Ppt chemical reactions

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Ppt chemical reactions

  1. 1. Chemical ReactionWhat is a chemicalreaction?• Atoms rearrange to create one or morenew compounds.• In other words, old bonds break andnew bonds form.
  2. 2. Chemical ReactionOLD NEW
  3. 3. Chemical ReactionOLD NEWReactants Products
  4. 4. Chemical EquationReactants  ProductsYEILD OR =Reactants and products can berepresented by usingchemical formulas orcompound names.
  5. 5. Chemical Equation2 H2 (g) + 1 O2 (g)  2 H2O (g)Reactants ProductsYield or =
  6. 6. Chemical Reactions can1.Absorb or releaseenergy.1.Fast or Slow
  7. 7. Absorb energy or releaseenergy?
  8. 8. Exothermic- release of energy. Exo- Think exit! Thermic – heatEndothermic- absorption ofenergy Endo- Taken in Thermic – heatChemical Reactions canbe…
  9. 9. 2. Fast or slowThe speed of a chemical reaction isdifferent for all!Depends on the reactants.Chemical Reactions canbe…
  10. 10. Reaction Rate Activity- thespeed a reaction going fromreactants to products.
  11. 11. Law of Conservation ofMatterThe law of conservation of matterstates that matter (mass) can neitherbe created nor destroyed. Itcan, however, can be rearranged.In a chemical reaction, the mass of thereactants must equal the mass of theproducts.
  12. 12. Law of Conservation ofMatterThe law of conservation of matterstates that matter (mass) can neitherbe created nor destroyed. It can,however, can be rearranged.In a chemical reaction, the mass of thereactants must equal the mass of theproducts.WHAT??????
  13. 13. Think of a Balance Everything must be equal. When matter goes through a physical orchemical change, the amount (or mass) ofthe substances that you begin with mustequal the amount (or mass) of thesubstances that you end with. BEFORE MASS MUST = THE AFTER MASS!WHY you ask!!!!!!!
  14. 14. How do we balancechemical equations?!?!?!1.USE A PENCIL!!2.Identify reactants and products3. Make a Table!!!
  15. 15.  EXAMPLE:H2O2 O2 + H2OHow do we balancechemical equations?!?!?!How many of each element is in thereactants?How many of each element is in theproducts?Element w/o coeff. X coeff. Total Element w/o coeff. X coeff. Total
  16. 16.  EXAMPLE:KClO3KCl + O2How do we balancechemical equations?!?!?!How many of each element is in thereactants?How many of each element is in theproducts?Element w/o coeff. X coeff. Total Element w/o coeff. X coeff. Total
  17. 17.  EXAMPLE:CH4 + O2 CO2 + H2OHow do we balancechemical equations?!?!?!How many of each element is in thereactants?How many of each element is in theproducts?Element w/o coeff. X coeff. Total Element w/o coeff. X coeff. Total
  18. 18. Types of Reactions
  19. 19.  1. Synthesis- Two or more simple substances are combined toform one new and more complex substance.Types of ReactionsA + B  AB
  20. 20.  1. Synthesis- Two or more simple substances are combined toform one new and more complex substance.Types of ReactionsA + B  AB2Na + Cl2 2NaCl
  21. 21.  2. Decomposition Reaction- A more complex substance breaks down into its moresimple parts.Types of ReactionsAB  A + B
  22. 22.  2. Decomposition Reaction- A more complex substance breaks down into its moresimple parts.Types of ReactionsAB  A + BH2O2 O2 + H2O
  23. 23.  3. Single-Replacement- A free uncombined element replaces another combinedelement in a compound.Types of ReactionsAB + C  AC + B
  24. 24.  3. Single-Replacement- A free uncombined element replaces another combinedelement in a compound.Types of ReactionsAB + C  AC + BLiCl + Br2LiBr + Cl2
  25. 25.  4. Double Replacement Reaction- The reacting parts of two compounds switch places toform two new compounds.Types of ReactionsAB + CD  AD + BC
  26. 26.  4. Double Replacement Reaction- The reacting parts of two compounds switch places toform two new compounds.Types of ReactionsAB + CD  AD + BCCaF2 + LiSO4 CaSO4 + LiF
  27. 27.  5. Combustion Reaction- OR Burning Reaction Involves the combination of a substance with oxygen to giveoff heat and light.Types of ReactionsAB + O2 Heat+ Light
  28. 28.  5. Combustion Reaction- OR Burning Reaction Involves the combination of a substance with oxygen to giveoff heat and light.Types of ReactionsAB + O2 Heat+ LightCH4 + O2 CO2 + H2O
  29. 29. Types of ReactionsUse the code below to classify each reaction.S = Synthesis D = Decomposition SR = Single Replacement DR = Double Replacement____ P + O2 → P4O10 ____ Mg + O2 → MgO____ HgO → Hg + O2____ Al2O3 → Al + O2____ Cl2 + NaBr → NaCl + Br2 ____ H2 + N2 → NH3

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