Textbook Question
Aspirin has the following connections among atoms. Completethe electron-dot structure for aspirin, tell how many s bondsand how many p bonds the molecule contains, and tell thehybridization of each carbon atom.
Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure
All textbooks
McMurry 8th EditionCh.8 - Covalent Compounds: Bonding Theories and Molecular StructureProblem 96
McMurry 8th EditionCh.8 - Covalent Compounds: Bonding Theories and Molecular StructureProblem 96Chapter 8, Problem 96
What is the difference in spatial distribution between electrons in a bonding MO and electrons in an antibonding MO?
Verified step by step guidance1
1. Molecular Orbitals (MOs) are formed when atomic orbitals overlap. The overlap can be constructive or destructive. Constructive overlap leads to the formation of bonding MOs, while destructive overlap leads to the formation of antibonding MOs.
2. In a bonding MO, the electron density is concentrated between the two nuclei. This is because the wave functions of the atomic orbitals combine constructively, leading to an increase in electron density between the nuclei. This increased electron density helps to hold the two nuclei together, hence the term 'bonding'.
3. On the other hand, in an antibonding MO, the electron density is found primarily outside the region between the two nuclei. This is due to the destructive combination of the wave functions of the atomic orbitals, which leads to a node (a region of zero electron density) between the nuclei. This lack of electron density between the nuclei does not help to hold them together, hence the term 'antibonding'.
4. Therefore, the main difference in spatial distribution between electrons in a bonding MO and electrons in an antibonding MO is that in a bonding MO, the electron density is concentrated between the nuclei, while in an antibonding MO, the electron density is found outside the region between the nuclei.
5. This difference in spatial distribution is crucial as it determines whether a molecular orbital will contribute to the formation of a chemical bond (in the case of a bonding MO) or hinder it (in the case of an antibonding MO).
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Orbitals (MOs)
Molecular orbitals are formed by the combination of atomic orbitals when atoms bond together. They can be classified as bonding or antibonding. Bonding MOs are lower in energy and result from the constructive interference of atomic orbitals, leading to increased electron density between the nuclei, which stabilizes the molecule. Antibonding MOs, on the other hand, arise from destructive interference and have higher energy, resulting in decreased electron density between the nuclei.
Recommended video:
Guided course
03:06
Molecular Orbital Theory
Spatial Distribution of Electrons
The spatial distribution of electrons in molecular orbitals refers to how electron density is arranged in relation to the nuclei of the bonded atoms. In bonding MOs, electron density is concentrated in the region between the nuclei, promoting attraction and stability. Conversely, in antibonding MOs, electron density is found outside the internuclear region, which can lead to repulsion between the nuclei and destabilization of the molecule.
Recommended video:
Guided course
01:30Spatial Orientation of Bonds
Energy Levels of MOs
The energy levels of molecular orbitals play a crucial role in determining the stability of a molecule. Bonding MOs are lower in energy compared to the original atomic orbitals, making them favorable for electron occupancy. Antibonding MOs, being higher in energy, are less stable and can destabilize a molecule if occupied by electrons. The filling of these orbitals according to the Aufbau principle influences the overall bond order and stability of the molecule.
Recommended video:
Guided course
03:46Homonuclear Diatomic Molecules MO Diagram Example
Related Practice
Textbook Question
The odor of cinnamon oil is due to cinnamaldehyde, C9H8O. What is the hybridization of each carbon atom in cinnamaldehyde? How many s and how many p bonds does cinnamaldehyde have?
Textbook Question
The following molecular model is a representation of caffeine. Identify the position(s) of multiple bonds in caffeine, and tell the hybridization of each carbon atom. 1Red = O, blue = N, gray = C, ivory = H.2
Textbook Question
For a given type of MO, use a s2s as an example, is the bonding or antibonding orbital higher in energy? Explain.
Textbook Question
Use the MO energy diagram in Figure 8.22b to describe thebonding in O2+, O2, and O2-. Which of the three is likely tobe stable? What is the bond order of each? Which containunpaired electrons?
Textbook Question
The C2 molecule can be represented by an MO diagram similar to that in Figure 8.22a. (b) To increase the bond order of C2, should you add or remove an electron?