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IONS

IONS. ION: Charged particle - Metals LOSE electrons= cation (+) e.g . Na + - Non-metals GAIN electrons = anion (-) e.g . Cl -. Ionic Bond: Attraction between positive ions and negative ions. . *** All atoms want a full outer shell in order to be stable !! ***. Compounds.

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IONS

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  1. IONS

  2. ION: Charged particle - Metals LOSE electrons= cation (+) e.g. Na+ - Non-metals GAIN electrons = anion (-) e.g. Cl- Ionic Bond: Attraction between positive ions and negative ions. *** All atoms want a full outer shell in order to be stable!! ***

  3. Compounds Compound: composed of 2 or more elements that are chemically combined (e.g. NaCl). There are 2 types of compounds: Ionic Compounds (metal + non-metal) Molecular Compounds (non-metal + non-metal) Ionic Compound: metal + non-metal combine. Ions are formed when the compound is dissolved in an aqueous solution.

  4. Counting Atoms

  5. Counting Atoms • The symbol represents 1 atom of that element (e.g. NaCl= 1 sodium atom & 1 chlorine atom) • A subscript represents the # of atoms (e.g. H2= 2 hydrogen atoms) *no subscript means there is 1 atom present* (e.g. Li = 1 lithium atom) • A coefficient in front of an ATOM represents the # of atoms (e.g. 3 C= 3 carbon)

  6. Counting Atoms • A coefficient in front of a chemical formula represents the # of molecules. (** If you multiply a coefficient # by the subscript it indicates the # of atoms) e.g. 3 H2O 3 H20= 3 H20 molecules O= 3 x 1(subscript) = 3 oxygen atoms H= 3 x 2 (subscript) = 6 hydrogen atoms

  7. Example #1: count the # of atoms present GLUCOSE C6H12O6

  8. ESTRADIOL Example #2: count the # of atoms present

  9. Example #3: count the # of atoms present 3 C2H4O2

  10. C3H8 + 5O2 3CO2 + 4H2O(Complete Combustion) Reactants: C= H= O= Products: C= H= O=

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