Standard Oxidation Petantials When we see the reaction: L'(aq) e-Lifs) with a reduction potential of -3.05 V, we can conclude that the lithium ion has little to no tendency to be reduced and return to a metallic atom. Reduction Li' (aq) + e Li 12. Write the half reaction for the oxidation of Lifs). Oxidation: End = -3.05 V 13. Which version of lithium has an octet? 14. Which of the two Sithium half-reactions represents lithium's natural tendency more accurately? Explain your reasoning. 15. Compare and contrast the two lithium half-reactions Compare Contrast/nalso serves as an E chart. The reverse reactions are oxidation reactions. The fact that the lithium ion es not want to be reduced suggests that the lithium atom really wants to be oxidized. Changing the sign on Egives E value. The larger the E' value the greater the tendency to be oxidized. 16. What would the E'ox be for the oxidation half-reaction for U/s/? 17. Looking at the E'red chart, circle the species that is more likely to be oxidized. Explain your reasoning ('s) a) Al(s) or Mg/s) 18. Define reducing agent. b) Sn(aq) and Cr(og) 19. Circle the species that is a better reducing agent? Explain your reasoning. ('s) a) Snag) and Cr(aq) b) Fe(s) and Ni(s) 20. On the SRP chart, which side of the equation do we find our reducing agents? Explain your reasoning. On your standard reduction potential table, highlight top ten reducing agents (not the whole equation). Teacher check

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