**Educational Content on Molecular Orbital Theory:** **Procedure: Answer the following questions related to Molecular Orbital Theory.** 1) The Molecular Orbital diagram for He₂⁺ is shown. a) **Identify the bond order:** Bond order: __________ b) **Identify if this molecule is paramagnetic or diamagnetic.** Answer: __________ --- **Description of Diagram:** The diagram is a molecular orbital (MO) diagram for the He₂⁺ ion. It illustrates the energy levels and the interactions between atomic orbitals as they combine to form molecular orbitals. - **Vertical Axis (Energy):** Represents the relative energy levels. Higher positions indicate higher energy. - **Left Side:** - The 1s atomic orbital of a helium atom. - The energy level is occupied by two electrons, represented by two arrows (one up, one down), signifying paired electrons. - **Right Side:** - The 1s atomic orbital of a helium ion. - The energy level is not occupied, indicating an absence of electrons. - **Center:** - σ (sigma) 1s bonding molecular orbital with one electron. - σ* (sigma star) 1s antibonding molecular orbital, which is not occupied. - The single electron in the σ 1s bonding orbital suggests a bond between the helium atom and the helium ion. **Explanation:** - **Bond Order Calculation:** - The bond order is calculated using the formula: \[ \text{Bond Order} = \frac{(\text{Number of electrons in bonding MOs}) - (\text{Number of electrons in antibonding MOs})}{2} \] - **Magnetic Property:** - A molecule is **paramagnetic** if it has unpaired electrons and **diamagnetic** if all electrons are paired. Based on the diagram, determine whether the He₂⁺ ion is paramagnetic or diamagnetic.

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