the mole and avogadro’s number. mole (n): the amount of substance 6.02x10 23 particles (atoms or...

The Mole and Avogadro’s Number

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The Moleand Avogadro’s Number

• Mole (n): the amount of substance• 6.02x1023 particles (atoms or

molecules) of a substance• The same number of particles as

atoms in 12 grams of carbon-12

mole

particlesx

1002.6 23

particlesx

mole231002.6

Page 3: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

Review

• How many atoms are there in 1.2 moles of oxygen?

• Calculate the number of moles of nitrogen equal to 3.45x1015 atoms of nitrogen.

Page 4: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

Counting Atoms

• CO• CO2

• Fe(NO3)3

• C6H12O6

• potassium carbonate

Page 5: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

• How many molecules in 5 moles of water?

• How many hydrogen atoms in 5 moles of water?

• How many atoms in 5 moles of water?

Page 6: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

1. How many chloride ions are there in zinc chloride?

2. A sample of zinc chloride contains 3.1x1019 molecules. a. How many moles is this?

b. How many zinc ions?

c. How many chloride ions?

Page 7: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

• Stop.

Page 8: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

Masses of Compounds

Page 9: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

• Atomic mass (A): the mass of an atom of an element relative to (compared to) other elements (g/mol)

Page 10: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

• Ionic: formula unit• Molecular (covalent): molecule

Page 11: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

• Formula mass: sum of the atomic masses of the atoms in the compound’s formula (IONIC) (g/mol)

• Molecular mass: sum of the atomic masses of all the atoms in one molecule (COVALENT) (g/mol)

Page 12: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

• Molar mass (M): the mass of one mole of any substance (g/mol)–atoms, molecules, ions, etc.

Page 13: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

IonicFormula

Mass

CovalentMolecular

Mass

MolarMass

Page 14: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

Calculating Molar Mass

• Stop.

Page 15: The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles

1. Calculate the mass of 1.98 moles of iron (II) nitrate.

2. How many molecules are there in 1.00 grams of iron (II) nitrate?

3. Calculate the mass of one molecule of iron (II) nitrate.

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