1. Notes Date SPI 0807.9.9 Periodic Table Tennessee SPI Objective:
Use the periodic table to determine the properties
of an element.
Essential Question(s)
How do I use the periodic table to…
a) …determine the atomic number?
b) …determine the atomic mass?
c) …determine the number of sub-atomic particles?
d) …determine other properties in an atom?
Success Criteria
I can use the periodic table to determine the properties of an element.

2. (on the left and middle)
Periodic Table in 3 Sections
(1) Metals, (2) Metalloids, and (3) Nonmetals
Metals: (on the left & middle)
Metalloids: (on the zig-zag line)
Nonmetals: (on the right)
Nonmetals
(on the right)
Groups 3 to 12
are called the
transition metals
Metals
(on the left and middle)
More Metals
These are actually located above
in the 6th & 7th periods (rows) in group (column) three)

3. Notes Science Periods: SPI 0807.9.9 Periodic Table
The rows are called periods, and there are seven of them
Per 1
Per 2
Per 3
Per 4
Per 5
Per 6
Per 7
From period 6
From period 7

4. The period number tells you the number of electron shells
All elements in the same period have the same number of electron shells
1st Period = 1 Shell
2nd Period = 2 Shells
3rd Period = 3 Shells
4th Period = 4 Shells
Lithium Atom
This atom has two electron shells.
So it is located in the second period.

5. The period numbers reveal the number of electron shells
Example: Every element in period 2 has 2 electron shells
Example: Every element in period 3 has 3 electron shells
Per 1
Per 2
Period 2 (Each element here has 2 electron shells)
Per 3
Period 3 (Each element here has 3 electron shells)
Per 4
Per 5
Per 6
Per 7

6. SPI
Periodic Table
Notes
Science
Groups: The columns are called groups (also called families)
There are 18 groups 1 18 2 13 14 15 16 17 3 4 5 6 7 8 9 10 11 12

7. Lithium Atom Beryllium Atom
The group number (in some cases) can reveal how many electrons are in the outer most shells.
Note: Electrons in the outer most shells are called valence electrons
Example: Lithium (see below-left) has one valence electron, so it is in group (column) one.
Example: Beryllium (see below-right) has two valence electrons, so it is in group (column) two.
Lithium Atom
Beryllium Atom
x 4
x 5
2 Valence Electrons
1 Valence Electron

8. Memory Help: Remember V =V V for vertical = V for valence electrons
Group numbers can reveal the number of valence electrons
Note: However this only works for groups 1 to 2 and 13 to 18
(see arrows below)
See next few slides for details about how this “trick” works 1 18 2 13 14 15 16 17
This "trick" does not work with groups 3 to 12
(called transition metals)
Memory Help:
Remember V =V
V for vertical = V for valence electrons

9. Rules for Groups One and Two
Group numbers can reveal the number of valence electrons 1 2
Rules for Groups One and Two
Example:
Every element in group one has only one valence electron.
Example:
Every element in group two has exactly two valence electrons.

10. Rule for Groups 13 to 18
Group numbers can reveal the number of valence electrons 13 14 15 16 17 18
For Groups 13 to 18:
Subtract ten from each number
Example:
For group 13 subtract ten, and you get three. So every element in group 13 has three valence electrons
Example:
For group 14 subtract ten, and you get four. So every element in group 14 has four valence electrons
Number of valence electrons 3 4 5 6 7 8

11. Reactivity in Elements
For groups 1 to 2:
Reactivity increases from right to left
Ignore group 18
(called Noble Gases)
…are non-reactive/inert
For groups 13 to 17:
Reactivity increases from left to right
Groups 1 to 2
Groups 13 to 17 1 2 13 14 15 16 17
Non-reactive
Again, ignore groups
3 to 12 for now
(called transition metals)

12. Review Question For groups 13 to 17:
Reactivity increases from left to right
So it decreases from right to left
Review Question

13. Review Question
Period Four

14. Review Question
Period Two

15. Review Question
Groups 3 to 12
are called the
transition metals

16. Note: The atoms get bigger, are heavier, and have more mass as you go to the right and down the periodic table.
Review Question