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Reaction Types

This guide explores the various types of chemical reactions, including combustion, synthesis, decomposition, single replacement, and double replacement reactions. It emphasizes recognizing patterns of reactivity to predict outcomes in chemical interactions, such as the reactions of alkali metals with water. Each reaction type is illustrated with balanced equations and examples, including acid-base and precipitation reactions. By studying these patterns, students can develop a broader understanding rather than relying solely on memorized equations.

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Reaction Types

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  1. Reaction Types

  2. How do we know what will be produced in a chemical reaction? • Recognizing a pattern of reactivity gives a broader understanding than memorizing a large number of reactions • Would expect elements of the same family to behave similar • 2K + 2H2O → 2KOH + H2 • What will happen if Na combines with water?

  3. Five Types of Reactions • Combustion – rapid reaction that produces flame • Occurs in hydrocarbons (compounds of C, H, and sometimes O) • Reaction of hydrocarbon with oxygen to produce carbon dioxide and water • C3H8 + 5O2 → 3CO2 + 4H2O • 2CH3OH + 3O2 → 2CO2 + 4H2O

  4. Combination or Synthesis • Two reactants combine to form a single product • A + B → AB • Examples • C + O2→ CO2 • N2 + 3H2→ 2NH3 • CaO + H2O → Ca(OH)2

  5. Decomposition • Single reactant breaks apart to form two or more substances • AB → A + B • Examples • 2KClO3 → 2KCl + 3O2 • CaCO3 → CaO + CO2

  6. Single Replacement • One element replaces another similar element in a compound • A + BX → AX + B • Examples • Fe + 2HCl → FeCl2 + H2 • Zn + CuSO4 → ZnSO4 + Cu • Na + 2H2O → 2NaOH + H2

  7. Double Replacement • Atoms exchange partners • Also called metathesis reactions • AX + BY → AY + BX • We will look at two types of double replacement • Acid-base reactions • Precipitation reactions

  8. Acid-Base Reactions • Acid – substance that increases the H+ concentration in aqueous solutions • HCl → H+ + Cl- • H2SO4→ H+ + HSO4- • HSO4→ H+ + SO42-

  9. Base • Increases the OH- concentration • NaOH → Na + OH- • NH3 + H2O → NH4+ + OH-

  10. Neutralization • Acids and bases react together to produce a salt (ionic compound) and water • HCl + NaOH → NaCl + H2O • Write a balanced equation for the reaction of hydrobromic acid, HBr, with barium hydroxide, Ba(OH)2.

  11. Write the balanced equation for the reaction between phosphoric acid, H3PO4, and potassium hydroxide.

  12. Precipitation Reaction • Double replacement that forms a precipitate • KI (aq) + Pb(NO3)2 (aq) → PbI2 (s) + 2KNO3 (aq)

  13. Example • When sodium phosphate and barium nitrate are mixed, a precipitate of barium phosphate forms. Write the balanced equation.

  14. Example • When aqueous sodium hydroxide and magnesium nitrate are mixed, a magnesium hydroxide precipitate forms. Write the balanced chemical equation.

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