1. The Mole: A Measurement of Matter
Sand Activity
Is it practical to count each grain of sand?
How else might you measure or quantify the sand?
mass, volume
just a small amount of sand contains millions of smaller particles, just like chemical substances

2. The Mole: A Measurement of Matter
Scientists answer questions such as:
How many kilograms of iron can be obtained from one kilogram of iron ore?
How many grams of the elements hydrogen and nitrogen must be combined to make 200 grams of the fertilizer ammonia (NH3)?
How do we measure matter?
by counting
determine its mass and volume

3. The Mole: A Measurement of Matter
There are ways that everyday things are measured
how many is a couple?
how many is one dozen?
how many is a few?
how many sodas are in one case?
how many are in one gross?
Example: apples can be measured three different ways, all of which can be equated to a dozen apples
By count:
1 dozen apples = 12 apples
for average-sized apples the following approximations can be used:
By mass:
1 dozen apples = 2.0 kg apples
By volume:
1dozen apples = 0.20 bushel apples

4. The Mole: A Measurement of Matter
Knowing how the count, mass, and volume of apples relate to a dozen apples allows you to convert between these units. For example, you could calculate the mass of a bushel of apples or the mass of 90 average-sized apples using conversion factors based on the unit relationships given above.

5. The Mole: A Measurement of Matter
In chemistry you will do calculations using a measuring unit called a mole. The mole, the SI unit that measures the amount of substance, is a unit just like the dozen.
The mole can be related to the number of particles (a count), the mass, and the volume of an element or a compound just as a dozen was related to these three units for apples

6. The Mole: A Measurement of Matter
Example:
What is the mass of 90 average-sized apples?
Knowns:
Number of apples = 90 apples
12 apples = 1 dozen apples
1 dozen apples = 2.0 kg apples
Unknowns:
Mass of 90 apples = ? kg
Convert:
Number of apples to mass of apples
This conversion can be carried out by performing the following sequence of conversions:
number dozens mass of apples

7. The Mole: A Measurement of Matter
Calculate:
First conversion factor: 1 dozen apples/ 12 apples
Second conversion factor: 2.0 kg apples/ 1 dozen apples
Multiplying the original number of apples by these two conversion factors yields the answer in kilograms,

8. The Mole and Molar Mass
The mole is the standard method in chemistry for communicating how much of a substance is present (just like one dozen is equal to the quantity twelve).
Definition:
The mole is the amount of substance of a system which contains as many elementary entities as there are atoms in kilogram of carbon-12. When the mole is used, the elementary entities must be specified and may be atoms, molecules, ions, electrons, other particles, or specified groups of such particles.

9. The Mole and Molar Mass
One mole contains as many entities as there are in 12 grams of carbon-12 (or kilogram)
In one mole, there are x 1023 atoms. Here's another way: there are x 1023 atoms of carbon in 12 grams of carbon-12
Let's say that clearly: one mole of ANYTHING contains x 1023 entities.

10. The Mole and Molar Mass
The word "entities" is simply a generic word. For example, if we were discussing atoms, then we would use "atoms" and if molecules were the subject of discussion, the word entities would be replaced in actual use by "molecules."
The mole has been very carefully measured in a number of ways over many decades. The symbol for mole is "mol."

11. The Mole and Molar Mass
One mole of ANY specified entity contains x 1023 of that entity. For example:
One mole of donuts contains x 1023 donuts
One mole of H2O contains x 1023 molecules
One mole of nails contains x 1023 nails
One mole of Fe contains x 1023 atoms
One mole of dogs contains x 1023 dogs
One mole of electrons contains x 1023 electrons
One mole of 11th grade chemistry students contains x 1023 poor, suffering (I mean happy, joyful) Monaca students

12. The Mole and Molar Mass
6.023 x 1023 is so important in chemistry that it has a name. It is called Avogadro's Number and has the symbol N.
It is so named in honor of Amedeo Avogadro, an Italian chemist, who, in 1811, made a critical contribution (recognized only in 1860 after his death) which helped greatly with the measurement of atomic weights.

13. The Mole and Molar Mass
Avogadro's Number has a unit associated with it. It is mol¯1, as in x 1023 mol¯1.
The superscripted minus one means the unit mol is in the denominator. There is an understood numerator of one, as in 1/mol.

14. The Mole and Molar Mass 6.022 x 1023 mol¯1
Why is there no unit in the numerator? There could be, but it would vary based on the entity involved. If we were discussing an element, we might write atoms/mol.
If we were discussing a compound, we would say "molecules per mol." What is in the numerator depends on what "entity" (atom, molecule, ion, electron, etc.) is being used in the problem.

15. The Mole and Molar Mass
Getting back to Avogadro's Number and its role in chemistry; please note that counting atoms or molecules is very difficult since they are so small. However, we can "count" atoms or molecules by weighing large amounts of them on a balance.
Examples
Atoms/mol
Molecules/mol
Ions/mol
Electrons/mol
Pencils/mol
Chairs/mol
etc

16. Molar Mass
When we weigh one mole of a substance on a balance, this is called a "molar mass" and has the units g/mol (grams per mole). This idea is very critical because it is used all the time.
A molar mass is the weight in grams of one mole.
One mole contains x 1023 entities.
Therefore, a molar mass is the mass in grams of x 1023 entities.

17. Molar Mass OK. How does one calculate a molar mass?
The molar mass of a substance is the molecular weight in grams. The molecular weight of a substance is the weight in atomic mass units of all the atoms in a given formula.
All you need to do is calculate the molecular weight and place the unit "g/mol" after the number and that is the molar mass for the substance in question.

18. Molar Mass Calculate the molar mass of Al(NO3)3
Al(1 x 26.98) + N(3 x ) + O(9 x 16.00) = g/mol
grams is the mass of one mole of aluminum nitrate.
grams of aluminum nitrate contains x 1023 entities of Al(NO3)3

19. Review Calculate the molar mass of Pb(ClO2)2
Pb( 1 x 207.2) + Cl( 2 x ) + O( 4 x ) = g/mol
Calculate the molar mass of NH4MnO4
N( 1 x ) + H( 4 x 1.01) + Mn( 1 x ) + O( 4 x )
= g/mol

20. Mole and Weight Relationships of Water and its Parts
2 moles H +
1 mole O =
1 mole water
2 * 1.01 g
16.00 g
18.02 g
A bottle filled with exactly g water will contain 6.02 x 1023 water molecules.  The concept of fractions and multiples described above also applies to molecules: 9.01 g of water would contain 1/2 mole, or 3.01 x 1023 molecules. 

21. Activity: How Many?