1. Chapter 5: The Periodic Table

2. Now, we are going to color the Periodic Table
First, pick 4 separate colors.
Color 1- Metals Color 3- Metalloids
Color 2- Non-Metals Color 4- Liquids

3. Types of Elements Metals Non-metals Metalloids Noble Gases Left Side
Right Side
Metalloids
Touch the zig-zag staircase
Noble Gases
All the way Right

4. Periodic Table Label the names of the different Groups (columns)
Group 1- Alkali Metals
Group 2- Alkali Earth Metals
Group Transition Metals
Group 17- Halogens
Group 18- Noble Gases

5. Periodic Table Created by Dmetri Mendeleev
The Periodic Table is based on Trends
Atomic Number
Periodic Law: The Periodic Table arranged the elements in order of increasing atomic number
The Atomic Number equals what?
Which element in the row has the highest Atomic Number?
Rh Ag Sn
Rb K Na
Cu Co Ni

6. Periodic Table Periods Horizontal Rows Written on the Left Hand Side
The Period number equals the number of Principle Energy Levels
How many electrons are in the first principle energy level?
The second?
The third?
The fourth?
How many principle energy levels do each of the following elements have? C? H?
Al?
Ge?
Hg?

7. Periodic Table Groups Vertical Columns
Written on the Top Side
The Group number equals the number of Valence Electrons
These elements will have similar chemical properties and react similarly
Exceptions are the Transition Elements
How many valence electrons do each of the following elements have? C? H?
Al?
Si? B?
Na?
Which of the above pairs will react similarly?

8. Metals Left of the staircase- Except Hydrogen (H)
Low ionization energy
Low electronegativity
Tend to lose electrons and form positive ions
Smaller radius
Metallic luster
Malleable
Able to be made into sheets
Ductile
Can be made into wires
Good conductors of heat and electricity
Most are solids at room temperature
Exception? Which is a liquid?

9. Non-Metals Right of the staircase High ionization energy
High electronegativity
Tend to gain electrons and form negative ions
Larger radius
Lack a metallic luster
Brittle
Not malleable or ductile
Poor conductors of heat and electricity
Usually gases, molecular solids, or network solids
Exception? Which is a volatile liquid?

10. Metals
Non-Metals
Ionization energy
Low
High
Electronegativity
Electrons
Lose
Gain
Ions
Positive
Negative
Luster
Metallic
Non-metallic
Malleable
Yes
No- Brittle
Ductile
Conductors
Good
Poor
Usual Phase
Solid
Gas

11. Metalloids
They touch the staircase
All solids
Have properties of both

12. Noble Gases Group 18 All have a FULL valence shell Monatomic gases
Complete outer principle energy shell
All have 8 valence electrons
Except He. Why?
Monatomic gases
Stable
Elements with an oxidation number of 0 are completely unreactive
He, Ne, Ar, Rn
Elements that contain oxidation numbers other than zero have SOME reactivity
Kr, Xe
As you go DOWN in Group 18, dispersion forces increase
We will talk more about this in another chapter
Forces of attraction holding the atoms together
This causes the boiling point to increase

13. Allotropes Different forms of the same element
Different molecular formulas or different crystalline formulas
Allotropes have different properties of the element
For example:
Oxygen has 2 allotropes
O2 is what we breathe and O3 is the ozone layer
Carbon has many allotropes
Diamond: Every carbon is bonded in a tetrahedron
Graphite: Carbons are attached in sheets or layers
Coal: Carbon atoms have no pattern
Buckminsterfullerene: Carbon atoms are arranged like a soccer ball

14. Open your workbook to p. 83-85 (1-29)1* 2 3 7 1 1 4 3 1 4 3 2

15. Ions What is the charge of an electron? Good, negative
So, if you lose a negative charge, what charge will you gain?
Think…if you subtract a negative in math
Or, 0 – (-1) = ?
If a metal loses an electron, it gains a positive charge
Vice versa, if you gain a negative charge, what charge will you get?
Think…if you add a negative in math
Or, 0 + (-1) = ?
If a nonmetal gains an electron, it gains a negative charge
Ions and atoms differ only in their number of electrons
Ions always have a COMPLETE outer shell
Full valence electrons

16. Review What are the three types on subatomic particles? Protons (+)
Neutrons (o)
Electrons (-)
Similariteis
Differences
Isotopes
Same
Differ
Charge
Mass
Ions

17. Group 1 Alkali Metals Soluble Soft VERY reactive
Cuts easily with a plastic knife
VERY reactive
Never occur free in nature
Fluorine is also very reactive and does not occur free in nature
As you go down, reactivity increases
Which element has the greatest reactivity?
Lose e- to form stable, positive compounds

18. Group 2 Called Alkali Earth Metals Some form soluble compounds
Some are insoluble
More dense than Group 1
Harder than Group 1
Cuts with a steel knife
Doesn’t react in cold water
Only HOT water and it reacts slowly
As you go down, reactivity increases
Which element in Group 2 has the greatest reactivity?
In nature, they are only found in compounds
Lose e- to form stable, positive ions

19. Group 3-12 Called Transition Metals
Contain multiple positive oxidation states
Ions form COLORED SOLUTIONS

20. Group 17 Called Halogens Very active! Reacts VERY fast
Only exists in compounds
As you go up, reactivity increases
Which element in Group 17 has the greatest reactivity?
Fluorine is so reactive that it will react with heavier Noble Gases

21. Group 18 Called Noble Gases Smaller ones DO NOT react
Heavier ones will react with Fluorine and Oxygen
Kr, Xe, and Rn

22. Properties of Elements
Two types of Properties
Physical and Chemical
Physical
Characteristic of a substance that you can notice without changing the substance into anything else
Can you think of some physical properties?
Color, odor, soluble, malleable, conductors, density, phases, boiling point, melting point, hardness, etc
Table S

23. Properties of Elements
Two types of Properties
Physical and Chemical
Chemical
How an element will react in a chemical reaction- how will it change
Can you think of some chemical properties?
Reactivity? Is it able to burn? Does it react with water? Valence electrons? etc.
Table S
What weapon can you make from the elements potassium, nickel and iron?
KNiFe

24. Ionization Energy Amount of energy needed to remove an electron
The smaller the amount of ionization energy, the easier it is to lose an electron
Groups
Ionization energy decreases as you go down
Further away from protons, so easier to remove
Periods
Ionization energy increases as you go across
If you forget, LOOK ON TABLE S

25. Electronegativity Attractions for electrons Groups
Larger the electronegativity, the more the atoms attracts electrons
Groups
Electronegativity decreases as you go down
Further away from protons, so less attraction
Periods
Electronegativity increases as you go across
If you forget, LOOK ON TABLE S

26. Atomic Radius Distance from the nucleus to the valence electrons
Period
As you go across, the radius decreases
Larger positive nucleus charge causes electrons to pull in closer
Group
As you go down, the radius increases
Due to the extra electron shell
TABLE S

27. Ionic Radius
Distance from the nucleus to the valence electrons on an ion
Metals tend to lose electrons
Ca (loses 2 electrons) -> Ca+2
Because it loses electrons, its outer shell is closer. So, radius is smaller
Nonmetals tend to gain electrons
O (gains 2 electrons) -> O-2
Because it gains electrons, its outer shell is fuller. So, radius is bigger

28. Open your workbook to p. 1, 1 4, 4 4 3 1 3, 3 Don’t worry 2 2 3 1
Nonmetal, High Reactivity
p. 3:13
Don’t worry