Chapter 5: Problem 19
The number of \(\sigma\) bonds and \(\pi\) bonds in \(\mathrm{CO}_{2}\) molecule are \(\quad\) respectively.
Short Answer
Expert verified
Answer: In a CO₂ molecule, there are 2 sigma (σ) bonds and 2 pi (π) bonds.
Step by step solution
01
Determine the molecular structure of CO₂
First, we need to figure out the structure of the CO₂ molecule. A CO₂ molecule consists of one carbon atom double bonded to two oxygen atoms (O=C=O).
02
Identify the sigma (σ) and pi (π) bonds in the molecule
In a double bond, there is always one sigma (σ) bond and one pi (π) bond. As there are two double bonds in CO₂ molecule (each between the carbon and an oxygen atom), we can now calculate the number of sigma (σ) and pi (π) bonds:
03
Calculate the number of sigma (σ) bonds
Since there is one σ bond in each double bond, CO₂ will have:
1 σ bond (from C=O) + 1 σ bond (from C=O) = 2 σ bonds
04
Calculate the number of pi (π) bonds
As there is one π bond in each double bond, CO₂ will have:
1 π bond (from C=O) + 1 π bond (from C=O) = 2 π bonds
In conclusion, the number of sigma (σ) bonds and pi (π) bonds in a CO₂ molecule are 2 and 2, respectively.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Sigma Bonds
Sigma bonds (\(\sigma\) bonds) are the strongest type of covalent chemical bond. These bonds are formed by the "head-on" overlapping of atomic orbitals.
When we look at molecules such as \(\mathrm{CO}_{2}\), understanding sigma bonds gives us a window into the stability and structural integrity of the molecule. They are foundational to the molecule's strength.
When we look at molecules such as \(\mathrm{CO}_{2}\), understanding sigma bonds gives us a window into the stability and structural integrity of the molecule. They are foundational to the molecule's strength.
- Formation: A sigma bond can form between two s orbitals, or an s and a p orbital, or even two p orbitals aligned properly, stretching directly between two nuclei.
- Characteristics: Sigma bonds allow for free rotation of bonded atoms. This is because the electron cloud in sigma bonds is symmetrically distributed along the axis connecting the two nuclei.
Pi Bonds
Pi bonds (\(\pi\) bonds) are a form of covalent chemical bond where the "sideways" overlapping of atomic orbitals creates bonding above and below the plane of the atoms involved. They often exist in conjunction with sigma bonds, adding complexity and rigidity to molecular structures.
In double bonds like those in \(\mathrm{CO}_{2}\), pi bonds are crucial to maintaining the molecule's planar structure.
In double bonds like those in \(\mathrm{CO}_{2}\), pi bonds are crucial to maintaining the molecule's planar structure.
- Formation: Pi bonds occur when parallel p orbitals overlap, allowing electrons to be shared across the bond in two lobes (above and below the plane).
- Characteristics: Pi bonds prevent the rotation of the bonded atoms. One pi bond, occurring in addition to a sigma bond in double bonds, adds to the rigidity of the molecule.
Molecular Structure
The molecular structure of a molecule such as \(\mathrm{CO}_{2}\) is a combination of its spatial arrangement of atoms and the type of chemical bonds that hold these atoms.
Understanding molecular structure is critical to predicting a molecule's reactivity, polarity, phase of matter, color, magnetism, biological activity, and other properties.
Understanding molecular structure is critical to predicting a molecule's reactivity, polarity, phase of matter, color, magnetism, biological activity, and other properties.
- Linear Structure: In \(\mathrm{CO}_{2}\), the molecule is linear. The central carbon atom forms double bonds with each oxygen atom, leading to a straight-line configuration — denoted as O=C=O.
- Bond Angles: In a linear molecule like \(\mathrm{CO}_{2}\), the angle between the bonds is 180°.
- Nonpolar Nature: Due to its linear shape and even distribution of charge, \(\mathrm{CO}_{2}\) is a nonpolar molecule. The dipole moments cancel out, resulting in zero net dipole moment.