Question

Use the Lewis acid-base model to explain the following reaction. $$\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2}\mathrm{CO}_{3}(a q)$$

Short answer

In the given reaction, CO2 acts as a Lewis acid (electron-pair acceptor) and H2O acts as a Lewis base (electron-pair donor). The oxygen atom in the water molecule donates an electron pair to the carbon atom in the carbon dioxide molecule, forming a new bond and resulting in the formation of carbonic acid (H2CO3) in aqueous form. The reaction can be summarized as: \( \mathrm{CO}_{2}(g) \, \text{(Lewis acid)} + \mathrm{H}_{2} \mathrm{O}(l) \, \text{(Lewis base)} \longrightarrow \mathrm{H}_{2}\mathrm{CO}_{3}(a q) \).

Step-by-step solution

Identify the Lewis acid and base

To apply the Lewis acid-base model, first identify the Lewis acid and base in the given reaction. A Lewis acid is an electron-pair acceptor, while a Lewis base is an electron-pair donor. Here, CO2 is the Lewis acid, and H2O is the Lewis base.

Analyze the electron-pair donation and acceptance

In the reaction, the Lewis base (H2O) donates an electron pair, while the Lewis acid (CO2) accepts the electron pair. The oxygen atom in the water molecule has two lone electron pairs that can be donated. On the other hand, the carbon atom in the carbon dioxide molecule has empty orbitals that can accept electron pairs.

Formation of the product

As the Lewis base (H2O) donates an electron pair to the Lewis acid (CO2), a new bond is formed between the oxygen atom of the water molecule and the carbon atom of the carbon dioxide molecule. This results in the formation of carbonic acid (H2CO3), which exists in aqueous form (aq). The reaction can be summarized as follows: \( \mathrm{CO}_{2}(g) \, \text{(Lewis acid)} + \mathrm{H}_{2} \mathrm{O}(l) \, \text{(Lewis base)} \longrightarrow \mathrm{H}_{2}\mathrm{CO}_{3}(a q) \).

Key concepts

Electron-Pair Acceptor

The term **electron-pair acceptor** is crucial in understanding the Lewis acid-base model of chemical reactions. In this model, a Lewis acid is defined as an electron-pair acceptor. This basically means that the molecule or atom lacks sufficient electrons and has the capacity to accept electron pairs from another atom or molecule.
In the given reaction involving carbon dioxide \(\mathrm{CO}_{2}\) and water \(\mathrm{H}_{2}\mathrm{O}\), \(\mathrm{CO}_{2}\) acts as the electron-pair acceptor. Carbon dioxide is well-suited for this role because the carbon atom in \(\mathrm{CO}_{2}\) has empty orbitals. This enables it to accept electron pairs from other atoms, such as the oxygen in water.
The effectiveness of \(\mathrm{CO}_{2}\) as an electron-pair acceptor is why it functions as a Lewis acid in this reaction. When \(\mathrm{CO}_{2}\) accepts an electron pair, it forms a new chemical bond, facilitating the creation of a new compound. This process is central to many important chemical reactions and showcases the versatility of Lewis acid-base interactions.

Electron-Pair Donor

In contrast to a Lewis acid, a **Lewis base** is known as an electron-pair donor. Being an electron-pair donor means the molecule or atom has extra electron pairs that it can provide to another atom or molecule. This characteristic defines its ability to participate in chemical reactions.
In the reaction we are analyzing, water \(\mathrm{H}_{2}\mathrm{O}\) serves as the electron-pair donor. Water is a good Lewis base because it has lone pairs of electrons on its oxygen atom. These lone pairs make it possible for water to donate an electron pair to another molecule like \(\mathrm{CO}_{2}\).
During the reaction with \(\mathrm{CO}_{2}\), the oxygen atom in water donates a pair of electrons to form a new bond with the carbon atom in \(\mathrm{CO}_{2}\). This act of donation is crucial because it triggers the subsequent steps where a new compound is formed. Choosing water as an electron-pair donor is a natural fit in many reactions, as it is abundantly available and highly reactive due to its ability to donate electrons.

Carbonic Acid Formation

***Carbonic acid formation*** is the final outcome of this Lewis acid-base reaction between \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2}\mathrm{O}\). This process results in \(\mathrm{H}_{2}\mathrm{CO}_{3}\) being formed.
In this process, the Lewis base, \(\mathrm{H}_{2}\mathrm{O}\), donates an electron pair to the carbon atom in the Lewis acid, \(\mathrm{CO}_{2}\). This donation results in a new bond being formed, ultimately creating carbonic acid.
Carbonic acid itself is a weak acid that exists mainly in aqueous form. It plays a pivotal role in biological and geological systems, serving key functions in the human body as well as in the carbon cycle. In our everyday lives, carbonic acid is present in carbonated beverages, offering an example of its practical use.
Understanding the formation of carbonic acid through the Lewis acid-base model helps us appreciate how simple interactions at the molecular level can have significant consequences across wide-ranging fields from physiology to ecology.