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Ch.12 - Liquids, Solids & Intermolecular Forces
Tro - Chemistry: A Molecular Approach 5th Edition
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Tutti i libri di testoTro 5th EditionCh.12 - Liquids, Solids & Intermolecular ForcesProblema 36b
Capitolo 12, Problema 36b

Determine the kinds of intermolecular forces that are present in each element or compound. b. NCl3

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Identify the molecular structure of NCl_3. It is a trigonal pyramidal molecule with nitrogen at the center and three chlorine atoms bonded to it.
Determine the polarity of the molecule. NCl_3 is a polar molecule because the nitrogen-chlorine bonds are polar due to the difference in electronegativity between nitrogen and chlorine.
Recognize the types of intermolecular forces present in polar molecules. Polar molecules like NCl_3 exhibit dipole-dipole interactions due to the presence of permanent dipoles.
Consider the presence of London dispersion forces. All molecules, including NCl_3, have London dispersion forces, which are weak intermolecular forces arising from temporary dipoles.
Conclude that NCl_3 exhibits both dipole-dipole interactions and London dispersion forces as its intermolecular forces.

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Intermolecular Forces

Intermolecular forces are the attractive forces between molecules that influence physical properties such as boiling and melting points. These forces include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Understanding these interactions is crucial for predicting the behavior of substances in different states of matter.
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Intermolecular vs Intramolecular Forces

Polarity

Polarity refers to the distribution of electrical charge over the atoms in a molecule. A molecule is polar if it has a significant difference in electronegativity between its atoms, leading to a dipole moment. In the case of NCl3, the nitrogen atom is less electronegative than chlorine, resulting in a polar molecule that exhibits dipole-dipole interactions.
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Molecular Polarity

Molecular Geometry

Molecular geometry describes the three-dimensional arrangement of atoms within a molecule. The shape of a molecule affects its polarity and the types of intermolecular forces it can exhibit. For NCl3, the trigonal pyramidal shape influences its dipole moment and the presence of dipole-dipole interactions, as well as potential London dispersion forces due to its molecular size.
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Molecular Geometry with Two Electron Groups
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