Regents Chem Bonding
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| molecular compound | compound with covalent bonds containing nonmetals and/or semi-metals
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| ionic compound | compound with ionic bonds; usually between metals and nonmetals that transferred electrons.
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| covalent bonds | Bond formed when nonmetals and/or semi-metals share electrons
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| coordinant covalent bonds | covalent bonds where the 2 shared electrons come from the same atom. Hydronium (H3O+) and ammonium (NH4+) contain this special type of bond.
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| polar molecules | molecule with an uneven distribution of electrons. Positive and negative regions exist
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| nonpolar molecules | molecule with even distribution of electrons due to its SYMMETRY.
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| network bonding/network solid | strongest intermolecular force. Covalent bonds continue in all directions. Ex. Diamond, graphite and silicon dioxide, silicon carbide
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| metallic bonding | nuclei surrounded by a “sea of moving electrons’ – this is why metals conduct.
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| intermolecular forces | attractive forces between molecules, the stronger they are, the higher the boiling and melting points will be
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| hydrogen bonding | strong attraction between certain polar molecules containing hydrogen bonded to small, highly electronegative elements like N, O and F
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| molecule ion attractions | polar molecules are attracted to ionic compounds. This is how water dissolves salts, by attacking and surrounding the ions
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| octet rule | all elements want 8 valence electrons to become stable. H and He only require 2 electrons (duet rule)
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| ion | a charged element or compound, formed by a gain or loss of electrons
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| cation | The special name for a positive ion; "MEOW"
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| anion | A-Negative ION
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| formula unit | a single piece of an ionic compound
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| formula | represents a compound, using element symbols and their subscripts
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| electronegativity | ability to attract electrons
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| polar covalent bond | unequal sharing of electrons; END is 0.4-2.0
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| nonpolar covalent bond | equal sharing of electrons, usually in diatomic molecules; END 0-0.3
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| diatomic element | 7 elements that cannot exist alone in nature. They bond to themselves (ex: F2)
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| structural formula | Shows bonded and non-bonded e's, element symbols, and the geometry of a molecule
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| unshared (lone) electron pair | Non-bonded electrons. These repel all bonded e's and change symmetry of a molecule.
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| symmetry | A molecule with evenly distributed e's
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| Has both ionic and covalent bonds | Any ionic compound that has a table E ion in it. (the polyatomic ion contains covalent bonds, but the overall bonding is ionic)
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