1 / 14

Reactions

Reactions. • Electrolytes, non-electrolytes and weak electrolytes. Ionic solutions can be identified by their ability to conduct electricity. If a large number of ions are present in a solution, the solution will be an excellent conductor of electricity.

Download Presentation

Reactions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Reactions

  2. • Electrolytes, non-electrolytes and weak electrolytes • Ionic solutions can be identified by their ability to conduct electricity. • If a large number of ions are present in a solution, the solution will be an excellent conductor of electricity. • Such a substance is completely ionized and is a strong electrolyte. All soluble ionic compounds, but very few molecular compounds are strong electrolytes.

  3. • Electrolytes, non-electrolytes and weak electrolytes • If the solution conducts electricity only weakly, there is likely to be only a few ions present. Such a substance is partially ionized and is a weak electrolyte. • Non-electrolytes have no ions present in solution and therefore cannot conduct electricity. • Such a substance is NOT ionized and is a non-electrolyte. Most molecular compounds are either nonelectrolytes or weak electrolytes

  4. Net Ionic Equation • Net ionic equation: a chemical equation that shows only ions or pure substances that are changed in the reaction • Spectator ion: an ion that remains in solution and does not participate in a chemical reaction

  5. Net Ionic Equation • If you mixed aqueous solutions of calcium chloride (CaCl2 (aq)) and sodium nitrate (NaNO3 (aq)), you might be tempted to predict that the following chemical reaction would occur: CaCl2 (aq) + 2NaNO3 (aq) Ca(NO3)2 (aq) + 2NaCl (aq)

  6. Dissociation occurs:

  7. Detailed Ionic Equation • This means that what we really have in the beaker is: Ca2+ (aq) + Cl− (aq) + Na+ (aq) + NO3− (aq)  Ca2+ (aq)  +  NO3− (aq) + Na+ (aq) + Cl− (aq) • Did a reaction occur?

  8. Detailed Ionic Equation • Now consider the reaction of aqueous silver nitrate with aqueous sodium carbonate: • AgNO3 (aq) + Na2CO3 (aq)  Ag2CO3 (s) + NaNO3 (aq) • What is different about this reaction?

  9. Detailed Ionic Equation • The detailed ionic equation would look like this: • Ag+ (aq) + NO3− (aq) + Na+ (aq) + CO32− (aq)  Ag2CO3 (s) + Na+ (aq) + NO3− (aq) • If we cancel out the spectator ions… • What would be left?

  10. Net Ionic Equation • we are left with the unbalancednet ionic equation for this reaction: Ag+ (aq) + CO32− (aq)  Ag2CO3 (s) • The balancednet ionic equation would therefore be: 2 Ag+ (aq) + CO32− (aq)  Ag2CO3 (s)

  11. Strong acids and bases are written in ionic form; weak acids and bases are written in molecular form • Polyprotic Acids: The second and subsequent ionizations are always weak, whether or not the original is strong or weak. • Soluble Salts are written in ionic form • Insoluble Salts are written in the molecular form • Solids, liquids and gases are always written in molecular form.

  12. Solubility Rules

  13. Predict if a reaction takes place between the following solutions. If it does, write a net ionic equation for the reaction. • KOH(aq) + MgBr2(aq) → • BaS(aq) + NiSO4(aq) → • (NH4)2SO4(aq) + ZnCl2(aq) → • AlCl3(aq) + LiOH(aq) →

More Related