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Chapter 8 Chemical Reactions

Chapter 8 Chemical Reactions. Evidence of Chemical Change. Evidence of Chemical Change Color change Formation of a solid Formation of a gas Absorption or release of heat energy Emission of light energy. Evidence of Chemical Change. Color change. Formation of a solid.

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Chapter 8 Chemical Reactions

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  1. Chapter 8Chemical Reactions

  2. Evidence of Chemical Change Evidence of Chemical Change • Color change • Formation of a solid • Formation of a gas • Absorption or release of heat energy • Emission of light energy

  3. Evidence of Chemical Change Color change

  4. Formation of a solid Evidence of Chemical Change

  5. Formation of a gas Evidence of Chemical Change

  6. Evolution of heat and light Evidence of Chemical Change

  7. Emission of light Evidence of Chemical Change

  8. Heat transfer as evidence of physical change Many physical changes are accompanied by heat transfer, so be cautious in using this form of evidence of a chemical change. Evidence of Chemical Change

  9. Evolution of a Chemical Equation When solid potassium is added to liquid water, a reaction occurs, producing hydrogen gas, potassium hydroxide solution, and heat:

  10. Evolution of a Chemical Equation Chemists have developed a standardized shorthand method for describing chemical reactions, such as the reaction of sodium and water, in writing. State Symbols and Their Meanings SymbolMeaning (s) solid (l) liquid (g) gas (aq) aqueous (dissolved in water)

  11. Evolution of a Chemical Equation Solid potassium K(s) plus + liquid water H2O(l) yields hydrogen gas H2(g) plus + potassium hydroxide solution KOH(aq)

  12. Evolution of a Chemical Equation The equation K(s) + H2O(l) H2(g) + KOH(aq) is said to be unbalanced because the number of atoms of each element is not the same before and after the chemical change. An equation is balanced when the number of atoms of each element is the same before and after the chemical change 2 K(s) + 2 H2O(l) H2(g) + 2 KOH(aq)

  13. Interpreting Chemical Equations The particulate-level interpretation of a chemical equation: 2 H2(g) + O2(g) 2 H2O(g) Two molecules of hydrogen react with one oxygen molecule to form two water molecules.

  14. Interpreting Chemical Equations The particulate-level interpretation of a chemical equation:

  15. Interpreting Chemical Equations The molar-level interpretation of a chemical equation: 2 H2(g) + O2(g) 2 H2O(g) Two moles of hydrogen react with one mole of oxygen to form two moles of water.

  16. Writing Chemical Equations • Write the formulas of the given reactants to the left of an arrow and the formulas of the products to the right. • Balance the equationby adding coefficients, but do not change the qualitative description of the reaction by adding, removing, or altering any chemical formula.

  17. Combination Reactions Combination Reaction Two or more substances combine to form a single product:

  18. Combination Reactions Example: Potassium combines with oxygen to form potassium oxide. Solution: Write the qualitative description: K + O2K2O Balance the O: K + O22 K2O Balance the K: 4 K + O22 K2O

  19. Combination Reactions Reactants: Any combination of elements and/or compounds Reaction type: Combination Equation type: A + X AX Products: One compound

  20. Decomposition Reactions Decomposition Reaction A compound breaks down into simpler substances:

  21. Decomposition Reactions Example: Water is decomposed into its elements. Solution: Write the qualitative description: H2O (l)  H2 (g) + O2 (g) Balance the O: 2 H2O (l)  2 H2 (g) + O2 (g)

  22. Decomposition Reactions Example: Calcium carbonate (limestone) is decomposed into carbon dioxide and calcium oxide (lime). CaCO3(s)  CaO (s) + CO2 (g)

  23. Decomposition Reactions Reactants: One compound Reaction type: Decomposition Equation type: AX A + X Products: Any combination of elements and compounds

  24. Single-Replacement Reactions Single-Replacement Reaction One element appears to replace another in a compound:

  25. Single-Replacement Reactions Example: Potassium is able to replace hydrogen in water. 2 K(s) + 2 HOH (l)  H2 (g) + 2 KOH (aq)

  26. Single-Replacement Reactions Example: A copper strip is placed in a solution of silver nitrate. Solution: Copper displaces silver from silver nitrate Cu (s) + 2AgNO3 (aq)  Cu(NO3)2 (aq) + 2 Ag (s) The reverse reaction does not occur

  27. Single-Replacement Reactions Example: A magnesium strip is placed in a solution of hydrochloric acid. Mg (s) + 2HCl (aq)  MgCl2 (aq) + H2 (g) Magnesium displaces hydrogen from acid

  28. Single-Replacement Reactions Summary: Single-Replacement Reactions Reactants: Element (A) plus a solution of an acid or an ionic compound (BX) Reaction type: Single-replacement Equation type: A + BX AX + B Products:Element (B) must be less active than element A

  29. Double-Replacement Reactions Double-Replacement Reaction Ions of two reactants appear to change partners:

  30. Double-Replacement Reactions Double-Replacement Reaction between two ionic compounds. When solutions of two ionic compounds are mixed, positive ions from one compound may combine with negative ions from the other compound to form a solid (precipitate) or a molecular compound (water, weak acid, weak base, gas)

  31. Formation of a precipitate Formation of silver chloride precipitate from sodium chloride and silver nitrate. NaCl (aq) + AgNO3 (aq)  NaNO3 (aq) + AgCl (s) Formation of barium sulfate precipitate from barium chloride and sodium sulfate. BaCl2 (aq) + Na2SO4 (aq)  BaSO4 (s) + 2 NaCl (aq)

  32. Neutralization Reactions: Formation of water Neutralization reaction is a reaction between an acid and a base. One hydrogen ion from acid reacts with one hydroxide ion from a base to form one water molecule. Neutralization of hydrochloric acid by sodium hydroxide. HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l) Reaction between sulfuric acid and solid aluminum hydroxide. 3 H2SO4 (aq) + 2 Al(OH)3 (s)  Al 2(SO4)3 (aq) + 3 H2O (l)

  33. Formation of weak acid Reaction of hydrochloric acid and sodium acetate to form acetic acid (weak acid) HCl (aq) + NaCH3CO2 (aq) NaCl (aq) + HCH3CO2 (aq) Reaction between hydrochloric acid and sodium sulfide to form hydrosulfuric acid (weak acid) Na2S(aq) + 2 HCl (aq)  2 NaCl(aq) + H2S (aq)

  34. Formation of a gas Reaction between hydrochloric acid and sodium carbonate to form carbon dioxide gas Na2CO3 (aq) + 2 HCl (aq)  2 NaCl(aq) + H2O(l) + CO2(g)

  35. Double-Replacement Reactions Summary: Double-Replacement Reactions Reactants: Solutions of two ionic compounds,(AX + BY) Reaction type: Double-replacement Equation type: AX + BY AY + BX Products: Two new compounds (AY + BX), one of which may be a solid, water, weakacid, weak base, or a gas

  36. Summary

  37. Homework Homework: 9, 15, 19, 23, 27, 29, 31, 35, 39, 53, 59, 69, 76

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