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What You Will Learn Today

What You Will Learn Today. Write balanced ionic equations. Note: Please ensure that you’ve downloaded and printed the accompanied notes before you embark on this e-learning journey. Ionic equations. A chemical equation shows the number of atoms and molecules of the reactants and products.

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What You Will Learn Today

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  1. What You Will Learn Today • Write balanced ionic equations. Note: Please ensure that you’ve downloaded and printed the accompanied notes before you embark on this e-learning journey.

  2. Ionic equations • A chemical equation shows the number of atoms and molecules of the reactants and products. • Also shows physical state of reactants and products. • However, does not show clearly the reactions of ionic compounds.

  3. Ionic equations • An ionic equation shows only the ions taking part in the reaction and leaves out the ions that do not react.

  4. Writing ionic equations • Procedure is similar as writing chemical equations. • A) Ionic compounds when dissolved in water dissociate completely into ions. • B) Spectator ions i.e ions that do not take part in the reaction are omitted on both sides of the ionic equation.

  5. Writing ionic equations Example 1 • Step 1 • Write word equation and chemical formula. • Silver nitrate + sodium chloride  silver chloride + sodium nitrate AgNO3 (aq) + NaCl (aq)  AgCl (s) + NaNO3(aq)

  6. Writing ionic equations Example 1 • Step 2 • Write formula of ions formed AgNO3 (aq) + NaCl (aq)  AgCl (s) + NaNO3(aq) Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) AgCl (s) + Na+ (aq) + NO3-(aq) Not able to dissolve in water to form ions

  7. Writing ionic equations Example 1 • Step 3 • Omit spectator ions (NO3- and Na+ appear both sides. Do not take part in the reaction. Can be cancelled) Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) AgCl (s) + Na+ (aq) + NO3-(aq) Ag+ (aq) + Cl- (aq) AgCl (s)

  8. Writing ionic equationsExample 2 • Step 1 • Write word equation and chemical formula. • Sodium hydroxide + hydrochloric acid  sodium chloride + water NaOH (aq)+ HCl (aq)  NaCl (aq)+ H2O (l)

  9. Writing ionic equationsExample 2 • Step 2 • Write formula of ions formed NaOH (aq)+ HCl (aq)  NaCl (aq)+ H2O (l) Na+ (aq) + OH- (aq) + H+ (aq) + Cl- (aq)Na+ (aq) + Cl-(aq) + H2O (l) Covalent compound. Does not form ions

  10. Writing ionic equationsExample 2 • Step 3 • Omit spectator ions (Na+ and Cl- appear both sides. Do not take part in the reaction. Can be cancelled) Na+ (aq) + OH- (aq) + H+ (aq) + Cl- (aq)Na+ (aq) + Cl-(aq) + H2O (l) H+ (aq) + OH- (aq)  H2O (l)

  11. Writing ionic equationsExample 3 • Step 1 • Write word equation and chemical formula. • Sodium carbonate + dilute hydrochloric acid  sodium chloride + water + carbon dioxide Na2CO3 (aq)+ 2HCl (aq)  2NaCl (aq)+ H2O (l) + CO2 (g)

  12. Writing ionic equationsExample 3 • Step 2 • Write formula of ions formed Na2CO3 (aq)+ 2HCl (aq) 2NaCl (aq)+ H2O (l) + CO2 (g) 2Na+ (aq) + CO3- (aq) + 2H+ (aq) + 2Cl- (aq)2Na+ (aq) + 2Cl-(aq) + H2O (l) + CO2 (g)

  13. Writing ionic equationsExample 3 • Step 3 • Omit spectator ions (Na+ and Cl- appear both sides. Do not take part in the reaction. Can be cancelled) 2Na+ (aq) + CO3- (aq) + 2H+ (aq) + 2Cl- (aq)2Na+ (aq) + 2Cl-(aq) + H2O (l) + CO2 (g) 2H+ (aq) + CO3- (aq)  CO2 (g) + H2O (l)

  14. QUESTION Write balanced chemical equations and then the ionic equations (with state symbols) for the following questions. 1 Magnesium + sulfuric acid  magnesium sulfate + hydrogen 2 Sodium hydroxide + nitric acid  Sodium nitrate + water

  15. QUESTION Write balanced chemical equations and then the ionic equations (with state symbols) for the following questions. 3 Magnesium oxide + hydrochloric acid  Magnesium chloride + water 4 Silver nitrate solution + potassium iodide solution  silver iodide (AgI is insoluble) + potassium nitrate

  16. Answers in red box (take a peek only after you’ve done the questions in your notes. Your integrity counts!)

  17. 1. Magnesium + sulfuric acid  magnesium sulfate + hydrogen Mg (s) + H2SO4 (aq)  MgSO4 (aq) + H2 (g) Mg (s) + 2H+ (aq) + SO42- (aq) Mg2+ (aq) + SO42- (aq) + H2 (g) Mg (s) + 2H+ (aq) Mg2+ (aq) + H2 (g)

  18. 2. Sodium hydroxide + nitric acid  Sodium nitrate + water NaOH (aq) + HNO3 (aq)  NaNO3 (aq) + H2O (l) Na+ (aq) + OH- (aq) + H+ (aq) + NO3- (aq) Na+ (aq) + NO3- (aq) + H2O (l) OH- (aq) + H+ (aq)  H2O (l)

  19. 3. Magnesium oxide + hydrochloric acid  Magnesium chloride + water MgO (s) + 2HCl (aq)  MgCl2 (aq) + H2O (l) MgO (s) + 2H+ (aq) + 2Cl- (aq) Mg2+ (aq) + 2Cl- (aq) + H2O (l) MgO (s) + 2H+ (aq) Mg2+ (aq) + H2O (l)

  20. 4. Silver nitrate + potassium iodide  silver iodide + potassium nitrate AgNO3 (aq) + KI (aq)  AgI (s) + KNO3 (aq) Ag+ (aq) + NO3- (aq) + K+ (aq) + I- (aq) AgI (s) + K+ (aq) + NO3- (aq) Ag+ (aq) + I- (aq) AgI (s)

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