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Chemical Reactions. Section 9.1 Reactions and Equations Section 9.2 Classifying Chemical Reactions. Click a hyperlink or folder tab to view the corresponding slides. Exit. Chapter Menu. Section 9.1 Reactions and Equations. Recognize evidence of chemical change.

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  1. Chemical Reactions Section 9.1 Reactions and Equations Section 9.2 Classifying Chemical Reactions Click a hyperlink or folder tab to view the corresponding slides. Exit Chapter Menu

  2. Section 9.1 Reactions and Equations Recognizeevidence of chemical change. Representchemical reactions with equations. Balancechemical equations. Section 9-1

  3. Section 9.1 Reactions and Equations chemical change:a process involving one or more substances changing into a new substance chemical reaction reactant product chemical equation coefficient Section 9-1

  4. Chemical Reactions Chemical reaction: The process by which one or more substances are rearranged to form different substances. Section 9-1

  5. Chemical Reactions (cont.) Evidence of a chemical reaction • Change in temperature • Change in color • Odor, gas, or bubbles Section 9-1

  6. Representing Chemical Reactions (cont.) A chemical equationis a statement that uses chemical formulas to show the identities and relative amounts of the substances involved in a chemical reaction. Section 9-1

  7. Representing Chemical Reactions Two parts of chemical equations Reactantsare the starting substances. Productsare the substances formed in the reaction. Section 9-1

  8. Section 9-1

  9. Representing Chemical Reactions (cont.) Chemical Reaction in words aluminum(s) + bromine(l) → aluminumbromide(s) What state are the reactants? What state is the product? Section 9-1

  10. Representing Chemical Reactions (cont.) Skeleton equations use atomic symbols Al(s) + Br(l) → AlBr3(s) Notice the product is a correct molecular formula Section 9-1

  11. Solid lithium reacts with chlorine gas to produce solid lithium chloride. Example 1

  12. Solid lithium reacts with chlorine gas to produce solid lithium chloride. lithium(s) + chlorine(g)  lithium chloride(s) Example 1 word equation

  13. Solid lithium reacts with chlorine gas to produce solid lithium chloride. lithium(s) + chlorine(g)  lithium chloride(s) Li(s) + Cl2(g)  LiCl(s) Remember a lot of atoms are diatomic in nature Example 1 skeleton equation

  14. Nitrogen gas reacts with oxygen gas to produce nitrogen dioxide gas. Example 2

  15. Nitrogen gas reacts with oxygen gas to produce nitrogen dioxide gas. nitrogen(g) + oxygen(g)  nitrogen dioxide(g) Example 2 word equation

  16. Nitrogen gas reacts with oxygen gas to produce nitrogen dioxide gas. nitrogen(g) + oxygen(g)  nitrogen dioxide(g) N2(g) + O2(g)  NO2(g) Example 2 skeleton equation

  17. Solid iron reacts with aqueous copper (II) nitrate to produce solid copper and aqueous iron (II) nitrate. Example 3

  18. Solid iron reacts with aqueous copper (II) nitrate to produce solid copper and aqueous iron (II) nitrate. Iron(s) + copper(II) nitrate(aq)  copper(s) + iron(II) nitrate(aq) Remember nitrate is (NO3)- Example 3 word equation

  19. Solid iron reacts with aqueous copper (II) nitrate to produce solid copper and aqueous iron (II) nitrate. Iron(s) + copper(II) nitrate(aq)  copper(s) + iron(II) nitrate(aq) Fe(s) + Cu(NO3)2(aq)  Cu(s) + Fe(NO3)2(aq) Example 3 skeleton equation

  20. Balancing Chemical Equations Balanced equation for the reaction between aluminum and bromine. Section 9-1

  21. Balancing Chemical Equations (cont.) A coefficientin a chemical equation is the number written in front of a reactant or product. It describes the lowest whole-number ratio. Yeah!!!! Section 9-1

  22. Balancing Chemical Equations (cont.) Balanced equations represent the Law of Conservation of Mass Section 9-1

  23. Balancing Chemical Equations (cont.) Section 9-1

  24. Li(s) + Cl2(g)  LiCl(s) 1 Li 2 Cl 1 Li 1 Cl Example 1 balanced equation

  25. Li(s) + Cl2(g)  LiCl(s) 1 Li 2 Cl 1 Li 1 Cl need 2 Cl on this side Example 1 balanced equation

  26. Li(s) + Cl2(g)  LiCl(s) 1 Li 2 Cl 1 Li 1 Cl need 2 Cl on this side put 2 in front of LiCl Li(s) + Cl2(g)  2LiCl(s) 1 Li 2 Cl 2 Li 2 Cl Example 1 balanced equation

  27. Li(s) + Cl2(g)  LiCl(s) 1 Li 2 Cl 1 Li 1 Cl need 2 Cl on this side Li(s) + Cl2(g)  2LiCl(s) 1 Li 2 Cl 2 Li 2 Cl bc molecule need 2 Li on this side put 2 in front of Li only Example 1 balanced equation

  28. Li(s) + Cl2(g)  LiCl(s) 1 Li 2 Cl 1 Li 1 Cl need 2 Cl on this side Li(s) + Cl2(g)  2LiCl(s) 1 Li 2 Cl 2 Li 2 Cl bc molecule Need 2 Li 2Li(s) + Cl2(g)  2LiCl(s) 2 Li 2 Cl 2 Li 2 Cl all balanced Example 1 balanced equation

  29. N2(g) + O2(g)  NO2(g) Example 2 balanced equation

  30. N2(g) + O2(g)  NO2(g) 2N 2O 1N 2O not balanced put 2 in front of NO2 N2(g) + O2(g)  2NO2(g) 2N 2O 2N 4O not balanced put 2 in front of O2 N2(g) + 2O2(g)  2NO2(g) 2N 4O 2N 4O balanced Example 2 balanced equation

  31. Fe(s) + Cu(NO3)2(aq)  Cu(s) + Fe(NO3)2(aq) Example 3 balanced equation

  32. Fe(s) + Cu(NO3)2(aq)  Cu(s) + Fe(NO3)2(aq) 1Fe 1Cu 2(NO3) 1Cu 1Fe 2(NO3) balanced Example 3 balanced equation

  33. Solid potassium reacts with liquid water to produce hydrogen gas and a water (aqueous) solution of potassium hydroxide. Hydroxide is OH- Practice 1 balanced equation

  34. Solid potassium reacts with liquid water to produce hydrogen gas and a water (aqueous) solution of potassium hydroxide. Potassium(s) + water(l)  hydrogen(g) + potassium hydroxide(aq) K(s) + H2O(l)  H2(g) + KOH(aq) Practice 1 balanced equation

  35. Solid potassium reacts with liquid water to produce hydrogen gas and a water (aqueous) solution of potassium hydroxide. Potassium(s) + water(l)  hydrogen(g) + potassium hydroxide(aq) K(s) + H2O(l)  H2(g) + KOH(aq) 2K(s) + 2H2O(l)  H2(g) + 2KOH(aq) Practice 1 balanced equation

  36. Calcium chloride and sodium carbonate in water (aqueous) solution produce solid calcium carbonate and a water solution of sodium chloride. Carbonate is (CO3)-2 Practice 2 balanced equation

  37. Calcium chloride and sodium carbonate in water (aqueous) solution produce solid calcium carbonate and a water solution of sodium chloride. Calcium chloride(aq) + sodium carbonate(aq)  calcium carbonate(s) + sodium chloride(aq) CaCl2(aq) + Na2(CO3)(aq)  Ca(CO3)(s) + NaCl(aq) Practice 2 balanced equation

  38. Calcium chloride and sodium carbonate in water (aqueous) solution produce solid calcium carbonate and a water solution of sodium chloride. Calcium chloride(aq) + sodium carbonate(aq)  calcium carbonate(s) + sodium chloride(aq) CaCl2(aq) + Na2(CO3)(aq)  Ca(CO3)(s) + NaCl(aq) CaCl2(aq) + Na2(CO3)(aq)  Ca(CO3)(s) + 2NaCl(aq) Practice 2 balanced equation

  39. Liquid bromine and solid lithium iodide react to form solid lithium bromide and solid iodine. Practice 3 balanced equation

  40. Liquid bromine and solid lithium iodide react to form solid lithium bromide and solid iodine. bromine(l) + lithium iodide(s)  lithium bromide(s) + iodine(s) Br2(l) + LiI(s)  LiBr(s) + I2(s) Practice 3 balanced equation

  41. Liquid bromine and solid lithium iodide react to form solid lithium bromide and solid iodine. bromine(l) + lithium iodide(s)  lithium bromide(s) + iodine(s) Br2(l) + LiI(s)  LiBr(s) + I2(s) Br2(l) + 2LiI(s)  2LiBr(s) + I2(s) Practice 3 balanced equation

  42. A B C D Section 9.1 Assessment Which of the following is NOT a chemical reaction? A.a piece of wood burning B.a car rusting C.an ice cube melting into water D.red litmus paper turning blue Section 9-1

  43. A B C D Section 9.1 Assessment What is the coefficient of bromine in the equation 2Al(s) + 3Br2(l) → 2AlBr3(s)? A.1 B.2 C.3 D.6 Section 9-1

  44. End of Section 9-1

  45. Section 9.2 Classifying Chemical Reactions Classify chemical reactions. Identify the characteristics of different classes of chemical reactions. Section 9-2

  46. Section 9.2 Classifying Chemical Reactions (cont.) Types of chemical reactions: • Synthesis • Combustion • Decomposition • Replacement reactions Section 9-2

  47. Section 9.2 Classifying Chemical Reactions synthesis reaction combustion reaction decomposition reaction single-replacement reaction double-replacement reaction precipitate metal: an element that is a solid at room temperature, a good conductor of heat and electricity, and is generally shiny Section 9-2

  48. Types of Chemical Reactions Synthesis reaction two or more substances react produce a single product. Section 9-2

  49. Types of Chemical Reactions (cont.) Synthesis Example Section 9-2

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