crystal-properties

crystal-properties - Ionic, H-bonding, Dipole, or London?...

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Ionic, H-bonding, Dipole, or London? Ionic, H-bonding, Dipole, or London? Details Bond Molecule IMF EN = 0 - 0.5 nonpolar nonpolar London EN = 0.5 - 1.7 polar polar dipole-dipole* EN = 1.7 - 3.2 ionic Ionic ionic* H + N,O,F polar polar H-bonding* Symmetrical molecule (any EN) -- nonpolar London *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.
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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
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Metallic crystals Metallic crystals Metals normally occur as solids (high melting points).
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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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crystal-properties - Ionic, H-bonding, Dipole, or London?...

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