Both NH3, NCl3, and NF3 are all polar. Here is a data table with some additional information: Name Melting Point (°C) Boiling Point (°C) Molecular Geometry Nitrogen trihydride (ammonia) -77.7 -33.3 Trigonal Pyramidal Nitrogen trichloride -40.0 71.0 Trigonal Pyramidal Nitrogen trifluoride -207 -129 Trigonal Pyramidal Considering intermolecular forces, for what reason would nitrogen trichloride have such a high boiling point? choose one: 1.The molecular geometry makes it the most polar of the compounds 2.The larger mass and larger electron cloud means stronger LDF 3.It can participate in H-bonding 4.Unlike the other substances, it is polar. 5.The small mass means it takes less energy to break the IMF
Both NH3, NCl3, and NF3 are all polar. Here is a data table with some additional information: Name Melting Point (°C) Boiling Point (°C) Molecular Geometry Nitrogen trihydride (ammonia) -77.7 -33.3 Trigonal Pyramidal Nitrogen trichloride -40.0 71.0 Trigonal Pyramidal Nitrogen trifluoride -207 -129 Trigonal Pyramidal Considering intermolecular forces, for what reason would nitrogen trichloride have such a high boiling point? choose one: 1.The molecular geometry makes it the most polar of the compounds 2.The larger mass and larger electron cloud means stronger LDF 3.It can participate in H-bonding 4.Unlike the other substances, it is polar. 5.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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Both NH3, NCl3, and NF3 are all polar. Here is a data table with some additional information:
| Name | Melting Point (°C) | Boiling Point (°C) | Molecular Geometry |
| Nitrogen trihydride (ammonia) | -77.7 | -33.3 | Trigonal Pyramidal |
| Nitrogen trichloride | -40.0 | 71.0 | Trigonal Pyramidal |
| Nitrogen trifluoride | -207 | -129 | Trigonal Pyramidal |
Considering intermolecular forces, for what reason would nitrogen trichloride have such a high boiling point?
choose one:
1.The molecular geometry makes it the most polar of the compounds
2.The larger mass and larger electron cloud means stronger LDF
3.It can participate in H-bonding
4.Unlike the other substances, it is polar.
5.The small mass means it takes less energy to break the IMF
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