1. Atomic Structure

2. The Basic Analogy Atom Element Compound Molecule Element-
Cannot be broken down into another substance
Is made up of only one type of atom

3. Molecules & Compounds
Analogy: It’s like putting two lego blocks together and getting
a Cow! (but there are reasons why this happens)

4. So…What’s in an Atom?

5. AnATOMy of An ATOM
Electron
Nucleus with
Protons &
Neutrons

6. Some Typical Atoms
Hydrogen
1P+
1e-
Carbon
6P+ 6N
6e-

7. Rules for Atoms The Net Charge for any atom should equal … 0
This means that there should be the same number of Protons and Electrons!
The number of PROTONS defines the element (This is the Atomic Number)

8. More About Atoms
The MASS NUMBER of an atom is the sum of the number of PROTONS and the number of NEUTRONS.

9. What happens if... An atom gains or loses electrons?
you get an ION…a charged particle
An atom gains or loses neutrons?
you get an ISOTOPE…a heavier or lighter form of the same substance
An atom gains or loses protons?
you get a different element (happens in nuclear fission or fusion)

10. Atomic Mass (not Mass Number)
Definition: the weighted average of all of the isotopes of an element.
What’s a weighted average?
Take carbon for example. You’ll notice that the atomic mass is very close to 12. There are heavier forms of carbon, but they occur much less frequently than Carbon 12. If you take the average based on how frequently they occur, the relative amount of Carbon 12 brings the average close to 12.

11. More History (Yippeeee!)
Ernie’s (Rutherford) Big Adventure
Thin Sheet of Gold
Atoms

12. Rutherford’s Conclusion
Atoms are made of mostly EMPTY SPACE!
Actually, the ratio of the size of the nucleus to the diameter of the orbits of electrons can be compared with placing a marble in the middle of a football stadium!

13. Constructing Atoms…
An atom has an atomic number of “6”, and a mass number of “14”.
Sketch the Atom
Use the 2-8-8…rule for electron orbitals
Identify the Element (Periodic Table)
Is the atom the most common form for the element?
An atom has an atomic number of “14”. Sketch its most common form!

14. Periodic Table
Groups
Periods

15. Group... Within a Group or Family Moving Down a Group
Same number of electrons in outer level
React similarly
Are likely to form similar Ions
Moving Down a Group
Add one electron shell each time
Elements on the left (Group 1) get more reactive as you go down a column.
Elements on the right (Group 7) get less reactive as you go down a column.

16. Periods... Elements in the same period… As you go across a period…
Have the same number of energy levels
As you go across a period…
Atomic number increases by “1”
One electron is added to the outer shell each time
Change in reactivity
Form different types of Ions