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

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Multiple Choice

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

NCl_3 is a nonpolar molecule.

NCl_3 is ionic.

NCl_3 is amphiprotic.

NCl_3 is a polar molecule.

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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 it has one lone pair of electrons. This gives NCl_3 a trigonal pyramidal shape.

Step 2: Consider the electronegativity difference between nitrogen and chlorine. Chlorine is more electronegative than nitrogen, so each N–Cl bond is polar with a dipole moment pointing toward the chlorine atoms.

Step 3: Analyze the symmetry of the molecule. Because of the lone pair on nitrogen, the molecule is not symmetrical, so the individual bond dipoles do not cancel out.

Step 4: Conclude that due to the asymmetrical shape and polar bonds, NCl_3 has a net dipole moment, making it a polar molecule.

Step 5: Understand why the other options are incorrect: NCl_3 is not ionic because it involves covalent bonds; it is not amphiprotic because it does not donate or accept protons; and it is not nonpolar due to its molecular geometry and bond polarity.