1.1 Electronegativity and Bonding Note

1.1 Electronegativity and Bonding Note - ions attract one...

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Electronegativity and Bonding Electronegativity - affinity for electrons - ability of an element to attract electrons that it is sharing in a covalent bond - normally elements that need only 1 or 2 electrons to fill the outer energy levels are more electronegative - increases as you go horizontally across the table from Li to F and decreases as you go vertically from F to I, for example Bonding A: Intramolecular Forces - intra means within thus these forces are found within the molecule between atoms 1. covalent bonding – sharing of valence electrons (a) nonpolar covalent - share valence electrons equally or almost equally - electronegativity difference is from 0 to 0.5 (b) polar covalent - share valence electrons, but not equally - electronegativity difference is from 0.5 to 1.7 2. ionic bonding - forces between ions (which are charged atoms) where oppositely charged
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Unformatted text preview: ions attract one another - electronegativity difference is greater than 1.7 B: Intermolecular Forces- forces that exist between molecules 1. London dispersion forces-a weak force that exists between all molecules -due to a temporary charge -the larger the molecules the longer the temporary force lasts; usually liquids or solids like lipids-the smaller the molecules the shorter the temporary force lasts; usually in gases like methane 2. dipole-dipole forces-forces between polar molecules 3. hydrogen bonding-forces that exist between H (which is part of a molecule) and O, N, F (something with a high electronegativity that is also part of another molecule)-a type of dipole-dipole Electronegativity Table p. 14...
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