Chapter 9: Problem 37
Specify which hybrid orbitals are used by carbon atoms in the following species: (a) CO (b) \(\mathrm{CO}_{2},(\mathrm{c}) \mathrm{CN}^{-}\)
Short Answer
Expert verified
Carbon is sp hybridized in CO, CO₂, and CN⁻.
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
sp hybrid orbitals
Hybridization is a model that explains the molecular structure and geometry by mixing atomic orbitals to form new hybrid orbitals. In particular, sp hybridization occurs when one s orbital and one p orbital from the same atom combine. This results in two equivalent sp hybrid orbitals. These orbitals align linearly, 180 degrees apart, and are often involved in forming linear structures.
For example, carbon, an element capable of forming covalent bonds, frequently exhibits sp hybridization when it forms multiple bonds like triple bonds. The sp hybrid orbitals participate in forming sigma (\(\sigma\)) bonds, while the unhybridized p orbitals overlap to create pi (\(\pi\)) bonds. This configuration is usually found in molecules like carbon monoxide (CO), carbon dioxide (CO2), and the cyanide ion (CN⁻). Understanding this helps explain their linear shapes and bonding properties.
For example, carbon, an element capable of forming covalent bonds, frequently exhibits sp hybridization when it forms multiple bonds like triple bonds. The sp hybrid orbitals participate in forming sigma (\(\sigma\)) bonds, while the unhybridized p orbitals overlap to create pi (\(\pi\)) bonds. This configuration is usually found in molecules like carbon monoxide (CO), carbon dioxide (CO2), and the cyanide ion (CN⁻). Understanding this helps explain their linear shapes and bonding properties.
carbon monoxide
Carbon monoxide (CO) is a simple and toxic molecule formed by a carbon atom triple bonded to an oxygen atom. In this molecule, the carbon atom is sp hybridized. Here's how: one s orbital and one p orbital in carbon mix to form two sp hybrid orbitals. Carbon uses one of these sp orbitals to form a sigma bond with oxygen.
The remaining two p orbitals on carbon contribute to forming two pi bonds with the p orbitals of oxygen, completing the triple bond structure. The sp hybridization results in a linear molecular geometry, reflecting the nature of the bond between carbon and oxygen.
CO is an example of sp hybridization where significant overlap between atomic orbitals creates strong bonds, contributing to its stability despite being a small molecule. This characteristic explains CO's role as an important ligand in coordination chemistry.
The remaining two p orbitals on carbon contribute to forming two pi bonds with the p orbitals of oxygen, completing the triple bond structure. The sp hybridization results in a linear molecular geometry, reflecting the nature of the bond between carbon and oxygen.
CO is an example of sp hybridization where significant overlap between atomic orbitals creates strong bonds, contributing to its stability despite being a small molecule. This characteristic explains CO's role as an important ligand in coordination chemistry.
carbon dioxide
In carbon dioxide (CO2), the central carbon atom is sp hybridized, similar to the CO molecule. Each of the two sp hybrid orbitals forms sigma bonds with the oxygen atoms, accounting for the double bonds in CO2.
The linear shape of CO2 is a direct result of the 180-degree arrangement of these sp hybrid orbitals. Carbon's unhybridized p orbitals form pi bonds with the p orbitals of the oxygen atoms, completing the carbon-oxygen double bonds.
Understanding this hybridization explains how CO2 maintains a linear structure, which is vital for its role in various processes such as photosynthesis and respiration. The sp hybrid orbitals help shed light on the molecule's unique properties, including its non-polarity despite having polar bonds.
The linear shape of CO2 is a direct result of the 180-degree arrangement of these sp hybrid orbitals. Carbon's unhybridized p orbitals form pi bonds with the p orbitals of the oxygen atoms, completing the carbon-oxygen double bonds.
Understanding this hybridization explains how CO2 maintains a linear structure, which is vital for its role in various processes such as photosynthesis and respiration. The sp hybrid orbitals help shed light on the molecule's unique properties, including its non-polarity despite having polar bonds.
cyanide ion
The cyanide ion (CN⁻) is a negatively charged linear molecule consisting of a carbon and nitrogen atom connected by a triple bond. In this case, the carbon atom exhibits sp hybridization.
Similar to carbon monoxide, the carbon in CN⁻ uses one of its sp hybrid orbitals to form a strong sigma bond with nitrogen. The remaining p orbitals create two pi bonds with the p orbitals on nitrogen, reinforcing the triple bond strength.
As a result, the cyanide ion is highly stable and linear, a testament to effective sp hybridization. This configuration also contributes to its high toxicity, as the ion can penetrate biological membranes easily. Understanding CN⁻'s structure is critical to grasping its behavior in biological contexts and chemical reactions.
Similar to carbon monoxide, the carbon in CN⁻ uses one of its sp hybrid orbitals to form a strong sigma bond with nitrogen. The remaining p orbitals create two pi bonds with the p orbitals on nitrogen, reinforcing the triple bond strength.
As a result, the cyanide ion is highly stable and linear, a testament to effective sp hybridization. This configuration also contributes to its high toxicity, as the ion can penetrate biological membranes easily. Understanding CN⁻'s structure is critical to grasping its behavior in biological contexts and chemical reactions.
