Chapter Seventeen: Chemical Change

2. Chapter Seventeen: Chemical Change • 17.1 Chemical Reactions • 17.2 Balancing Equations • 17.3 Classifying Reactions

3. 17.1 Chemical Reactions • A chemical reaction is the process of breaking of chemical bonds in one or more substances, and the reforming of new bonds to create new substances. • When you make pizza, which changes are physical and which are chemical changes?

4. 17.1 Evidence of chemical change Four indicators of chemical change are: • Formation of new gas • Formation of new solid • Release of energy (heat or light) • Color change

5. 17.1 Products and reactants • In chemical reactions, you start with reactants that are combined to make products. • The reactants are the starting substances. • The products are the new substances which result from the chemical reaction.

7. 17.1 Reactants and products • In the reaction, methane (a natural gas) is burnedor combusted. • Some energy is added to get the reaction started.

8. 17.2 Balancing Equations • Antoine Laurent Lavoisier, established an important principal based on his experiments with chemical reactions. • He stated that the total mass of the products of a reaction is equal to the total mass of the reactants. • The law of conservation of mass holds true for even a burning mass of wood.

9. 17.2 Balancing Equations • The combined mass of the burning wood and oxygen is converted into carbon dioxide and water.

10. 17.2 Conservation of mass • Lavoisier showed that a closed system must be used when studying chemical reactions. • When chemicals are reacted in a closed container, you can show that the mass before and after the reaction is the same.

11. 17.2 Formula mass • The sum of the atomic mass values of the atoms in a chemical formula is called the formula mass.

12. 17.2 Avogadro’s Number • The Avogadro number was named in honor of Amedeo Avogadro who discovered that a mole of any gas under the same conditions has the same number of molecules. • Johann Josef Loschmidt, a German physicist, named and discovered the Avogadro number. • Loschmidt realized that a mole of any substance—be it a gas, liquid, or solid—contains 6.02 x 1023 atoms or molecules.

13. 17.2 Molar Mass • The mass (in grams) of one mole of a compound is called its molar mass.

14. Solving Problems What is the molar mass of one mole of CaCO3? • Looking for: • … molar mass of CaCO3 • Given • … chemical formula • Relationships: • no. amu in formula = molar mass in grams

15. Solving Problems • Solution Formula mass CaC03 = 100.19 g 1 mole CaC03 = 100.19 g CaCO3

16. 17.2 Chemical Equations • When a chemical reaction is written using chemical formulas and symbols, it is called a chemical equation.

17. 17.2 Chemical equations • An arrow is always included between reactants and products. • It means “to produce” or “to yield.” to produce Reactants Products “Methane combines with oxygen gas to produce carbon dioxide gas and water vapor.”

18. 17.2 Numbers in equations

19. 17.2 Balancing equations • The law conservation of mass is applied by balancing the number and type of atoms on either side of the equation.

20. 17.2 Balancing equations • Counting atoms is necessary to balance an equation. How many carbon atoms? How many hydrogen atoms? How many oxygen atoms?

21. 17.2 Steps for balancing • If not provided, write the word form of the equation. • Calcium carbonate reacts with hydrochloric acid to produce calcium chloride, carbon dioxide and water.

22. 17.2 Steps for balancing • If not provided, write the chemical equation from the word form.

23. 17.2 Steps for balancing • Count the number of each type of atom on both sides.

24. 17.2 Steps for balancing • Add coefficients to balance the equation.

25. Solving Problems • In this reaction, chalcocite (a mineral) reacts with oxygen in the presence of heat. The products are a type of copper oxide and sulfur dioxide. Balance this equation: Cu2S + O2 → Cu2O + SO2

26. Solving Problems • Looking for: • …the coefficients for each molecule • Given • … chemical formulas which show types and no. of atoms

27. Solving Problems • Relationships • Coefficients can be added in front of any chemical formula in a chemical equation. • When a coefficient is added in front of a chemical formula, all atoms in that formula are multiplied by that number. • Use common denominators to help choose coefficients to try.

28. Solving Problems • Solution- Trial and error

29. 17.3 Addition reactions • The process of creating large molecules from small ones is called polymerization.

30. 17.3 Addition reactions • In an addition reaction, two or more substances combine to form a new compound.

31. 17.3 Decomposition reactions • A chemical reaction in which a single compound is broken down to produce two or more smaller compounds is called a decomposition reaction.

32. 17.3 Single Displacement • In a single-displacement reaction, one element replaces a similar element in a compound.

33. 17.3 Double Displacement • In a double-displacement reaction, ions from two compounds in solution exchange places to produce two new compounds. • One of the compounds formed is usually a precipitate that settles out of the solution, a gas that bubbles out of the solution, or a molecular compound such as water.

34. 17.3 Precipitation reactions • A precipitate is a new solid product that comes out of solution in a chemical reaction. • The formation of a cloudy precipitate is evidence that a double-displacement reaction has occurred.

35. 17.3 Precipitation • The limewater test for carbon dioxide is a precipitation reaction.

36. 17.3 Combustion reactions • A combustion reaction, also called burning, occurs when a substance such as wood, natural gas, or propane combines with oxygen and releases a large amount of energy in the form of light and heat.

37. 17.3 Combustion reactions • What do reactants like wood, natural gas, and propane have in common?

39. Chapter 18.1 Learning Goals • Contrast endothermic and exothermic reactions. • Explain why activation energy is needed to begin chemical reactions. • Describe what happens when ionic compounds are dissolved in water.

40. 18.1 Energy and Reactions • Energy is involved in chemical reactions in two ways: • to break some (or all) bonds between atoms in the reactants so the atoms can form new bonds or • when the atoms or products form new bonds to make new products.

41. 18.1 Two Types of Reactions • We classify chemical reactions based on how the energy of the reactants compares to the energy of the products.

42. 18.1 Exothermic reactions • If forming new bonds releases more energy than it takes to break the old bonds, the reaction is exothermic.

43. 18.1 Exothermic reactions • A good example is the reaction of hydrogen with oxygen. Once started, exothermic reactions tend to keep going as each reaction releases more energy to fuel neighboring molecules.

44. 18.1 Endothermic reactions • If forming new bonds in the products releases less energy than it took to break the original bonds, the reaction is endothermic.

45. 18.1 Endothermic reactions • An important endothermic reaction is photosynthesis. • Plants need energy from sunlight to make glucose and oxygen from carbon dioxide and water.

46. 18.1 Activation Energy • Activation energy is the energy needed to begin a reaction and break chemical bonds in the reactants.

47. 18.1 Activation Energy • This is why a flammable material like gasoline does not burn without a spark or flame.

48. 18.1 Carbon Reactions • Carbon dioxide and other atmospheric gases are called “greenhouse gases.” Scientists believe the rise in amount of greenhouse gases will result in rises in sea level and changes in weather.

49. 18.1 Examples of Endothermic Reactions • Most of the reactions used in industry to produce useful materials require more energy than they produce. • One process that uses endothermic reactions is the refining of ores to produce useful metals.

50. 18.1 Examples of Endothermic Reactions • Most of the reactions used in industry to produce useful materials require more energy than they produce. • The reaction taking place inside an instant cold pack is endothermic.