crystal-properties-handout - Ionic, H-bonding, Dipole, or...

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Ionic, H Ionic, H -bonding, Dipole, or London? bonding, Dipole, or London? ionic* Ionic ionic Δ EN = 1.7 - 3.2 London nonpolar -- Symmetrical molecule (any Δ EN) H-bonding* polar polar H + N,O,F polar nonpolar Molecule dipole-dipole* polar Δ EN = 0.5 - 1.7 London nonpolar Δ EN = 0 - 0.5 IMF Bond Details *Since all compounds have London forces. London forces are also present. However, their affect is minor and overshadowed by the stronger forces present. Note: the term “polar” is used interchangeable with “polar covalent”. Likewise, “nonpolar” and “nonpolar covalent” mean the same thing. Network solids (covalent crystals) Network solids (covalent crystals) • There are some compounds that do not have molecules, but instead are long chains of covalent bonds (E.g. diamond) C C C C C C C C C C C C C C C C C • This happens in 3 dimensions, creating a crystal • Because there are only covalent bonds, network solids are extraordinarily strong Metallic crystals Metallic crystals
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This note was uploaded on 04/12/2011 for the course CHEM 1010 taught by Professor Marshall during the Spring '11 term at North Texas.

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