1. The Mole

2. Define the following: 144 Pair = Dozen = Gross = Ream = Mole = 2 12
500
6.02 x 1023

3. A. What is the Mole? A large amount!!!! VERY
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 ( ) is called Avogadro’s number
A large amount!!!!
VERY

4. A. What is the Mole? HOW LARGE IS IT???
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!

5. Ionic Compounds = Molecular Compounds = 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) =
Ionic Compounds =
Molecular Compounds =
atoms
Formula units
molecules

6. The representative particle in a mole of water is the water molecule.
1 mol H2O = x 1023 molecules H2O

7. The representative particle in a mole of copper is the copper atom.
1 mol Cu = x 1023 atoms Cu

8. 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.

9. 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)

10. B. Molar Mass Examples 12.011 g/mol 26.982 g/mol 65.38 g/mol carbon
aluminum
zinc
g/mol
g/mol
65.38 g/mol

11. B. Molar Mass Examples H2O 2(1.008) + (1)15.999 = ______ g/mol NaCl
water
sodium chloride
H2O
2(1.008) + (1) = ______ g/mol
NaCl
(1) (1) = _______ g/mol

12. B. Molar Mass Examples NaHCO3
sodium hydrogen carbonate
sucrose
NaHCO3
(15.999) = ______ g/mol
C12H22O11
12(12.011) + 22(1.008) + 11(15.999) = ______ g/mol

13. Find the molar masses of the following substances:Fe Hg
SO3
(NH4)1+
NaBr
Ca(OH)2
Na3PO4
(NH4)2CO3
Zn(C2H3O2)2