Questions: Given the following chemical equation, identify the Lewis acid: Zn^2+(aq) + 4 NH3(aq) -> [Zn(NH3)4]^2+ (aq) Zn^2+ (aq) NH3(aq) [Zn(NH3)4]^2+ (aq)

Transcript text: Given the following chemical equation, identify the Lewis acid: \[ \mathrm{Zn}^{2+}(\mathrm{aq})+4 \mathrm{NH}_{3(\mathrm{aq})} \rightarrow\left[\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}{ }_{(\mathrm{aq})} \] $\mathrm{Zn}^{2+}$ (aq) $\mathrm{NH}_{3(\mathrm{aq})}$ $\left[\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}$ (aq)

Solution

Solution Steps

Step 1: Identify the Lewis Acid and Lewis Base

In a chemical reaction, a Lewis acid is a species that accepts an electron pair, while a Lewis base is a species that donates an electron pair.

Step 2: Analyze the Reactants

In the given reaction: \[ \mathrm{Zn}^{2+}(\mathrm{aq}) + 4 \mathrm{NH}_{3(\mathrm{aq})} \rightarrow \left[\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}{ }_{(\mathrm{aq})} \]

$\mathrm{Zn}^{2+}$ is a cation with a positive charge, indicating it can accept electron pairs.
$\mathrm{NH}_3$ is a neutral molecule with a lone pair of electrons on the nitrogen atom, indicating it can donate electron pairs.

Step 3: Determine the Lewis Acid

Since $\mathrm{Zn}^{2+}$ accepts electron pairs from $\mathrm{NH}_3$, $\mathrm{Zn}^{2+}$ is the Lewis acid.