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THE PERIODIC TABLE
Chapter 4
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HOW ARE ELEMENTS ORGANIZED?
Groups of elements share certain properties
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PERIODIC PATTERN
Newlands (1865) – Arranged elements
according to increasing atomic mass
Properties repeated every 8 elements
Law of octaves
Dobereiner (early 1800s)
Groups of 3 elements have similar properties
Triads
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MENDELEEV
First periodic table
63 known elements at the time
Mendeleev’s table contains gaps that unknown elements should fill
He predicted the properties of these unknown elements & gave them names
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MOSELEY
Arranged elements according to atomic number
Erased the discrepancies in Mendeleev’s table
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OTHER CONTRIBUTIONS
Seaborg – pulled out inner transition elements
to condense periodic table
Ramsey – discovered noble gases
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PERIODIC LAW
Elements with similar properties appear at
regular intervals (when arranged by atomic #)
Valence electrons – outermost electrons in an
atom of an element
Electrons that participate in chemical reactions
with other atoms
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GROUPS/FAMILIES & PERIODS
Group/family = vertical column on the periodic
table
Elements have similar chemical properties because
of same # of valence electrons
Period = horizontal row
Elements have same number of occupied energy
levels (i.e. energy level 2)
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GROUPS AND PERIODS
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THE PERIODIC TABLE
Main Group elements
Transition elements
Inner transition elements
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METALS, NONMETALS, METALLOIDS
Metals – occupy the majority of the periodic table
Located to the left of the “staircase”
Lustrous, Malleable, Ductile, Conductors
Alloy = a solid or liquid mixture of 2 or more metals
Nonmetals – generally opposite properties of metals
Metalloids – have properties of both, located along the “staircase”
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METALS, NONMETALS, METALLOIDS
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TRANSITION METALS
d-block elements
Groups 3-12
Do NOT have identical outer electron
configurations
May lose different #’s of valence electrons
Good conductors, ductile, malleable
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LANTHANIDE & ACTINIDE SERIES
f-block elements
Lanthanides – first row of inner transition
elements
Shiny metals, similar in reactivity to alkaline earth
metals
Actinides – second row
Radioactive
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ns
1
ns
2
ns
2n
p1
ns
2n
p2
ns
2n
p3
ns
2n
p4
ns
2n
p5
ns
2n
p6
d1
d5
d1
0
4f
5f
Ground State Electron Configurations of the Elements
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ALKALI METALS – GROUP 1A (GROUP 1)
React with water to make alkaline solutions
One valence electron = VERY reactive
Lose their 1 valence electron to achieve noble gas configuration (octet)
Soft texture, dull or shiny, good conductors
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Group 1A Elements (ns1, n 2)
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ALKALINE EARTH METALS – GROUP 2A (GROUP
2)
Highly reactive
2 valence electrons
Harder and have higher melting points than
alkali metals
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Group 2A Elements (ns2, n 2)
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COMMON GROUP ELEMENTS – 3A TO 5A
(GROUPS 13-15)
3, 4, or 5 valence electrons (depending on group)
Some metals, some metalloids, some nonmetals
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Group 3A Elements (ns2np1, n 2)
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Group 4A Elements (ns2np2, n 2)
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Group 5A Elements (ns2np3, n 2)
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CHALCOGENS – GROUP 6A (GROUP 16)
Oxygen group
6 valence electrons
Name means “ore former”
Nonmetals, metalloids, metals
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Group 6A Elements (ns2np4, n 2)
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HALOGENS – GROUP 7A (GROUP 17)
Highly reactive nonmetals
7 valence electrons (1 short of a noble gas
configuration)
Often react with alkali metals
“Salt maker”
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Group 7A Elements (ns2np5, n 2)
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NOBLE GASES – GROUP 8A (GROUP 18)
Inert = unreactive
8 valence electrons (full set); except He (2 e-)
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HYDROGEN
Most common element in
the universe
1 electron
Extremely flammable
Reacts unlike any other
element
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PERIODIC TRENDS
Predictable change in a particular direction
Reactivity of Alkali metals
Increases as you down the group
Reactivity of Halogens
Increases as you go up the group
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IONIZATION ENERGY
Energy supplied to remove an electron
IE + X (g) X+(g) + e-
Filled n=1 shell
Filled n=2
shell
Filled n=3
shell Filled n=4 shell
Filled n=5
shell
Electron Shielding – outermost electrons
are not held as tightly to the nucleus due
to the inner electrons “shielding” them
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General Trend in Ionization Energies
Increasing First Ionization Energy
Incre
asin
g F
irst Io
niz
atio
n E
ne
rgy
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ATOMIC RADIUS
Atomic radius = ½ the distance from the center to the center of
2 like atoms that are bonded
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Atomic Radii
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ELECTRONEGATIVITY
Ability of an atom in a compound to attract
electrons
Fluorine has highest electronegativity value
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ELECTRON AFFINITY
Electron affinity = energy change when a
neutral atom gains an electron
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Cation is always smaller than atom from which it
is formed.
Anion is always larger than atom from which it is
formed.
ION SIZE
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Comparison of Atomic Radii with Ionic Radii