Multiple Choice
Which of the following molecules will have a net dipole moment?
1
views
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 statements about the polar and non-polar nature of a molecule is true?
A
Non-polar molecules cannot contain any polar bonds.
B
A molecule is polar if it has polar bonds and its molecular geometry does not allow the dipoles to cancel out.
C
All molecules with polar bonds are always polar, regardless of their geometry.
D
A molecule with a symmetrical geometry is always polar.
Verified step by step guidance1
Step 1: Understand the concept of polarity in molecules. A molecule's polarity depends on both the presence of polar bonds and the overall molecular geometry, which determines if the individual bond dipoles cancel out or add up to a net dipole moment.
Step 2: Analyze the statement 'Non-polar molecules cannot contain any polar bonds.' This is false because a molecule can have polar bonds but still be non-polar if its geometry causes the dipoles to cancel each other out (e.g., carbon dioxide, CO\_2).
Step 3: Consider the statement 'A molecule is polar if it has polar bonds and its molecular geometry does not allow the dipoles to cancel out.' This is true because both polar bonds and an asymmetrical shape are required for a molecule to be polar.
Step 4: Evaluate the statement 'All molecules with polar bonds are always polar, regardless of their geometry.' This is false because molecular geometry can cause dipoles to cancel, making the molecule non-polar despite having polar bonds.
Step 5: Review the statement 'A molecule with a symmetrical geometry is always polar.' This is false because symmetrical molecules often have dipoles that cancel out, resulting in a non-polar molecule.
Related Videos
Related Practice
Molecular Polarity practice set
Problem sets built by lead tutorsExpert video explanations