Draw Lewis structures for the \(\mathrm{AsCl}_{4}^{+}\) and \(\mathrm{AsCl}_{6}^{-}\) ions. What type of reaction (acid-base, oxidation- reduction, or the like) is the following?$$2 \mathrm{AsCl}_{5}(g) \longrightarrow \mathrm{AsCl}_{4} \mathrm{AsCl}_{6}(s)$$.

First, we need to draw the Lewis structures for \(\mathrm{AsCl}_{4}^{+}\) and \(\mathrm{AsCl}_{6}^{-}\) ions. In these ions, arsenic (As) is the central atom surrounded by chlorine (Cl) atoms. For \(\mathrm{AsCl}_{4}^{+}\): 1. Determine the total number of valence electrons: \(5\) (from As) + \(4 \times 7\) (from 4 Cl atoms) + \(1\) (due to positive charge) = \(33\). 2. Place As in the center and add single bonds to each Cl atom: \(_{As}|\text{Cl}¢\text{Cl}¢\text{Cl}¢\text{Cl}=\). 3. Place remaining electrons as lone pairs, following the octet rule, yielding \(_{\large{\bullet}}^{\large{\bullet}}\text{As}(_{\large{\bullet}}^{\large{\bullet}}\text{Cl}\ _{\large{\bullet}}^{\large{\bullet}}\text{Cl}\ _{\large{\bullet}}^{\large{\bullet}}\text{Cl}\ _{\large{\bullet}}^{\large{\bullet}}\text{Cl}\ _{\large{\bullet}}^{\large{\bullet}}|\). 4. Calculate the formal charge on each atom to confirm the best structure: As (\(0\)), all Cl atoms (\(-1\)), and check that the sum is equal to the overall charge of \(\mathrm{AsCl}_{4}^{+}\). For \(\mathrm{AsCl}_{6}^{-}\): 1. Determine the total number of valence electrons: \(5\) (from As) + \(6 \times 7\) (from 6 Cl atoms) - \(1\) (due to negative charge) = \(47\). 2. Place As in the center and add single bonds to each Cl atom. 3. As As can accommodate more than 8 electrons (expanded octet), add remaining electrons as lone pairs, following the octet rule for Cl atoms. 4. Calculate the formal charge on each atom to confirm the best structure. In this case, As has a formal charge of \(-1\) and all Cl atoms have a formal charge of \(0\). The sum is equal to the overall charge of \(\mathrm{AsCl}_{6}^{-}\).

Now, let's examine the given reaction: $$2 \mathrm{AsCl}_{5}(g) \longrightarrow \mathrm{AsCl}_{4}^{+} \mathrm{AsCl}_{6}^{-}(s)$$. To classify this reaction, we observe that: - There is no transfer of protons (H+), so it's not an acid-base reaction. - There is no change in oxidation states of As or Cl, so it's not an oxidation-reduction reaction. This reaction involves the transfer of a chlorine atom (Cl) between two \(\mathrm{AsCl}_{5}\) molecules, forming one \(\mathrm{AsCl}_{4}^{+}\) and one \(\mathrm{AsCl}_{6}^{-}\) species. Therefore, this is a **ligand-exchange reaction**.