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• Chemist measure atoms and molecule in moles (unit only available for chemistry).
• Mole is a unit used to count number of particles.
• Avogadro´s Number = 6.022 x 10 ^23 named after Amedeo Avogadro (he was Italian, so he was very cool).
• Avogadro´s Number: the number of particles in a mole. Is used to convert mass in grams to atomic mass units or vice versa.
• Molar Mass: Mass of 1 mole of unit of a substance. Same value as Atomic Mass.
• The most accurate method for determining atomic and molecular masses. In other words measures the mass of the atom.
• Molecular Mass: the sum of atomic masses in a molecule.
• With the molecular mass we can determine the molar mass of a molecule or compound. We can calculate the number of moles and individual atoms in a given quantity of a compound.
• Molar Mass (g) = Molecular Mass (amu)
• Theoretical yield: the amount of product that would result is all the limiting reagent reacted.
• Actual yield: is the amount of product actually obtained from a reaction.
• Percent yield: the proportion of the actual yield to the theoretical yield.
• The mass of an atom depends on the number of protons, neutrons, and electrons it contains.
• Atomic Mass is the mass of the atom in atomic mass units or also called amu; located above the element symbol in the periodic table.
• Example: C = 12amu
• Average Atomic Mass. Average mass of naturally occurring isotopes. Example: Carbon- 12 (98.90 percent abundance, 12amu) Carbon-13 (1.10 percent abundance, 13amu). To calculate the average atomic mass we must multiply the percent and the amu of each. Then add these values and divide them by 100, the answer id the average atomic mass for Carbon.
• Percent composition of mass is the percent by mass of each element in a compound.
• Used to determine the purity in a compound by calculating the percent of the total mass of the compound and comparing the result to the present composition.
• With the percent composition we can determine the empirical formula.