The three most stable oxides of carbon are carbon monoxide \((\mathrm{CO}),\) carbon dioxide \(\left(\mathrm{CO}_{2}\right),\) and carbon suboxide \(\left(\mathrm{C}_{3} \mathrm{O}_{2}\right) .\) The space-filling models for these three compounds are For each oxide, draw the Lewis structure, predict the molecular structure, and describe the bonding (in terms of the hybrid orbitals for the carbon atoms).

Start by counting the number of valence electrons for each atom in the molecule. Carbon has 4 valence electrons, and oxygen has 6 valence electrons. Now, arrange the atoms to form a molecule and share the electrons such that each atom obeys the octet rule. For CO, we have a total of 10 valence electrons. Lewis structure for CO: ``` O ≡ C ``` Where each line represents a pair of shared electrons. Here, CO has a triple bond between the carbon and oxygen atoms with two lone pairs on the oxygen atom. For CO2, we have a total of 16 valence electrons. Lewis structure for CO2: ``` O = C = O ``` Here, CO2 has a double bond between the central carbon atom and each oxygen atom with two lone pairs on each oxygem atom. For C3O2, we have a total of 22 valence electrons. Lewis structure for C3O2: ``` O=C=C=C=O ``` Here, C3O2 has a double bond between the terminal carbon and oxygen atoms, and a double bond between the carbon atoms.

To predict the molecular structure, we'll use the Valence Shell Electron Pair Repulsion (VSEPR) theory. CO has a triple bond between the carbon and oxygen atoms and two lone pairs on the oxygen atom, making it a linear molecule. CO2 has a double bond between the central carbon atom and each oxygen atom with two lone pairs on each oxygen atom, making it a linear molecule as well. C3O2 has double bonds between the terminal carbon and oxygen atoms, and a double bond between the carbon atoms, also making it a linear molecule.

For this step, we will use the hybridization concept to determine the types of hybrid orbitals involved in the bonding of each carbon atom in the molecules. For CO, the central carbon atom is sp hybridized. This is because it forms a total of two sigma bonds (one from the triple bond and one from the lone pair on oxygen), which corresponds to the linear geometry of the molecule. For CO2, the central carbon atom is sp hybridized as well. Each carbon-oxygen double bond consists of one sigma bond and one pi bond, so the central carbon atom forms two sigma bonds, corresponding to the linear molecular geometry. For C3O2, the terminal carbon atoms that form double bonds with oxygen are also sp hybridized. In this case, each carbon atom forms one sigma bond with oxygen and one sigma bond with the neighboring carbon atom, leading to the linear molecular geometry. The middle carbon atom is sp2 hybridized since it forms one sigma bond with each neighboring carbon atom and has one non-bonding electron pair. This indicates a trigonal planar geometry around the middle carbon atom. However, due to the linear arrangement of the entire molecule, the overall structure still appears linear.