Periodic Table E Config

1. Komperda
ORGANIZATION OF THE
PERIODIC TABLE
November 2
nd
, 3
rd
& 4th, 2009

2. Komperda
How is the periodic table arranged?
Periodic table is arranged by increasing atomic
number
How did they decide when to add a new row?
A new row is needed so that elements are
arranged with repeating properties in each column
The properties of the elements repeat periodically
Hence… the periodic table!
There are many different ways to organize the
elements…

3. Komperda
Circular

4. Komperda
Long Form

5. Komperda
Spiral

6. Komperda
Pyramid

7. Komperda
Layers

8. Komperda
Which one do you like the best?

9. Komperda
Why so many versions?
Everybody sees their own pattern in the elements
What patterns did we see?
Shells
Outer Electrons

10. Komperda
Groups and Families
The columns in the periodic table are called groups, or
families.
Each group has the same number of outer shell electrons
Group 1: Alkali Metals
Group 2: Alkaline
Earth Metals
Group 7: Halogens
Group 8: Noble Gases

11. Komperda
Valence Electrons
All elements in a group have the same number of
outer shell, or valence electrons
Valence electrons determine how an element will
behave and what it bonds with
How many
valence electrons
does each group
have?

12. Komperda
Typical Charge (Ion Formed)
You should remember that 8 is great!
Elements will either gain or lose electrons to try to have 8
Elements with 3 or less electrons will LOSE electrons
Becoming _____________
Elements with 4 or more will GAIN electrons
Becoming _____________
For Hydrogen and Helium, 2 is good too!
They can’t possibly hold 8 electrons, so they are full at 2

13. Komperda
Label:
•Group name or number
•# of valence electrons
•Typical Charge
Practice

14. Komperda
Where are the electrons?
-The Bohr Atom
 Problems with Bohr Model
Only worked for
Hydrogen
Couldn’t explain where
the electrons were in
atoms that had more than
one electron
What Bohr got right
Energy Levels

15. Komperda
The difference between continuous
and quantized energy levels
How do we think energy levels work?

16. Komperda
Quantum Mechanical Model
aElectrons do not follow definite paths like the planets
pElectrons have a probability of being found in a
cloud of negative charge around the nucleus. These
clouds have specific shapes.
iThere are areas around the nucleus that correspond
with certain energy levels (like the Bohr Model)
rThe areas around the nucleus where the electron
probably is (energy levels) are called orbitals

17. Komperda
Orbitals
Do not have sharp edges
We can never map exactly where an electron is at any
given moment
All we know is the probability of an electron being in a certain
place
You know I’m probably in this room all day, you just don’t know if I’m
at my desk or in the storeroom or walking around

18. Komperda
The s Orbital

19. Komperda
The p orbitals (three of them)
The d orbitals
(five of them)

20. Komperda
Relative size of the 1s, 2s, 3s orbitals

21. Komperda
Electron Filling
Electrons like to be close to the nucleus because that
requires the least amount of energy
Electrons will fill the orbitals in this order:
1s orbital, then 2s, 2p, 3s, 3p, 4s, 3d, and so on.
This order can be seen just by looking at the periodic
table
Larger numbers mean larger orbitals, which means the
electrons is farther away from the nucleus
The farther away an electron is, the more energy it has
Think about where the office of a CEO is…

22. Komperda
Color in or outline the sections on your blank periodic
table to match this diagram

23. Komperda
Electron Configuration
When we write out the location of all electrons in
an atom, we are writing its electron configuration
Think of it like a map
Fill in the missing information on your map
Now locate the element with this electron configuration
1s
1
1s
2
2s
1
1s
2
2s
2
2p
4
Write the electron configuration for Boron