Westonci.ca connects you with experts who provide insightful answers to your questions. Join us today and start learning! Discover a wealth of knowledge from professionals across various disciplines on our user-friendly Q&A platform. Our platform provides a seamless experience for finding reliable answers from a network of experienced professionals.
Sagot :
Molecular Orbital Theory (MOT) provides an excellent framework for understanding the electronic structure and properties of molecules, including oxygen gas, [tex]\(O_2\)[/tex].
In the case of [tex]\(O_2\)[/tex], the molecular orbital configuration can be constructed by combining the atomic orbitals of the two oxygen atoms. Here is a step-by-step explanation:
1. Atomic Configuration of Oxygen: Each oxygen atom has an atomic number of 8, so its electronic configuration is [tex]\(1s^2 2s^2 2p^4\)[/tex].
2. Molecular Orbitals Formation: When two oxygen atoms combine, their atomic orbitals overlap to form molecular orbitals. The [tex]\(2p\)[/tex] orbitals combine to form two sets of molecular orbitals ([tex]\(\sigma\)[/tex] and [tex]\(\pi\)[/tex]) and their corresponding antibonding orbitals.
The ordering of these molecular orbitals for oxygen is:
[tex]\[ \sigma_{2s} < \sigma_{2s} < \sigma_{2p_z} < \pi_{2p_x} = \pi_{2p_y} < \pi_{2p_x} = \pi_{2p_y} < \sigma_{2p_z} \][/tex]
3. Population of Molecular Orbitals:
- The total number of electrons in [tex]\(O_2\)[/tex] is [tex]\(16\)[/tex] since each oxygen atom contributes [tex]\(8\)[/tex] electrons.
- These electrons are placed in the molecular orbitals in the following order:
[tex]\[ 2\sigma_{1s}^2, 2\sigma_{1s}^2, 2\sigma_{2s}^2, 2\sigma_{2s}^2, 2\sigma_{2p_z}^2, 4\pi_{2p_x}^2 = 4\pi_{2p_y}^2, 2\pi_{2p_x}^1 = 2\pi_{2p_y}^1 \][/tex]
4. Unpaired Electrons in [tex]\(O_2\)[/tex]: The critical observation here is the filling of the [tex]\(\pi_{2p_x}\)[/tex] and [tex]\(\pi_{2p_y}\)[/tex] orbitals. Each of these [tex]\(\pi_{2p}\)[/tex] antibonding orbitals hosts one unpaired electron.
5. Paramagnetism of [tex]\(O_2\)[/tex]: According to Molecular Orbital Theory, the presence of unpaired electrons in an orbital leads to paramagnetism. Since [tex]\(O_2\)[/tex] has two unpaired electrons in the [tex]\(\pi_{2p_x}\)[/tex] and [tex]\(\pi_{2p_y}\)[/tex] orbitals, it exhibits paramagnetism.
To summarize, the correct reason why Molecular Orbital Theory correctly predicts the paramagnetism of oxygen gas, [tex]\(O_2\)[/tex], is:
[tex]\[ \text{there are two unpaired electrons in the MO electron configuration of } O_2. \][/tex]
Therefore, the correct answer is:
- there are two unpaired electrons in the MO electron configuration of [tex]\(O_2\)[/tex].
In the case of [tex]\(O_2\)[/tex], the molecular orbital configuration can be constructed by combining the atomic orbitals of the two oxygen atoms. Here is a step-by-step explanation:
1. Atomic Configuration of Oxygen: Each oxygen atom has an atomic number of 8, so its electronic configuration is [tex]\(1s^2 2s^2 2p^4\)[/tex].
2. Molecular Orbitals Formation: When two oxygen atoms combine, their atomic orbitals overlap to form molecular orbitals. The [tex]\(2p\)[/tex] orbitals combine to form two sets of molecular orbitals ([tex]\(\sigma\)[/tex] and [tex]\(\pi\)[/tex]) and their corresponding antibonding orbitals.
The ordering of these molecular orbitals for oxygen is:
[tex]\[ \sigma_{2s} < \sigma_{2s} < \sigma_{2p_z} < \pi_{2p_x} = \pi_{2p_y} < \pi_{2p_x} = \pi_{2p_y} < \sigma_{2p_z} \][/tex]
3. Population of Molecular Orbitals:
- The total number of electrons in [tex]\(O_2\)[/tex] is [tex]\(16\)[/tex] since each oxygen atom contributes [tex]\(8\)[/tex] electrons.
- These electrons are placed in the molecular orbitals in the following order:
[tex]\[ 2\sigma_{1s}^2, 2\sigma_{1s}^2, 2\sigma_{2s}^2, 2\sigma_{2s}^2, 2\sigma_{2p_z}^2, 4\pi_{2p_x}^2 = 4\pi_{2p_y}^2, 2\pi_{2p_x}^1 = 2\pi_{2p_y}^1 \][/tex]
4. Unpaired Electrons in [tex]\(O_2\)[/tex]: The critical observation here is the filling of the [tex]\(\pi_{2p_x}\)[/tex] and [tex]\(\pi_{2p_y}\)[/tex] orbitals. Each of these [tex]\(\pi_{2p}\)[/tex] antibonding orbitals hosts one unpaired electron.
5. Paramagnetism of [tex]\(O_2\)[/tex]: According to Molecular Orbital Theory, the presence of unpaired electrons in an orbital leads to paramagnetism. Since [tex]\(O_2\)[/tex] has two unpaired electrons in the [tex]\(\pi_{2p_x}\)[/tex] and [tex]\(\pi_{2p_y}\)[/tex] orbitals, it exhibits paramagnetism.
To summarize, the correct reason why Molecular Orbital Theory correctly predicts the paramagnetism of oxygen gas, [tex]\(O_2\)[/tex], is:
[tex]\[ \text{there are two unpaired electrons in the MO electron configuration of } O_2. \][/tex]
Therefore, the correct answer is:
- there are two unpaired electrons in the MO electron configuration of [tex]\(O_2\)[/tex].
We appreciate your visit. Hopefully, the answers you found were beneficial. Don't hesitate to come back for more information. We hope you found what you were looking for. Feel free to revisit us for more answers and updated information. Thank you for trusting Westonci.ca. Don't forget to revisit us for more accurate and insightful answers.
