Question

All are examples of Lewis acid-base reactions except:

(A) Cu²⁺(aq) + 4NH₃(aq) → [Cu(NH₃)₄]²⁺(aq)
(B) HCl(g) + NH₃(g) → NH₄Cl(s)
(C) H⁺(aq) + OH⁻(aq) → H₂O(l)
(D) 2Na(s) + Cl₂(g) → 2NaCl(s)

Answer 1

Option (D) 2Na(s) + Cl₂(g) → 2NaCl(s) is an oxidation-reduction reaction, not a Lewis acid-base reaction because it involves the transfer of electrons between sodium and chlorine, changing their oxidation states.

Step-by-step explanation:

All the given options are examples of Lewis acid-base reactions except for (D) 2Na(s) + Cl₂(g) → 2NaCl(s). This particular reaction is not a Lewis acid-base reaction; instead, it is an oxidation-reduction (redox) reaction. In a Lewis acid-base reaction, a Lewis base donates an electron pair, and a Lewis acid accepts an electron pair. In the case of option (D), sodium (Na) is losing electrons (oxidation), and chlorine (Cl₂) is gaining electrons (reduction), which classifies it as a redox reaction rather than a Lewis acid-base reaction.

• Lewis acid-base reactions involve the transfer of an electron pair.
• Redox reactions involve the transfer of electrons between species, resulting in changes in oxidation states.
• Examples (A), (B), and (C) involve Lewis acids and bases, whereas example (D) involves the transfer of electrons indicative of a redox reaction.