1. 3.3 Counting Atoms

2. Counting Atoms

3. Isotopes Atoms of the same element with different masses Isotopes do not differ significantly in their chemical behavior Writing Isotopes: – Hyphen notation: element-mass # (hydrogen-3) – Nuclear symbol: 235 U 92

4. Atomic Mass Atomic mass is a relative measure One atomic mass unit (amu) is exactly 1/12 th the mass of a carbon-12 atom. Average atomic mass is the weighted average of the atomic masses of the isotopes of an element (it takes into account the relative abundance of the isotopes).

5. Calculating Average Atomic Mass What is the average atomic mass of copper if naturally occurring copper consists of 69.15% copper-63 and 30.85% copper-65?

6. Expressing Quantities of Atoms The mole = SI unit for amount of substance, it is a counting unit like a dozen, it stands for a specific number of atoms. Avogadro’s Number = the number of particles in a mole of a substance 6.02 x 10 23 Molar Mass = the mass of one mole of a pure substance, its units are g/mol

7. What is the mass in grams of 3.50 mol of the element copper, Cu?

8. A chemist produced 11.9g of Al. How many moles of aluminum were produced?

9. How many moles of lead, Pb, are in 1.50 x 10 12 atoms of lead?

10. How many atoms of sulfur, S, are in 4.00 g of sulfur?

11. Beaker A contains 2.06 mol of copper, and Beaker B contains 222 grams of silver. Which beaker contains the larger mass? Which beaker has the larger number of atoms?