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.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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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