Final answer:
FeCl3 (iron(III) chloride) functions as a Lewis acid in an aqueous solution, while Cl2 (chlorine gas) does not act as an acid or a base under Brønsted-Lowry theory. Therefore, none of the provided options perfectly fits; however, FeCl3 can be considered an acid in the context of Lewis acid-base theory.
Step-by-step explanation:
In chemistry, an acid is a substance that can donate a proton or H+ ion, whereas a base is a substance that can accept a proton. When discussing whether a substance is an acid or a base, we refer to the Brønsted-Lowry theory.
Looking at FeCl3 (iron(III) chloride), when it is dissolved in water, it can lead to the formation of the Fe3+ ion, which has a high charge density and can act as a Lewis acid by accepting electron pairs. It does not donate protons, so it isn't an acid in the Brønsted-Lowry sense but rather a Lewis acid. On the other hand, Cl2 (chlorine gas) is neither an acid nor a base because it does not interact with water to either donate H+ ions or accept them.
Thus, answer (1) FeCl3 is an acid and Cl2 is a base is partially correct if we consider the Lewis acid definition. However, under Brønsted-Lowry theory, Cl2 wouldn't qualify as a base, so none of the four options provided perfectly fits the Brønsted-Lowry definitions of acids and bases. It is important to note that while FeCl3 behaves as a Lewis acid in aqueous solution, it is generally identified as a salt rather than simply an acid.