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CHEMICAL REACTIONS

CHEMICAL REACTIONS. Chemistry: the study of matter & the changes it undergoes. Types of Chemical Reactions. The Law of Conservation of Matter: Matter can neither be created nor destroyed in any chemical or physical process. Synthesis Reactions.

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CHEMICAL REACTIONS

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  1. CHEMICAL REACTIONS Chemistry: the study of matter & the changes it undergoes

  2. Types of Chemical Reactions The Law of Conservation of Matter: Matter can neither be created nor destroyed in any chemical or physical process.

  3. Synthesis Reactions • a.k.a.: Direct Combination Reactions • Two substances combine to form one new, more complex substance

  4. Synthesis Reactions • Form: R + S  RS • C(s) + O2(g) CO2(g)

  5. Combustion Reactions • The reactants are O2(g) and an organic molecule of carbon, hydrogen and perhaps oxygen • CO2(g) and H2O (g) are produced in complete combustion reactions

  6. Combustion Reactions • Form: CxHyOz+ O2(g) CO2(g) + H2O(g) • CH4(g) + 2 O2(g)CO2(g) + 2 H2O(g)

  7. Decomposition Reactions • a.k.a. Analysis Reactions • one complex substance breaks down into two or more “simpler” substances • Used to determine % composition of substances in laboratories.

  8. Decomposition Reactions • Form: RS  R + S • CaCO3(s) CaO (s) + CO2(g)

  9. Single Replacement Reactions • An element becomes an ion in solution and an ion that was in solution becomes a neutral element. • metals replace cations and non-metals replace anions. • Reactions based upon Activity Series ranking of elements.

  10. Single Replacement Reactions • Form: T + RS  TS + R • Mg(s)+ 2 AgNO3(aq) Mg(NO3)2(aq) + 2 Ag(s) • Cl2(g)+ 2 NaBr(aq) 2 NaCl(aq) + Br2(l)

  11. Oxidation and Reduction LEO goes GER Li (s) + AuCl (aq)  LiCl (aq) + Au (s) Li (s)  Li+1 (aq) + 1 e- Loss of Electrons = Oxidation Au+1 (aq) + 1 e-  Au (s) Gain of Electrons = Reduction

  12. Double Replacement Reactions • The cations of two aqueous ionic solutions switch with each other to make two new neutral ionic compounds. • One product must be one of the following: • water (from an acid / base reaction) • insoluble in water (see solubility chart) • Gas (bubbles)

  13. Double Replacement Reactions • Form: RS + TU RU + TS • HCl(aq) + NaOH(aq)  HOH (l) + NaCl(aq) (H2O) • NaI(aq) + AgNO3(aq)NaNO3(aq)+ AgI(s)

  14. Synthesis Decomposition Single Replacement Double Replacement Combustion 5 types of reactions

  15. Identify these types 9 O2 (g) + C6H12 (l)  6 CO2 (g) + 6 H2O (g) 2 H2O (g)  2 H2 (g)+O2 (g) 2 Na (s) + 2 HCl (aq)  H2 (g) + 2 NaCl (aq) combustion Decomposition Single Replacement

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