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Redox Reactions

Redox Reactions. I. Oxidation & Reduction. -_________-_________ ________, or _____ ________, are ________ in which ________ are __________ from one ____ to _______ ____. -when _______ reacts with _______, each ______ _____ ________ ___ _______ to each _______ _____.

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Redox Reactions

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  1. Redox Reactions I. Oxidation & Reduction -_________-_________ ________, or _____ ________, are ________ in which ________ are __________ from one ____ to _______ ____ -when _______ reacts with _______, each ______ _____ ________ ___ _______ to each _______ _____

  2. Redox Reactions I. Oxidation & Reduction -_________ is defined as the ____ of ________ from the _____ of a ________ -during its reaction with _______, ______ _____ ________: -_______ is ________ -_________ is defined as the ____ of ________ by the _____ of a ________ -during its reaction with _______, ________ _____ ________: -________ is _______

  3. Redox Reactions I. Oxidation & Reduction -a substance which ________ another substance by ________ its ________ is called an ________ _____, which is also the substance that is _______ -a substance which _______ another substance by ______ ________ is called an ________ _____, which is also the substance that is ________ -________ _________ become _______ ________ and _______ _______ by the _______ _______ of ________; the more _____________ is considered to be _______ and the less _____________ is considered to be ________

  4. Redox Reactions I. Oxidation & Reduction Identify each of the following changes as oxidation or reduction: Identify what is oxidized and what is reduced in each of the following:

  5. Redox Reactions I. Oxidation & Reduction Identify the oxidizing agent and the reducing agent in each of the following reactions:

  6. Redox Reactions I. Oxidation & Reduction Determine the oxidation number of the boldface element in each of the chemical formulas below:

  7. Redox Reactions I. Oxidation & Reduction Determine the oxidation number of the boldface element in each of the polyatomic ions below:

  8. Redox Reactions II. Balancing Redox Equations Use the oxidation-number method to balance the redox equation below:

  9. Redox Reactions II. Balancing Redox Equations

  10. 5. If necessary, use the conventional method to balance the remainder of the equation. Use the oxidation-number method to balance the redox equations below:

  11. Redox Reactions II. Balancing Redox Equations Use the oxidation-number method to balance the equation: The _____ ______ gains nearly ____ of its ___ from its _____ ______ _______ (_____) during the ____ ___ _______ of ______. The ______ each _______ _______ ___ of a _______ of __________ and ___________ __________ http://alanrider.files.wordpress.com/2009/01/space_shuttle_launch.jpg

  12. Redox Reactions II. Balancing Redox Equations While in _____ the _____ _______ uses a ___________ __________ _______ to ________, which involves ___________________ as the _________ and __________ _________ as the_______ https://secure.reservexl.net/wwwimg/img/tours/38-2.jpg

  13. Redox Reactions II. Balancing Redox Equations Use the oxidation-number method to balance the equation: http://www.arcadiastreet.com/cgvistas/spacexp/images/se_spaceshuttle_orbit_insert_600.jpg

  14. Redox Reactions II. Balancing Redox Equations Use the oxidation-number method to balance the following equations:

  15. Redox Reactions II. Balancing Redox Equations 1. Hypothesis: How do you know if an oxidation-reductions reaction has occurred? 2. Prediction: 3. Gather Data: A. Safety: Copper(II) sulfate is mildly toxic, with an LD50 = 300mg/kg. Avoid ingestion (don’t eat or drink it). Wash hands thoroughly with soap and water before leaving lab. Goggles mandatory. Copper(II) sulfate is an environmental hazard, being extremely toxic to aquatic organisms like algae. B. Procedure: 1. Use a piece of sandpaper to polish the end of an iron nail.

  16. 3. Gather Data: B. Procedure: 2. Add about 3 mL of 1.0 M CuSO4 solution to a test tube. 3. Place the polished end of the nail in the CuSO4 solution. Let stand and observe for about 10 minutes. Record your observations. ___________________________________ 4. Analyze Data: 1. What is the substance found clinging to the nail? _______ 2. What happened to the color of the CuSO4 solution? _____ ______________________________________________ 3. Write the balanced chemical equation for the reaction you observed: ______________________________________ 4. What substance was oxidized? _____________________ 5. What substance was reduced? _____________________

  17. Redox Reactions III. Half-Reactions -in the _________-_________ _______ ___ + ____ ______, each ____ _____ is ________ by ______ __ ________ -the _________ ____-_______ is: -each ________ ________ is _______ by _______ __ ________ -the _________ ____-_______ is:

  18. Redox Reactions III. Half-Reactions -in the _________-_________ _______ ___ + _______ ________ + ___, each ______ _____ is ________ by ______ __ ________ -the _________ ____-_______ is: -each ______ ____ is _______ by _______ __ ________ -the _________ ____-_______ is:

  19. Redox Reactions III. Half-Reactions Write the oxidation and reduction half-reactions for the following oxidation-reduction equations: Pb (s) + Pd(NO3)2 (aq) Pb(NO3)2 (aq) + Pd (s) KMnO4(aq) + SO2 (g) K2SO4(aq) + MnSO4 (aq)

  20. Redox Reactions III. Half-Reactions Write the oxidation and reduction half-reactions for the following oxidation-reduction equations: PbO (s) + NH3 (g) N2 (g) + Pb (s) + H2O (l) Na2S2O3(aq) + I2 (s) Na2S2O4(aq) + NaI (aq)

  21. Redox Reactions III. Half-Reactions Write the oxidation and reduction half-reactions for the following oxidation-reduction equations: NaOH (aq) + NO2 (g) NaNO2 (aq) + NaNO3 (aq) + H2O (l) HCl (aq) + Sn (s) SnCl2(aq) + H2 (g)

  22. Redox Reactions III. Half-Reactions Write the oxidation and reduction half-reactions for the following oxidation-reduction equations: H3PO3(aq) + HNO3 (aq) H3PO4 (aq) + NO (g) + H2O (l) HCl (aq) + KMnO4 (aq) KCl (aq) + MnCl2 (aq) + H2O (l) + Cl2 (g)

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