Multiple Choice
Which of the following best describes the molecular polarity of CH2F2 (difluoromethane)?
13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which of the following best describes the polarity of a carbon dioxide (CO_2) molecule?
A
CO_2 is a polar molecule because it contains polar bonds.
B
CO_2 is a polar molecule because it has a bent molecular geometry.
C
CO_2 is a nonpolar molecule because it contains only nonpolar bonds.
D
CO_2 is a nonpolar molecule because its linear shape causes the dipoles to cancel.
Verified step by step guidance1
Step 1: Identify the molecular geometry of CO_2. Carbon dioxide has a central carbon atom double bonded to two oxygen atoms, and the molecule is linear in shape due to the arrangement of electron pairs around the carbon atom.
Step 2: Determine the polarity of the individual bonds. The C=O bonds are polar because oxygen is more electronegative than carbon, creating dipole moments pointing from carbon to oxygen.
Step 3: Analyze the overall molecular polarity by considering the vector sum of the bond dipoles. Since CO_2 is linear, the two bond dipoles are equal in magnitude but point in opposite directions.
Step 4: Understand that because the bond dipoles are equal and opposite, they cancel each other out, resulting in no net dipole moment for the molecule.
Step 5: Conclude that despite having polar bonds, the linear geometry of CO_2 causes the dipoles to cancel, making the molecule nonpolar overall.
Related Videos
Related Practice
Molecular Polarity practice set
Problem sets built by lead tutorsExpert video explanations