Chapter 8 The Mole.

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Presentation transcript:

Chapter 8 The Mole

8.1Avogadro’s Constant and the Mole 1 mole = 6.02 x 1023 atoms (molecules, ions, formula units) This is an equality that can be turned into conversion factors.

8.1 Relative atomic mass and the PTE Atomic mass units= amu 1 amu= 1.66x10-24 g amu is a measurement of mass One atom of an element is equivalent to the mass of that element on the periodic table in amu’s Atomic mass is a weighted average of isotopes for that element.

8.1 Molar mass relates moles to grams Mole- the number equal to the number of carbon atoms in 12.01 grams of carbon Avogadro’s number = 6.022x1023 units A mole in context is similar to describing something in dozens. Therefore 1 mole (any element) = 6.02 x 1023 atoms 1 mole (any element) = mass in grams from PTE (molar mass) 6.02 x 1023 atoms = mass in grams from PTE

8.2 Molar Mass Molar mass of a substance is the mass(in grams) of 1 mole of that substance Molar mass can be found by adding up the masses of the atoms in the compound

8.2 % Composition of Compounds % composition can be found by: Mass of element(s) present in 1 mol of the compound/1 mol of compound All percents should add up to 100%

8.2 Calculation of Empirical Formulas Find how many moles of each element are present in the compound Divide each elements mol number by the lowest mol number Multiply the numbers from the previous step to make sure all numbers are whole numbers Empirical formula is the smallest form of the compound

8.2 Calculation of Molecular Formulas Calculate the empirical formula Find the molar mass Molar mass/ empirical formula mass Round to a whole by multiplying Multiply each element in the empirical formula to find the molecular formula