Multiple Choice
Which of the following best describes the polarity of the molecule CF_4?
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 nitrogen trifluoride (NF_3)?
A
NF_3 is a polar molecule.
B
NF_3 is ionic.
C
NF_3 is a nonpolar molecule.
D
NF_3 has no net dipole moment.
Verified step by step guidance1
Step 1: Determine the molecular geometry of NF_3 by considering the central atom nitrogen (N) and its bonding with three fluorine (F) atoms. Nitrogen has one lone pair and forms three single bonds with fluorine atoms, resulting in a trigonal pyramidal shape.
Step 2: Recall that fluorine is more electronegative than nitrogen, so each N-F bond is polar with the dipole moment pointing from nitrogen toward fluorine.
Step 3: Analyze the vector sum of the bond dipoles considering the trigonal pyramidal shape. Because of the lone pair on nitrogen, the bond dipoles do not cancel out completely.
Step 4: Conclude that the molecule has a net dipole moment due to the asymmetrical shape and polar bonds, making NF_3 a polar molecule.
Step 5: Understand that NF_3 is a covalent molecule, not ionic, and since it has a net dipole moment, it is not nonpolar or without dipole moment.
Related Videos
Related Practice
Molecular Polarity practice set
Problem sets built by lead tutorsExpert video explanations