1. Chapter 11 Honors Chemistry Glencoe
The Mole
Chapter 11
Honors Chemistry
Glencoe

2. Section 11-1: Measuring Matter
The Mole
Some numbers used in chemistry can be quite large, such as with the quantity of small items, such as atoms, molecules and ions.
One mole of an object is equivalent to 6.02 x 1023 objects (Avogadro’s #)

3. Section 11-2: Atomic and Molar Mass
Atomic Mass (AMU)
Describes the mass of atoms as compared to carbon-12.
1 AMU = 1.66 x grams (do not need to memorize)
The mass of an atom of each element is found on the periodic table.
The molecular (or formula) mass can be found by adding together the atomic masses of all elements.

4. Molar Mass
The mass of one mole of atoms, molecules or ions in grams. The mass of 6.02 x 1023 atoms.
The molar mass of elements are also found on the periodic table. For molecules, the masses are added up.
The calculations for individual atoms, molecules or ions (AMU) and Molar Mass (gram) are the same, except for the units.

5. Examples What is the mass of 1 atom of K? What is the molar mass of K?
What is the mass of 1 molecule of NaCl?
What is the molar mass of NaCl?
What is the mass of 1 molecule of Cu(NO3)2?
What is the molar mass of Cu(NO3)2?

6. Answers to the last slide…
39.10 amu (from PT)
39.10 g
58.44 amu (add up masses from PT)
58.44 g
amu g