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9 Cards in this Set
- Front
- Back
Electron affinity
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the tendency of an atom to accept an electron.
- increases as atomic number increases within a period (left-right) - increases as atomic number increases within a group (bottom-top) |
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electronegativity
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the relative ability of an atom to attract electrons in a chemical bond
- differences in electronegativity can be used to predict the character and type of a chem bond |
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polar covalent bonds
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a covalent bond formed between atoms of different elements that does not have equal sharing of the electron pair b/c there is a difference in electronegativity
*unequal sharing* |
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pure covalent bond
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or nonpolar covalent
occurs for identical atoms w/ an electronegativity different of 0 so that the electrons are equally shared between the 2 atoms |
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electronegativity differences
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1.70 = 50% ionic and 50% covalent
>1.70 = ionic bond |
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molecular polarity
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depends on the location and nature of the covalent bonds in the molecule
- nonpolar molecules are NOT attracted by an electric field - a polar molecular has a partial positive charge on one side and a partial negative charge on the other (a dipole) so it aligns w/ an electron field b/c of a greater electron density on one side |
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solubility
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polar molecules and ionic substances = soluble in polar substances
nonpolar molecules = soluble in nonpolar substances |
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dipole - dipole force
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the attraction of one end of the dipole to the oppositely charged end of the other dipole
- >dipole-dipole force = >molecular polarity |
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polar vs. nonpolar molecules
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Polar:
- molecule has a definite positive and negative end - bonds are NOT symmetric Non-polar: - symmetric--the electrical charge measured at any distance from its center is identical to the charge measured at the same idstance on the opp side - partial charges are balanced |