Chapter 4: Problem 62
Which orbital is used by oxygen atom to form a sigma bond with other oxygen
atom in
Short Answer
Expert verified
The sigma bond in is formed using the hybrid orbital.
Step by step solution
01
Understand the oxygen-oxygen bond in molecule
In an oxygen molecule ( ), two oxygen atoms form a double bond. One of these bonds is a sigma ( ) bond and the other is a pi ( ) bond.
02
Identify the hybridization state of oxygen atoms in
Each oxygen atom in undergoes hybridization. This is because hybridization allows for the formation of a sigma bond and also provides one unhybridized p-orbital needed for the pi bond.
03
Determine the orbital used for the sigma bond
During hybridization, one and two orbitals mix to form three hybrid orbitals. The sigma bond between the two oxygen atoms is formed using one of these hybrid orbitals.
04
Conclusion
Therefore, the sigma bond in the molecule is formed using the hybrid orbital.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Orbital Hybridization
Orbital hybridization is a key concept in understanding how atoms bond together to form molecules. It involves the mixing of atomic orbitals to create new hybrid orbitals, which can then participate in bonding. This mixing process happens because atoms strive to achieve the lowest possible energy state, and hybrid orbitals often offer a more stable configuration compared to pure atomic orbitals. When atoms like oxygen form bonds, they tend to undergo hybridization to achieve this stability.
For instance, in an molecule, each oxygen atom undergoes hybridization. This hybridization involves the combination of one and two orbitals to form three hybrid orbitals. These hybrid orbitals are then used to form stronger and more stable bonds between the atoms.
Understanding the concept of orbital hybridization can help you predict the geometry and bond angles in molecules. This concept is fundamental to mastering more complex topics in chemistry.
For instance, in an
Understanding the concept of orbital hybridization can help you predict the geometry and bond angles in molecules. This concept is fundamental to mastering more complex topics in chemistry.
Sigma and Pi Bonds
In the molecule, two types of covalent bonds are present: sigma ( ) bonds and pi ( ) bonds.
Sigma ( ) Bonds:
These are the strongest type of covalent bond and are formed by the direct overlap of orbitals. The electron density in a sigma bond is concentrated along the axis connecting the two bonding nuclei. In , the sigma bond is formed using one of the hybrid orbitals from each oxygen atom.
Pi ( ) Bonds:
These bonds are formed when parallel p-orbitals overlap sideways. In , after the formation of the sigma bond, each oxygen atom has an unhybridized p-orbital left, which are perpendicular to the internuclear axis. These unhybridized p-orbitals overlap side-by-side to form a pi bond. The electron density in a pi bond is concentrated above and below the plane of the nuclei.
Understanding the distinction between sigma and pi bonds is crucial for grasping the nature of multiple bonds in molecules. Sigma bonds provide the framework, while pi bonds add additional strength and rigidity.
Sigma (
These are the strongest type of covalent bond and are formed by the direct overlap of orbitals. The electron density in a sigma bond is concentrated along the axis connecting the two bonding nuclei. In
Pi (
These bonds are formed when parallel p-orbitals overlap sideways. In
Understanding the distinction between sigma and pi bonds is crucial for grasping the nature of multiple bonds in molecules. Sigma bonds provide the framework, while pi bonds add additional strength and rigidity.
sp2 Hybrid Orbitals
The hybrid orbitals are formed by the combination of one orbital and two orbitals from an atom. In the case of an oxygen atom in the molecule, this process creates three equal-energy hybrid orbitals oriented in a trigonal planar arrangement.
These hybrid orbitals are essential in the formation of sigma bonds. Each oxygen atom in employs one of its hybrid orbitals to form a sigma bond with the other oxygen atom. The remaining two hybrid orbitals on each oxygen atom hold lone pairs of electrons, which do not participate directly in bonding but influence the molecule's shape.
The unhybridized orbital that remains after hybridization is used to form the pi bond. This unhybridized orbital overlaps with the corresponding unhybridized orbital from the other oxygen atom, creating the double bond characteristic of oxygen molecules.
Thus, hybridization plays a pivotal role in the structure and bonding of oxygen in the molecule. It provides the necessary orbitals for both sigma and pi bonding, leading to a stable double-bonded framework.
These
The unhybridized
Thus,