1. Section 3 Counting Atoms
Chapter 3
Atomic Number
Atoms of the same element all have the same number of protons.
atomic number (Z) - number of protons of each atom of that element

2. Visual Concepts
Chapter 3
Atomic Number

3. Section 3 Counting Atoms
Chapter 3
Isotopes
Isotopes - atoms of the same element that have different masses
The isotopes of a particular element all have the same number of protons and electrons but different numbers of neutrons.
Most of the elements consist of mixtures of isotopes.

4. Section 3 Counting Atoms
Chapter 3
Mass Number
mass number - total number of protons and neutrons that make up the nucleus of an isotope

5. Visual Concepts
Chapter 3
Mass Number

6. Chapter 3 Designating Isotopes
Section 3 Counting Atoms
Chapter 3
Designating Isotopes
Hyphen notation: The mass number is written with a hyphen after the name of the element.
uranium-235
Nuclear symbol: The superscript indicates the mass number and the subscript indicates the atomic number.

7. Chapter 3 Designating Isotopes
Section 3 Counting Atoms
Chapter 3
Designating Isotopes
The number of neutrons is found by subtracting the atomic number from the mass number.
mass number  atomic number = number of neutrons
235 (protons + neutrons)  92 protons = 143 neutrons
Nuclide is a general term for a specific isotope of an element.

8. Chapter 3 Designating Isotopes Sample Problem A
Section 3 Counting Atoms
Chapter 3
Designating Isotopes
Sample Problem A
How many protons, electrons, and neutrons are there in an atom of chlorine-37?

9. Relative Atomic Masses
Section 3 Counting Atoms
Chapter 3
Relative Atomic Masses
atomic mass unit, or 1 amu - exactly 1/12 the mass of a carbon-12 atom
The atomic mass of any atom is determined by comparing it with the mass of the carbon-12 atom.

10. Average Atomic Masses of Elements
Section 3 Counting Atoms
Chapter 3
Average Atomic Masses of Elements
Average atomic mass - weighted average of the atomic masses of the naturally occurring isotopes of an element
Calculating Average Atomic Mass
The average atomic mass of an element depends on both the mass and the relative abundance of each of the element’s isotopes.

11. Average Atomic Masses of Elements
Section 3 Counting Atoms
Chapter 3
Average Atomic Masses of Elements
Calculating Average Atomic Mass
Copper consists of 69.15% copper-63, which has an atomic mass of amu, and 30.85% copper-65, which has an atomic mass of amu.

12. Relating Mass to Numbers of Atoms
Section 3 Counting Atoms
Chapter 3
Relating Mass to Numbers of Atoms
The Mole
The mole is the SI unit for amount of substance.
A mole (abbreviated mol) is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12.
Avogadro’s Number
Avogadro’s number—  1023—is the number of particles in exactly one mole of a pure substance.

13. Relating Mass to Numbers of Atoms
Section 3 Counting Atoms
Chapter 3
Relating Mass to Numbers of Atoms
Molar Mass
molar mass - mass of one mole of a pure substance
Molar mass is usually written in units of g/mol.
The molar mass of an element is numerically equal to the atomic mass of the element in atomic mass units.

14. Relating Mass to Numbers of Atoms
Section 3 Counting Atoms
Chapter 3
Relating Mass to Numbers of Atoms
Gram/Mole Conversions
The molar mass of helium is 4.00 g He/mol He.
To find how many grams of helium there are in two moles of helium, multiply by the molar mass.

15. Relating Mass to Numbers of Atoms
Section 3 Counting Atoms
Chapter 3
Relating Mass to Numbers of Atoms
Sample Problem B
What is the mass in grams of 3.50 mol of the element copper, Cu?

16. Relating Mass to Numbers of Atoms
Section 3 Counting Atoms
Chapter 3
Relating Mass to Numbers of Atoms
Sample Problem C
A chemist produced 11.9 g of aluminum, Al. How many moles of aluminum were produced?
The molar mass of aluminum from the periodic table is rounded to g/mol.

17. Chapter 3 Avogadro’s Number Visual Concepts
Click below to watch the Visual Concept.
Visual Concept

18. Section 3 Counting Atoms
Chapter 3
Solving Mole Problems

19. Determining the Mass from the Amount in Moles
Section 3 Counting Atoms
Chapter 3
Determining the Mass from the Amount in Moles

20. Relating Mass to Numbers of Atoms
Section 3 Counting Atoms
Chapter 3
Relating Mass to Numbers of Atoms
Sample Problem D
How many moles of silver, Ag, are in 3.01  1023 atoms of silver?

21. Relating Mass to Numbers of Atoms
Section 3 Counting Atoms
Chapter 3
Relating Mass to Numbers of Atoms
Sample Problem E
What is the mass in grams of 1.20  108 atoms of copper, Cu?