The hypochlorite ion, ClO-, acts as a weak base. (b) When ClO- acts as a base, which atom, Cl or O, acts as the proton acceptor? (c) Can you use formal charges to rationalize your answer to part (b)?
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insert step 1> Identify the role of the hypochlorite ion (ClO-) as a base, which means it will accept a proton (H+).
insert step 2> Consider the structure of the hypochlorite ion: Cl is bonded to O, and O has a lone pair of electrons.
insert step 3> Determine which atom, Cl or O, is more likely to accept a proton. Oxygen is more electronegative than chlorine and has lone pairs, making it a better candidate for proton acceptance.
insert step 4> Use formal charges to rationalize: In ClO-, the formal charge on O is typically -1, while Cl is 0. The negative charge on O indicates a higher electron density, making it more likely to attract and accept a proton.
insert step 5> Conclude that the oxygen atom in ClO- acts as the proton acceptor due to its higher electronegativity and negative formal charge.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Theory
Acid-base theory explains the behavior of substances in terms of proton transfer. According to the Brønsted-Lowry definition, an acid is a proton donor, while a base is a proton acceptor. In the case of the hypochlorite ion (ClO-), understanding its role as a weak base is crucial for determining which atom accepts the proton during a reaction.
In the context of acid-base reactions, the proton acceptor is the species that gains a hydrogen ion (H+). For the hypochlorite ion, the oxygen atom is typically the site of protonation due to its higher electronegativity compared to chlorine. This property allows oxygen to stabilize the positive charge that results from accepting a proton, making it the more likely proton acceptor.
Formal charge is a theoretical concept used to determine the distribution of electrons in a molecule. It is calculated by comparing the number of valence electrons in an atom to the number of electrons it owns in a Lewis structure. In the case of ClO-, analyzing formal charges can help rationalize which atom (Cl or O) is more stable after protonation, thus supporting the identification of the proton acceptor.
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