Considering intermolecular forces, for what reason would nitrogen trichloride have such a highboiling point?The molecular geometry makes it the most polar of the compoundsO The larger mass and larger electron cloud means stronger LDFO It can participate in H-bondingUnlike the other substances, it is polar.The small mass means it takes less energy to break the IMF NH3, NCI3, and NF3 are all polar. Here is a data table with some additional information:Melting PointMolecularNameBoiling Point (°C)(°C)GeometryNitrogen trihydride-77.7-33.3Trigonal Pyramidal(ammonia)Nitrogen trichloride-40.071.0Trigonal PyramidalNitrogen trifluoride-207-129Trigonal PyramidalConsidering intermolecular forces, for what reason would nitrogen trichloride have such a highboiling point?

NCl3 have higher boiling point in comparison to NH3 and NF3.

Considering intermolecular forces, for what reason would nitrogen trichloride have such a high boiling point? The molecular geometry makes it the most polar of the compounds The larger mass and larger electron cloud means stronger LDF It can participate in H-bonding Unlike the other substances, it is polar. The small mass means it takes less energy to break the IMF

Considering intermolecular forces, for what reason would nitrogen trichloride have such a high boiling point? The molecular geometry makes it the most polar of the compounds The larger mass and larger electron cloud means stronger LDF It can participate in H-bonding Unlike the other substances, it is polar. The small mass means it takes less energy to break the IMF

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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