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Strength of following bases decrease in the order? 


(I) Br-    (II) F-      (III) NH2    (IV) CH3-

  • a)
    IV > III > I>II

  • b)
    III > IV > I > II  

  • c)
    II > I > III > IV 

  • d)
    IV > I > II > III

Correct answer is option 'A'. Can you explain this answer?
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Most Upvoted Answer
Strength of following bases decrease in the order?(I) Br- (II) F- (...


  1. Br⁻ (bromide ion): This is a halide ion. Halide ions become stronger bases as the size of the ion increases (i.e., as we move down the periodic table). Bromide is quite large, but it is not as large as iodide, making it a relatively weaker base compared to other larger halides.



  2. F⁻ (fluoride ion): Fluoride is a small ion with high electronegativity, which means it holds onto its electron pair tightly and is less inclined to share it to form a bond with a proton. Thus, in an aqueous solution, fluoride is a weaker base than larger halide ions.



  3. NH₂⁻ (amide ion): This ion has a nitrogen atom, which is less electronegative than fluorine, holding the negative charge. Nitrogen can share its electron pair more easily than fluorine. Also, the negative charge on the amide ion is not as effectively stabilized because nitrogen is less electronegative than fluorine.



  4. CH₃⁻ (methide ion): This ion has a carbon atom bearing the negative charge. Carbon is less electronegative than nitrogen and fluorine, so it is more ready to share its electron pair compared to NH₂⁻ and F⁻. However, the negative charge is not delocalized and is concentrated on a single carbon atom, making it a strong base.




Considering these factors, the order of increasing base strength from weakest to strongest should be:


F⁻ < Br⁻ < NH₂⁻ < CH₃⁻


This order takes into account that fluoride is very electronegative and holds onto its electron pair tightly, bromide is a larger halogen and can distribute its negative charge over a larger volume, the amide ion is less stable due to the higher energy of nitrogen-based anions, and the methide ion is a strong base due to carbon's low electronegativity and the localized negative charge.
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Strength of following bases decrease in the order?(I) Br- (II) F- (...
As electro negativity increase central element can attracted its electrons more powerfully so electronegative element is less basic..as electronegative order is F>Cl>N>C..so it follows reverse order
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