Question

In addition to \(\mathrm{CO}_{2}\), two additional stable oxides of carbon form. The space-filling models for \(\mathrm{CO}_{2}\) and the other two stable oxides are: What are the formulas for the two additional stable oxides of carbon? Explain the bonding in each of these two forms using the localized electron model.

Short answer

The two additional stable oxides of carbon are carbon monoxide (CO) and carbon suboxide (C3O2). In carbon monoxide, a triple bond (1σ and 2π bonds) between carbon and oxygen satisfies the octet rule for both atoms. Carbon suboxide has a linear structure O=C=C=C=O, in which the central carbon atom is doubly bonded (1σ and 1π bond) to the two adjacent carbon atoms, which are also doubly bonded to oxygen atoms.

Step-by-step solution

Identify the two additional stable oxides of carbon

The two additional stable oxides of carbon are carbon monoxide (CO) and carbon suboxide (C3O2).

Describe the bonding in CO using the localized electron model

First, let's analyze carbon monoxide (CO). Carbon has 4 valence electrons, and oxygen has 6 valence electrons. Using the localized electron model, we can represent the bonding as follows: 1. Place a single bond (2 electrons shared) between the carbon and oxygen atoms. 2. Assign the remaining 6 electrons to the oxygen atom in three lone pairs. 3. Assign the remaining 2 electrons to the carbon atom in a lone pair. 4. Since carbon needs to have 8 electrons in its outer shell to achieve an octet, it forms a triple bond with the oxygen atom. The Lewis structure would look like this: C≡O In the localized electron model, carbon monoxide consists of a triple bond between carbon and oxygen, with one sigma (σ) bond and two pi (π) bonds. It has no formal charge, as the octet rule is satisfied for both atoms.

Describe the bonding in C3O2 using the localized electron model

Now, let's analyze carbon suboxide (C3O2). The molecule consists of 3 carbon atoms and 2 oxygen atoms. Carbon has 4 valence electrons, and oxygen has 6 valence electrons. Using the localized electron model, we can represent the bonding as follows: 1. Place a single bond (2 electrons shared) between each pair of carbon atoms. 2. Place a single bond (2 electrons shared) between each carbon at the ends and an oxygen atom. 3. Assign the remaining electrons in such a way that each atom achieves an octet. 4. The resulting Lewis structure would look like this: O=C=C=C=O In the localized electron model, carbon suboxide consists of a central carbon atom doubly bonded to two adjacent carbon atoms, which are in turn doubly bonded to oxygen atoms. There is a σ bond between adjacent carbon atoms and π bonds between the adjacent double-bonded atoms (C=C and C=O). Each atom has no formal charge, as the octet rule is satisfied.

Key concepts

Localized Electron Model

The localized electron model helps us understand how atoms bond together. In this model, we represent molecules by showing the sharing of electrons between atoms.
Each shared pair of electrons forms a bond, represented in diagrams as lines or sticks. - It is most effective for explaining how covalent bonds are formed. - The model highlights which electrons participate in bonding and which form lone pairs. Unlike more complex models, the localized electron model focuses on fixed positions, making it accessible and simpler for beginners learning molecular structures.

Lewis Structure

A Lewis structure is a diagrammatic way to represent the atoms and bonding in a molecule. It shows the arrangement of valence electrons around atoms. Structure is key in learning how atoms share electrons to reach a stable configuration. - Lewis structures use dots to represent valence electrons. - Lines between atoms symbolize shared pairs, i.e., bonds. For example, in carbon monoxide (CO), a Lewis structure clearly illustrates the triple bond between carbon and oxygen. By providing a visual guide, Lewis structures make complex bonding concepts more accessible for students.

Triple Bond

A triple bond involves the sharing of three pairs of electrons between two atoms. This is a strong type of chemical bond and is essential for the stability of molecules like carbon monoxide. - Consists of one sigma (σ) bond and two pi (π) bonds.
- Provides high bond strength and short bond length. In the case of CO, a triple bond forms due to carbon's need for more electrons to complete its octet. This triple bond ensures both carbon and oxygen achieve their stable electron configurations, making CO a remarkably stable molecule.

Carbon Monoxide

Carbon monoxide is a well-known compound with the formula CO. It features a triple bond between carbon and oxygen, which provides its remarkable stability. - It has one carbon atom and one oxygen atom. - Formed by sharing 8 valence electrons between the two atoms. Due to its stable triple bond, CO remains a prevalent molecule in various industrial processes. However, despite its uses, it is also a toxic gas, such as when burning fuels without adequate ventilation.

Carbon Suboxide

Carbon suboxide, with the formula C3O2, is an intriguing molecule with unique bonding. - It includes three carbon atoms and two oxygen atoms.
- Each carbon atom connects through double bonds, creating a linear chain. Bonded as O=C=C=C=O, this structure is fascinating in its arrangement but less common as it can rapidly polymerize under certain conditions. Understanding carbon suboxide enriches the study of organic chemistry, showcasing different ways carbon-based compounds can exhibit stability.