Multiple Choice
Which of the following best describes the molecular polarity of SF_4?
13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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How many of the following molecules are polar: BrCl_3, CS_2, SiF_4, SO_3?
A
2
B
3
C
1
D
4
Verified step by step guidance1
Step 1: Determine the molecular geometry of each molecule using the VSEPR theory. This involves counting the number of bonding pairs and lone pairs around the central atom to predict the shape.
Step 2: Analyze the symmetry of each molecule's shape. A symmetrical molecule with identical surrounding atoms usually results in nonpolar molecules because the dipole moments cancel out.
Step 3: Evaluate the electronegativity differences between the central atom and the surrounding atoms to determine if individual bonds are polar.
Step 4: Combine the bond polarities and molecular geometry to decide if the overall molecule has a net dipole moment (polar) or if the dipoles cancel out (nonpolar).
Step 5: Apply these principles to each molecule: BrCl_3, CS_2, SiF_4, and SO_3, then count how many are polar based on their shapes and bond polarities.
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