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REACTION TYPES

REACTION TYPES. REACTION TYPES. A quick review… Evidences of a chemical change: Production of light, heat, sound Absorption of heat (container gets cold) New color, new odor Appearance of a new substance. SELF TEST: True/False. T F F T T. Paper burning is a chemical change.

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REACTION TYPES

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  1. REACTIONTYPES

  2. REACTION TYPES A quick review… Evidences of a chemical change: • Production of light, heat, sound • Absorption of heat (container gets cold) • New color, new odor • Appearance of a new substance

  3. SELF TEST: True/False T F F T T • Paper burning is a chemical change. • Salt dissolving in water is a chemical change. • Ice melting is a chemical change • Wood burning is a chemical change • Fruit rotting is a chemical change.

  4. I. CHEMICAL EQUATIONS Defined • Are a condensed statement of facts about a chemical reaction 2Na + Cl2 2NaCl

  5. II. Information in an Equation • Reactants: • are all substances that exist before the reaction • are always located to the left of the arrow 2Na + Cl2 2NaCl

  6. II. Information in an Equation • Products: • are all substances that exist after the reaction • are always located to the right of the arrow 2Na + 1Cl2 2NaCl

  7. II. Information in an Equation • Arrows: • Horizontal Arrows Stand for yields or produces 2Na + 1Cl2 2NaCl

  8. II. Information in an Equation HCl + Zn H2+ ZnCl2 • Arrows: • Vertical Arrows  indicates that the substance will leave the reaction as a gas(effervescence)

  9. II. Information in an Equation AgNO3 + Zn Ag + Zn(NO3)2 • Arrows: • Vertical Arrows  indicates that the substance settles to the bottom of the solution as a solid • (precipitate is formed)

  10. II. Information in an Equation H2(g) + O2(g) H2O(l) D. Showing Phase: (g) gas (l) liquid (s) solid (aq) dissolved in H2O

  11. 2H2(g)+ 1O2(g)+ energy 2H2O(l) F. Showing Energy Changes: 1.Endothermic Rx: • Absorb energy • Have + energy on reactant side • Exothermic Rx: • Release energy • Have + energy on product side

  12. III. Balanced Equations A. Obey the Law of Conservation of Matter • States: • Matter cannot be created or destroyed

  13. 2AlCl3 B. Coefficients • Are whole numbers that indicate how many atomsor mc of each substance are involved in the reaction • Are written in front of formulas • Are used to balance an eq.

  14. III. Balancing Equations C. General Rules for Balancing Eq. 1.Write the equations in ink balance in pencil. 2.Count the number of atoms of each element in the reactants and products. 3. Balance the elements one at a time by using coefficients. Never change subscripts!

  15. III. Balancing Equations D. Steps to Balancing an Eq. 1. Check for Diatomic Mc H2 N2 O2 F2 Cl2 Br2 I2 if these elements appear by themselves in an equation,they must be written with the subscript 2

  16. III. Balancing Equations D. Steps to Balancing an Eq. 2. Balance metals 3. Balance nonmetals 4. Balance oxygen 5. Balance hydrogen 6. Recount all atoms 7. If every coefficient will reduce, rewrite in the simplest whole-number ratio.

  17. III. Balancing Equations • Sample Problems Cl2+ NaBr Br2 + NaCl

  18. III. Balancing Equations • Sample Problems Al2(SO4)3 + CaCl2 AlCl3 + CaSO4

  19. REACTION TYPES • Synthesis Reaction – a reaction of at least two substances that forms a new, more complex compound A + B AB 2 Na + Cl2 2 NaCl

  20. REACTION TYPES 2. Decomposition Reaction – a reaction in which one compound breaks into at least two products AB  A + B 2 H2O  2 H2+ O2

  21. REACTION TYPES 3. Combustion Reaction – a reaction in which a hydrocarbon and oxygen burn yielding the products carbon dioxide and water. CH4+ 2O2 CO2+ 2H2O

  22. REACTION TYPES 4. Single Displacement Reaction – a reaction in which atoms of one element take the place of atoms of another element in a compound. AX+B BX + A 3 CuCl2+ 2 Al 2 AlCl3+ 3 Cu

  23. REACTION TYPESsingle replacement Predict the products for the following: * Pb + H3PO4 * Ca + H2O  * F2 + KCl 

  24. REACTION TYPESsingle replacement Predict the products for the following: * Pb + H3PO4H2 + Pb3(PO4)2 * Ca + H2O  * F2 + KCl

  25. REACTION TYPESsingle replacement Predict the products for the following: * 3Pb + 2H3PO43H2 + Pb3(PO4)2 * Ca + H2O  * F2 + KCl

  26. REACTION TYPESsingle replacement Predict the products for the following: * 3Pb + 2H3PO43H2 + Pb3(PO4)2 * Ca + H2O  Ca(OH)2 +H2 * F2 + KCl

  27. REACTION TYPESsingle replacement Predict the products for the following: * 3Pb + 2H3PO43H2 + Pb3(PO4)2 * Ca + 2 H2O  Ca(OH)2 +H2 * F2 + KCl

  28. REACTION TYPESsingle replacement Predict the products for the following: * 3Pb + 2H3PO43H2 + Pb3(PO4)2 * Ca + 2 H2O  Ca(OH)2 +H2 * F2 + KClKF + Cl2

  29. REACTION TYPESsingle replacement Predict the products for the following: * 3Pb + 2H3PO43H2 + Pb3(PO4)2 * Ca + 2 H2O  Ca(OH)2 +H2 * F2 + 2KCl2 KF + Cl2

  30. No, Ni is below Na Yes, Li is above Zn Yes, Al is above Cu Yes, Fe is above Cu We have looked at several reactions: Fe + CuSO4  Cu + Fe2(SO4)3 Li + H2O  LiOH + H2 Such experiments reveal trends. The activity series ranks the relative reactivity of metals. It allows us to predict if certain chemicals will undergo single displacement reactions when mixed: metals near the top are most reactive and will displace metals near the bottom. Q: Which of these will react? Fe + CuSO4  Ni + NaCl  Li + ZnCO3  Al + CuCl2  Cu + Fe2(SO4)3 NR (no reaction) Zn + Li2CO3 Cu + AlCl3

  31. REACTION TYPES 5. Double Displacement Reaction – a reaction in which new compounds are formed from the exchange of ions between two compounds. AX + BY  AY + BX Pb(NO3)2+ K2CrO4  PbCrO4+ 2 KNO3

  32. REACTION TYPESdouble replacement Predict the products for the following: Pb(NO3)2 + H3PO4 AgF + NiCl2 NaOH + CaBr2

  33. REACTION TYPESdouble replacement Predict the products for the following: Pb(NO3)2 + H3PO4 HNO3 + Pb3(PO4)2 AgF + NiCl2 NaOH + CaBr2

  34. REACTION TYPESdouble replacement Predict the products for the following: 3Pb(NO3)2 + 2H3PO4 6HNO3 + Pb3(PO4)2 AgF + NiCl2 NaOH + CaBr2

  35. REACTION TYPESdouble replacement Predict the products for the following: 3Pb(NO3)2 + 2H3PO4 6HNO3 + Pb3(PO4)2 AgF + NiCl2 NiF2 + AgCl NaOH + CaBr2

  36. REACTION TYPESdouble replacement Predict the products for the following: 3Pb(NO3)2 + 2H3PO4 6HNO3 + Pb3(PO4)2 2AgF + NiCl2 NiF2 + 2AgCl NaOH + CaBr2

  37. REACTION TYPESdouble replacement Predict the products for the following: 3Pb(NO3)2 + 2H3PO4 6HNO3 + Pb3(PO4)2 2AgF + NiCl2 NiF2 + 2AgCl NaOH + CaBr2 NaBr + Ca(OH)2

  38. REACTION TYPESdouble replacement Predict the products for the following: 3Pb(NO3)2 + 2H3PO4 6HNO3 + Pb3(PO4)2 2AgF + NiCl2 NiF2 + 2AgCl 2NaOH + CaBr2 2NaBr + Ca(OH)2

  39. REACTION TYPESdouble replacement Sometimes a double replacement reaction occurring in water will result in a precipitate. How would you predict whether a solid would form in a reaction? With a…

  40. REACTION TYPESdouble replacement Sometimes a double replacement reaction occurring in water will result in a precipitate. How would you predict whether a solid would form in a reaction? With a… SOLUBILITY TABLE!!!

  41. What’s soluble and what ain’t!!! • Solubility rules that apply to water solution: • (1) All alkali metal and ammonium compounds are soluble. • (2) All acetate, perchlorate, chlorate, and nitrate compounds are soluble. • (3) Silver, lead, and mercury(I) compounds are insoluble. • (4) Chlorides, bromides, and iodides are soluble

  42. What’s soluble and what ain’t!!! • (5) Carbonates, hydroxides, oxides, phosphates, silicates, and sulfides are insoluble. • (6) Sulfates are soluble except for calcium and barium. • These rules are to be applied in the order given.

  43. So…are we done or what???

  44. REACTION TYPES 6. Neutralization Reaction – a special double replacement reaction in which an acid is combined with a base and yields water and a salt. HCl+ NaOH NaCl+ H2O HCl + NaOH  NaCl+ H2O

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