Avogadro’s Number and the Mole
Atoms, ions, and molecules are very small, so even tiny samples have a hugenumber of particles. To make counting such large numbers easier, scientistsuse the same approach to represent the number of ions or molecules in asample as they use for atoms. The SI unit for amount is called the mole(mol). A mole is the number of atoms in exactly 12 grams of carbon-12.
The number of particles in a mole is called Avogadro’s number orAvogadro’s constant. One way to determine this number is to count thenumber of particles in a small sample and then use mass or particle sizeto find the amount in a larger sample. This method works only if all of theatoms in the sample are identical. Thus, scientists measure Avogadro’snumber using a sample that has atoms of only one isotope.
The most recent measurement of Avogadro’s number shows that it is6.02214199 × 1023 units/mole. In this class, the measurement is roundedto 6.022 × 1023 units/mol. Avogadro’s number is used to count any kind ofparticle.
The Mole Is a Counting Unit
Moles
# of Particles
Multiply by 6.022 x 1023
Divide by 6.022 x 1023
1. How many ions are there in 0.187 mol of Na+ ions?
2. How many atoms are there in 1.45 × 10−17 mol of arsenic?
3. How many molecules are there in 4.224 mol of acetic acid, C2H4O2?
4. How many formula units are there in 5.9 mol of NaOH?
1.13 x 1023 ions of Na+
8.73 x 106 ions of arsenic or 8,730,000 ions of arsenic
2.544 x 1024 ions of C2H4O2
3.6 x 1024 ions of NaOH
1. How many moles of xenon do 5.66 × 1023 atoms equal?
2. How many moles of silver nitrate do 2.888 × 1015 formula units equal?
3. A biologist estimates that there are 2.7 × 1017 termites on Earth. How many moles of termites is this?
4. How many moles do 5.66 × 1025 lithium ions, Li+, equal?
0.940 moles of xenon
4.796 x 10-9 moles of silver nitrate
4.5 x 10-7 moles of termites
9.40 x 101 moles of Li+ or 94.0 moles of Li+