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Common Types of Reactions

Common Types of Reactions. N 2 (g) + O 2 (g). 4Al(s) + 3O 2 (g). NH 3 (g) + HCl(g). 2NO(g). NH 4 Cl(s). 2Al 2 O 3 (s). Combination Rxns. Between non-metals to give a molecular product Between metal and non-metal to yield an ionic product Between compounds.

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Common Types of Reactions

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  1. Common Types of Reactions

  2. N2(g) + O2 (g) 4Al(s) + 3O2 (g) NH3(g) + HCl(g) 2NO(g) NH4Cl(s) 2Al2O3(s) Combination Rxns • Between non-metals to give a molecular product • Between metal and non-metal to yield an ionic product • Between compounds (Al3+, O2-)

  3. CuSO4.5H2O(s) MgCO3(s) CuSO4(s) + 5H2O(g) MgO(s) + CO2(g) Decomposition Rxns

  4. Zn(s) + 2HCl(aq) Na(s) + 2H2O(l) ZnCl2(aq) + H2(g) 2NaOH(aq) + H2(g) Single Replacement Rxns

  5. H2O(l) + NaNO3(aq) PbI2(s) + 2KNO3(aq) HNO3(aq) + NaOH(aq) Pb(NO3)2(aq) + 2KI(aq) yellow solid acid base salt Double Replacement(Metathesis)Rxns • Precipitation Reactions • Acid-Base (Neutralization) Reactions

  6. H2O(l) + NaNO3(aq) PbI2(s) + 2KNO3(aq) HNO3(aq) + NaOH(aq) Pb(NO3)2(aq) + 2KI(aq) ZnCl2(aq) + H2(g) Zn(s) + 2HCl(aq) More Than One Way to Categorize • Acid-Base (Neutralization) Rxns • Oxidation-Reduction(Redox, Electron Transfer) Rxns • Precipitation Rxns

  7. More About Acids and Bases... • Acids • Taste sour (vinegar, lemon juice) • Turn litmus red • React with bases to make H2O • React with many metals to make H2 • React with carbonates to make CO2 and H2O • Bases • Taste bitter • Turn litmus blue • React with acids to make water • Feel slippery

  8. The Arrhenius View • Acid- yields H+ when added to water • HCl(g) + H2O(l)g H+(aq) + Cl- (aq) unbalanced • Base - yields OH- when added to water • NaOH(s) + H2O(l)g Na+(aq) + OH-(aq) unbalanced

  9. acid + base a salt + water HCl (aq) + NaOH (aq) NaCl (aq) + H2O Arrhenius View of Neutralization

  10. The BrønstedView • More general approach, not limited to water • Brønsted acid= H+ donor • Brønstedbase = H+ acceptor • Neutralization = “proton” (H+) transfer

  11. hydronium ion, H3O+ Why is HCl a BrønstedAcid?

  12. Why is Ammonia a Brønsted Base? base acid

  13. Redoxe- transfer rxns

  14. 2Fe (s) + 3Cl2 (g) 2FeCl3 (s) Fe3+, Cl- Fe is oxidized (loses e-): Fe Fe3+ + 3e- Cl2 is reduced (gains e-):Cl2 + 2e- 2Cl- reducing agent (supplier of e-): Fe oxidizing agent (acceptor of e-): Cl2 Oxidation-Reduction

  15. oxidation reduction overall 2Fe 2Fe3+ + 6e- 3Cl2 + 6e- 6Cl- 2Fe + 3Cl2 2FeCl3 Adding Half Rxns Yields Overall Rxn

  16. Cu Cu2+ + 2e- Cu(s) + 2AgNO3(aq) Cu(NO3)2(aq) + 2Ag(s) Ag+ + 1e- Ag Problem: What is the oxidizing agent when copper reacts with silver nitrate to form silver and copper(II) nitrate? Ag+ is the oxidizing agent (consumes electrons from Cu)

  17. 2KClO3 2KCl + 3O2 Problem: Is Cl reduced or oxidized when KClO3 decomposes? ?

  18. Tracking e- Transfers Oxidation State (Oxidation Number): The charge an element carries either alone or when combined with other elements in a compound. oxidation: O# goes up reduction: O# goes down change in O# tells whether ox or red occurs

  19. Simple Oxidation Number Rules • Free element O# = zero. Fe, Cl2, Na, Pb, H2, O2, P4 = 0 2. In monatomic ions, the O# = ion charge Li+, Li = +1; Fe3+, Fe = +3; O2-, O = -2 • Certain elements have same O# in ~all their compounds. O usually -2, H usually +1 ... 4. S (O# in cmpd) = overall charge of cmpd/ion. More extensive rules are in text...

  20. +5 -2 +1 -1 0 +1 2KClO3 2KCl + 3O2 2KClO3 2KCl + 3O2 Problem: Is Cl reduced or oxidized when KClO3 decomposes ? 1 potassium + 1 chlorine + 3 oxygens = 0 charge on KClO3 1(+1) + 1(?) + 3(-2) = 0 ?= +5 Oxidation number drops (+5 to -1), so Cl is reduced.

  21. H = +1 O#’s according to rules O = -2 Problem: What are the oxidation numbers of all the elements inHCO3- ? HCO3- C = ? no simple rule 1 hydrogen + 1 carbon + 3 oxygens = -1 charge anion 1(+1) + 1(?) + 3x(-2) = -1 ? = O# of C =+4

  22. The Activity Series for Metals Not important to memorize any of this. You’ll see it again next semester.

  23. Net Ionic EquationsTo Describe Pptn and A-B Rxns

  24. Problem: Pb(NO3)2 and NaCl g ? • NaCl solution: • contains Na+(aq) + Cl-(aq) • Pb(NO3)2 solution: • contains Pb2+(aq) + NO3-(aq) • How do we know ions are separated?

  25. Problem: Pb(NO3)2 and NaCl g ? New Combinations? • Na+ with NO3- • NaNO3 is a strong electrolyte g ions stay separated • Represent as “NaNO3(aq)” or “Na+(aq) + NO3-(aq)” • Pb2+ with Cl- • PbCl2 is a weak electrolyteg ions mostly together • Represent as “PbCl2(s)”

  26. 2Na+ (aq) + 2Cl-(aq) + Pb2+(aq) + 2NO3-(aq) • --> PbCl2(s) + 2Na+ (aq) + 2NO3-(aq) • Pb2+(aq) + 2Cl-(aq) --> PbCl2(s) Problem: Pb(NO3)2 and NaCl g ? • Ionic equation shows ions in correct state • Net ionic equation excludes spectator ions

  27. 2NaCl(aq) + Pb(NO3)2(aq) PbCl2(s) + 2NaNO3(aq) • 2Na+ (aq) + 2Cl-(aq) + Pb2+(aq) + 2NO3-(aq) • PbCl2(s) + 2Na+ (aq) + 2NO3-(aq) • Pb2+(aq) + 2Cl-(aq) PbCl2(s) Summary • Whole formula equation • Ionic equation • Net ionic equation

  28. Problem: Write the net ionic equation for the reaction of sodium hydroxide and acetic acid in water. whole formula ionic eqn net ionic eqn

  29. NaOH(aq) + HC2H3O2(aq) NaC2H3O2(aq) + H2O(l) whole formula strong electrolyte weak electrolyte strong electrolyte weak/non- electrolyte ionic eqn Na++OH-+HC2H3O2 Na+ +C2H3O2-+H2O net ionic eqn OH- +HC2H3O2 C2H3O2- + H2O (l) Problem: Write the net ionic equation for the reaction of sodium hydroxide and acetic acid in water.

  30. Ca2+ + CO32- CaCO3 NH3 + H+ NH4+ Problem:Classify the following reactions. Zn + 2HCl ZnCl2 + H2 Ca + F2 CaF2 Precipitation Acid-Base Redox (Single Displacement) Redox (Combination)

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