Mr. Shields
Regents Chemistry
U08 L02
1
Periodic Table
-The periodic table has 115 natural and man made elements
- 1 through 118
- 1-92 are naturally occurring
- 23 are man made
- 113, 115, 117 not yet produced
- 112 of 115 are named (112=Copernicium Cn)
- Everything above 83 is radioactive
- Through 112: 2 liquids, 11 gases, 99 solids
- 86 of the 112 named elements (78%) are metals!
2
The Gases
At STP we know there are 11 gases and 2 liquids
- 6 Noble gases
- These gases are all monoatomic
- He, Ne, Ar, Kr, Xe, Rn
- 5 other elements are gases
- These gases are always diatomic
- H2, N2, O2, F2 and Cl2
- Mercury and Bromine are liquids
3
Periodic Table
-Elements that have similar chemical properties are
aligned in COLUMNS called GROUPS
The periodic table also organizes the elements
in ROWS called PERIODS
- There are 18 groups and 7 periods
- Groups are numbered 1-18
- Periods are numbered 1-7
- corresponds to principle energy levels
4
Column numbering (1  18) is from left to right
Period numbering (1  7) goes from top to bottom
5
The Inner Transition Elements
Look at the bottom of the periodic table:
Notice the group of elements known as the Lanthanides
And Actinides are separated From the main periodic
table.
This is done strictly to help organize the periodic table.
- Table would be too large if we included them
Lanthanides/Actinides fit into period 6 & 7
- These two groups are known collectively as the
INNER TRANSITION ELEMENTS
6
These groups of elements
Actually belong here
Pulled to the bottom
to help Reduce Table size
7
Periodic Table Columns
- Numbering of Columns from 1 – 18 is new since mid 1980’s
-Tall columns on left and right originally numbered IA-VIIIA
-These are the current Groups 1,2, 13-18
- Known as the REPRESENTATIVE OR MAIN GROUPS
- Short columns in middle were originally numbered IB-VIIIB
- Corresponds to Current Croups 3 – 12
- These are known as the TRANSITION METALS
- Let’s see what this looks like…
8
Representative or Main Group
Transition Elements
1
2
3
4
5 6
7
8
9
10 11 12 13 14 15 16 17 18
9
PERIODS
The rows of the periodic table are called PERIODS
- Presently there are 7
The length of each period grows in size as we go from
Period 1 to 7
- Period 1
- Period 2&3
- Period 4&5
- Period 6
- Period 7
The change has
To do with the
Filling of the
s,p,d,f sublevels
2 elements
8 elements
18 elements
32 elements
25 (up to element 111)
10
Periods
The periods of the periodic table represent the
Number of principle energy levels contained by the
atoms in that row.
For example,
K has electrons
In the 4th Principle
Energy level:
K = 2-8-8-1
11
Blocks
As we’ve discussed before, electrons fill orbitals in
specific sublevels.
This leads to
Sections of the
the periodic table
being designated as
“Blocks” based on
what sublevel
is being filled.
12
Some Characteristics of Blocks
S Block:
- Elements in group 1-2 are very reactive metals
- Group 1 metals are so reactive they are never
found free in nature
D Block:
- Transition metal compounds are very colorful
- Copper compounds tends to form blues
- Chrome compounds tend to form yellows
P Block:
- Contains a mix of metals, metalloids, and
non-metals
F Block:
- All of the Actinides metals are radioactive
13
Common Family Names
Recall that the vertical columns of elements are called
Groups.
They are also known as families because the elements
In any given column have similar chemical Properties
Elements forming a Family have
specific Common names.
The Smiths
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Common Family Names
Family Names
Transition Metals
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
Group #
15
We’ve discussed how the periodic table is organized by:
1) Atomic number
2) Groups and periods
3) Family names
4) Block names based on which sublevels are filling
5) The representative or main group elements vs
transition & inner transition elements
And lastly, the periodic table is also organized by
6) CLASSIFICATION of the elements
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Classification by element type:
By far ….Metals are the majority (abt 80%)
85
12
7
6
17
Properties of Metals & Non-Metals
Metals
Non-Metals
HIGH
LOW (or None)
Malleable & Ductile
Brittle
CONDUCTIVITY OF
HEAT AND
ELECTRICITY
Good to Excellent
Poor or Non-Conductor
PHASE at STP
Solid (except Hg)
Gas or Solid (except Br)
Loses e- to form
positive ions
Gains e- to form
negative ions
IONIZATION ENERGY
Low (lowest is Fr)
High (noble gases are
the highest
ELECTRONEGATIVITY
Low (lowest is Fr)
High (highest is F)18
LUSTER
DEFORMABILITY
Ion FORMATION