1. Section 4.4—The Periodic Table

2. History of the Periodic Table
Different scientists organized the elements differently—this lead to confusion
In 1869, Dimitri Mendeleev designed a periodic table based on atomic mass.
This way showed patterns in properties that repeated across rows and similarities down columns
He couldn’t find elements to fit all the property trends, so he left holes

3. History of the Periodic Table
The holes he left were later filled in as more elements were discovered
The modern periodic table is arranged by atomic number rather than atomic mass
This caused a few “switches” in placement, but overall is very similar to Mendeleev’s

4. Organization of the Periodic Table

5. Groups and Periods Groups Columns are called “groups” or “families”
Rows are called “periods”

6. Information for Each Element
Most periodic tables give the following information, but it can be in a different location
Atomic Number
Whole number—elements are ordered by this on the periodic table. 6 C
Carbon
12.01
Element Symbol
If there’s a second letter, it’s lower-case
Element Name
Atomic Mass
Number with decimals
Gives the mass for 1 mole of atoms, in grams

7. Parts of the Periodic Table

8. The rows at the bottom
Most periodic tables are written with 2 rows at the bottom.
This is done to allow the font to be bigger on a piece of paper.

9. The rows at the bottom
Most periodic tables are written with 2 rows at the bottom.
This is done to allow the font to be bigger on a piece of paper.
But they really belong here!
Follow the atomic numbers on your periodic table to see it!

10. Electron Configurations and the Periodic Table.

11. Configurations Within a Group
Look at the electron configurations for the Halogens F
1s2 2s2 2p5 Cl
1s2 2s2 2p6 3s2 3p5 Br
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 I
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5
All of the elements in Group 7 end with 5 electrons in a p subshell.
In fact, every Group ends with the same number of electrons in the highest energy subshell

12. Configurations and the Periodic Table
s-block
p-block
d-block s1 s2 p1 p2 p3 p4 p5 p6 d1 d2 d3 d4 d5 d6 d7 d8 d9
d10
f-block f1 f2 f3 f4 f5 f6 f7 f8 f9
f10
f11
f12
f13
f14

13. How to remember the filling order?1s 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d
s subshells begin in level 1, so begin the s-block with “1s”
p subshells begin in level 2, so begin the p-block with “2p”
d subshells begin in level 3, so begin the d-block with “3d”
f subshells begin in level 4, so begin the f-block with “4f”

14. How to remember the filling order?1s 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d
To see the filling order of subshells, read from left to right, top to bottom!
Note that this tool shows that the 3d energy level is filled after the 4s energy level!

15. Where Does the Noble Gas Leave Off?
How do you know where to start off after using a noble gas?
Use the periodic table! 1s He 2s 2p Ne 3s 3p Ar 4s 3d 4p Kr 5s 4d 5p Xe 6s 4f 5d 6p Rn 7s 5f 6d
The noble gas fills the subshell that it’s at the end of.
Begin filling with the “s” subshell in the next row to show valence electrons.