1 / 21

Chemical Reactions

Chemical Reactions. Determining Products of Reactions AP Chemistry 2012-2013. Types of Reactions. Metathesis – no transfer of electrons Double Replacement Precipitation Reactions Solids Gases Acid-Base Reactions. Types of Reactions Continued.

gaille
Download Presentation

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. Chemical Reactions Determining Products of Reactions AP Chemistry 2012-2013

  2. Types of Reactions • Metathesis – no transfer of electrons • Double Replacement • Precipitation Reactions • Solids • Gases • Acid-Base Reactions

  3. Types of Reactions Continued • Oxidation-Reduction Reactions – transfer of electrons • Some types of redox reactions include • Single Replacement • Combustion • Synthesis • Decomposition

  4. Writing the equations • NET IONIC ONLY • Balanced for mass and charge • Examples

  5. Two Elements as Reactants • Two elements as reactants • Synthesis • Be sure to assign the most common oxidation states to the elements • Examples • Solid zinc is heated in chlorine gas. • Solid sulfur is burned in oxygen

  6. Example Reactions • Answers • Zn + Cl2 ZnCl2 • S + O2  SO2

  7. Single Reactant • Must be a Decomposition • When unsure, break the compound into its elements • Most do not completely decompose but produce • Ionic salts and • oxide gases • Example • Solid calcium carbonate is heated • A piece of solid potassium nitrate is heated

  8. Example Reactions • Answers • CaCO3 CaO + CO2 • 2 KNO3  2 KNO2 + O2

  9. Water is a Reactant • Three variations • Pure metal or metal hydride in water makes a base and hydrogen gas. • Sodium metal is added to distilled water • Lithium hydride is added to distilled water • A metal oxide in water will produce a base. • Solid barium oxide is added to water. • A nonmetal oxide in water will produce an acid. • Solid dinitrogenpentoxide is added to water. • Carbon dioxide gas is bubbled through water.

  10. Examples • Answers • Na + 2 H2O  Na+ + 2 OH- + H2 • LiH + 2 H2O  Li+ + 2 OH- + H2 • BaO + H2O  Ba2+ + 2 OH- • N2O5 + H2O  2 H+ + 2 NO3- • CO2 + H2O  H2CO3

  11. Mixture of two salt solutions • Precipitation Reactions – KNOW YOUR SOLUBILITY RULES AND COMMON IONS • Net ionic and balanced • Examples • A solution of silver nitrate is added to a solution of potassium iodide • Solutions of lead(II) nitrate and tri-potassium phosphate are mixed

  12. Examples • Ag+ + I-  AgI • 3 Pb2+ + 2 PO43-  Pb3(PO4)2

  13. Combustion of carbon compounds • Combustion is the reaction with oxygen • Produces carbon dioxide and water when enough oxygen is present • Examples • Propane is burned in air. • Carbon disulfide is burned in excess oxygen.

  14. Examples • C3H8 + 5 O2 3 CO2 + 4 H2O • CS2 + 3 O2  CO2 + 2 SO2

  15. Single replacement • Transition metal placed in a solution • Oxidation-reduction reaction • Metal will always be oxidized M+x • Neutral conditions • Ion in solution will be reduced • Examples • Solid manganese flakes are placed in a solution of copper (II) sulfate • Iron filings are placed in a solution of iron (III) sulfate.

  16. Examples • Mn + Cu2+  Mn2+ + Cu • Fe + 2 Fe3+ 3 Fe 2+ • Fe  Fe 2+ + 2e- • Fe 3+ + 1 e-  Fe 2+

  17. Single replacement (2) • Acidic conditions with an oxoacid • Anion of the oxoacid will be reduced to an oxide gas and water will form • Examples • Copper is immersed in dilute nitric acid • Lead is immersed in concentrated warm sulfuric acid

  18. Examples • Cu + H+ + NO3- Cu2+ + NO + H2O • Pb + H+ + HSO4-2  Pb2+ + SO2 + H2O

  19. Formation of complex ions • Look for transition metal ions in solution with NH3, OH-, CN-, or SCN- • Don’t worry about how many you put on the metal ion • Usually combine in 1, 2, 4, or 6 • Add the charges together to determine the charge on the whole ion • Example • Excess ammonia is added to a solution of silver nitrate • Ag+ + NH3 Ag(NH3)2+

  20. More examples of complex ions • A solution of sodium cyanide is added to a solution of iron(II) chloride • Fe 2+ + CN- Fe(CN)64- • Charges are determined by adding all the ions in the complex • 2+ + 6 x -1 = -4

  21. Videos of reactions – alkali metals and water • http://www.youtube.com/watch?v=oqMN3y8k9So • http://www.youtube.com/watch?v=Jy1DC6Euqj4 • http://www.youtube.com/watch?v=92Mfric7JUc

More Related