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

💡 Solution & Explanation

# Why $C_nH_{2n+2}$ Hydrides Don't Act as Lewis Acids/Bases **Step 1: Identify the hydrocarbon type** $C_nH_{2n+2}$ represents **alkanes** (saturated hydrocarbons) with only single C—C and C—H bonds. **Step 2: Recall Lewis acid/base definitions** - **Lewis acid**: accepts electron pairs (has empty orbitals) - **Lewis base**: donates electron pairs (has lone pairs) **Step 3: Analyze electron availability in alkanes** - All valence electrons in alkanes are **engaged in C—C and C—H bonds** - No lone pairs available on carbon or hydrogen atoms - All electrons are **localized in bonding pairs** between atoms **Step 4: Check orbital status** - Carbon in alkanes uses sp³ hybridization (tetrahedral geometry) - **No empty p-orbitals** available for accepting electron pairs - Cannot act as Lewis acid **Step 5: Conclusion** Since alkanes have: - No lone pairs (cannot donate) → not Lewis bases - No empty orbitals (cannot accept) → not Lewis acids **Therefore, they behave as normal covalent compounds** with inert bonding—their electrons are fully occupied in bonds with no additional interactions possible. This is why alkanes are chemically inert under normal conditions and don't participate in acid-base reactions.