1. 6.1
The Periodic Table

2. Mendeleev’s Periodic Table
Set up by atomic mass v. atomic number-modern

3. Numbering the Periodic Table

4. Groups: vertical
Similar properties in each
Periods: horizontal
No similar properties
Increasing atomic number

5. Mapping the Periodic Table: Metals, Nonmetals, Metalloids

6. Definitions
Metal: good conductor of heat and electricity, high luster (sheen), ductile, malleable
With the exception of mercury (Hg), all metals are solid at RT
Nonmetal: Most are gases at RT (Sulfur and phosphorous are solids, bromine is a liquid)
Generally poor conductors of heat and electricity
solids tend to be brittle
Semi-metal (metalloid): has a mix of properties of metals and nonmetals]
Ex: pure silicon is a poor conductor of electricity, but when mixed with boron, it becomes a good conductor of electric current

7. Group Names, Representative, Transition metals and Inner transition (rare earth) metals

8. Name the 3 broad classes of elements
Which of these sets of elements have similar physical and chemical properties?
oxygen, nitrogen, carbon, boron
strontium, magnesium, calcium, beryllium
nitrogen, neon, nickel, niobium
Identify each as a metal, nonmetal, or semi-metal
gold
sulfur
silicon
barium
Name 2 elements that have similar properties to sodium

9. Electron configuration Ions and charges Periodic Trends
Ch. 6.2 and 6.3
Electron configuration
Ions and charges
Periodic Trends

10. Electron config. Blocks

11. Valence electrons Valence Electrons (v.e.):
electrons used in bonding elements
Electrons in the highest energy level
s and p sublevels – maximum is 8
Valence electrons is the same as the group number (for representative elements)
Example: Mg is group 2A, has 2 v.e.

12. Valence electrons in P.T.

14. Lewis Dot Structures

15. Ions Atoms gain or lose electrons to obtain a noble gas configuration
Cations: positive charge bc they LOSE electrons.
Ca: loses 2 e- becomes +2 charge to be like Ar (Ca2+)
Anions: negative charge bc they GAIN electrons
Cl: gains 1 e- become 1- charge to be like Ar (Cl-)

16. Charges of the Ions

17. Atomic Size (radius): one half the distance between the nuclei of 2 atoms of the same element when 2 atoms are joined.
Ions: atom (or group of atoms) that has a positive or negative charge by losing or gaining electrons.
Anions: larger than original atom
Cations: smaller than original atom

18. Atomic Radius

19. Vocabulary
Ionization Energy: energy required to remove the first electron from an atom. 
Electronegativity: the ability of an atom to attract an electron when an atom is in a compound. (number value assigned arbitrarily )

23. Increasing electronegativity and ionization energy