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| a strong attractive force that exists between atoms in a molecule |
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| a bond between oppositely charged ions; the ions are formed from atoms by transfer of one or more electrons |
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| a bond formed between two or more atoms by a sharing of electrons |
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| bonding, usually in solid metals, in which the bonding electrons are relatively free to move throughout the 3D structure |
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| the chemical symbol for an element with a dot for each valence electron |
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| a rile stating that bonded atoms tend to possess or share a total of eight valence-shell electrons |
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| the energy required to separate completely ions in an ionic solid |
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| a thermodynamic cycle based on Hess's law that relates the lattice energy of an ionic substance to its enthalpy of formation an d to other measurable quantities |
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| a representation of covalent bonding in a molecule that is drawn using Lewis symbols; shared electron pairs are shown as lines, and unshared electron parts are shown as pairs of dots; only the valence-shell electrons are shown |
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| a covalent bond involving one electron pair |
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| a covalent bond involving two electron pairs |
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| a covalent bond involving three electron pairs |
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| a measure of the degree to which the electrons are shared unequally between two atoms in a chemical bond |
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| a covalent bond in which the electrons are shared equally |
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| a covalent bond in which the electrons are not shared equally |
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| a measure of the ability of an atom that is bonded to another atom to attract electrons to itself |
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| a molecule that possess a nonzero dipole moment |
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| a molecule with one end having a partial negative charge and the other end having a partial positive charge; a polar molecule |
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| a measure of the separation and magnitude of the positive and negative charges in polar molecules |
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| the number of valence electrons in an isolated atom minus the number of electrons assigned to the atom in the Lewis structure |
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| individual Lewis structures in cases where two or more Lewis structures are equally good descriptions of a single molecule; the resonance structures in such an instance are "averaged" to give a more accurate description of the real molecule |
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| the enthalpy change required to break a particular bond when the substance is in the gas phase |
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