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Intro to reactions

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Transcript

  • 1. Chemical ReactionsI. Intro to Reactions I II III IV V
  • 2. A.Signs of a ChemicalReactions Evolution of heat and lights Formation of a gass Formation of a precipitates Color change
  • 3. B.Law of Conservation ofMasss mass is neither created nor destroyed in a chemical reactions total mass stays the sames atoms can only rearrange4H 4H 36 g2O 2O 4g 32 g
  • 4. C. Chemical EquationsA+B → C+DREACTANTS PRODUCTS
  • 5. C. Chemical Equations
  • 6. D. Writing Equations 2H2(g) + O2(g) → 2H2O(g)s Identify the substances involved.s Use symbols to show: • How many? - coefficient • Of what? - chemical formula • In what state? - physical states Remember the diatomic elements.
  • 7. D. Writing Equations Two atoms of aluminum react with three units of aqueous copper(II) chloride to produce three atoms of copper and two units of aqueous aluminum chloride. • How many? • Of what? • In what state?2Al(s) + 3CuCl2 (aq) → 3Cu(s) + 2AlCl3 (aq)
  • 8. E. Describing Equationss Describing Coefficients: • individual atom = “atom” • covalent substance = “molecule” • ionic substance = “unit”3CO2 ⇒ 3 molecules of carbon dioxide2Mg ⇒ 2 atoms of magnesium4MgO ⇒ 4 units of magnesium oxide
  • 9. E. Describing Equations Zn(s) + 2HCl(aq) → ZnCl2(aq) + • How many? H2(g) • Of what? • In what state? One atom of solid zinc reacts with two molecules of aqueous hydrochloric acid to produce one unit of aqueous zinc chloride and one molecule of hydrogen gas.