Multiple Choice
Which of the following correctly represents the molecular orbital (MO) energy diagram for Li\(_2^+\), considering only the 1s and 2s atomic orbitals?
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12. Molecular Shapes & Valence Bond Theory
Molecular Orbital Theory
Multiple Choice
According to molecular orbital theory, what is the bond order of the Ne_2^{2+} ion?
A
0.5
B
1
C
2
D
0
Verified step by step guidance1
Identify the total number of electrons in the neutral Ne_2 molecule. Each neon atom has 10 electrons, so Ne_2 has 20 electrons in total.
Since the ion is Ne_2^{2+}, remove 2 electrons from the total count, resulting in 18 electrons to place in molecular orbitals.
Write the molecular orbital electron configuration for Ne_2^{2+} using the molecular orbital energy ordering for homonuclear diatomic molecules in the second period: \(\sigma_{2s}\), \(\sigma_{2s}^*\), \(\sigma_{2p_z}\), \(\pi_{2p_x} = \pi_{2p_y}\), \(\pi_{2p_x}^* = \pi_{2p_y}^*\), \(\sigma_{2p_z}^*\).
Fill the molecular orbitals with 18 electrons according to the Aufbau principle and Pauli exclusion principle, pairing electrons in lower energy orbitals first.
Calculate the bond order using the formula: \(\text{Bond order} = \frac{(\text{number of bonding electrons}) - (\text{number of antibonding electrons})}{2}\). Count the electrons in bonding and antibonding orbitals from your configuration and apply this formula.
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