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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Transcribed Image Text:On the educational webpage, you need to use the unfilled (unpopulated) molecular-orbital (MO) diagram for a homonuclear diatomic molecule or ion, such as O₂, F₂, O₂⁺, F₂⁺, O₂⁻, or F₂⁻.
**IMPORTANT:** This diagram includes only valance orbitals.
### Diagram Overview:
The MO diagram depicted includes orbitals arranged as follows:
- **Left Side (Atomic Orbitals for One Atom):**
- 2s orbital
- 2p orbitals (three lines of equal energy)
- **Middle (Molecular Orbitals):**
- σ (sigma) 2s
- σ* (sigma star) 2s
- π (pi) 2p (two orbitals of equal energy)
- σ (sigma) 2p
- π* (pi star) 2p (two orbitals of equal energy)
- σ* (sigma star) 2p
- **Right Side (Atomic Orbitals for Another Atom):**
- 2s orbital
- 2p orbitals (three lines of equal energy)
Dashed lines connect corresponding atomic orbitals to molecular orbitals, highlighting the interactions forming the molecular orbitals.
### Instructions:
1. **Complete the Diagram:**
- Focus on the O₂⁺ molecular cation.
- Indicate the electron populations for all valance molecular orbitals on scratch paper.
2. **Determine the Bond Order:**
- After filling in the electrons, calculate the bond order.
### Question:
What is the bond order in O₂⁺?
- Options:
- 0
- 1
- 1.5
- 2
- 2.5
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