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Predicting Products of Chemical Reactions

Predicting Products of Chemical Reactions. Adapted from “The Ultimate Chemical Equation Handbook, 2 nd Edition”. Thousands of known chemical reactions occur in living systems, in industrial processes, and in chemical laboratories.

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Predicting Products of Chemical Reactions

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  1. Predicting Products of Chemical Reactions Adapted from “The Ultimate Chemical Equation Handbook, 2nd Edition”

  2. Thousands of known chemical reactions occur in living systems, in industrial processes, and in chemical laboratories. • Often it is necessary to predict the products formed in one of these reactions.

  3. Synthesis or Composition Reactions • Two or more substances combining to form a new compound. • A + X → AX • A metal combines with a nonmetal to form a binary salt. • Example: • A piece of lithium metal is dropped into a container of nitrogen gas. • 6Li + N2 → 2Li3N

  4. Metallic oxides and water form bases (metallic hydroxides). • Example: • Solid sodium oxide is added to water. • Na2O + HOH → 2NaOH • Solid magnesium oxide is added to water. • MgO + 2HOH → Mg(OH)2

  5. Nonmetallic oxides and water form acids. The nonmetal retains its oxidation number. • Example: • Carbon dioxide is bubbled into water. • CO2 + H2O → H2CO3 (oxidation number of C is +4) • Dinitrogen pentoxide is bubbled into water. • N2O5 + H2O → 2HNO3 (oxidation number of N is +5)

  6. Metallic oxides and nonmetallic oxides form salts. • Example: • Solid sodium oxide is added to carbon dioxide. • Na2O + CO2 → Na2CO3 • Sodium calcium oxide is added to sulfur trioxide. • CaO + SO3 → CaSO4

  7. Decomposition Reactions • Decomposition Reactions occur when a single reactant is broken down into two or more products. • AX → A + X • Most decomposition reactions take place only when energy in the form of electricity or heat is added.

  8. Metallic carbonates decompose into metallic oxides and carbon dioxide. • Example: • A sample of magnesium carbonate is heated. • MgCO3 → MgO + CO2 • Metallic chlorates decompose into metallic chlorides and oxygen. • Example: • A sample of magnesium chlorate is heated. • Mg(ClO3)2 → MgCl2 + 3O2

  9. Ammonium carbonate decomposes into ammonia, water, and carbon dioxide. • Example: • A sample of ammonium carbonate is heated. • (NH4)2CO3 → 2NH3 + H2O + CO2 • Sulfurous acid decomposes into sulfur dioxide and water. • Example: • A sample of sulfurous acid is heated. • H2SO3 → H2O + SO2

  10. Carbonic acid decomposes into carbon dioxide and water. • Example: • A sample of carbonic acid is heated. • H2CO3 → H2O + CO2 • A binary compound may break down to produce two elements. • Example: • Molten sodium chloride is electrolyzed. • 2NaCl → 2Na + Cl2

  11. Hydrogen peroxide decomposes into water and oxygen. • Example: • 2H2O2 → 2H2O + O2 • Ammonium hydroxide decomposes into ammonia and water. • Example: • NH4OH → NH3 + HOH

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