Unit 2: Elements & Matter January 29, 2016

How is the periodic table organized?

Part 2

4. Transition Metals

4. Transition Metals ¤ These are the metals you are probably most familiar:

copper, tin, zinc, iron, nickel, gold, and silver.

¤ They are good conductors of heat and electricity.

¤ Very hard, High melting points, High boiling points, and are Malleable

¤ The compounds of transition metals are usually brightly colored and are often used to color paints.

5. Halogens

5. Halogens ¤ Halogens have 7 valence electrons, which

explains why they are the most active non-metals. They are never found free in nature.

¤ Halogen atoms only need to gain 1 electron to fill their outermost energy level.

¤ They react with alkali metals to form salts. ¤ Very reactive, volatile, diatomic, nonmetals ¤ Used as disinfectants and to strengthen teeth.

6. Noble Gases

6. Noble Gases ¤ Noble Gases are colorless gases that are

extremely un-reactive.

¤ One important property of the noble gases is their inactivity.

¤ Because they do not readily combine with other elements to form compounds, the noble gases are called inert.

¤ All the noble gases are found in small amounts in the earth's atmosphere.

7. Rare Earth Metals

7. Rare Earth Metals ¤  The thirty rare earth elements are composed of the lanthanide and

actinide series.

Metals Metalloids

Nonmetals

8. Metalloids

8. Metalloids ¤ Metalloids (metal-like) have properties of both

metals and non-metals.

¤ They are solids that can be shiny or dull.

¤ They conduct heat and electricity better than non-metals but not as well as metals.

¤ They are ductile and malleable.

9. Nonmetals

9. Nonmetals ¤ Non-metals are poor conductors of heat and electricity.

¤ Non-metals are not ductile or malleable.

¤ Solid non-metals are brittle and break easily.

¤ They are dull.

¤ Many non-metals are gases.

How can we communicate the location of each element?

Electron Configuration

1

2

3

4

5

6

7

6

7

1A

2A

3B 4B 5B 6B 7B 8B 8B 8B 1B 2B

3A 4A 5A 6A 7A

8A

group # = # valence (outside) e-

d p

f

s Row

= # shells

An arrangement of electrons based on the elements location on the periodic table.

Format for electron configuration

1s1

row # shell #

possibilities are 1-7 7 rows

subshell possibilities are

s, p, d, or f 4 subshells

group # # valence e-

possibilities are: s: 1 or 2 p: 1-6

d: 1-10 f: 1-14

Total e- should equal Atomic #

What element has an electron configuration of 1s1?

Example Problems ¤ Write the electron configuration for the

following elements

1. O 2. Al 3. Br 4. Ar 5. Ca2+