Unit 2: Elements & Mattermsmorrischemistry.weebly.com/uploads/3/8/9/5/38951057/jan_29.pdf · Format...
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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+