6: Lewis Structures, Shapes, and Intermolecular Forces
- Page ID
- 409004
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- 6.1: The Octet Rule
- According to the octet rule, atoms will tend to lose, gain, or share electrons such that their valence electron shell resembles that of a noble gas. In most cases, the noble gas has 8 electrons in his valence shell, hence the word octet to describe the number 8.
- 6.2: Writing Lewis Structures for Covalent Compounds
- A procedure is introduced for determining Lewis structures for more complex molecules and ions.
- 6.3: Predicting the Shapes of Molecules
- The approximate shape of a molecule can be predicted from the number of electron groups and the number of surrounding atoms.
- 6.4: Electronegativity and Polarity
- Covalent bonds can be nonpolar or polar, depending on the electronegativities of the atoms involved. Molecules can be polar or nonpolar, depending both on the polarity of the bonds which make them up and the overall geometry of the molecule.
- 6.5: Intermolecular Forces- Dispersion, Dipole–Dipole, Hydrogen Bonding
- All substances experience dispersion forces between their particles. Substances that are polar experience dipole-dipole interactions. Substances with covalent bonds between an H atom and N, O, or F atoms experience hydrogen bonding. The preferred phase of a substance depends on the strength of the intermolecular force and the energy of the particles.
- 6.E: Electrons and Chemical Bonds (Exercises)
- The following questions are related to the material covered in this chapter.