The Mole

Define the following:

Pair = Dozen = Gross = Ream = Mole =

2

12

144500

6.02 x 1023

A. What is the Mole?

A counting number (like a dozen)1 mol = 6.02 1023 particles“particles” may be atoms, molecules, formula units,

or ionsThe number 6.02 x 1023 (602 000 000 000 000 000 000

000 ) is called Avogadro’s number

A large amount!!!!

1 mole of hockey pucks would equal the mass of the moon!

A. What is the Mole?

1 mole of pennies would cover the Earth 1/4 mile deep!

1 mole of basketballs would fill a bag the size of the earth!

Now that we know…

1 mol = 6.02 x 1023 particlesWe must be able to recognize what type of

particles we’re dealing with based on the substance

Think back Elements (by themselves) =

Ionic Compounds =

Molecular Compounds =

atoms

Formula units

molecules

• The representative particle in a mole of water is the water molecule.

• 1 mol H2O = 6.02 x 1023 molecules H2O

• The representative particle in a mole of copper is the copper atom.

• 1 mol Cu = 6.02 x 1023 atoms Cu

• The representative particle in a mole of sodium chloride is the formula unit.

• 1 mol NaCl =6.02 x 1023

formula units NaCl

• The term “formula unit”is used to represent one“unit” of an ionic compound.

B. Molar Mass

Mass of 1 mole of an element or compound.

Atomic mass tells the... atomic mass units per atom (amu) grams per mole (g/mol)

B. Molar Mass Examples

carbon

aluminum

zinc

12.011 g/mol

26.982 g/mol

65.38 g/mol

B. Molar Mass Examples

water

sodium chloride

H2O

2(1.008) + (1)15.999 = ______ g/mol

NaCl (1)22.990 + (1)35.453 = _______ g/mol

B. Molar Mass Examples

sodium hydrogen carbonate

sucrose

NaHCO3

22.990 + 1.008 + 12.011 + 3(15.999)

= ______ g/mol

C12H22O11

12(12.011) + 22(1.008) + 11(15.999)

= ______ g/mol

Find the molar masses of the following substances:

Fe

Hg

SO3

(NH4)1+

NaBr

Ca(OH)2

Na3PO4

(NH4)2CO3

Zn(C2H3O2)2