See image — GOC and Organic Chemistry Basics Chemistry Question

💡 Solution & Explanation

# Solution: Basicity Order of Anions/Compounds **Key Principle:** Stronger bases have greater tendency to accept protons. Basicity is determined by: 1. **Electronegativity** of the central atom (lower = more basic) 2. **Charge stability** (negative charge on less electronegative atoms = more basic) 3. **Hybridization** (higher s-character = more electronegative, less basic) --- ## Analysis of Each Species: **$OH^-$** → O is highly electronegative; charge on O is stabilized. **Weakest base** **$NH_2^-$** → N is less electronegative than O; lone pair readily available. **Strong base** **$H-C \equiv C^-$** → C is $sp$ hybridized (50% s-character, very electronegative); charge highly stabilized. **Weak base** **$CH_3-CH_2^-$** → C is $sp^3$ hybridized (25% s-character); least electronegative carbon; charge least stabilized. **Strongest base** --- ## Correct Order: $$CH_3-CH_2^- > NH_2^- > H-C \equiv C^- > OH^-$$ **Why (A) is correct:** - Alkyl anion (ethyl) is most basic because $sp^3$ carbon is least electronegative - $NH_2^-$ is next (N less electronegative than O) - Acetylide ion stabilized by $sp$ hybridization - $OH^-$ is weakest (highly electronegative oxygen stabilizes negative charge) **Why others fail:** (B), (C), (D) all incorrectly place $OH^-$ as strongest or $CH_3CH_2^-$ lower in the series.