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Chapter 10 Notes, Part I

Chapter 10 Notes, Part I. Parts of an equation Types of reactions. What is a chemical reaction?. A chemical reaction is the act of changing substances into new substances with new and different chemical and physical properties. A Chemical Equation.

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Chapter 10 Notes, Part I

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  1. Chapter 10 Notes, Part I Parts of an equation Types of reactions

  2. What is a chemical reaction? • A chemical reaction is the act of changing substances into new substances with new and different chemical and physical properties.

  3. A Chemical Equation • A chemical equation shows what is going on in a chemical reaction. • Instead of writing down the entire sentence “hydrogen reacts with oxygen to form dihydrogen monoxide (water)”, you could write…

  4. reactants The substances you have before a chemical reaction occurs (found on the left side of the equation) products The substances you have after a chemical reaction occurs (found on the right side of the equation) 2H2 + O2a2H2O

  5. subscripts How many atoms of an element are in a compound coefficients How many substances are in the reaction 2H2 + O2a2H2O

  6. 2H2 + O2a2H2O The arrow reads as “produces”, “yields” or “reacts to form”

  7. Word Equation • This indicates the reactants and products of chemical reactions. reactant 1 + reactant 2 → product 1 iron (s) + chlorine (g) → iron(III) chloride (s) This reads: “Iron and chlorine react to produce iron(III) chloride.”

  8. Skeleton Equation • Uses chemical formulas instead of words to identify your reactants and products. Word: iron (s) + chlorine (g) → iron(III) chloride (s) Skeleton: Fe (s) + Cl2 (g) → FeCl3 (s)

  9. Chemical Equation • A skeleton equation that shows that the number of atoms of each reactant and each product is equal on both sides of the arrow, also called balanced. Word: iron (s) + chlorine (g) → iron(III) chloride (s) Skeleton: Fe (s) + Cl2 (g) → FeCl3 (s) Chemical: 2Fe (s) + 3Cl2 (g) → 2 FeCl3

  10. Iron reacts with oxygen gas to produce iron (III) oxide 4Fe + 3O2a2Fe2O3

  11. Other symbols in an Equation • (s) = substance is solid • (l) = substance is liquid • (g) = substance is a gas • (aq) = substance is dissolved in water • D = heat • A formula written above or below an arrow means it is a catalyst (a substance that speeds up a reaction without being used up by it.)

  12. What is: • The name of something that speeds a reaction, but is not used up? • The name of what you have before a reaction takes place? • The symbol for heat? • The number that shows there are more than one of the entire compound?

  13. Types of reactions • There are five types of reactions • Synthesis • Decomposition • Single replacement • Double replacement • Combustion

  14. Synthesis Reaction • A synthesis reaction occurs when two or more elements or compounds combine to form a single substance. • It will follow the form A + B a AB • Example: Fe + S aFeS

  15. Decomposition Reaction • A decomposition reaction occurs when one substance breaks down into two or more substances. • It will follow the pattern AB a A + B • Example: CaCO3aCaO+CO2

  16. Single Replacement Reaction • One element replaces another element in a compound. • Generally follows the formula: AB + C a A + BC • Example: Mg+Zn(NO3)2aZn+Mg(NO3)2

  17. Double Replacement Reaction • The exchange of two positive ions between two reacting compounds, forming two new compounds as a product. • Generally follows the formula: AB + CD a AD + CB • Example: Na2S+Cd(NO3)2aCdS+2NaNO3

  18. Combustion Reaction • A compound reacts with oxygen to producing energy as heat and light. • Most of the time, it is a hydrocarbon reacting with oxygen, and the outcome is always carbon dioxide and water • Follows the form: A + O2a CO2 + H2O • Example: CH4 + O2a CO2 + 2H2O

  19. What type of reaction is: • NaCN + H2SO4a 2HCN + Na2SO4 • Zn + 2HCl a ZnCl2 + H2 • 2C2H6 + 7O2a 4CO2 + 6H2O • 2H2 + O2a 2H2O

  20. Tell which of the five types of reactions the following are:

  21. 2Na + 2H2O a 2NaOH + H2 Single replacement

  22. Fe + S a FeS combination

  23. Al(OH)3 + 3NaCl aAlCl3 + 3NaOH Double replacement

  24. CH4 + 2O2a CO2 + 2H2O combustion

  25. KClO2a KCl + O2 decomposition

  26. NaOH + HCl a NaCl + H2O Double replacement

  27. 4Fe + 3O2a 2Fe2O3 combination

  28. 2C2H2 + 5O2a 4CO2 + 2H2O combustion

  29. H2 + Cl2a 2HCl combination

  30. MgO + 2KF a MgF2 + K2O Double replacement

  31. Na + Al(NO3)3aNaNO3 + Al Single replacement

  32. 2PbO2a 2PbO + 3O2 decomposition

  33. Ba(CN)2 + H2SO4a BaSO4 + HCN Double replacement

  34. C3H8 + 5O2a 3CO2 + 4H2O combustion

  35. 4Li + O2a 2Li2O combination

  36. 2Ag + 2HCl a 2AgCl + H2 Single replacement

  37. 2H2O2a 2H2O + O2 decomposition

  38. C2H2 + O2a CO2 + H2O combustion

  39. 2HBr a H2 + Br2 decomposition

  40. CrSO4 + 2AgNO3a Cr(NO3)2 + Ag2SO4 Double replacement

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