QQuestionAnatomy and Physiology
QuestionAnatomy and Physiology
1. Draw the Lewis structure for $\mathrm{ICI}_{4}{ }^{-}$in the window below and then answer the questions that follow.
- Do not include overall ion charges or formal charges in your drawing.
2. Draw the Lewis structure for $\mathbf{S O}_{3}$ in the window below and then answer the questions that follow.
- Do not include overall ion charges or formal charges in your drawing.
- Do not draw double bonds to oxygen atoms unless they are needed for the central atom to obey the octet rule.
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Step 1I'll solve this problem step by step for both Lewis structures, following the precise LaTeX formatting guidelines:
For $$\mathrm{ICI}_{4}^{-}$$ Lewis Structure:
Step 2: Count total valence electrons
- Total valence electrons: $$7 + 28 + 1 = 36$$ electrons
- Iodine (I): 7 valence electrons - Chlorine (Cl): 7 valence electrons × 4 = 28 - Negative charge adds 1 electron
Final Answer
- For \mathrm{ICI}_{4}^{-}: A Lewis structure with iodine at center, four chlorines bonded, with additional lone pairs - For \mathrm{SO}_{3}: A Lewis structure with sulfur at center, three oxygen atoms bonded, potentially with double bonds to satisfy octet rule Note: Precise visual representation would require drawing the actual Lewis structure, which cannot be done in text format.
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