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

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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
O The larger mass and larger electron cloud means stronger LDF
O 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
Transcribed Image Text: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 O The larger mass and larger electron cloud means stronger LDF O 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
NH3, NCI3, and NF3 are all polar. Here is a data table with some additional information:
Melting Point
Molecular
Name
Boiling Point (°C)
(°C)
Geometry
Nitrogen trihydride
-77.7
-33.3
Trigonal Pyramidal
(ammonia)
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?
Transcribed Image Text:NH3, NCI3, and NF3 are all polar. Here is a data table with some additional information: Melting Point Molecular Name Boiling Point (°C) (°C) Geometry Nitrogen trihydride -77.7 -33.3 Trigonal Pyramidal (ammonia) 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?
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