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 Chemical Properties Conductors
Luster: reflects light
Ductile
Malleable
Solids at room temperature
Exception: Mercury
High melting point
Lose valence e- easily
Low Electronegativity
Corrode easily

7. Metals
Alkali Metals
React with water
1 ve-

8. Metals
Alkaline earth Metals
React with Halogens
2 ve-

9. Metals
Transition Metals
Many oxidation states
Different number of ve-

10. Nonmetals Physical Properties Chemical Properties
Mostly gas at room temperature.
Some solids
One liquid: Bromine
Opposing properties to metals.
Poor conductors.
Exception: Carbon
Gain or share ve-
High electronegativity

11. Nonmetals
Halogens
Form salts
Form acids when bonded to Hydrogen
7 ve-

12. Nonmetals
Noble Gases
Unreactive/inert
Odorless and colorless
8 ve-

13. Metalloids Similar to both metals and nonmetals.
Different conditions change properties.
Form alloys with metals.
Stairstep elements

14. Atomic Radii (AR)
Measured from center of the nucleus to edge of the electron cloud.
Increases down a group/family
Adds energy levels
Decreases across a period/series
More p+ and e- increases the attraction, pulling electron cloud closer to the nucleus

16. Atomic Radius Practice
Which of the following in each pair has a greater atomic radius?
Lithium or rubidium
Aluminum or chlorine
Sodium or lead
Magnesium or fluorine

17. Electronegativity (EN)
Ability to gain or hold electrons
A + e- A- + E
Forms negative ions called anions
Anion: negative “AN(t)ion”
Does not include Noble Gases

18. Electronegativity (EN)
Decreases down a group
More energy levels
More space for electrons to be lost
Less energy to lose e-
Increases across a period
More e- in energy levels
Held more tightly
More energy needed to give up e-

19. Electronegativity Practice
Which of the following in each pair has a lower electronegativity?
potassium or arsenic
Chlorine or Iodine
calcium or fluorine
Strontium or barium

20. Ionic Radii (IR) Opposite trend from atomic radii
Decreases down a family
Increases across a series
Larger atoms lose e- to become cations
Cation: positive “CATion”
Smaller atoms gain e- to become anions
Anion: negative “AN(t)ion”

22. Ionization Energy (IE)
Energy to remove outer electrons (ve-)
A + E A+ + e-
Forms positive ions called cations
Cation: positive “CATion”

23. Ionization Energy (IE)
Decreases down a group
More energy levels, electrons further from nucleus
e- easier to remove, less energy needed
Increases across a period
More e-
Held tighter to nucleus
More energy to remove e-

24. Ionization Energy Practice
Which element in the following pairs has the lowest Ionization Energy?
Boron or Nitrogen
Lithium or Neon
Sodium or phosphorus
Iodine or argon

25. Trends Practice Potassium or Hydrogen Sodium or Cesium
Which element has the lowest of all four trends? The highest?
Potassium or Hydrogen
Sodium or Cesium
Carbon or bromine
Zinc or tin