Transcript Periodic Table and Electron Configurations Honors Chemistry

Periodic Table
and
Electron Configurations
Honors Chemistry
Unit 3
Modern Periodic Table
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Elements are arranged by increasing
atomic number.
– Recall that atomic number gives the number
of protons in the nucleus of an atom.
The Periodic Law says:
When elements are arranged in order
of increasing atomic number, there is a
periodic repetition of their physical
and chemical properties.
 Horizontal rows = periods
– There are 7 periods
– Each row (or period) is the energy level
 Vertical column = group (or family)
– Similar physical & chemical properties
– Identified by number (1 - 18)
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Periods
Groups/Families
Areas of the periodic table
Three classes of elements are:
1. Metals
2. Nonmetals
3. Metalloids
Notice the heavy, stair-step line?
• This is the dividing line between
the Metals and Non-Metals
Properties of Metals
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 Most are silver/grey in
On the Left side of the
color
table
Does not include hydrogen  Conducts heat and
electricity
Solids at room
 Will lose electrons to
temperature (except for
form (+) ions (cations)
Mercury)
Shiny
Ductile: can be made into
wires
Malleable: can be pounded
& easily shaped, like
knives and swords
Properties of Non-metals
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On the right side of
the periodic table
Most are gases (H,
He, Ne, etc.)
Brittle, or break
easily
Dull texture
Poor conductors of
heat and electricity
Will Gain electrons to
become negative
ions (anions)
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Come in a variety of
colors
Properties of Metalloids
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Properties are intermediate between metals
and nonmetals
Also called semi-metals
They are on the stair step line in between the metals
and non-metals
They have a combination of both metallic and nonmetallic properties
– Ex: they are shiny but don’t conduct electricity
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Semiconductors – conduct electricity under certain
circumstances (some used in computer technology)
Metallic Character
Metals
 Nonmetals
 Metalloids
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Blocks
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Main Group Elements – groups 1, 2 &13-18
Transition Metals – groups 3-12
Inner Transition Metals
Sublevel Blocks
1
2
3
Period
Number
4
5
6
7
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Each row (or period) is the energy level
for s and p orbitals.
s1
1s1
Elements in the s - blocks
s2
2s2
He
Group 1 metals all end in s1
 Group 2 metals all end in s2
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– really should include He, but it fits
better in a different spot, since He has
the properties of the noble gases, and
has a full outer level of electrons.
7s1 7s2
The P-block – groups 13 - 18
p1 p2
2p1
p3
p4
p5
p6
2p6
3p1
6p1
6p6
Transition Metals - d block
Groups 3 - 12
1
d
3d1
4d1
5d1
2
d
3
d
d4
9
5
6
7
8
d
d d d d
10
d
3d10
F - block
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Called the “inner transition elements”
f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14
4f1
5f1
1
2
3
4
5
6
7
4f
f
5f
orbitals start filling at 4f, and
are 2 less than the period
number
The “f” Block
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The “d” orbitals fill up in levels 1 less
than the period number, so the first d is
3d even though it’s in row 4.
1
2
3
4
4d
5d
5
6
7
3d
Writing Electron Configuration from
the Periodic Table
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The way an electron configuration ends
will tell you what element you have.
Examples:
Mn
1. 3d5
Rb
2. 5s1
Ge
3. 4p2
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Chemistry Crash Course video - Periodic
Table