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20 Cards in this Set
- Front
- Back
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ELECTRON DOT STRUCTURES
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an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element’s symbol. The inner-shell electrons are not shown.
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VALENCE ELECTRONS
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a single electron or one of two or more electrons in the outer shell of an atom that is responsible for the chemical properties of the atom
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HALIDE ION
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a halogen atom bearing a negative charge
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OCTET RULE
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atoms are most stable when they have a full outer energy level – usually this means 8 electrons in the highest numbered energy level
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COORDINATE COVALENT BOND
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a description of covalent bonding between two atoms in which both electrons shared in the bond come from the same atom
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LONDON DISPERSION FORCES
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the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
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STRUCTURAL FORMULA
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indicates the kind, number, and arrangement, and bonds but not the unshared pairs of the atoms in a molecule.
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NETWORK SOLID
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a chemical compound in which the atoms are bonded by covalent bonds in a continuous network
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BOND DISSOCIATION ENERGY
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one measure of the bond strength in a chemical bond
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IONIC BONDING
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a type of chemical bond that involves a metal and a nonmetal ion through electrostatic attraction
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COVALENT BONDING
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a form of chemical bonding that is characterized by the sharing of pairs of electrons between atoms, or between atoms and other covalent bonds
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POLAR
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the bonded elements have an unbonded pair of electrons
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NONPOLAR
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the bonded elements do not have unbonded pairs of electrons
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MONATOMIC
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has one atom in it
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DIATOMIC
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has 2 atoms in it
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POLYATOMIC
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has multiple atoms in it
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SINGLE COVALENT BONDS
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a covalent bond in which one pair of electrons is shared between two atoms
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TRIPLE COVALENT BONDS
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a covalent bond in which three pairs of electrons are shared between two atoms
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RESONANCE
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occurs when there are 2 correct Lewis Structures
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VSEPR THEORY
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it is used to predict the geometries of more-complicated molecules, one must consider the locations of all electron pairs surrounding the bonding atoms
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