QQuestionChemistry
QuestionChemistry
Predict the shape and bond angle for the compound carbon tetrafluoride, CF^4.
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 Central Atom and Valence Electrons
- Total valence electrons: $$4 + (4 \times 7) = 32$$ electrons
- The central atom is carbon (C) - Carbon has 4 valence electrons - Fluorine (F) has 7 valence electrons
Step 3:: Draw the Lewis Structure
- Carbon will form 4 single bonds with fluorine atoms - Each fluorine atom will have 3 lone pairs - Total electron arrangement follows the octet rule
Step 4:: Apply VSEPR Theory
- Count electron domains around the central carbon - 4 bonding domains (C-F bonds) - 0 lone pair domains - Total electron domains: 4
Step 5:: Predict Molecular Geometry
- With 4 electron domains and 0 lone pairs - Molecular geometry is tetrahedral - Electron domain geometry is also tetrahedral
Step 6:: Determine Bond Angle
- Bond angle between any two bonds is $$109.5^\circ
- In a perfect tetrahedral arrangement
Final Answer
- Shape: Tetrahedral - Bond Angle: 109.5^\circ
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