Download 6.02 10 23

The Mole
Define the following:
Pair = 2
Dozen = 12
Gross = 144
Ream = 500
Mole = 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 ions
 The number 6.02 x 1023 (602 000 000 000 000 000 000
000 ) is called Avogadro’s number
A
large amount!!!!
A. What is the Mole?

1 mole of hockey pucks would
equal the mass of the moon!

1 mole of basketballs would fill a
bag the size of the earth!
1 mole of pennies would cover the
Earth 1/4 mile deep!
Now that we know…
1 mol = 6.02 x 1023 particles
We must be able to recognize what type of
particles we’re dealing with based on the
substance
Think back
Elements (by themselves) = atoms
Formula
units
Ionic
Compounds
=

molecules
Molecular
Compounds
=

• 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
12.011 g/mol
aluminum
26.982 g/mol
zinc
65.38 g/mol
B. Molar Mass Examples
water
 H2O
 2(1.008) + (1)15.999 = ______ g/mol
sodium chloride
 NaCl
 (1)22.990 + (1)35.453 = _______ g/mol
B. Molar Mass Examples
sodium hydrogen
carbonate
 NaHCO3
 22.990 + 1.008 + 12.011 + 3(15.999)
= ______ g/mol
sucrose
 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