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Chemical Reactions

Chemical Reactions. Reaction Types. Chemical equation – contains all necessary info about a reaction ( like a recipe ). +. +. The Law of Conservation of Mass: In any chemical reaction matter cannot be created or destroyed. H 2 (g) + O 2 (g) H 2 O (g). O. O. O. O. H.

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Chemical Reactions

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  1. Chemical Reactions Reaction Types

  2. Chemical equation – contains all necessary info about a reaction (like a recipe). + +

  3. The Law of Conservation of Mass: In any chemical reaction matter cannot be created or destroyed. H2 (g) + O2 (g) H2O (g) O O O O H H H H H H H H 2 2 We call this equation unbalanced because the atoms are not conserved.

  4. Balancing Rules: You cannotchange the formulaof any reactant or product. You canonlychange the coefficients in front of the reactants and products. 3 H2O

  5. 2 HCl + MgBr2 MgCl2 + HBr 2 (2) = 2 (2) = 2 H: 1 H: 1 Cl: 1 Cl: 2 Mg: 1 Mg: 1 Br: 2 Br: 1 (2) = 2 (2) = 2 BALANCED

  6. 2 2 K(NO3) + MgMg(NO3)2 + K (2) = 2 (2) = 2 K: 1 K: 1 NO3: 1 NO3: 2 Mg: 1 Mg: 1 (2) = 2 BALANCED

  7. Solid potassium oxide and chlorine gas react to produce potassium chloride and oxygen gas. +1 -2 +1 -1 potassium oxide potassium chloride + + chlorine oxygen (s) 2 2 (g) K2O + ClKCl + O (g) 4 2 2

  8. In nature there are millions of possible chemical reactions. • Chemists have discovered that many reactions are similar. • Once the chemist knows the type of reaction, then the products of the reaction can be predicted. • So, the chemists have classified the reactions.

  9. Key Words • Synthesis reactions • Decomposition reactions • Single replacement reactions • Double replacement reactions • Combustion reactions

  10. Synthesis Reactions (Combination): 2 or more substances react to form a single substance. A + B  C S S O O O O +

  11. 2 Na + S Na2S H2 + O2 H2O K + Cl2 KCl Fe + O2 Fe2O3 2 2 2 2 2 4 3

  12. Decomposition Reactions: A single compound splits apart, into two or more simpler compounds. C  A + B S S O O O O +

  13. MgCl2 Mg + Cl2 CO2 CO + O2 Al2S3 Al + S 2 2 2 3

  14. Single Replacement Reactions: One element replaces another element in a compound. More active elements replace less active elements. A + BC  AC + B A + B C

  15. 2 2 Cu + AgI Ag + CuI2 I2 + CuCl Cl2 + CuI Al + ZnBr2 Zn + AlBr3 Ba + K(NO3) K + Ba(NO3)2 2 2 2 3 3 2 2 2

  16. Double Replacement Reactions: 2 compounds split and exchange positive ions AB + CD  AD + CB

  17. 2 2 BaF2 + LiBr BaBr2 + LiF HCl + AlBr3 HBr + AlCl3 BeF2 + Na2O BeO + NaF 3 3 2

  18. Combustion Reactions: Oxygen reacts with a carbon compound to produce water, carbon dioxide and heat. CxHy + O2  CO2 + H2O

  19. 8 7 3 C7H6O + O2 CO2 + H2O C3H8 + O2 CO2 + H2O CH4 + O2 CO2 + H2O 5 3 4 2 2

  20. Synthesis or combination A + B  C Decomposition C  A + B Single replacement A + BC  B + AC Double replacement AC + BD  AD + BC Combustion reactions CxHy + O2  CO2 + H2O

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