Final answer:
In the given reactions, the highlighted reactants have different roles. HCIO(aq) acts as a Brønsted-Lowry acid. Heptane (C10H22), CH4(g), and Br2(g) do not act as Brønsted-Lowry acids or bases. Br2(g) acts as a Lewis acid. HCN(aq) acts as a Brønsted-Lowry acid, and CH3NH2(aq) acts as a Brønsted-Lowry base.
Step-by-step explanation:
In the given reactions, we need to identify the roles of the highlighted reactants as Brønsted-Lowry acids, Brønsted-Lowry bases, Lewis acids, and Lewis bases.
Reactant 1: HCIO(aq)
- Acts as a Brønsted-Lowry acid because it donates a proton (H+ ion) to another species.
Reactant 2: Heptane (C10H22)
- Does not act as a Brønsted-Lowry acid or base as there is no proton transfer involving this compound.
- Does not act as a Lewis acid or base as it does not accept or donate electron pairs.
Reactant 3: CH4(g)
- Does not act as a Brønsted-Lowry acid or base as there is no proton transfer involving this compound.
- Does not act as a Lewis acid or base as it does not accept or donate electron pairs.
Reactant 4: Br2(g)
- Does not act as a Brønsted-Lowry acid or base as there is no proton transfer involving this compound.
- Acts as a Lewis acid because it accepts a pair of electrons from another species.
Reactant 5: HCN(aq)
- Acts as a Brønsted-Lowry acid because it donates a proton (H+ ion) to another species.
Reactant 6: CH3NH2(aq)
- Acts as a Brønsted-Lowry base because it accepts a proton (H+ ion) from another species.