Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the neutral compound S2F2?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
After drawing the Lewis structure of CCl4, determine whether the molecule is polar or nonpolar.
A
CCl4 is ionic.
B
CCl4 is a polar molecule.
C
CCl4 has both polar and nonpolar bonds.
D
CCl4 is a nonpolar molecule.
Verified step by step guidance1
Step 1: Draw the Lewis structure of CCl\_4 by placing the carbon atom in the center and surrounding it with four chlorine atoms, each connected by a single bond. Carbon has 4 valence electrons, and each chlorine has 7 valence electrons, so the structure satisfies the octet rule for all atoms.
Step 2: Identify the type of bonds between carbon and chlorine. Since chlorine is more electronegative than carbon, each C–Cl bond is polar, with a dipole moment pointing from carbon to chlorine.
Step 3: Analyze the molecular geometry of CCl\_4. The molecule has a tetrahedral shape because there are four bonding pairs and no lone pairs on the central carbon atom, leading to bond angles of approximately 109.5°.
Step 4: Determine the overall polarity by considering the symmetry of the molecule. In a tetrahedral geometry with four identical polar bonds symmetrically arranged, the individual bond dipoles cancel each other out.
Step 5: Conclude that despite having polar bonds, the symmetrical arrangement causes the dipoles to cancel, making CCl\_4 a nonpolar molecule overall.
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