1. Describing Chemical Reactions On May 6, 1937, the huge airship Hindenburg erupted into a fireball. Within a short time, 210,000 cubic meters of hydrogen had burned and the airship was destroyed. The chemical reaction that occurred is “hydrogen combines with oxygen to produce water.” You will learn to represent this chemical reaction by a chemical equation. 11.1

2. Writing Chemical Equations – Word Equations – To write a word equation, write the names of the reactants to the left of the arrow separated by plus signs; write the names of the products to the right of the arrow, also separated by plus signs. – Reactant + Reactant  Product + Product 11.1

3. Writing Chemical Equations Methane + Oxygen  Carbon dioxide + Water 11.1

4. Writing Chemical Equations – Chemical Equations A chemical equation is a representation of a chemical reaction; the formulas of the reactants (on the left) are connected by an arrow with the formulas of the products (on the right). 11.1

5. Writing Chemical Equations – Write the formulas of the reactants to the left of the yields sign (arrow) and the formulas of the products to the right. 11.1

6. Writing Chemical Equations – A skeleton equation is a chemical equation that does not indicate the relative amounts of the reactants and products. – Here is the equation for rusting: – Fe + O 2  Fe 2 O 3 11.1

7. Writing Chemical Equations A catalyst is a substance that speeds up the reaction but is not used up in the reaction. 11.1

8. Writing Chemical Equations 11.1

10. for Conceptual Problem 11.1

11. Balancing Chemical Equations – To write a balanced chemical equation, first write the skeleton equation. Then use coefficients to balance the equation so that it obeys the law of conservation of mass. 11.1

12. Balancing Chemical Equations This is a balanced equation for making a bicycle. The numbers are called coefficients—small whole numbers that are placed in front of the formulas in an equation in order to balance it. 11.1

13. Balancing Chemical Equations A chemical reaction is also described by a balanced equation in which each side of the equation has the same number of atoms of each element and mass is conserved. 11.1

15. for Conceptual Problem 11.2

18. Types of Chemical Reactions The heat and smoke of burning charcoal are the products of a combustion reaction. Combustion is one of the five general types of chemical reactions. If you can recognize a reaction as being a particular type, you may be able to predict the products of the reaction. 11.2

19. Classifying Reactions – The five general types of reaction are combination, decomposition, single-replacement, double-replacement, and combustion. 11.2

20. Classifying Reactions – Combination Reactions A combination reaction is a chemical change in which two or more substances react to form a single new substance. 11.2

23. for Conceptual Problem 11.4

24. Classifying Reactions – Decomposition Reactions A decomposition reaction is a chemical change in which a single compound breaks down into two or more simpler products. 11.2

27. for Conceptual Problem 11.5

28. Classifying Reactions – Single-Replacement Reactions A single-replacement reaction is a chemical change in which one element replaces a second element in a compound. 11.2

29. Classifying Reactions The activity series of metals lists metals in order of decreasing reactivity. 11.2

32. for Conceptual Problem 11.6

33. Classifying Reactions – Double-Replacement Reactions A double-replacement reaction is a chemical change involving an exchange of positive ions between two compounds. 11.2

35. for Conceptual Problem 11.7

36. Classifying Reactions – Combustion Reactions A combustion reaction is a chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light. 11.2

38. for Conceptual Problem 11.8

39. Predicting the Products of a Chemical Reaction – The number of elements and/or compounds reacting is a good indicator of possible reaction type and thus possible products. 11.2

40. Predicting the Products of a Chemical Reaction 11.2

41. Predicting the Products of a Chemical Reaction 11.2

42. Predicting the Products of a Chemical Reaction 11.2

43. Predicting the Products of a Chemical Reaction 11.2

44. Predicting the Products of a Chemical Reaction 11.2

45. Reactions in Aqueous Solution Structures in limestone caverns are formed when carbon dioxide converts calcium hydrogen carbonate into calcium carbonate. The calcium carbonate precipitates and forms dramatic stalactites and stalagmites. You will learn to predict the formation of precipitates and write equations to describe the reactions that produce them. 11.3

46. Net Ionic Equations A complete ionic equation is an equation that shows dissolved ionic compounds as dissociated free ions. 11.3

47. Net Ionic Equations An ion that appears on both sides of an equation and is not directly involved in the reaction is called a spectator ion. The net ionic equation is an equation for a reaction in solution that shows only those particles that are directly involved in the chemical change. 11.3

48. Net Ionic Equations – A net ionic equation shows only those particles involved in the reaction and is balanced with respect to both mass and charge. 11.3

49. Net Ionic Equations Sodium ions and nitrate ions are not changed during the chemical reaction of silver nitrate and sodium chloride so the net ionic equation is 11.3

52. for Conceptual Problem 11.9

53. Predicting the Formation of a Precipitate – You can predict the formation of a precipitate by using the general rules for solubility of ionic compounds. 11.3

54. Predicting the Formation of a Precipitate 11.3

55. Predicting the Formation of a Precipitate Will a precipitate form when a sodium carbonate solution is mixed with a barium nitrate solution? 11.3

56. Predicting the Formation of a Precipitate Sodium nitrate is soluble but barium carbonate is insoluble. The net ionic equation is 11.3