)  FeCl 2 (aq) + Cu(s) II: 2Ag(s) + CuCl 2 (aq)  2AgCl(aq) + Cu(s) Iron will replace copper, but silver will not. So reaction I will occur, but reaction II will not.

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

25. 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)

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

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

28. 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 Zinc metal reacts with aqueous copper(II) sulfate. Aqueous silver nitrate reacts with aqueous potassium chloride. Potassium metal reacts with chlorine.

29. 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 (produces oxygen and hydrogen gas). Aqueous sodium carbonate reacts with (aqueous) nitric acid (HNO 3 ).

30. Precipitation reactions Double replacement reactions often (but not always) form a precipitate Pb(NO 3 ) 2 (aq) + 2 KI (aq)  PbI 2 (s) + 2 KNO 3 (aq) These reactions are known as precipitation reactions

31. Ionic equations Precipitation reaction in ions: Pb 2+ (aq) + 2 NO 3 - (aq) + 2 K + (aq) + 2 I - (aq)  PbI 2 (s) + 2 K + (aq) + 2 NO 3 - (aq) Such an ionic equation can be simplified by omitting the non reacting ions, giving the net ionic equation. K + and NO 3 - are not reacting and therefore are called spectator ions.

32. Net ionic equation Equation (in water) showing only the reacting ions: Pb 2+ (aq) + 2 I - (aq)  PbI 2 (s) PbI 2 is a precipitate (so not in ionic form anymore).

33. Acid Base reaction A double replacement reaction between an acid and a base is called an acid-base reaction. The reaction products are a salt and water. HCl(aq) + NaOH(aq)  H 2 O(l) + NaCl(aq)

34. As ionic equation: H + (aq) + Cl - (aq) + Na + (aq) + OH - (aq)  H 2 O(l) + Na + (aq) + Cl - (aq) So the net ionic equation is: H + (aq) + OH - (aq)  H 2 O(l)

35. Gas forming reactions Reactions in which a gas is formed. Mg(s) + 2 HCl(aq)  H 2 (g) + MgCl 2 (aq)