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Electrochemistry Unit 12 Pages 1-3 Learning Target: I can determine the oxidation state for any atom in an element, ion, or compound. I can explain what happens in an oxidation-reduction, or redox, reaction. Criteria for Success: I can determine the oxidation state for an atom in an element. I can determine the oxidation state for an atom in an ion. I can determine the oxidation state for an atom in a compound. I can identify the species being oxidized in a redox reaction. I can identify the species being reduced in a redox reaction. Introduction to Oxidation-Reduction Reactions A. Any chemical process in which electrons are transferred from one atom to another is an _________-__________ reaction. 1. The name for this type of reaction is often shortened to what is called a ________ reaction. 2. A species _____ _________ when _______ (LEO). A species _____ ________ when _______ (GER). 3. ___________________________ (OIL). ____________________________(RIG). Oxidation Numbers/States A. Chemists assign a number to each element in a reaction called an _________________ state that allows him/her to determine the electron flow in the reaction. 1. Even though they look like them, oxidation states are not _________ charges! 2. Oxidation numbers can be assigned to each atom in an element, ion, or compound…whether the compound is ____________ or ___________________! 3. Oxidation states are imaginary charges assigned based on a set of rules simply used to determine _________________ flow. Rules for Assigning Oxidation Numbers (In order of priority): 1. The oxidation number of any pure element is _________. 2. The oxidation number of a monatomic ion is __________ to its charge. 3. The ______ of the oxidation numbers in a compound is zero if ____________, or equal to the ___________ if a polyatomic ion. 4. The oxidation number of alkali metals in compounds is _____, and that of alkaline earths in compounds is ______. The oxidation number of F is ______ in all its compounds. 5. The oxidation number of H is _____ in most compounds. Exceptions are H2 (where H = 0) and the ionic hydrides, such as NaH (where H = -1). 6. The oxidation number of oxygen (O) is ______ in most compounds. Exceptions are O2 (where O = 0) and peroxides, such as H2O2 or Na2O2, where O = -1. 7. For other elements, you can usually use rule (3) to solve for the unknown oxidation number. Examples: N2(g) elemental state, so N = 0. N3-(g) monatomic ion, so N = -3. NO(g) has O = -2, so N = +2. NO2(g) has O = -2, so N = +4. SO42- has O = -2. Thus x + 4(-2) = -2. Solving the equation gives x = -2 + 8 = +6. K2Cr2O7 has K = +1 and O = -2. Thus 2(+1) + 2 x + 7(-2) = 0; 2 x = 12; Cr = +6. B. In general, redox reactions will be any type of reaction except ___________________________________. 1. However, there are exceptions so you should always check if electrons have been_____________. Identifying Oxidation-Reduction Reactions A. In order to identify a REDOX reaction, write the _________ number for each ________ in the reaction as outlined in the rules above. 1. A substance that has the element that has been ________ (LOST electrons) will have an oxidation number that becomes more ________. 2. A substance that has the element that has been ________ (GAINED electrons) will have an oxidation number that becomes more ________. B. ___________ are produced in oxidation and acquired in reduction. Therefore, for reduction to occur, oxidation must occur _____________. Each process is referred to as a ___________. Oxidation Half-Reaction Zn(s) → Zn2+(aq) + 2e- Reduction Half-Reaction Fe2+(aq)+ 2e- → Fe(s) Guided/ Independent Practice Directions: In the following questions, give the oxidation number of the indicated atoms/ion. 1. N in N2O3 12. Fe in Fe(ClO2)3 2. S in H2SO4 13. N in NO3- 3. C 14. Cu2+ 4. C in CO 15. Zn2+ 16. C in CH4 5. Na in NaCl 17. Mn in MnO2 6. H in H2O 18. S in SO32- 7. Ba in BaCl2 19. Mg2+ 8. N in NO2- 20. Cl- 9. S in Al2S3 21. O2 10. S in HSO4- 22. P4 11. Cl in Fe(ClO2)3 23. Na in Na2S 24. S in H2S 28. Mn in KMnO4 25. Ca2+ 29. I in Mg(IO3)2 26. C in CN30. C in C2O42- 27. H in OH Directions: In each of the following equations, label the oxidation state of each atom before and after the process occurs. Indicate the element that has been oxidized and the one that has been reduced. Write the oxidation and reduction half reactions. 1. 2 Na + FeCl2 → 2 NaCl + Fe 2. 2 C2H2 + 5 O2 → 4 CO2 + 2 H2O 3. 2 PbS + 3 O2 → 2 SO2 + 2 PbO 4. 2 H2 + O2 → 2 H2O 5. Cu + HNO3 → CuNO3 + H2 6. AgNO3 + Cu → CuNO3 + Ag