Carbon hydride of the type, CnH2n+2 do not act as Lewis acid or Lewis base. They behave as normal co — Hydrogen Chemistry Question

💡 Solution & Explanation

# Solution: Why $C_nH_{2n+2}$ Hydrides Are Neither Lewis Acids nor Bases **Understanding the compound type:** $C_nH_{2n+2}$ represents **alkanes** (saturated hydrocarbons) — compounds with only single C-C and C-H bonds. **Lewis acid requirement:** Needs empty orbitals to accept electron pairs - Carbon in alkanes: **sp³ hybridized** with 4 bonding pairs, **no vacant orbitals** available - Therefore, cannot accept electrons → **not a Lewis acid** **Lewis base requirement:** Needs lone pairs to donate - Carbon: All valence electrons engaged in bonding (4 bonds) - Hydrogen: All electrons in C-H bonds, **no lone pairs** - Therefore, cannot donate electrons → **not a Lewis base** **Why they behave as normal covalent hydrides:** Alkanes are **completely saturated** with: - All valence orbitals of carbon filled - All electrons localized in σ-bonds - No lone pairs, no empty orbitals, no polar C-H bonds This makes them **inert** and unreactive with electron acceptors or donors, exhibiting pure covalent character without acid-base behavior. **Answer: C** — The structure lacks both empty orbitals (for Lewis acidity) and lone pairs (for Lewis basicity), making them incapable of acid-base interactions.