Determine the intermolecular forces for each of the following molecules: Compound N₂ CH4 CH3CI H₂O HF CCl4 NH3 NF3 total valance electrons Lewis Structure Molecular Geometry For a molecule to be polar, it must satisfy the following two requirements: 1. The molecule must have polar bonds 2. The molecule must have a lack of symmetry, so the bond dipoles do not cancel each other. The lack of symmetry will exist if the central atom is bonded to different elements, and/or contains at least one lone pair. 1. Does the molecule contain polar bonds? yes or no? 2. Does the molecule have a lack of symmetry? yes or no? Is the molecule polar? yes or no? Dominant Intermolecular Force for Molecul

Determine the intermolecular forces for each of the following molecules: Compound N₂ CH4 CH3CI H₂O HF CCl4 NH3 NF3 total valance electrons Lewis Structure Molecular Geometry For a molecule to be polar, it must satisfy the following two requirements: 1. The molecule must have polar bonds 2. The molecule must have a lack of symmetry, so the bond dipoles do not cancel each other. The lack of symmetry will exist if the central atom is bonded to different elements, and/or contains at least one lone pair. 1. Does the molecule contain polar bonds? yes or no? 2. Does the molecule have a lack of symmetry? yes or no? Is the molecule polar? yes or no? Dominant Intermolecular Force for Molecul

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter8: Molecules And Materials

Section: Chapter Questions

Problem 8.43PAE: 8.43 Identify the kinds of intermolecular forces (London dispersion, dipoledipole, or hydrogen...

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