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The Periodic Table
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Period
• The 7 horizontal
rows
Example:
• Period 1 has 2
elements: Hydrogen
(H) and Helium (He)
• Period 2 has 8
elements
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Group
• Vertical column of the
Periodic Table
• A group is also called
a family of elements
because all elements
in the same group
share some physical
and chemical
properties
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Metals • Include all members of
Groups 1 through 12 as
well as some elements
of Groups 13 through 16
• All metals are good
conductors of electricity
• Conductivity increases
as temperature
decreases
• All are solid at room
temperature except
Mercury
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Transition Metals
• Elements in Groups 3 through 12 including
the two long rows below the main table
• Have varied properties
• Not as reactive as Group
1 and 2 elements
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Nonmetals • Elements in Groups 17
and 18 as well as some
members of Groups 14
through 16
• Poor conductors of
electricity
• Conductivity increases
as temperature
increases
• Can be gases, solids or
liquids at room
temperature
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Semiconductors
(metalloids)
• Not in one group but spread across groups
13-16 starting with Boron, Silicon,
Germanium, Arsenic, Antimony and
Tellurium
• Conduct electricity better than nonmetals
but not as well as metals
• Useful in electronic devices
• Solid at room temperature
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Lanthanides and Actinides
• Lanthanides –
rare earth metals
(lanthanum)
• Actinides –
radioactive elements
(uranium)
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Group Names
• Group 1: Alkali Metals (Note – Hydrogen
is not a metal but it is in group 1)
• Group 2: Alkali Earth Metals (Be, …)
• Groups 3 – 12: Transition Metals
• Metalloids/Semiconductors: Not in one
group but spread across groups 13-16
starting with Boron, Silicon, Germanium,
Arsenic, Antimony and Tellurium
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Group Names (cont.)
• Group 17: Halogens (F, Cl, Br, I, …)
• Group 18: Noble Gases (He, Ne, Ar, …)
• Lathanides: elements after Lanthanum to
Lutetium
• Actinides: Actinium to Lawrencium
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6
C Carbon
12.011
Atomic #: # of Protons
Element Symbol
Element Name
Atomic Mass: # of
Protons + # of Neutrons
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Julius Meyer
• 1830-1895
• Used atomic weights
to arrange 28
elements into 6
families that had
similar chemical and
physical properties
• Incomplete periodic
table
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Dmitri Mendeleev
• 1834-1907
• Left gaps (worked on Meyers)
• Predicted that new elements would be discovered
• Arranged elements known at
the time by similarities in their
physical and chemical
properties
• Ordered by increasing atomic mass
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Henry Moseley
• 1888-1915
• Arranged elements by increasing atomic number
• Discrepancies disappeared
• Similar physical and chemical properties occur at regular intervals (periodic law)
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Moseley (cont.)
• Moseley’s discovery was consistent with
Mendeleev’s ordering of the periodic table
by properties rather than strictly atomic
number
• He showed that there were gaps in the
sequence at numbers 43, 61 and 75 (now
known to be radioactive, non-naturally-
occurring, technetium and promethium,
and the last discovered naturally-occurring
element rhenium, respectively)
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Periodic Law
• Periodic Law states: ‘the physical and
chemical properties of the elements are
periodic functions of their atomic
numbers’
• The periodic table is an arrangement of
the elements in order of their atomic
numbers so the elements with similar
properties fall in the same group or column
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Past to Present
• The periodic table has changed since
Mendeleev’s time
• Chemists have discovered new elements
• In recent years chemists have synthesized
new elements in the laboratory
• Significant addition to the periodic table
was discovery of the noble gases
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