Objective 3.02

What is a MOLE????
• An amount of a substance
• A unit of measurement specific to chemistry
• mole
• mol
• n

The Mole
“like a dozen”
• Specific quantity
• Does not change
• Avogadro’s Number:
• The # of “things” in 1 mole
• 6.022 x 10 23

The Mole
How its used in Chemistry:
Elements are made up of _______________.
1 mole Cu =
1 mole Na =
1 mole O =

The Mole
How its used in Chemistry:
Compounds are made up of _____________.
1 mole NaCl =
1 mole LiOH =
1 mole CaF
2
=

The Mole
How its used in Chemistry:
1 mole Ca
3
(PO
4
)
2
* Subscripts = # of moles of the element in the compound

The Mole
How its used in Chemistry:
2 H
2
+ O
2
 2 H
2
O
* Coefficients = # of moles of a substance in a reaction

• 1 mole of each substance has a “molar mass” – a specific weight
• It is the same as atomic mass only in g
• Ex:
• 1 mole Na =
• 1 mole C =
• 1 mole Li =
•The units for molar mass are g/mol

• 1 mole H
2
O =
• 1 mole NaCl =
• 1 mole Pb(NO
3
)
2
=

Convert the following:
1. 4.3g of calcium hydroxide into moles
2. 0.82 moles of aluminum oxide into grams
3. 7.90 x 10 24 molecules of water into moles
4. 2.56 moles of sodium carbonate into molecules
5. 8.73 grams of beryllium bromide into molecules
6. 3.17 x 10 23 atoms of copper into grams of copper.
7. How many atoms of iron are there in 5.6 moles of iron (III) phosphate?
8. What is the mass of cobalt in 0.31 moles of cobalt
(II) nitride?