### Construct the Molecular Orbital Diagram for \( \text{H}_2^- \)The diagram above illustrates the molecular orbital (MO) energy levels for the \( \text{H}_2^- \) ion.- **Atomic Orbitals (AO):** - The diagram starts with hydrogen atom orbitals labeled as \( 1s \) on both sides. Each hydrogen atom A has one electron in its 1s orbital.- **Molecular Orbitals:** - The molecular orbitals (\( \sigma_{1s} \) and \( \sigma^*_{1s} \)) are formed by the combination of these atomic orbitals. - **\( \sigma_{1s} \):** This is a bonding molecular orbital and is lower in energy. - **\( \sigma^*_{1s} \):** This is an antibonding molecular orbital and is higher in energy.- **Electron Configuration:** - Electrons are then placed in these molecular orbitals according to the Aufbau principle, starting with the lowest energy level. - Ensure to fill in all electrons from the available answer bank.### Answer Bank- This section includes two electron options: one electron with a single arrow \( \uparrow \) and another option with a double arrow \( \uparrow\downarrow \), suggesting one position can be filled completely.### Identify the Bond OrderTo determine the bond order, use the formula:\[\text{Bond Order} = \frac{(\text{Number of electrons in bonding MOs} - \text{Number of electrons in antibonding MOs})}{2}\]- Options for bond order are: - 0 - 0.5 - 1 - 1.5 - 2Select the bond order based on the electron placements in the molecular orbitals.

Answered: Construct the molecular orbital diagram…

Construct the molecular orbital diagram for H,. H H; H- Answer Bank 1 11 1s 1s 1s Identify the bond order. 0.5 1 1.5 O O O O

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

### Construct the Molecular Orbital Diagram for \( \text{H}_2^- \)

The diagram above illustrates the molecular orbital (MO) energy levels for the \( \text{H}_2^- \) ion.

- **Atomic Orbitals (AO):**
- The diagram starts with hydrogen atom orbitals labeled as \( 1s \) on both sides. Each hydrogen atom A has one electron in its 1s orbital.

- **Molecular Orbitals:**
- The molecular orbitals (\( \sigma_{1s} \) and \( \sigma^*_{1s} \)) are formed by the combination of these atomic orbitals.
- **\( \sigma_{1s} \):** This is a bonding molecular orbital and is lower in energy.
- **\( \sigma^*_{1s} \):** This is an antibonding molecular orbital and is higher in energy.

- **Electron Configuration:**
- Electrons are then placed in these molecular orbitals according to the Aufbau principle, starting with the lowest energy level.
- Ensure to fill in all electrons from the available answer bank.

### Answer Bank

- This section includes two electron options: one electron with a single arrow \( \uparrow \) and another option with a double arrow \( \uparrow\downarrow \), suggesting one position can be filled completely.

### Identify the Bond Order

To determine the bond order, use the formula:

\[
\text{Bond Order} = \frac{(\text{Number of electrons in bonding MOs} - \text{Number of electrons in antibonding MOs})}{2}
\]

- Options for bond order are:
- 0
- 0.5
- 1
- 1.5
- 2

Select the bond order based on the electron placements in the molecular orbitals.

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