energy, are o3s, 3s", T3p, 03p, T3p* and o3p*; in other words, the o2s to o2,* pattern is repeated. Determine the bond order of a Mg, molecule. 2p bond order: 2p Predict the stability of a Mg, molecule. stable 2s 2s 2s O unstable

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The energy-level diagram shown can be continued to higher energies. The next few orbitals, in order of increasing energy, are \( \sigma_{3s}, \sigma_{3s}^*, \pi_{3p}, \sigma_{3p}, \pi_{3p}^*, \) and \( \sigma_{3p}^* \); in other words, the \( \sigma_{2s} \) to \( \sigma_{2p}^* \) pattern is repeated.

**Determine the bond order of a Mg\(_2\) molecule.**

Bond order: \_\_\_\_\_\_

**Predict the stability of a Mg\(_2\) molecule.**

- [ ] stable
- [ ] unstable

### Diagram Explanation

The diagram illustrates the molecular orbital configuration for a Mg\(_2\) molecule:

- **\( \sigma_{1s} \) and \( \sigma_{1s}^* \)**: Two filled orange boxes indicate completely filled bonding and antibonding orbitals from the 1s atomic orbitals.
- **\( \sigma_{2s} \) and \( \sigma_{2s}^* \)**: Two filled orange boxes depict filled orbitals from the 2s atomic orbitals.
- **\( \pi_{2p} \) and \( \pi_{2p}^* \)**: Green rectangles show that the π bonding orbitals are filled, while the antibonding π* orbitals are not.
- **\( \sigma_{2p} \) and \( \sigma_{2p}^* \)**: One filled orange box and one unfilled indicate a filled bonding orbital but an unfilled antibonding orbital.

To find the bond order, use the formula:

\[ \text{Bond order} = \frac{\text{Number of bonding electrons} - \text{Number of antibonding electrons}}{2} \] 

The stability of a molecule typically depends on whether the bond order is greater than zero.
Transcribed Image Text:The energy-level diagram shown can be continued to higher energies. The next few orbitals, in order of increasing energy, are \( \sigma_{3s}, \sigma_{3s}^*, \pi_{3p}, \sigma_{3p}, \pi_{3p}^*, \) and \( \sigma_{3p}^* \); in other words, the \( \sigma_{2s} \) to \( \sigma_{2p}^* \) pattern is repeated. **Determine the bond order of a Mg\(_2\) molecule.** Bond order: \_\_\_\_\_\_ **Predict the stability of a Mg\(_2\) molecule.** - [ ] stable - [ ] unstable ### Diagram Explanation The diagram illustrates the molecular orbital configuration for a Mg\(_2\) molecule: - **\( \sigma_{1s} \) and \( \sigma_{1s}^* \)**: Two filled orange boxes indicate completely filled bonding and antibonding orbitals from the 1s atomic orbitals. - **\( \sigma_{2s} \) and \( \sigma_{2s}^* \)**: Two filled orange boxes depict filled orbitals from the 2s atomic orbitals. - **\( \pi_{2p} \) and \( \pi_{2p}^* \)**: Green rectangles show that the π bonding orbitals are filled, while the antibonding π* orbitals are not. - **\( \sigma_{2p} \) and \( \sigma_{2p}^* \)**: One filled orange box and one unfilled indicate a filled bonding orbital but an unfilled antibonding orbital. To find the bond order, use the formula: \[ \text{Bond order} = \frac{\text{Number of bonding electrons} - \text{Number of antibonding electrons}}{2} \] The stability of a molecule typically depends on whether the bond order is greater than zero.
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