QQuestionChemistry
QuestionChemistry
For the molecule CF₄, determine the following:
Lewis structure
Bonding pairs/lone pairs
Electron geometry
Molecular shape
Polarity of the molecule
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: $$4 + (7 \times 4) = 32$$ electrons
- Carbon (C): 4 valence electrons - Fluorine (F): 7 valence electrons × 4 = 28
Step 3:: Draw the Lewis Structure
\begin{array}{c}
- Carbon will be the central atom - Four fluorine atoms will bond to carbon - Electron arrangement: F \ \downarrow \ F-C-F \ \uparrow \ F \end{array}
Step 4:: Bonding Analysis
- Total electron pairs used: $$8 + 24 = 32$$ electrons
- Bonding pairs: 4 single bonds between C and F
Step 5:: Electron Geometry
- Geometry follows $$AX_{4}$$ classification
- Central carbon has 4 bonding groups - Electron geometry is tetrahedral
Step 6:: Molecular Shape
- No lone pairs on central carbon - Molecular shape is identical to electron geometry - Tetrahedral molecular shape
Step 7:: Polarity Analysis
- C-F bonds are polar (electronegativity difference) - Symmetrical tetrahedral arrangement - Net dipole moments cancel out - Molecule is NON-POLAR
Final Answer
- Lewis Structure: Tetrahedral carbon with four single C-F bonds - Bonding Pairs: 4 single bonds - Electron Geometry: Tetrahedral - Molecular Shape: Tetrahedral - Polarity: Non-polar
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