QQuestionChemistry
QuestionChemistry
F₂ is diamagnetic while O₂ is paramagnetic. Explain this on the basis of molecular orbital theory.
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Answer
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Step 1:I'll solve this problem step by step, explaining the molecular orbital theory behind the magnetic properties of F₂ and O₂.
Step 2:: Understand Molecular Orbital Theory Basics
Molecular orbital theory describes how atomic orbitals combine to form molecular orbitals. The electronic configuration of these orbitals determines the magnetic properties of molecules.
Step 3:: Electron Configuration of F₂
(\sigma_{1s})^{2}(\sigma^{*}_{1s})^{2}(\sigma_{2s})^{2}(\sigma^{*}_{2s})^{2}(\sigma_{2p})^{2}(\pi_{2p})^{4}(\pi^{*}_{2p})^{0}
For F₂, the electron configuration is:
Step 4:: Analyze F₂ Electron Pairing
In F₂, all molecular orbitals are completely filled and paired. This means: - All electrons are paired - No unpaired electrons exist - Paired electrons have opposite spins - Result: Diamagnetic behavior
Step 5:: Electron Configuration of O₂
(\sigma_{1s})^{2}(\sigma^{*}_{1s})^{2}(\sigma_{2s})^{2}(\sigma^{*}_{2s})^{2}(\sigma_{2p})^{2}(\pi_{2p})^{4}(\pi^{*}_{2p})^{2}
For O₂, the electron configuration is:
Step 6:: Analyze O₂ Electron Pairing
- The $$\pi^{*}_{2p}$$ orbitals have two unpaired electrons
In O₂: - Unpaired electrons have parallel spins - Result: Paramagnetic behavior
Final Answer
F₂ is diamagnetic due to all electrons being paired, while O₂ is paramagnetic due to two unpaired electrons in its \pi^{*}_{2p} molecular orbitals.
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