See image — GOC and Organic Chemistry Basics Chemistry Question

💡 Solution & Explanation

# Analysis: Which Species Cannot Function as an Electrophile? An **electrophile** is a species that accepts electron density (electron-poor species). Let me analyze each option: ## (A) HCl - $H$ in $HCl$ is slightly positive ($\delta^+$) due to $Cl$ being more electronegative - However, $HCl$ is a **Brønsted acid**, not a Lewis electrophile - $H$ cannot accept an electron pair—it can only donate a proton - **Cannot function as a Lewis electrophile** ✗ ## (B) $\overset{..}{C}Cl_2$ (Dichlorocarbene) - Carbon has only 6 electrons (electron-deficient) - Readily accepts electron pairs from nucleophiles - **Excellent electrophile** ✓ ## (C) $SiF_4$ - Silicon is electron-deficient and can expand its octet - Highly polarized $Si-F$ bonds make Si very electron-poor - Readily accepts nucleophiles (forms $SiF_6^{2-}$ complexes) - **Strong electrophile** ✓ ## (D) $CH_2=CH_2$ (Ethene) - $\pi$-electrons are available for donation to electrophiles - Acts as a nucleophile in electrophilic addition reactions - Can also accept electrons through back-bonding (acts as electrophile toward strong nucleophiles) - **Can function as electrophile** ✓ **Answer: (A) HCl** — It functions as a Brønsted acid (proton donor), not a Lewis electrophile (electron pair acceptor).