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| the attractive forces between atoms in molecules result in their formation |
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| formed when two atoms share a pair of electrons |
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| results from the electrostatic attraction of a cation for an anion |
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| consists of the nuclei of metal atoms surrounded by a "sea" of shared electrons |
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| a set of eight electrons in the outermost (valence) shell of an atom |
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| states that atoms of main group elements make bonds by gaining, losing, or sharing electrons to achieve an outer shell containing eight electrons or four electron pairs |
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| the maximum of two electrons that the outermost shell of a hydrogen atom can contain |
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| a two-dimensional representation of a molecule that provides a view of the connections between its atoms' valence electrons are depicted as dots around the atomic symbol |
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| the chemical symbol for an atom surrounded by one or more dots representing the valence electrons |
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| results when two atoms share one pair of electrons |
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| a pair of electrons that is not shared |
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| a pair of electrons shared between two atoms |
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| results when two atoms share two pairs of electrons |
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| results when two atoms share three pairs of electrons |
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| the distance between the nuclear centers of two atoms joined together in a bond |
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| contains bonds that have an uneven distribution of charge because electrons in the bonds re not shared equally by the two atoms |
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| contains bonds that have an even distribution of charge; electrons in the bonds are shared equally by the two atoms; pure covalent bonds give rise to nonpolar diatomic molecules |
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| results from unequal sharing of bonding pairs of electrons between atoms |
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| a relative of the ability of an atom to attract electrons to itself |
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| a measure of the extent to which bonding electrons are shared between two atoms in a covalent bond; the less equally they are shared, the more uneven the distribution, the more polar the bond |
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| different forms of the same element, such as oxygen and ozone |
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| occurs when two or more equivalent Lew structures can be drawn for one compound |
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| one of two or more Lewis structures with the same arrangement of atoms but different arrangements of electrons for a molecule |
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| equals the number of valence electrons on the free atom in the Lewis structure minus the sum of the number of electrons in its lone pairs plus half the number of electrons in its bonding pairs |
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| reflects the number of covalent bonds an element forms when it has a formal charge of zero |
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| Electron-Deficient Compounds |
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| substances who central atoms in Lewis structures have fewer than four electron pairs (less than an octet of electrons) |
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| molecules having an odd umber of valence electrons and hence unpaired electrons in their Lewis structures |
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| the number of bonds between atoms |
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| the energy needs to break one mole of a covalent bond in the gas phase |
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