Q50. Which factors are responsible for making fluorine the strongest oxidising agent?
(A) Highest el

Q: What is the correct answer for CUET UG Chemistry Q50?

The correct answer is b. Fluorine's strong oxidizing power is due to a combination of factors, mainly: 1. Its high electron gain enthalpy (though its magnitude is less negative than chlorine's due to interelectronic repulsion in the small 2p orbital). 2. Its low F-F bond dissociation enthalpy (making it easier to break the bond and form atoms). 3. The high hydration enthalpy of the F⁻ ion (due to its small size and high c

Q: Q50. Which factors are responsible for making fluorine the strongest oxidising agent? (A) Highest electronegativity (B) High electron gain enthalphy (C) High bond dissociation enthalphy (D) Small…

The correct answer is b. Fluorine's strong oxidizing power is due to a combination of factors, mainly: 1. Its high electron gain enthalpy (though its magnitude is less negative than chlorine's due to interelectronic repulsion in the small 2p orbital). 2. Its low F-F bond dissociation enthalpy (making it easier to break the bond and form atoms). 3. The high hydration enthalpy of the F⁻ ion (due to its small size and high c

Q: What are the options for this CUET UG Chemistry question?

A. (A), (B) and (D) only · B. (B), (C) and (D) only · C. (A), (C) and (D) only · D. (B) and (C) only

Question

Q50. Which factors are responsible for making fluorine the strongest oxidising agent?
(A) Highest electronegativity
(B) High electron gain enthalphy
(C) High bond dissociation enthalphy
(D) Small size of flourine
Choose the correct answer from the options given below:

FirstInTest · Accepted Answer

Fluorine's strong oxidizing power is due to a combination of factors, mainly: 1. Its high electron gain enthalpy (though its magnitude is less negative than chlorine's due to interelectronic repulsion in the small 2p orbital). 2. Its low F-F bond dissociation enthalpy (making it easier to break the bond and form atoms). 3. The high hydration enthalpy of the F⁻ ion (due to its small size and high charge density). Highest electronegativity (A) also contributes. Statement (C) 'High bond dissociation enthalpy' is factually incorrect for fluorine (F₂ has a low bond dissociation enthalpy). However, the provided correct answer (b) includes (C) as a factor. Given this direct contradiction within the provided material (solution explicitly states F₂ bond dissociation energy is *much lesser* than chlorine's), a coherent explanation for the given answer is not possible.

Answer

(A), (B) and (D) only

Answer

(B), (C) and (D) only

Answer

(A), (C) and (D) only

Answer

(B) and (C) only

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