Consider the following (unbalanced) net ionic equation: IO3-(aq) + I-(aq) → I2(s) 1. Identify the oxidation numbers for each of the species shown here by placing them in the appropriate bin. Each number may be used once, more than once, or not at all. I in IO3-, I in I2, O in IO3-, I in I- oxidation number -2,-1,0,+5,+6 2. Identify the oxidizing agent (OA) and reducing agent (RA) by dragging the appropriate label onto the net ionic equation. IO3-(aq) + I-(aq) → I2(s) 3. Write the balanced equation for the reaction that takes place in acidic aqueous solution.
Consider the following (unbalanced) net ionic equation: IO3-(aq) + I-(aq) → I2(s) 1. Identify the oxidation numbers for each of the species shown here by placing them in the appropriate bin. Each number may be used once, more than once, or not at all. I in IO3-, I in I2, O in IO3-, I in I- oxidation number -2,-1,0,+5,+6 2. Identify the oxidizing agent (OA) and reducing agent (RA) by dragging the appropriate label onto the net ionic equation. IO3-(aq) + I-(aq) → I2(s) 3. Write the balanced equation for the reaction that takes place in acidic aqueous solution.
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter8: Reactions In Aqueous Solutions
Section: Chapter Questions
Problem 15A
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Consider the following (unbalanced) net ionic equation:
IO3-(aq) + I-(aq) → I2(s)
1. Identify the oxidation numbers for each of the species shown here by placing them in the appropriate bin. Each number may be used once, more than once, or not at all.
I in IO3-, I in I2, O in IO3-, I in I-
oxidation number -2,-1,0,+5,+6
2. Identify the oxidizing agent (OA) and reducing agent (RA) by dragging the appropriate label onto the net ionic equation. IO3-(aq) + I-(aq) → I2(s)
3. Write the balanced equation for the reaction that takes place in acidic aqueous solution.
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