QQuestionChemistry
QuestionChemistry
Using the molecular orbital model to describe the bonding in F^2 + 2 , F^2, and F^2−2, predict the bond orders and the relative bond lengths for these three species. How many unpaired electrons are present in each species?
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Answer
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Step 1:Let's solve this problem step by step using molecular orbital theory:
Step 2:: Determine the electron configuration for F atom
- Electron configuration: $$1s^{2} 2s^{2} 2p^{5}
- Atomic number of F is 9 - Valence electrons: 7 electrons
Step 3:: Construct molecular orbital diagram for F^2
\sigma_{1s}^{2} \sigma^{*}_{1s}^{2} \sigma_{2s}^{2} \sigma^{*}_{2s}^{2} \pi_{2p_{x}}^{2} \pi_{2p_{y}}^{2} \sigma_{2p_{z}}^{2} \pi^{*}_{2p_{x}}^{1} \pi^{*}_{2p_{y}}^{1}
- Molecular orbital filling order:
Step 4:: Calculate bond orders
- Bond order: $$\frac{1}{2}(10 - 6) = 2
F^2 + 2: - Total electrons: 12 - Unpaired electrons: 2 F^2: - Total electrons: 14 - Unpaired electrons: 0 F^2−2: - Total electrons: 16 - Unpaired electrons: 0
Step 5:: Predict relative bond lengths
- Bond order is inversely proportional to bond length - F^2 + 2 (bond order 3): Shortest bond - F^2 (bond order 3): Same length as F^2 + 2 - F^2−2 (bond order 2): Longest bond
Final Answer
- F^2 + 2: Bond order = 3, 2 unpaired electrons, shortest bond - F^2: Bond order = 3, 0 unpaired electrons, intermediate bond length - F^2−2: Bond order = 2, 0 unpaired electrons, longest bond
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