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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![**Title: Calculating the Bond Order for OF⁻ Using the Molecular Orbital Diagram**
**Introduction:**
To determine the bond order of the OF⁻ ion, we can utilize the molecular orbital (MO) diagram. This diagram represents the relative energy levels of molecular orbitals formed from the atomic orbitals of oxygen and fluorine.
**Molecular Orbital Diagram Overview:**
The MO diagram for OF⁻ features both bonding and antibonding orbitals. These orbitals are formed from the combination of atomic orbitals of the oxygen and fluorine atoms. The positions of these orbitals on the diagram typically correspond to their relative energy levels.
**List of Orbitals in the Diagram:**
1. **σ\*_p** - Highest energy antibonding sigma orbital formed from p orbitals.
2. **π\*_p (two orbitals)** - Antibonding pi orbitals.
3. **π_p (two orbitals)** - Bonding pi orbitals.
4. **σ_p** - Bonding sigma orbital formed from p orbitals.
5. **σ\*_s** - Antibonding sigma orbital formed from s orbitals.
6. **σ_s** - Bonding sigma orbital formed from s orbitals.
**Explaining the Diagram:**
- **σ and π Orbitals:** The σ (sigma) orbitals are typically associated with direct overlapping of atomic orbitals along the internuclear axis, while π (pi) orbitals result from parallel overlapping.
- **Bonding and Antibonding Distinction:** Bonding orbitals (σ, π) are lower in energy and help stabilize the molecule, whereas antibonding orbitals (σ\*, π\*) are higher in energy and can destabilize the molecule if occupied by electrons.
**Calculating Bond Order:**
The bond order is calculated using the formula:
\[ \text{Bond Order} = \frac{(\text{Number of electrons in bonding MOs} - \text{Number of electrons in antibonding MOs})}{2} \]
**Conclusion:**
By counting the electrons in the molecular orbitals for OF⁻ and applying the bond order formula, we can quantitatively determine the bond characteristics between oxygen and fluorine in the ion. Understanding and interpreting MO diagrams is crucial for predicting molecular stability and reactivity.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2c653cb9-ab7a-49e3-bea3-1c34e4b2ce5f%2F6f0b93c7-981b-4f3c-83c3-94a536d4e234%2F3umnix_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Calculating the Bond Order for OF⁻ Using the Molecular Orbital Diagram**
**Introduction:**
To determine the bond order of the OF⁻ ion, we can utilize the molecular orbital (MO) diagram. This diagram represents the relative energy levels of molecular orbitals formed from the atomic orbitals of oxygen and fluorine.
**Molecular Orbital Diagram Overview:**
The MO diagram for OF⁻ features both bonding and antibonding orbitals. These orbitals are formed from the combination of atomic orbitals of the oxygen and fluorine atoms. The positions of these orbitals on the diagram typically correspond to their relative energy levels.
**List of Orbitals in the Diagram:**
1. **σ\*_p** - Highest energy antibonding sigma orbital formed from p orbitals.
2. **π\*_p (two orbitals)** - Antibonding pi orbitals.
3. **π_p (two orbitals)** - Bonding pi orbitals.
4. **σ_p** - Bonding sigma orbital formed from p orbitals.
5. **σ\*_s** - Antibonding sigma orbital formed from s orbitals.
6. **σ_s** - Bonding sigma orbital formed from s orbitals.
**Explaining the Diagram:**
- **σ and π Orbitals:** The σ (sigma) orbitals are typically associated with direct overlapping of atomic orbitals along the internuclear axis, while π (pi) orbitals result from parallel overlapping.
- **Bonding and Antibonding Distinction:** Bonding orbitals (σ, π) are lower in energy and help stabilize the molecule, whereas antibonding orbitals (σ\*, π\*) are higher in energy and can destabilize the molecule if occupied by electrons.
**Calculating Bond Order:**
The bond order is calculated using the formula:
\[ \text{Bond Order} = \frac{(\text{Number of electrons in bonding MOs} - \text{Number of electrons in antibonding MOs})}{2} \]
**Conclusion:**
By counting the electrons in the molecular orbitals for OF⁻ and applying the bond order formula, we can quantitatively determine the bond characteristics between oxygen and fluorine in the ion. Understanding and interpreting MO diagrams is crucial for predicting molecular stability and reactivity.
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