1. The Basics of Atomic Structure

2. Terms you should know…
Atom: smallest unit of an element that maintains the identity of that element.
Chemical Reaction: Reaction where atoms combine in such a way to form new substances.

3. Atomic Structure Each element has a unique chemical identity.
- The key to understanding the identity of an atom is in it’s structure and the components that make up it’s structure.

4. Atomic Particle Distribution

5. Subatomic Particles Electron (e-) (-) charge 1/1840 amu
RELATIVE MASS
POSITION
(-) charge
1/1840 amu
located outside the nucleus
Proton (p+)
(+) charge
1 amu
Located inside the nucleus
Neutron (n0)
No charge

6. What’s amu? amu is shorthand for “Atomic Mass Unit (u)”
Atomic Mass Units are the units used to express atomic and molecular units.
One atomic mass unit (u) is roughly equal to the mass of one proton or one neutron. Scientists agreed to define one amu as 1/12th the mass of a carbon-12 atom. This is the standard by which all other atomic masses are compared.
In grams, one atomic mass unit (u) is equal to:
 × 10−24 g

7. Nucleus
In the center of the atom and contains the protons and neutrons
Makes up 99% of the mass of the atom.

8. Elements in the Periodic Table
Atomic Number:
This is the number of protons
In a neutral atom:
Number of protons = Number of electrons
Mass Number:
Protons + Neutrons (total number of particles in the nucleus)
Atomic mass:
the average mass of all known isotopes of the element 6 C
Carbon
12.001

9. What is the difference between mass number and atomic mass
Protons + neutrons
Whole number
Applies to only ONE isotope
NOT on the periodic table
Weighted average of ALL isotopes
Decimal number
Found on periodic table

10. So what’s your (atomic) number?
An element will always have the same number of protons regardless of the number of neutrons and electrons. An element can be identified by its Atomic Number.
Isotopes are atoms with the same number of protons but a different number of neutrons; therefore, the mass number will be different but the atomic number will be the same. All atoms of an element are considered an isotope, some are more common than others.
An Ion is an element with a number of electrons that differ from its number of protons. An ion is a charged atom.
Cation is a positive ion (created when an atom loses electrons)
Anion is an negative ion (created when an atom gains electrons)
Notice: it’s the number of electrons and neutrons that change, not the atomic number!

11. Introduction to Isotopes
All atoms of an element are considered an isotope, only some are more common than others.
Even though isotopes have different amounts of neutrons they are still chemically alike since they have the same number of protons and electrons.
Atomic mass is the average of all isotopes of the element.

12. Isotope Notation Mass number is written to the top left.
Atomic number is written at the bottom left.
What would the notation look like for Carbon 14?

14. So what are isotopes good for?
Dope testing
- one of the initial tests to determine if someone has been doping with synthetic testosterone is a test for a high concentration of an isotope that’s not contained within naturally produced testosterone, but within the synthetic testosterone derived from yams.
More tests will have to be conducted if it is revealed that the athlete is a vegetarian with an affinity for yams.

15. Radiometric Dating

16. Making Bombs