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 Alkanes ($C_nH_{2n+2}$) Don't Act as Lewis Acids/Bases **Step 1: Identify the compound class** $C_nH_{2n+2}$ represents saturated hydrocarbons (alkanes like methane, ethane, propane). **Step 2: Recall Lewis acid/base definitions** - **Lewis acid**: Electron pair acceptor (has empty orbitals) - **Lewis base**: Electron pair donor (has lone pairs) **Step 3: Analyze bonding in alkanes** Alkanes contain only $C-C$ and $C-H$ sigma bonds. Each carbon atom: - Forms 4 sigma bonds (sp³ hybridization) - Has **no lone pairs** of electrons - Has **no empty orbitals** available for bonding **Step 4: Why they can't donate or accept electrons** - Cannot act as **Lewis base**: No lone pairs to donate - Cannot act as **Lewis acid**: No vacant orbitals to accept electron pairs - All valence electrons are engaged in bonding **Step 5: Why they behave as normal covalent hydrides** Alkanes only undergo: - Non-polar covalent bonding (C-C and C-H bonds are nonpolar) - Physical interactions (van der Waals forces) - Substitution/addition reactions via free radicals or electrophilic mechanisms They are **inert** to Lewis acid-base reactions because they have **saturated bonding** with no available electron density or orbital space for electron pair exchange.