Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

13. Liquids, Solids & Intermolecular Forces

Molecular Polarity

General Chemistry

13. Liquids, Solids & Intermolecular Forces

Molecular Polarity

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which of the following best describes the polarity of nitrogen trichloride (NCl_3)?

NCl_3 is a polar molecule because it contains ionic bonds between nitrogen and chlorine.

NCl_3 is a polar molecule because it has a lone pair on nitrogen and asymmetrical charge distribution.

NCl_3 is a nonpolar molecule because all the N–Cl bonds are identical and the molecule is symmetrical.

NCl_3 is a nonpolar molecule because nitrogen and chlorine have similar electronegativities.

Previous problemNext problem

Verified step by step guidance

Step 1: Identify the molecular geometry of nitrogen trichloride (NCl_3). Nitrogen is the central atom bonded to three chlorine atoms and has one lone pair of electrons. This results in a trigonal pyramidal shape rather than a symmetrical shape like trigonal planar or tetrahedral.

Step 2: Understand the concept of polarity. A molecule is polar if it has an uneven distribution of electron density, which usually occurs when there is an asymmetrical shape or differences in electronegativity between atoms.

Step 3: Analyze the electronegativity difference between nitrogen and chlorine. Both atoms have different electronegativities, so the N–Cl bonds are polar covalent bonds, not ionic bonds.

Step 4: Consider the effect of the lone pair on nitrogen. The lone pair creates an asymmetrical charge distribution, causing the dipole moments of the N–Cl bonds not to cancel out, resulting in a net dipole moment.

Step 5: Conclude that NCl_3 is a polar molecule due to its trigonal pyramidal shape and the presence of a lone pair on nitrogen, which leads to an asymmetrical charge distribution and a net dipole moment.