QQuestionChemistry
QuestionChemistry
Draw the Lewis structure for the molecule XeF₄. Include all lone pairs of electrons. If resonance structures are needed to describe the Lewis structure, draw all possible resonance structures.
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Determine the total number of valence electrons
- Total valence electrons: $$8 + (4 \times 7) = 8 + 28 = 36$$ valence electrons
- Xe (Xenon) is in Group 18 and has 8 valence electrons - F (Fluorine) has 7 valence electrons
Step 3:: Arrange atoms and form single bonds
- Remaining electrons: $$36 - 8 = 28$$ electrons
- Place Xe in the center - Attach four F atoms to Xe with single bonds
Step 4:: Distribute remaining electrons as lone pairs
- Place 3 lone pairs on each F atom ($$3 \times 4 = 12$$ electrons)
- Remaining electrons: 28 - 12 = 16 electrons - Place the remaining 16 electrons as lone pairs on the central Xe atom
Step 5:: Lewis structure details
- Central Xe atom has 2 lone pairs - Each F atom has 3 lone pairs - All atoms have a complete octet Final Lewis Structure Representation: - Four F atoms bonded to central Xe - 3 lone pairs on each F atom - 2 lone pairs on central Xe atom
Final Answer
The Lewis structure for XeF₄ shows a square planar molecular geometry with the Xe atom in the center, four F atoms symmetrically arranged around it, with additional lone pairs as described above.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students