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CHEMICAL REACTIONS

Exploring the fundamental aspects of chemical reactions, including the types and the Law of Conservation of Matter. This guide covers synthesis reactions, decomposition reactions, single and double replacement reactions, and combustion reactions. Understand how substances combine, break down, or exchange ions through detailed chemical equations. The principles of oxidation and reduction (redox) are also discussed. Gain insights into the significance of these reactions in both laboratory chemistry and everyday phenomena.

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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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