**3.** **(a)** Rank the relative oxidizing strength of the halogens (Cl, Br and I), and explain your ranking.**(b)** Rank the relative reducing strength of the halide ions (Cl⁻, Br⁻, and I⁻), and explain your ranking.**(c)** Rank the oxidizing strength of Fe³⁺ and MnO₄⁻, and explain your ranking. ### Table 1: Oxidizing Power of Halogens**Fe Reference:** Clear on top and bottom **MnO4 Reference:** Clear on top, purple on bottom| | Cl⁻ | Br⁻ | I⁻ ||--------|--------------------|-------------------------|---------------------------|| Cl₂ | x | a) Gold on top, pale yellow on bottom | b) Pink-purple on top, orange on bottom || Br₂ | c) No reaction | x | d) Dark pink on top, orange on bottom || I₂ | e) No reaction | f) No reaction | x |### Table 2: Oxidizing Power of Fe³⁺ and MnO₄⁻| | Br⁻ | I⁻ ||--------|------------------------------|---------------------------------------|| Fe³⁺ | g) Bottom layer to light yellow, no change on top, therefore no reaction | h) Purple on top, red-orange on bottom || MnO₄⁻ | i) Orange on top, yellow on bottom | j) Purple on top, red band in middle, orange on bottom | ---**Explanation:**- **Table 1** demonstrates the reactivity trends among halogens: chlorine (Cl₂), bromine (Br₂), and iodine (I₂) in the presence of halide ions (Cl⁻, Br⁻, and I⁻). It shows the color changes indicating the oxidizing power when different halogens react, or do not react, with the various halide ions.- **Table 2** reflects the oxidizing power of iron ions (Fe³⁺) and permanganate ions (MnO₄⁻) when they interact with bromide (Br⁻) and iodide (I⁻) ions. This table describes the color changes or lack thereof, to indicate reactions or lack of reactions, helping in understanding oxidation-reduction relationships.Understanding these tables helps in illustrating the relative strength of oxidizing agents, as well as the application of color changes to determine reaction outcomes in chemical experiments.

A question based on general chemistry, which is to be accomplished.

3. (a) Rank the relative oxidizing strength of the halogens (Cl, Br and I), and explain your ranking. (b) Rank the relative reducing strength of the halide ions (Cl-, Br , and I), and explain your ranking. (c) Rank the oxidizing strength of Fe* and MnO4 , and explain your ranking.

3. (a) Rank the relative oxidizing strength of the halogens (Cl, Br and I), and explain your ranking. (b) Rank the relative reducing strength of the halide ions (Cl-, Br , and I), and explain your ranking. (c) Rank the oxidizing strength of Fe* and MnO4 , and explain your ranking.

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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Question

**3.**

**(a)** Rank the relative oxidizing strength of the halogens (Cl, Br and I), and explain your ranking.

**(b)** Rank the relative reducing strength of the halide ions (Cl⁻, Br⁻, and I⁻), and explain your ranking.

**(c)** Rank the oxidizing strength of Fe³⁺ and MnO₄⁻, and explain your ranking.

### Table 1: Oxidizing Power of Halogens

**Fe Reference:** Clear on top and bottom
**MnO4 Reference:** Clear on top, purple on bottom

| | Cl⁻ | Br⁻ | I⁻ |
|--------|--------------------|-------------------------|---------------------------|
| Cl₂ | x | a) Gold on top, pale yellow on bottom | b) Pink-purple on top, orange on bottom |
| Br₂ | c) No reaction | x | d) Dark pink on top, orange on bottom |
| I₂ | e) No reaction | f) No reaction | x |

### Table 2: Oxidizing Power of Fe³⁺ and MnO₄⁻

| | Br⁻ | I⁻ |
|--------|------------------------------|---------------------------------------|
| Fe³⁺ | g) Bottom layer to light yellow, no change on top, therefore no reaction | h) Purple on top, red-orange on bottom |
| MnO₄⁻ | i) Orange on top, yellow on bottom | j) Purple on top, red band in middle, orange on bottom |

---

**Explanation:**

- **Table 1** demonstrates the reactivity trends among halogens: chlorine (Cl₂), bromine (Br₂), and iodine (I₂) in the presence of halide ions (Cl⁻, Br⁻, and I⁻). It shows the color changes indicating the oxidizing power when different halogens react, or do not react, with the various halide ions.

- **Table 2** reflects the oxidizing power of iron ions (Fe³⁺) and permanganate ions (MnO₄⁻) when they interact with bromide (Br⁻) and iodide (I⁻) ions. This table describes the color changes or lack thereof, to indicate reactions or lack of reactions, helping in understanding oxidation-reduction relationships.

Understanding these tables helps in illustrating the relative strength of oxidizing agents, as well as the application of color changes to determine reaction outcomes in chemical experiments.

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