Question

In each row check off the boxes that apply to the highlighted reactant. reaction The highlighted reactant acts as a... (check all that apply) Brønsted-Lowry acid Brønsted-Lowry base HCIO(aq) + (CH3), N(aq) + C10(aq) + (CH3), NH Lewis acid (aq) Lewis base Brønsted-Lowry acid Brønsted-Lowry base 2 CH4(9) + Br2(9) ► 2CH2Br(g) + H2(9) Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base HCN(aq) + CH3NH2(aq) → CN (aq) + CH3NH; (aq) Lewis acid Lewis base x 6 ?

Answer 1

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.