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Like a recipe: Reactants Products 2H 2 (g) + O 2 (g)  2H 2 O(l)

Introduction. Like a recipe: Reactants Products 2H 2 (g) + O 2 (g)  2H 2 O(l). Introduction. Symbols  Yields or Produces (s) solid (l) liquid (aq) aqueous (g) or  gas. (l) or (aq)?. The Difference between (l) and (aq) Liquid – Pure liquid.Nothing is in it.

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Like a recipe: Reactants Products 2H 2 (g) + O 2 (g)  2H 2 O(l)

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  1. Introduction Like a recipe: ReactantsProducts 2H2(g) + O2(g)  2H2O(l)

  2. Introduction Symbols  Yields or Produces (s) solid (l) liquid (aq) aqueous (g) or  gas

  3. (l) or (aq)? The Difference between (l) and (aq) • Liquid – Pure liquid.Nothing is in it. H2O(l) • Aqueous – Dissolved in water. NaCl(aq) = Salt water

  4. (l) or (aq)? (l) or (aq)? Distilled water Tap Water Iced Tea Mouthwash Gasoline Paint

  5. Balancing Easy Examples: Hd10 + Bu8 HdBu

  6. Balancing

  7. Balancing

  8. Balancing

  9. Balancing

  10. Balancing 1. Must balance because of the Law of Cons. of Matter 2. Rules: • Can only change the coefficient, never the subscript • Coefficient multiplies every atom in a formula

  11. Balancing S + O2 SO P2(g) + H2(g)  PH3(g)

  12. Balancing Al + Cl2 AlCl3 H2O + C  H2 + CO C3H8 + O2 CO2 + H2O

  13. Balancing C2H6 + O2 CO2 + H2O C4H10 + O2 CO2 + H2O Na2SO4 + Fe(NO3)3  NaNO3 + Fe2(SO4)3

  14. Balancing Fe(OH)3 + H2SO4  Fe2(SO4)3 + H2O Sodium reacts with water to form sodium hydroxide and hydrogen gas

  15. Magnesium hydroxide reacts with hydrochloric acid (HCl) to form magnesium chloride and water.

  16. Balancing Calcium reacts with water to form hydrogen and calcium hydroxide Aluminum nitrate reacts with sodium hydroxide to form aluminum hydroxide and sodium nitrate

  17. Balancing Copper(II) chloride reacts with iron(III) sulfate to form copper(II)sulfate and iron(III) chloride Phosphoric acid (H3PO4) reacts with calcium hydroxide to form water and calcium phosphate

  18. Mg3(PO4)2 + Al2(SO4)3 MgSO4+ AlPO4 Fe2S3 + O2  Fe2O3 + SO2 Ru2O3 + CO  Ru + CO2 NaBr + Al(NO3)3  NaNO3 + AlBr3 Ba + AlCl3  BaCl2 + Al Propane (C3H8) is burned in oxygen to produce carbon dioxide and water Iron(III)nitrate reacts with lithium carbonate to form iron(III)carbonate and lithium nitrate. Sodium Chlorate decomposes to form sodium chloride and oxygen gas

  19. Mg3(PO4)2 + Al2(SO4)3 3MgSO4 + 2AlPO4 2Fe2S3 + 9O2  2Fe2O3 + 6SO2 Ru2O3 + 3CO  2Ru + 3CO2 3NaBr + Al(NO3)3  3NaNO3 + AlBr3 3Ba + 2AlCl3  3BaCl2 + 2Al C3H8 + 5O2 3CO2 + 4H2O 2Fe(NO3)3 + 3Li2CO3  Fe2(CO3)3 + 6LiNO3 2NaClO3  2NaCl + 3O2

  20. Sulfur trioxide reacts with water to form sulfuric acid (H2SO4) Boron sulfide, B2S3, reacts with water to form boric acid, H3BO3 and hydrogen sulfide, H2S. Mercury(II)nitrate decomposes to form mercury(II) oxide, nitrogen dioxide, and oxygen Hydrogen sulfide reacts with iron(III)hydroxide to form iron(III)sulfide and water.

  21. Types of Reactions Synthesis (Combination) Decomposition Combustion Single Replacement Double Replacement Dissolving

  22. Types of Reactions 1. Synthesis • Two or more elements or compounds combine to form a new compound • Examples Na(s) + Cl2(g)  NaCl(s) C(s) + O2(g)  CO2(g) CaO(s) + CO2(g)  CaCO3(s)

  23. Types of Reactions 2. Decomposition • Opposite of synthesis • One compound breaks down, usually requires heat energy

  24. Dima, a 40,000 year old frozen mammoth (Alaska)

  25. Types of Reactions • Examples: HgO(s)  Hg(l) + O2(g) CaCO3(s)  CaO(s) + CO2(g) KClO3(s)  KCl(s) + O2(g)

  26. Types of Reactions 3. Combustion • Fast reaction with O2 (Burning) • Hydrocarbons burn to form CO2 and H2O

  27. Types of Reactions • Examples: Mg(s) + O2(g)  MgO(s) C8H18 + O2 CO2 + H2O C6H12O6 + O2 CO2 + H2O

  28. Types of Reactions 4. Single replacement • One element replaces another • Not every element can replace every other element

  29. Zn + CuCl2 Cu + ZnCl2 Cr + Pb(NO3)2  Pb + Cr(NO3)3 Mg + HCl  MgCl2 + H2

  30. Types of Reactions 5. Double replacement • Two elements switch places ZnBr2 + AgNO3 Zn(NO3)2 + AgBr BaCl2 + H2SO4  BaSO4 + HCl Na2CO3 + CaCl2 CaCO3 + NaCl

  31. Types of Reactions Acid/Base Reactions • A special type of double replacement • Acids a. produce H+ b. Often start with H (HCl, H2SO4, H3PO4)

  32. Types of Reactions • Bases a. produce OH- b. Hydroxides (Drano, NaOH) NaOH + HCl  KOH + HCl 

  33. Types of Reactions 6. Dissolving A. Molecular Compounds 1) Contain all non-metals 2) Do not break up into ions in water 3) Some are still soluble: C12H22O11(s)  C12H22O11(aq)

  34. Types of Reactions

  35. Types of Reactions B. Ionic Compounds (and acids) 1) Contain a metal 2) Break up into ions in water. 3) Examples: NaCl(s)  Na+(aq) + Cl-(aq) CaCl2(s)  Ca2+(aq) + 2Cl-(aq) KNO3(s)  K+(aq) + NO3-(aq) 4) Different than decomp. because ions are produced.

  36. Types of Reactions What Ions are produced when these dissolve: AlCl3(s)  Na2CO3(s)  NH4Cl(s)  FeBr2(s)  (NH4)2Cr2O7(s) 

  37. Types of Reactions BaCO3(s)  BaO(s) + CO2(g) Ca(NO3)2(s)Ca2+(aq) + 2NO3-(aq) KOH + HBr  KBr + H2O N2 + H2 NH3 BaCl2 + MgSO4  BaSO4 + MgCl2 Cr + Pb(NO3)2  Pb + Cr(NO3)3 C5H12 + O2 CO2 + H2O

  38. Predicting Reactions Steps: • Identify the type of reaction • Break all elements into ions (generally keep polyatomic together) • Write the products • Balance the equation

  39. Predicting Reactions K + O2 Mg + O2 Al + Cl2 Na + N2 K + F2

  40. Predicting Reactions CuCl2(s) (placed in water) KNO3(s) (placed in water) Mg(NO3)2(s) (placed in water) Na3PO4(s) (placed in water)

  41. Predicting Reactions CuSO4 + NaOH  BaCl2 + AgNO3 HNO3 + LiOH  H2SO4 + KOH  AgNO3 + HCl 

  42. Predicting Reactions CH4 + O2 C2H6 + O2 C3H8 + O2 C6H6 + O2

  43. Types of Reactions K + Fe(OH)2  Al2O3 + Mg  Fe + CuCl2  HCl + Al  Na + Ca(NO3)2

  44. Types of Reactions HCl + Ba(OH)2  HClO4 + LiOH  Pb(NO3)2 + KI  H3PO4 + NaOH  H3PO4 + Ca(OH)2 

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