The oxidation power of halogens and the reducing power of halides is just reverse . Support based on the activity series.

Answer

To support the statement that the oxidation power of halogens and the reducing power of halides is just reverse based on the activity series, we can follow these steps:

### Step 1: Understanding Oxidation and Reduction
- **Oxidation** is the loss of electrons, while **reduction** is the gain of electrons. In the context of halogens and halides:
- Halogens (e.g., Cl2, Br2, I2) can act as oxidizing agents because they can gain electrons.
- Halides (e.g., Cl-, Br-, I-) can act as reducing agents because they can lose electrons.

### Step 2: Activity Series of Halogens
- The activity series for halogens is as follows:
- Fluorine (F2) > Chlorine (Cl2) > Bromine (Br2) > Iodine (I2)
- This indicates that fluorine is the strongest oxidizing agent among the halogens, while iodine is the weakest.

### Step 3: Standard Reduction Potentials (SRP)
- The standard reduction potentials (SRP) for halogens also reflect their oxidizing power:
- F2 + 2e- → 2F- (SRP is the highest)
- Cl2 + 2e- → 2Cl-
- Br2 + 2e- → 2Br-
- I2 + 2e- → 2I- (SRP is the lowest)
- Higher SRP values indicate stronger oxidizing agents.

### Step 4: Reducing Power of Halides
- Conversely, the reducing power of halides is inversely related to the activity series:
- I- > Br- > Cl- > F-
- This means that iodide (I-) is the strongest reducing agent, while fluoride (F-) is the weakest.

### Step 5: Conclusion
- From the above points, we can conclude that:
- The oxidation power of halogens increases from iodine to fluorine.
- The reducing power of halides decreases from iodide to fluoride.
- Thus, the statement that the oxidation power of halogens and the reducing power of halides is just reverse is supported by the activity series and the standard reduction potentials.