QuestionJuly 16, 2025

49. Us ng the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders . Which ones are paramagnetic? a. Li_(2) SHOW ANSWER b. C_(2) SHOW ANSWER C. S_(2)

49. Us ng the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders . Which ones are paramagnetic? a. Li_(2) SHOW ANSWER b. C_(2) SHOW ANSWER C. S_(2)
49. Us ng the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders . Which ones are paramagnetic? a. Li_(2) SHOW ANSWER b. C_(2) SHOW ANSWER C. S_(2)

Solution
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Answer

a. Li_{2}: Bond order = 1, Diamagnetic ### b. C_{2}: Bond order = 2, Diamagnetic ### c. S_{2}: Bond order = 2, Paramagnetic Explanation 1. Write Electron Configuration for Li_{2} For Li_{2}, the electron configuration is (\sigma_{1s})^2 (\sigma_{1s}^*)^2 (\sigma_{2s})^2. 2. Calculate Bond Order for Li_{2} **Bond order** = \frac{(n_b - n_a)}{2}, where n_b is the number of bonding electrons and n_a is the number of antibonding electrons. For Li_{2}, bond order = \frac{4 - 2}{2} = 1. 3. Determine Paramagnetism for Li_{2} Li_{2} has all paired electrons, so it is **diamagnetic**. 4. Write Electron Configuration for C_{2} For C_{2}, the electron configuration is (\sigma_{1s})^2 (\sigma_{1s}^*)^2 (\sigma_{2s})^2 (\sigma_{2s}^*)^2 (\pi_{2p_x})^2 (\pi_{2p_y})^2. 5. Calculate Bond Order for C_{2} Bond order = \frac{8 - 4}{2} = 2. 6. Determine Paramagnetism for C_{2} C_{2} has all paired electrons, so it is **diamagnetic**. 7. Write Electron Configuration for S_{2} For S_{2}, the electron configuration is (\sigma_{1s})^2 (\sigma_{1s}^*)^2 (\sigma_{2s})^2 (\sigma_{2s}^*)^2 (\sigma_{2p_z})^2 (\pi_{2p_x})^2 (\pi_{2p_y})^2 (\pi_{2p_x}^*)^2 (\pi_{2p_y}^*)^2. 8. Calculate Bond Order for S_{2} Bond order = \frac{10 - 6}{2} = 2. 9. Determine Paramagnetism for S_{2} S_{2} has unpaired electrons in \pi_{2p_x}^* and \pi_{2p_y}^* orbitals, so it is **paramagnetic**.

Explanation

1. Write Electron Configuration for $Li_{2}$<br /> For $Li_{2}$, the electron configuration is $(\sigma_{1s})^2 (\sigma_{1s}^*)^2 (\sigma_{2s})^2$.<br /><br />2. Calculate Bond Order for $Li_{2}$<br /> **Bond order** = $\frac{(n_b - n_a)}{2}$, where $n_b$ is the number of bonding electrons and $n_a$ is the number of antibonding electrons. For $Li_{2}$, bond order = $\frac{4 - 2}{2} = 1$.<br /><br />3. Determine Paramagnetism for $Li_{2}$<br /> $Li_{2}$ has all paired electrons, so it is **diamagnetic**.<br /><br />4. Write Electron Configuration for $C_{2}$<br /> For $C_{2}$, the electron configuration is $(\sigma_{1s})^2 (\sigma_{1s}^*)^2 (\sigma_{2s})^2 (\sigma_{2s}^*)^2 (\pi_{2p_x})^2 (\pi_{2p_y})^2$.<br /><br />5. Calculate Bond Order for $C_{2}$<br /> Bond order = $\frac{8 - 4}{2} = 2$.<br /><br />6. Determine Paramagnetism for $C_{2}$<br /> $C_{2}$ has all paired electrons, so it is **diamagnetic**.<br /><br />7. Write Electron Configuration for $S_{2}$<br /> For $S_{2}$, the electron configuration is $(\sigma_{1s})^2 (\sigma_{1s}^*)^2 (\sigma_{2s})^2 (\sigma_{2s}^*)^2 (\sigma_{2p_z})^2 (\pi_{2p_x})^2 (\pi_{2p_y})^2 (\pi_{2p_x}^*)^2 (\pi_{2p_y}^*)^2$.<br /><br />8. Calculate Bond Order for $S_{2}$<br /> Bond order = $\frac{10 - 6}{2} = 2$.<br /><br />9. Determine Paramagnetism for $S_{2}$<br /> $S_{2}$ has unpaired electrons in $\pi_{2p_x}^*$ and $\pi_{2p_y}^*$ orbitals, so it is **paramagnetic**.
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