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Chapter 11 Chemical Reactions

Chapter 11 Chemical Reactions. Hindenburg Ship. Hydrogen gas combined with Oxygen which caused the ship to catch fire. Chemical reactions. Take place after you eat. Photosynthesis. In a Chemical reaction. One or more substances change into one or more new substances.

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Chapter 11 Chemical Reactions

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  1. Chapter 11 Chemical Reactions

  2. Hindenburg Ship Hydrogen gas combined with Oxygen which caused the ship to catch fire

  3. Chemical reactions Take place after you eat

  4. Photosynthesis

  5. In a Chemical reaction One or more substances change into one or more new substances

  6. Writing chemical equations Word Equations Reactants Products Iron + Oxygen Iron(III) Oxide Hydrogen Peroxide Dihydrogen monoxide + Oxygen Methane + oxygen Carbon dioxide + Dihydrogen monoxide

  7. Chemical Equations Skeleton Equations - Equation that does not show the amounts of the reactants and the products Fe + O2 Fe2O3 Unbalanced equation !!!!!

  8. One can add more information to the skeleton equations: To indicate if the reactants and products are liquids, solids or gases you use parentheses Fe(s) + O2(g) Fe2O3 (s) To indicate a catalyst (a substance that speeds up the reaction but is not used in the reaction) you place the catalyst over the arrow MnO2 H2O2 (aq) H2O (l) + O2 (g)

  9. heat catalyst

  10. Balancing Equations Reactants Products Frame + wheel + hanlebar + pedal Bicycle F + 2 W + 1 H + 2 P FW2HP2

  11. Calcium + Oxygen Calcium Oxide First write the skeleton equation Ca + O2 CaO Now balance Balanced!! 2 Ca + O2 2 CaO 2 1 Ca 2 1 Ca 2O 2 1 O

  12. Hydrogen + oxygen Dihydrogen monoxide First write the skeleton equation H2 + O2 H2O Now balance 4 2 H 2 H 4 2 O 2 1 O Balanced!! 2 H2 + O2 2 H2O

  13. Types of Chemical Reactions 5 Types combination decomposition Single-replacement Double-replacement combustion

  14. Combination Reactions (Synthesis) Chemical change in which two or more substances react to form a single new substance 2 Mg(s) + O2(g) 2 MgO(s) Metal + nonmetal 2 K(s) + Cl2(g) 2 KCl(s) SO2 (g) S (s) + O2(g) Two nonmetals two possibilities 2 S (s) + 3 O2(g) SO3 (g)

  15. Decomposition Reactions Chemical change in which a single compound breaks down into two or more simpler products **Requires heat or electricity 2 HgO(s) heat 2 Hg(l) + O2(g) 2 H2O(l) electricity 2 H2(g) + O2(g)

  16. Single-replacement Reactions Chemical change in which one element replaces a second element in a compound Zn(s) + H2SO4(aq) ZnSO4(aq) + H2(g) Cl2(g) + 2 NaBr(aq) 2NaCl(aq) + Br2(aq)

  17. Double-replacement Reactions Chemical change involving an exchange of positive ions between two compounds 2 NaCN(aq) + H2SO4(aq) 2 HCN(aq) + Na2SO4(aq) NaOH(aq) + Fe(NO3)3 (aq) Fe(OH)3(s) + 3 NaNO3(aq) **Solution containing two ionic compounds

  18. Combustion Reactions Chemical change in which an element or compound reacts with oxygen often producing energy in the form of heat or light CH4 (g) + 2 O2(g) CO2 (g) + 2 H2O(l) 2HCOOH (aq) + O2(g) 2CO2 (g) + 2 H2O(l) hydrocarbon + oxygen  carbon dioxide + water

  19. ** The number of elements and/or compounds reacting is a good indicator of possible reaction types and possible products- you can make predictions

  20. Check what you know!! • What are the five different types of reactions? • What type of reaction are the following? • C3H6 + O2→ CO2 + H2O • Li + O2 → Li2O • Zn + AgNO3 → Ag + Zn(NO3)2 Combination, decomposition, single-replacement, double-replacement, combustion Combustion Combination Single-replacement

  21. Predict the type of reaction that will occur? • An aqueous solution of two ionic compounds. • Reactant is a single compound. • The reactants are two elements. • The reactants are oxygen and a compound of carbon and hydrogen. Double-replacement Decomposition Combination Combustion

  22. Reactions in Aqueous Solution Net Ionic Equations Many important reactions take place in water Net ionic equations are different that the equations we are used to writing. We used to write equations like this: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

  23. Complete Ionic Equations Shows the dissolved ionic compound as separate ions Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) AgCl(s) + Na+(aq) + NO3- (aq) Spectator ions - Ion that appears on both sides of the equation but is not involved in the reaction Net Ionic Equations Equation that shows only the particles that are directly involved in the reaction Ag+(aq) + Cl-(aq) AgCl(s)

  24. Predicting the formation of a precipitate

  25. Check what you know!!! • Write a balanced net ionic equation. • Pb(NO3)2(aq) + H2SO4(aq) → PbSO4(s) + HNO3(aq) First write the complete ionic equation Pb2+(aq) + NO3- (aq) + H+(g) + SO42-(aq) PbSO4(s) + H+(g) + NO3- (aq) Then find the spectator ions and cross them out Finally, write the net ionic equations Pb2+(aq) + SO42-(aq) PbSO4(s)

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