(11.8) Use the molecular orbital diagram shown, answer the following questions. a) Determine the bond order of C₂. b) Is C₂ paramagnetic or diamagnetic? Atomic orbitals 2p 2s Molecular orbitals I Tip 2p #2p afs σip B₂, C₂ N₂ 2s Atomic orbitals 2p
(11.8) Use the molecular orbital diagram shown, answer the following questions. a) Determine the bond order of C₂. b) Is C₂ paramagnetic or diamagnetic? Atomic orbitals 2p 2s Molecular orbitals I Tip 2p #2p afs σip B₂, C₂ N₂ 2s Atomic orbitals 2p
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
![### Molecular Orbital Theory
#### Example Question:
(11.8) Use the molecular orbital diagram shown to answer the following questions:
a) Determine the bond order of \( \text{C}_2^- \).
b) Is \( \text{C}_2^- \) paramagnetic or diamagnetic?
#### Molecular Orbital Diagram Explanation:
The diagram provided shows the molecular orbitals for diatomic molecules involving elements like Boron (\( \text{B}_2 \)), Carbon (\( \text{C}_2 \)), and Nitrogen (\( \text{N}_2 \)). The diagram includes atomic orbitals on the left and right sides labeled as "Atomic Orbitals" and molecular orbitals in the center labeled as "Molecular Orbitals".
##### Detailed Breakdown of the Molecular Orbitals:
1. **Atomic Orbitals (Left and Right):**
- 2s and 2p orbitals are shown for each atom.
2. **Molecular Orbitals (Center):**
- The molecular orbitals are arranged from bottom to top in the following order:
- \( \sigma_{2s} \)
- \( \sigma_{2s}^* \)
- \( \pi_{2p} \)
- \( \sigma_{2p} \)
- \( \pi_{2p}^* \)
- \( \sigma_{2p}^* \)
3. **Electron Configuration for \( \text{C}_2^- \):**
- The added electron in \( \text{C}_2^- \) must be placed in the appropriate molecular orbital according to Hund's rule and the Pauli exclusion principle.
#### Steps to Determine the Bond Order:
1. **Count the number of electrons in bonding molecular orbitals** and **non-bonding molecular orbitals**.
2. **Use the formula for bond order**:
\[
\text{Bond Order} = \frac{\text{Number of electrons in bonding MOs} - \text{Number of electrons in anti-bonding MOs}}{2}
\]
##### Example Calculation for \( \text{C}_2^- \):
- Considering the total number of valence electrons and the added electron due to the negative charge.
#### Magnetism:
- Determine if \( \text{C}_2^- \) is paramagnetic or diamagnetic by checking for unpaired electrons in the](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8ace3a86-4905-4025-b5a4-d5dbea0f3d2b%2F7a80351c-032f-421c-9bd5-8c0d09173d0d%2F0y5c1m9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Molecular Orbital Theory
#### Example Question:
(11.8) Use the molecular orbital diagram shown to answer the following questions:
a) Determine the bond order of \( \text{C}_2^- \).
b) Is \( \text{C}_2^- \) paramagnetic or diamagnetic?
#### Molecular Orbital Diagram Explanation:
The diagram provided shows the molecular orbitals for diatomic molecules involving elements like Boron (\( \text{B}_2 \)), Carbon (\( \text{C}_2 \)), and Nitrogen (\( \text{N}_2 \)). The diagram includes atomic orbitals on the left and right sides labeled as "Atomic Orbitals" and molecular orbitals in the center labeled as "Molecular Orbitals".
##### Detailed Breakdown of the Molecular Orbitals:
1. **Atomic Orbitals (Left and Right):**
- 2s and 2p orbitals are shown for each atom.
2. **Molecular Orbitals (Center):**
- The molecular orbitals are arranged from bottom to top in the following order:
- \( \sigma_{2s} \)
- \( \sigma_{2s}^* \)
- \( \pi_{2p} \)
- \( \sigma_{2p} \)
- \( \pi_{2p}^* \)
- \( \sigma_{2p}^* \)
3. **Electron Configuration for \( \text{C}_2^- \):**
- The added electron in \( \text{C}_2^- \) must be placed in the appropriate molecular orbital according to Hund's rule and the Pauli exclusion principle.
#### Steps to Determine the Bond Order:
1. **Count the number of electrons in bonding molecular orbitals** and **non-bonding molecular orbitals**.
2. **Use the formula for bond order**:
\[
\text{Bond Order} = \frac{\text{Number of electrons in bonding MOs} - \text{Number of electrons in anti-bonding MOs}}{2}
\]
##### Example Calculation for \( \text{C}_2^- \):
- Considering the total number of valence electrons and the added electron due to the negative charge.
#### Magnetism:
- Determine if \( \text{C}_2^- \) is paramagnetic or diamagnetic by checking for unpaired electrons in the
Transcribed Image Text:This image presents multiple-choice questions regarding bond order and magnetic properties of molecules. Below is the transcribed text from the image:
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**Question: Determine the bond order and magnetic property of the given molecule.**
1. ⃝ a) bond order = 2.0 b) paramagnetic
2. ⃝ a) bond order = 2.0 b) diamagnetic
3. ⃝ a) bond order = 1.5 b) paramagnetic
4. ⃝ a) bond order = 2.5 b) paramagnetic
---
### Explanation:
Each option consists of two parts:
- **Bond Order**: This indicates the number of chemical bonds between a pair of atoms. For example, a bond order of 2.0 means a double bond, 1.5 is an intermediate bond strength between single and double bonds, and 2.5 indicates a bond order stronger than a double bond.
- **Magnetic Properties**:
- **Paramagnetic**: Substances that have one or more unpaired electrons and are attracted by a magnetic field.
- **Diamagnetic**: Substances that have all electrons paired and are not attracted, but are slightly repelled by a magnetic field.
These questions test the understanding of molecular orbital theory and the relationship between electronic configuration, bond order, and magnetic properties.
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