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10 Cards in this Set
- Front
- Back
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atomic mass unit
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based on 1/12 of carbon 12 (standard)
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atomic mass
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average of the masses of the naturally occurring isotopes of elements
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Avagadro's Number
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6.022 x 10^23
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Molar mass
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summation of the atomic masses of all the atoms in the compound
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empirical formula
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simplest whole number ratio
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molecular formula
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actual # of atoms
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structural formula
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shows how atoms go together
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percent by mass of an element in a compound
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mass (g) of element/ molar mass of compound x 100%
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Steps To Obtain Empirical Formula
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1) Convert % masses into grams using 100g base
2) convert masses to moles by dividing by atomic mass of element 3) Divide each by smallest # in step two |
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Steps to Obtain Molecular Formula
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1) Compute empirical formula molar mass
2) Divide Molar Mass/EFM 3) Multply each element in the EF by Step Two to obtain MF |
