1 / 30

Types of Chemical Reactions

Types of Chemical Reactions. Synthesis, Combustion, Decomposition and Replacement. You can think of atoms as people getting together as couples. The Get Together…. Synthesis. Decomposition. Decomposition. Single Replacement Reactions. Single Replacement Reactions.

seth-johnston
Download Presentation

Types of Chemical 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. Types of Chemical Reactions Synthesis, Combustion, Decomposition and Replacement

  2. You can think of atoms as people getting together as couples...

  3. The Get Together…

  4. Synthesis

  5. Decomposition

  6. Decomposition

  7. Single Replacement Reactions

  8. Single Replacement Reactions

  9. Double Replacement Reaction

  10. Double Replacement Reaction

  11. Combustion

  12. Combustion

  13. How does this analogy break down?

  14. Let’s look at the reactions in more detail Synthesis Decomposition Single-Replacement Double-Replacement Combustion

  15. Combustion What are some types of combustion you are familiar with? Every cell in your body is carrying out combustion

  16. Combustion • Oxygen combines with a metal, non-metal, or compound • Creates a metal oxide, non-metal oxide, or 2 or more oxides • Releases energy – heat, light • Can be a slower process too…

  17. Synthesis • 2 or more reactants combine to make a product

  18. Decomposition • A compound breaks down into two or more substances

  19. Single Replacement • A metal replaces a hydrogen • A metal replaces another metal • We use an activity series to predict which metals are “stronger” and can knock out other metals from compounds

  20. Activity Series The most active metals are at the top. These will replace metals below them. The halogens are also listed in order of most active at the top to least active at the bottom. More active elements replace less active elements in single replacement reactions

  21. Single Replacement Examples • 2 AgNO3 + Cu  Cu(NO3)2 + 2 Ag • Fe + Cu(NO3)2   Fe(NO3)2 + Cu • Zn + 2HCL  ZnCl2 + H2

  22. Double Replacement Reactions • Produces a precipitate, liquid or gas • All four of the ions switch partners • Aqueous solution

  23. Double Replacement Examples • AgNO3(aq) + KCl(aq)  AgCl(s) + KNO3(aq) • CaCO3(aq) + 2 HCl(aq)  CaCl2(aq) + H2O(l) + CO2(g) • HCl(aq) + NaOH(aq)  HOH(l) + NaCl(aq)

  24. How to identify a reaction Be systematic – it will help you identify the reaction type and the products!

  25. How to identify a reaction Example: Solid calcium oxide and carbon dioxide gas react to produce solid calcium carbonate

  26. Summary The main types of reactions Replacement Reactions: 2 types Single replacement – a stronger cation steps in and replaces a weaker anion Double replacement – 2 cations switch places, forming a precipitate, a liquid, or a gas • Combustion – reaction with oxygen • Synthesis – two compounds or elements getting together • Decomposition – One compound splitting up • Replacement – Another ion moves in

  27. You try it! • Work on these examples together in pairs. • Write the reaction • Balance the equation • Classify the reaction • Be prepared to present your results on the board! • Magnesium and Hydrochloric acid form Magnesium Chloride and Hydrogen • Carbon Dioxide and Water form Carbonic Acid (H2CO3) • Silver Nitrate and Sodium Chloride form Silver Chloride and Sodium Nitrate • Heating sodium bicarbonate (NaHCO3) releases water and carbon dioxide and sodium carbonate

  28. You try it! • Magnesium and Hydrochloric acid form Magnesium Chloride and Hydrogen: • Mg + HCl  MgCl + H2 (skeleton equation) • 2Mg + 2HCl  2MgCl + H2 (balanced equation) • Single replacement (reaction type) • Carbon Dioxide and Water form Carbonic Acid (H2CO3): • CO2 + H2O  H2CO3 (skeleton equation) • CO2 + H2O  H2CO3 (it’s already balanced!) • Synthesis (reaction type)

  29. You try it! • Silver Nitrate and Sodium Chloride form Silver Chloride and Sodium Nitrate • AgNO3 + NaCl  AgCl + NaNO3 (skeleton equation) • AgNO3 + NaCl  AgCl + NaNO3 (already balanced) • Double replacement (reaction type) • Heating sodium bicarbonate releases water and carbon dioxide and sodium carbonate • NaHCO3 Na2CO3 + H2O + CO2 (skeleton equation) • 2NaHCO3 Na2CO3 + H2O + CO2 (balanced equation) • Decomposition (reaction type)

More Related