Stability of +2 oxidation state in Group 14 increases down the group due to?

1. Which element is the most powerful oxidizing agent? +

Correct Answer

Fluorine (F)

Why is Fluorine the Most Powerful Oxidizing Agent?

An oxidizing agent is a species that accepts electrons and gets reduced.

Oxidizing agent + e⁻ → Reduced species

Fluorine is the most powerful oxidizing element because it has the highest electronegativity and a very strong tendency to accept an electron.

F + e⁻ → F⁻

Fluorine also has a very high positive standard reduction potential:

F₂ + 2e⁻ → 2F⁻
E° ≈ +2.87 V

A higher positive reduction potential means a greater tendency to gain electrons and therefore a stronger oxidizing character.

Periodic Trend

Among the elements, oxidizing character generally increases:

Across a period → increases

Down a group ↓ decreases

Thus, fluorine, located at the top of Group 17, has the highest oxidizing power.

F > Cl > Br > I

for oxidizing strength of the halogen molecules.

Important JEE / NEET Point

Do not confuse oxidizing power with electron gain enthalpy. Although chlorine has a more negative electron gain enthalpy than fluorine, fluorine is still the strongest oxidizing agent. This is because oxidizing strength depends on the overall energetics of the redox process, including bond dissociation, electron gain and hydration effects.

Strongest elemental oxidizing agent = F₂

30 Related MCQs with Solutions

1. Which element is the most powerful oxidizing agent?

A. Cl

B. F

C. O

D. Br

Answer: B. Fluorine (F)

2. The strongest oxidizing agent among halogens is:

A. F₂

B. Cl₂

C. Br₂

D. I₂

Answer: A. F₂

3. Fluorine is a powerful oxidizing agent mainly because of its:

A. Low electronegativity

B. High electronegativity

C. Large atomic size

D. Low electron affinity

Answer: B. High electronegativity

4. An oxidizing agent undergoes:

A. Oxidation

B. Reduction

C. Sublimation

D. Neutralisation

Answer: B. Reduction

5. Which reaction represents the oxidizing action of fluorine?

A. F₂ → 2F⁺

B. F₂ + 2e⁻ → 2F⁻

C. F⁻ → F₂

D. F + e⁻ → F²⁻

Answer: B

6. The standard reduction potential of F₂/F⁻ is approximately:

A. −2.87 V

B. +2.87 V

C. +1.36 V

D. −1.36 V

Answer: B. +2.87 V

7. A more positive standard reduction potential generally indicates:

A. Stronger reducing ability

B. Stronger oxidizing ability

C. Lower electron affinity

D. Greater metallic character

Answer: B

8. The correct order of oxidizing strength of halogens is:

A. I₂ > Br₂ > Cl₂ > F₂

B. F₂ > Cl₂ > Br₂ > I₂

C. Cl₂ > F₂ > I₂ > Br₂

D. Br₂ > I₂ > F₂ > Cl₂

Answer: B

9. Which halogen has the highest electronegativity?

A. F

B. Cl

C. Br

D. I

Answer: A. F

10. The strongest elemental oxidant is:

A. O₂

B. F₂

C. Cl₂

D. N₂

Answer: B. F₂

11. Oxidizing character generally increases across a period because:

A. Atomic size increases

B. Effective nuclear charge generally increases

C. Metallic character increases

D. Ionization enthalpy decreases

Answer: B

12. Down Group 17, oxidizing power generally:

A. Increases

B. Decreases

C. Remains constant

D. First decreases then increases

Answer: B. Decreases

13. Which species accepts electrons in a redox reaction?

A. Reducing agent

B. Oxidizing agent

C. Catalyst only

D. Solvent

Answer: B. Oxidizing agent

14. Fluorine changes to fluoride ion by:

A. Losing one electron

B. Gaining one electron

C. Losing two electrons

D. Gaining two electrons

Answer: B. Gaining one electron

15. Which has the greatest tendency to get reduced?

A. F₂

B. I₂

C. Br₂

D. Cl₂

Answer: A. F₂

16. Which statement about F₂ is correct?

A. It is a strong reducing agent

B. It is a very strong oxidizing agent

C. It readily loses electrons

D. It has low electronegativity

Answer: B

17. The strongest oxidizing halogen has the:

A. Lowest reduction potential

B. Highest reduction potential

C. Lowest electronegativity

D. Largest atomic radius

Answer: B

18. Which is the weakest oxidizing agent among halogens?

A. F₂

B. Cl₂

C. Br₂

D. I₂

Answer: D. I₂

19. Fluorine has the highest:

A. Metallic character

B. Electronegativity

C. Atomic radius

D. Reducing power

Answer: B. Electronegativity

20. Which species is reduced when it acts as an oxidizing agent?

A. F₂

B. Na

C. K

D. Mg

Answer: A. F₂

21. The oxidizing strength of halogens follows:

A. F₂ > Cl₂ > Br₂ > I₂

B. I₂ > Br₂ > Cl₂ > F₂

C. Cl₂ > Br₂ > I₂ > F₂

D. Br₂ > F₂ > I₂ > Cl₂

Answer: A

22. Which element has the greatest tendency to attract bonding electrons?

A. F

B. O

C. Cl

D. N

Answer: A. F

23. A high positive E° value means the species has a strong tendency to:

A. Lose electrons

B. Gain electrons

C. Lose protons

D. Gain neutrons

Answer: B. Gain electrons

24. Which is more powerful as an oxidizing agent?

A. F₂

B. I₂

C. Both equal

D. I⁻

Answer: A. F₂

25. Oxidizing agents are electron:

A. Donors

B. Acceptors

C. Neutralisers

D. Catalysts

Answer: B. Acceptors

26. Which factor is especially important for the high oxidizing power of fluorine?

A. High electronegativity

B. Large atomic radius

C. Low effective nuclear charge

D. High metallic character

Answer: A

27. Which halogen can oxidize the largest number of other halide ions?

A. F₂

B. Cl₂

C. Br₂

D. I₂

Answer: A. F₂

28. Which equation shows reduction of fluorine?

A. F₂ → 2F⁺

B. F₂ + 2e⁻ → 2F⁻

C. F⁻ → F₂

D. F⁻ → F⁺ + 2e⁻

Answer: B

29. The most powerful oxidizing agent among the following is:

A. Li

B. Na

C. F₂

D. K

Answer: C. F₂

30. The key reason fluorine is the strongest elemental oxidizing agent is its:

A. Low electron-attracting ability

B. Very high tendency to accept electrons

C. Large atomic size

D. High metallic character

Answer: B

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