1. Periodic table

2. Arrangement Mendeleev arranged the first periodic table.
Arranged by increasing atomic mass.
Periodic Law: arranged in order of increasing atomic number.
Repetition of properties.

3. Arrangement
Periods/Series: horizontal rows

4. Arrangement
Groups/Families: vertical columns

6. Metals Physical Properties
Good electrical conductors
Solids at room temperature
Good heat conductors
High melting point
High density
Lustrous
High boiling point
Ductile
Malleable

7. Metals Chemical Properties
Lose valence e- easily
Low Electronegativity
Corrode easily

8. Alkali Metals React with water Not found in nature Soft
1 valence electron
Oxidation of +1
Loses 1 electron to form bonds
Lower melting and boiling points

9. Alkaline Earth Metals React with Halogens to form salts
Not found in nature
Low density
Found in molecules in earth’s crust
2 valence electrons
Oxidation of +2
Loses 2 electrons to form bonds

10. Transition Metals Vary in oxidation states
Different number of valence electrons
Mercury

11. Inner Transition Metals
Lanthanides
Actinides
“Pull out” rows in periods 6 and 7
Trans-uranium: man-made (nuclear chemistry)

12. Nonmetals Physical Properties
Mostly gas at room temperature.
Poor conductors of heat
Poor electrical conductors
Brittle
Non-lustrous
Low melting and boiling points

13. Non-metals Chemical Properties
Gain or share valence electrons

14. Halogens (Nonmetals) Form salts when bonded to alkaline earth metals
Form acids when bonded to Hydrogen
7 valence electrons
Oxidation of -1
Readily reactive

15. Noble Gases (Nonmetals)
Unreactive/inert
Odorless
Colorless
8 valence electrons (2 for He)
Full octet (outer shell)

16. Metalloids Similar to both metals and nonmetals.
Different conditions change properties.
Form alloys with metals.
“Stair-step” elements

17. Valence and trends

18. Valence Electrons
Valence electrons – Electrons in an atom’s highest-numbered energy level.
How many are in each of the examples?

19. Valence Electrons Shortcut
You can tell how many valence electrons any atom should have by its position in the periodic table. 1 2 3 4 5 6 7 8
variable

20. Octet Rule 8 electrons in outer shell is most stable (one exception)
Atoms will combine to make the octet full, giving them the same electron configuration as the closest noble gas.
How many electrons do each element (from the example) want to lose or gain?

21. Atomic Radii (AR)
Center of the nucleus to edge of the electron cloud.

22. Atomic Radii (AR) Increases down a group
Each new energy level adds radius
Electrons have more room to move around

23. Atomic Radii (AR) Decreases across a period
More protons and electrons in the same energy level (same amount of space)
Increased attraction pulls the e- cloud closer to the nucleus (like magnets)

24. Electronegativity (EN)
Ability to gain or hold electrons
Forms a negative ion (anion)
A + e- A- + E
Does not include Noble Gases

26. Electronegativity (EN)
Decreases down a group
As you move down, space is added between e- and nucleus
Lessens attractive force between p+ and e-
Easier for e- to be removed from atom

27. Electronegativity (EN)
Increases across a period
More e- in the same energy level,
e- are held more tightly by larger attractive force of nucleus

28. Ionization Energy (IE)
Energy put into molecule to remove outer shell electrons (valence electrons)
Forms a positive ion (cation)
A + E A+ + e-

30. Ionization Energy (IE)
Decreases down a group
More space between nucleus and electrons
Less energy to remove e- due to less attractive force

31. Ionization Energy (IE)
Increases across a period
More e- in the same energy level
Held tighter because of higher attractive force from nucleus
More energy to remove e-