1. The Periodic Table

2. History of the Periodic Table
1871 Mendeleev: The First Periodic Table
Arranged elements by increasing Atomic Mass
Noticed repetition, or periodic pattern, in the chemical and physical properties of known elements
Blank spaces – Predicted the existence of elements not yet discovered based on trends in properties
1913 Moseley
Determined that atoms of each element contain a unique number of protons in their nuclei – Number of Protons = Atomic Number
Arranged table by increasing Atomic Number
Clear periodic pattern observed

3. Atomic Structure Timeline
1869
1913
Dmitri Mendeleev’s arrangement of the periodic table
Henry Moseley’s arrangement of the periodic table

4. PERIODIC LAW
When elements are arranged in order of increasing atomic number:
There is a periodic repetition of their physical and chemical properties
You can determine the properties of an element based on its location on the periodic table
Write this on the back of your paper (up at the top)

5. Locate the Periodic Table on the bottom of the page
Color in the mini periodic table like you will see it on the next slide
Be sure to fill in the key with the colors you chose
Next to the word metal, put: (cation + charge)
Next to the work nonmetal, put: (anion - charge)
Next to the word group, put the definition on the following slide
Next to the word period, put the definition on the following slide

6. The periodic table can be divided into
Three main categories: metals,
Nonmetals, and metalloids
Group/Family
Period

7. The Modern Periodic Table
18 Groups/Families
Vertical Columns
Elements have similar physical and chemical properties and reactivities
Group/Family
Period
7 Periods
Horizontal Rows
Determines number
of energy levels

8. Locate the Periodic Table on the TOP of the page
In the appropriate space on the top of the page, write the definition for both valence electrons and oxidation number
Fill in the oxidation numbers and valence electrons for each of the groups on the periodic table

9. Oxidation Number
The charge on an ion of an element; The number of electrons lost, gained, or shared during chemical bonding
Oxidation # +1 -1 +2 +3
+/-4 -3 -2

10. Electrons in the outermost energy level (valence shell)
Valence Electrons
Electrons in the outermost energy level (valence shell)
Valence Electrons 1 7 8 2 3 4 5 6

11. Locate the Periodic Table on the TOP of the page
For each group that is on the page, write the important properties next to the group name and color in the group whatever color you choose.
Make sure to fill in the key with the appropriate colors that you chose

12. Groups/Families ALKALI METALS Most reactive metals Soft, shiny metals12

14. Groups/Families ALKALINE EARTH METALS Second most reactive metals
Gray-White luster 14

15. Groups/Families LANTHANIDES Rare Earth Elements Soft, malleable metals
Great conductors 15

16. Groups/Families ACTINIDES Rare Earth Elements Radioactive
Almost all are manmade 16

17. Groups/Families TRANSITION METALS Less active than Group 1 or 2 metals
Have variable numbers of valence electrons 17

18. Groups/Families HALOGEN FAMILY Most reactive Non-Metals
Fluorine most REACTIVE element!! 18

19. Groups/Families NOBLE GASES Valence shell is full
8 Valence Electrons (except Helium with 2)
Valence shell is full
Non-Reactive (why react when you already have 8 e-!) 19

20. Turn to the back of the page
Label each mini periodic table with the trends. Draw and label all arrows and any extra information that I added to the slide
Explanation of the trend – the third to the last slide has a summary of all of the trends for you to look over and summarize in that box.

21. Ionic Radius Ionic Radius Size of an ion
distance from nucleus to outermost e-

22. The size of an ion (distance from nucleus to outermost electrons)
Ionic Radius
The size of an ion (distance from nucleus to outermost electrons)
Increasing Ionic Radius
Increasing Ionic Radius Cs
Largest ion!!
Increasing Ionic Radius

23. Atomic Radius Atomic Radius Size of an atom
distance from nucleus to outermost e-

24. The size of an atom (distance from nucleus to outermost electrons)
Atomic Radius
The size of an atom (distance from nucleus to outermost electrons)
Increasing Atomic Radius
Increasing Atomic Radius Cs
Largest atom!!
Increasing Atomic Radius

25. Ionization Energy Ionization Energy:
Energy required to remove electrons from an atom
LOW ionization energy  EASY for an atom to lose electrons
Ex: Group 1 elements
HIGH ionization energy  HARD for an atom to lose electrons
Ex: Group 17 elements

26. The energy required to remove electrons from
Ionization Energy
The energy required to remove electrons from
an atom
Increasing Ionization Energy
Increasing Ionization Energy
Increasing Ionization Energy

27. Electronegativity Electronegativity:
Tendency for an atom to take electrons
HIGH Electronegativity  Tends to GAIN electrons easily
LOW Electronegativity  Tends to LOSE electrons

28. Electronegativity Increasing Electronegativity F
The tendency for an atom to take (attract) electrons
Increasing Electronegativity F
Increasing Electronegativity
Most electronegative element!!
Increasing Electronegativity