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| a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together. |
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| results from the sharing of electron pairs between two atoms. |
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| chemical bonding that results from the electrical attraction between large numbers of cations and anions. |
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| a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge. |
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| has an uneven distribution of charge. |
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| covalent bond in which the bonded atoms have an unequal attraction for shared electrons. |
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| neutral group of atoms that are held together by covalent bonds. |
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| chemical compound whose simplest units are molecules |
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| indicates the relative numbers of atoms in each kind in a chemical compound by using atomic symbols and numerical subscripts. |
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| shows the types and numbers of atoms combined in a single molecule of a molecular compound. |
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| molecule conataining only two atoms |
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| distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms. |
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| energy required to break a chemical bond and form neutral isolated atoms. |
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| chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level. |
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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 elements symbol. |
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| unshared pair and lone pair |
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| pair of electrons that is not involved in bonding and that belongs exclusively to one atom. |
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| formulas in which atomic symbols represent nuclei and inner- shell electrons, dot-pairs, or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons. |
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| indicates the kind, number, arragement, and bonds but not the unshared pairs of the atoms in a molecule. |
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| is a covalent bond produced by the sharing of one pair of electrons between two atoms. |
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| a covalent bond produced by the sharing of two pairs of electrons between two atoms. |
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| a covalent bond produced by the sharing of three pairs of electrons between two atoms. |
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| bonding in molecules or ions that can not be corrctly represented by a single Lewis Structure. |
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| composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal. |
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| the simplest collection of atoms from which an ionics compounds formula can be established. |
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| the energy released when one mole of an ionic crystalline compound is formed from gaseousions. |
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| a charged group of covalently bonded atoms. |
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| the chemical bonding that reults from the attraction between metal atoms and the surrounding sea of electrons. |
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| ability of a substance to be hammered or beaten into thin sheets. |
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| ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire. |
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| uneven distribution of molecular charge. |
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| states that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible. |
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| mixing of two or more atomic orbitals of similar energy's on the same atom to produce new orbitals of equal energies. |
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| orbitals of equal energy produced by the combination of two or more orbitals on the same atom. |
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| forces of attraction between molecules. |
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| created by equal but opposite charges that are seperated by a short distance. |
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| forces of attraction between polar molecules |
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| the intramolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a hearby molecule. |
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| the intramolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles. |
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| The forces of attraction within individual molecules. |
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