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Chemical Reactions

Chemical Reactions. Chemical reactions occur when bonds between the outermost parts of atoms are formed or broken. Chemical reactions involve changes in matter, the making of new materials with new properties, and energy changes.

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Chemical Reactions

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  1. Chemical Reactions

  2. Chemical reactions occur when bonds between the outermost parts of atoms are formed or broken

  3. Chemical reactions involve changes in matter, the making of new materials with new properties, and energy changes.

  4. Symbols represent elements, formulas describe compounds, chemical equations describe a chemical reaction

  5. Items to the LEFT of the arrow in a chemical equation are called REACTANTS. Na + Cl NaCl

  6. Items to the right of the arrow are called PRODUCTS. Ex: Na + Cl NaCl

  7. Important NOTE: No matter how many reactants and products are involved, all atoms present at the start of a reaction are present at the end.

  8. Conservation of Mass THE TOTAL MASS OF THE REACTANTS MUST EQUAL THE TOTAL MASS OF PRODUCTS. MATTER IS NEVER CREATED OR DESTROYED.

  9. Coefficient A number that tells how many molecules of a substance are involved in a chemical reaction. A coefficient of 1 is not written.

  10. Subscripts • A subscript indicates how many atoms of an element are in a compound Ex. H2SO4 H= 2 S = 1 O = 4

  11. Subscripts vs. Coefficients

  12. Symbols +-- used to separate two reactants or products. (yields) Separates reactants and products.

  13. Exothermic Reactions that release heat.

  14. Endothermic Reactions that absorb heat.

  15. Catalyst A substance that speeds up chemical reactions.

  16. Inhibitor A substance that slows down a chemical reaction.

  17. Types of Reactions

  18. Combustion Reactions that have hydrocarbons (CH4) and oxygen as reactants, and carbon dioxide and water as products.

  19. Example: C3H8 + 5O2 3CO2 + 4H2O

  20. Synthesis Reactions

  21. Examples 2Na + Cl2 2NaCl Na2O + CO2 Na2CO3

  22. Decomposition Reactions Starts with one reactant and ends with 2 or more products.

  23. Examples 2 KClO3 2KCl+3O2 2NaCl 2Na + Cl2

  24. Single Replacement Reactions One compound and a free element that recombine to yield a new compound and new free element.

  25. Examples Fe + CuSO4 Cu + FeSO4 2Na + 2HCl H2 + 2NaCl

  26. Double Replacement Reactions Starts with 2 compounds as reactants. These recombine to form 2 new compounds as products. + +

  27. Examples NaCl + AgNO3 NaNO3 + AgCl KOH + HNO3 HOH + KNO3 C:\Documents and Settings\mswilliams\Local Settings\Temporary Internet Files\OLK1B5\types.htm

  28. Let's Practice! The first slide shows the unbalanced equation, followed by the balanced equation.

  29. Unbalanced C + O2 ----- CO2

  30. Balanced C + O2 ----- CO2

  31. Unbalanced NaCl ---- Na + Cl2

  32. Balanced 2NaCl ---- 2Na + Cl2

  33. Unbalanced FeCl2 + K2S -- FeS + KCl

  34. Balanced FeCl2 + K2S -- FeS + 2KCl

  35. Unbalanced C2H4 + O2 CO2 + H2O

  36. Balanced C2H4 + 3O2 2CO2 + 2H2O

  37. Unbalanced AlCl3 + Na2CO3 Al2(CO3)3 + NaCl

  38. Balanced 2AlCl3 + 3Na2CO3 Al2(CO3)3 + 6NaCl

  39. Unbalanced CS2 + O2 CO2 + SO2

  40. Balanced CS2 + 3O2 CO2 + 2SO2

  41. Unbalanced Fe + H2O  Fe3O4 + H2

  42. Balanced 3Fe + 4H2O  Fe3O4 + 4H2

  43. Unbalanced AlCl3  Al + Cl2

  44. Balanced 2AlCl3  2Al + 3Cl2

  45. Unbalanced Na + H2SO4 ---> Na2SO4 + H2

  46. Balanced 2Na + H2SO4 ---> Na2SO4 + H2

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