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 CO, a triple bond forms between carbon and oxygen, with one lone pair on carbon and two lone pairs on oxygen. In C3O2, the first two carbon atoms form a double bond with a single oxygen atom and a single bond with another carbon atom, and the third carbon atom forms a single bond with the other oxygen atom. There is one lone pair on the first two carbon atoms, two lone pairs on the third carbon atom, and two lone pairs on each oxygen atom.

Step-by-step solution

Identify the formulas of two additional oxides of carbon

The three stable oxides of carbon are carbon dioxide (CO2), carbon monoxide (CO), and carbon suboxide (C3O2).

Explain bonding in CO using the localized electron model

In carbon monoxide (CO), carbon has 4 valence electrons, and oxygen has 6 valence electrons. According to the localized electron model: 1. Carbon forms a triple bond with oxygen, which means that there are 6 bonding electrons shared between carbon and oxygen. 2. Each atom also has a pair of non-bonding electrons. Carbon has one lone pair (2 non-bonding electrons), and oxygen has two lone pairs (4 non-bonding electrons). Therefore, the localized electron model for CO is a triple bond between carbon and oxygen, with one lone pair on the carbon atom and two lone pairs on the oxygen atom.

Explain bonding in C3O2 using the localized electron model

In carbon suboxide (C3O2), there are 3 carbon atoms and 2 oxygen atoms. Each carbon atom has 4 valence electrons, and each oxygen atom has 6 valence electrons. According to the localized electron model: 1. Two carbon atoms form a double bond with a single oxygen atom. This means that there are 4 bonding electrons shared between the carbon and oxygen atoms. 2. The remaining carbon atom forms a single bond with the other oxygen atom, meaning there are 2 bonding electrons shared between this carbon and oxygen atom. 3. The first two carbon atoms each have one lone pair (2 non-bonding electrons). 4. The third carbon atom has two lone pairs (4 non-bonding electrons). 5. Each oxygen atom also has two lone pairs (4 non-bonding electrons). Therefore, the localized electron model for C3O2 is: - A double bond between the first carbon atom and an oxygen atom, with a single bond connecting to the second carbon atom and double bond with the other oxygen atom. - A single bond between the third carbon atom and the other oxygen atom. - One lone pair on the first two carbon atoms, two lone pairs on the third carbon atom, and two lone pairs on each oxygen atom.

Key concepts

Localized Electron Model

The localized electron model is a way to visualize the arrangement of electrons between atoms in a molecule. It helps us understand how atoms bond and share electrons. This model assumes that electrons are localized on a particular atom or between a pair of atoms.

In this model:

• Electrons that participate in bonding are called bonding pairs.
• Electrons not involved in bonding are known as lone pairs.
• Bonds can be single, double, or triple, indicating the number of electron pairs shared.

In essence, it helps us depict the structure and electron placement, providing clarity on how molecules like carbon monoxide and carbon suboxide are bonded.

Carbon Monoxide

Carbon monoxide (CO) is one of the simplest oxides of carbon. It is composed of one carbon atom and one oxygen atom. The bond between carbon and oxygen in CO is a triple bond, which involves six electrons being shared.

For CO:

• Carbon, having 4 valence electrons, shares them with oxygen to satisfy the octet rule.
• Oxygen, with 6 valence electrons, pairs with carbon's electrons to achieve stability.
• Besides the triple bond, carbon possesses one lone pair, and oxygen holds two.

This arrangement of bonds and electrons can be better visualized and explained using the localized electron model, emphasizing the strong bond between the atoms.

Carbon Suboxide

Carbon suboxide ( C_3O_2 ) is an intriguing molecule comprising three carbon atoms and two oxygen atoms. Constructing this molecule involves multiple bonds and lone pairs, offering a complex structure to consider.

In C_3O_2 :

• The first carbon atom forms a double bond with an oxygen atom and a single bond with another carbon atom.
• This middle carbon is doubly bonded to both other carbons, creating a linear structure.
• The third carbon atom forms a double bond with the second oxygen.
• Lone pairs reside on each oxygen and the first and third carbon atoms, adding stability.

These elements combine to form a unique and relatively stable molecule, with its bonding structure well depicted through the localized electron model.

Chemical Bonding

Chemical bonding is a fundamental concept in chemistry that explains how atoms associate to form molecules. These bonds are essential to hold molecules together and determine their structure and properties.

Types of chemical bonds include:

• Covalent bonds: Form when atoms share electrons, like in carbon monoxide's triple bond.
• Ionic bonds: Involve electron transfer, usually between metals and non-metals.
• Metallic bonds: Found in metals where electrons are shared across many atoms.

Chemical bonding explains the intricate balance between forces that hold atoms together, providing us with the molecular structure essential for various chemical reactions and compounds.

Valence Electrons

Valence electrons are the outermost electrons of an atom and play a key role in chemical bonding and reactions. They determine an atom's ability to bond with others by either sharing or transferring to achieve a full outer shell.

Key points about valence electrons:

• They are crucial in the formation of bonds, especially in covalent molecules.
• The number of valence electrons influences how atoms interact and bond.
• Atoms strive for a stable electron configuration, often resembling the nearest noble gas.

Understanding valence electrons is critical to predicting and explaining how molecules, like carbon monoxide and carbon suboxide, achieve stability through bonding.