Multiple Choice
Which of the following best describes the molecular polarity of SCl_2?
13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following molecules is nonpolar?
A
NH3
B
H2O
C
SO2
D
CO2
Verified step by step guidance1
Step 1: Understand the concept of molecular polarity. A molecule is polar if it has a net dipole moment, which occurs when there is an uneven distribution of electron density due to differences in electronegativity and molecular geometry.
Step 2: Analyze the molecular geometry of each molecule using VSEPR theory. NH3 has a trigonal pyramidal shape, H2O has a bent shape, SO2 has a bent shape, and CO2 has a linear shape.
Step 3: Consider the electronegativity differences and the symmetry of the molecules. NH3, H2O, and SO2 have polar bonds and asymmetrical shapes, which result in a net dipole moment making them polar.
Step 4: For CO2, although the C=O bonds are polar, the molecule is linear and symmetrical, so the dipoles cancel each other out, resulting in a nonpolar molecule.
Step 5: Conclude that CO2 is nonpolar due to its linear geometry and symmetrical distribution of polar bonds, while the other molecules are polar because of their bent or pyramidal shapes causing an overall dipole moment.
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