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Lesson 7

Lesson 7. Ionic Equations. Learning Objectives: Recall the correct formulae for elements and ions Describe chemical reactions using balanced formulae equations Write ionic equations for the reactions of acids and the tests for other ions. Quick Quiz.

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Lesson 7

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  1. Lesson 7 Ionic Equations • Learning Objectives: • Recall the correct formulae for elements and ions • Describe chemical reactions using balanced formulae equations • Write ionic equations for the reactions of acids and the tests for other ions

  2. Quick Quiz • Pens out and flip to the back of your book! • Label 1-10

  3. OH- hydroxide ions

  4. CO32- carbonate ion

  5. NO3- nitrate ion

  6. Na+ sodium ion

  7. NH4+ ammonium ion

  8. SO42- sulphate ion

  9. Ca2+ calcium ion

  10. Al3+ aluminium ion

  11. SO32- sulphite ion

  12. Cl- chloride ions

  13. charge SO32- Number of atoms present of that element: if nothing there, theres only 1!

  14. How do ions form a compound? A cation and a anion come together to form a neutral compound. eg Na+ and Cl- NaCl Na+ and O2- Na2O

  15. Task Worksheet: ionic formula

  16. How to write an ionic equation • Give the relevant charge to the ions Na+Cl- • Work out how many of each there must be for the compound to be neutral eg Na+ and O2- Na+ + Cl- NaCl • Both sides of the equation must equal zero. If not, then you have to balance the equation, by putting numbers in front of the substances. • State symbols

  17. State Symbols These must go after every substance when writing an ionic equation: (g) Substance is a gas in the reaction • Substance is a pure liquid in the reaction (no water present) (s) Substance is a solid in the reaction (aq) Substance is in a solution which also contains water - aqueous

  18. Consider the following reaction….. AgNO3(aq) + NaCl(aq)  AgCl(s) + NaNO3(aq) Silver nitrate + sodiumchloride silver chloride + sodiumnitrate PRECIPITATE

  19. Ionic Equation Ag+NO3-(aq) + Na+Cl-(aq)  Ag+Cl-(s) + Na+NO3-(aq) Silver nitrate + sodiumchloride silver chloride + sodiumnitrate • The ions that do not take part in the reaction are called the SPECTATOR IONS. If we omit them, then the half equation for this reaction is: • Ag+(aq) + Cl−(aq) → AgCl(s) • Notice that the charges on both sides of the equation are BALANCED!

  20. Task • Worksheet: Ionic equations and spectator ions • Write ionic half equations for the reactions with NaOH

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