Question

in each row check off the boxes that apply to the highlighted reactant. the highlighted reactant acts as a... (check all that apply) row 2: your answer is incorrect. hclo(aq) + (ch3)3n(aq) → clo-(aq) + (ch3)3nh+(aq) h2(g) + br2(g) → 2 hbr(g) zn2+(aq) + 6 ch3cn(aq) → zn(ch3cn)62+(aq) lewis base lewis acid brønsted - lowry base brønsted - lowry acid lewis base lewis acid brønsted - lowry base brønsted - lowry acid lewis base lewis acid brønsted - lowry base brønsted - lowry acid

Explanation:

Step1: Recall acid - base definitions

A Brønsted - Lowry acid donates a proton ($H^+$), and a Brønsted - Lowry base accepts a proton. A Lewis acid accepts a pair of electrons, and a Lewis base donates a pair of electrons.

Step2: Analyze the first reaction $HClO(aq)+(CH_3)_3N(aq)

ightarrow ClO^-(aq)+(CH_3)_3NH^+(aq)$
$HClO$ donates a proton to $(CH_3)_3N$. So $HClO$ is a Brønsted - Lowry acid. $(CH_3)_3N$ accepts a proton, so it is a Brønsted - Lowry base. Also, $(CH_3)_3N$ donates a lone - pair of electrons to form a bond with the proton, so it is a Lewis base.

Step3: Analyze the second reaction $H_2(g)+Br_2(g)

ightarrow 2HBr(g)$
This is a redox reaction and not an acid - base reaction in the Brønsted - Lowry or Lewis sense as there is no proton transfer or electron - pair donation/acceptance in the acid - base context.

Step4: Analyze the third reaction $Zn^{2 + }(aq)+6CH_3CN(aq)

ightarrow Zn(CH_3CN)_6^{2+}(aq)$
$Zn^{2+}$ accepts electron pairs from $CH_3CN$. So $Zn^{2+}$ is a Lewis acid. $CH_3CN$ donates its lone - pair of electrons to $Zn^{2+}$, so $CH_3CN$ is a Lewis base.

Answer:

Reaction	Lewis acid	Lewis base	Brønsted - Lowry acid	Brønsted - Lowry base

| $HClO(aq)+(CH_3)_3N(aq)
ightarrow ClO^-(aq)+(CH_3)_3NH^+(aq)$ | | $(CH_3)_3N$ | $HClO$ | $(CH_3)_3N$ |
| $H_2(g)+Br_2(g)
ightarrow 2HBr(g)$ | | | | |
| $Zn^{2 + }(aq)+6CH_3CN(aq)
ightarrow Zn(CH_3CN)_6^{2+}(aq)$ | $Zn^{2+}$ | $CH_3CN$ | | |