QQuestionChemistry
QuestionChemistry
Draw the Lewis structure for CCl^4. What is the molecular geometry of this compound? Is the molecule polar or nonpolar?
Draw the Lewis structure for CCl^4. What is the molecular geometry of this compound? Is the molecule polar or nonpolar?
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Answer
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Step 1:I'll solve this step by step using proper LaTeX formatting:
Step 2:: Determine the total number of valence electrons
• Total valence electrons: $$4 + (4 \times 7) = 32$$ electrons
• Carbon (C) has 4 valence electrons • Chlorine (Cl) has 7 valence electrons
Step 3:: Arrange the atoms
• Carbon will be the central atom • Four chlorine atoms will bond to carbon
Step 4:: Draw the Lewis structure
• Place single bonds between carbon and each chlorine • Distribute remaining electrons as lone pairs • Each chlorine will have 3 lone pairs • Lewis structure looks like: \begin{array}{c} \text{Cl} \ \downarrow \ \text{Cl-C-Cl} \ \uparrow \ \text{Cl} \end{array}
Step 5:: Determine molecular geometry
• Bond angle: $$109.5^\circ
• Carbon has 4 bonds, no lone pairs • Molecular geometry is tetrahedral
Step 6:: Polarity analysis
• Although C-Cl bonds are polar • Symmetrical tetrahedral arrangement • Net dipole moments cancel out
Final Answer
CCl^4 has a tetrahedral molecular geometry and is a nonpolar molecule.
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