Final answer:
The compounds that act as Lewis acids are those that can accept pairs of electrons. In this case, the correct options would be (a) N≡C and (c) BeCl2.
Step-by-step explanation:
These compounds have an electron-deficient atom that can bond with electron pairs from a Lewis base. From the given options, the compounds that act as Lewis acids are −(CH3)3C (Tri-methyl carbocation) and BeCl2 (Beryllium dichloride), because they have vacant orbitals that can accept electron pairs.
The question asks to identify which of the following compounds are Lewis acids: a) N≡C b) −(CH3)3C c) BeCl2 d) NaHCO3. A Lewis acid is a compound that can accept a pair of electrons in a chemical reaction. Among the options given:
- N≡C (Cyanogen) doesn't conventionally act as Lewis acid because it does not have a vacant orbital to accept electrons.
- −(CH3)3C (Tri-methyl carbocation) is a carbocation and can act as a Lewis acid due to its vacant p-orbital.
- BeCl2 (Beryllium dichloride) is a classic example of Lewis acid, as Be has a vacant orbital that can accept electron pairs.
- NaHCO3 (Sodium bicarbonate) does not typically act as a Lewis acid; it's more commonly a reactant in Brønsted-Lowry reactions.
Therefore, the compounds that are Lewis acids from the given options are b) −(CH3)3C and c) BeCl2.