The potential set up when an electrode is in contact with 1M solution of its ions at 298 K is known as standard electrode potential (or standard reduction potential denoted by E°). All of the following statements about standard electrode potential are correct EXCEPT:
Correct answer: D. E°red of Cl2 is maximum (+2.87V)
- A. The smaller the E°red, the greater the reducing power of a metal
- B. E°red of Li+ is minimum (-3.04V)
- C. The greater the E°red, the greater the oxidizing power of a non-metal
- D. E°red of Cl2 is maximum (+2.87V)
Explanation
The correct answer is Option D. The statement that E°red of Cl2 is maximum (+2.87V) is incorrect because the maximum standard reduction potential is for fluorine, not chlorine. Chlorine does have a high E°red, indicating its strong oxidizing power, but it does not exceed that of fluorine.Option A is correct because a smaller E°red does indicate greater reducing power. Option B accurately states the low E°red of lithium, reflecting its strong reducing nature. Option C correctly describes the relationship between high E°red values and oxidizing power in non-metals.
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Electrochemistry describes electron transfer through oxidation and reduction, identifies oxidizing and reducing agents, and applies oxidation numbers to balance redox equations. It also covers electrode potential and the standard hydrogen electrode, which provides the reference for comparing the reduction tendencies of other electrodes.
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