Transcript Reading the Periodic Table

5.2 Reading the
Periodic Table
Vertical Columns
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Known as families or groups
Elements in a column tend to have
similar properties
Also have the same number of
valence, or outer electrons
Horizontal Rows
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Known as series or periods
Have the same number of electron
levels
Solids, liquids or gases?
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On the big periodic table
• Black – solids
• Blue – liquids
• Red - gases
Metals
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Found to the left of the stairstep
Properties
• Lusterous (shiny)
• Good conductors of heat and electricity
• Malleable: can be hammered into a thin
sheet
• Ductile: can be pulled into a thin wire
• Most are solids at room temperature
Non-Metals
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Found to the right of the stairstep,
includes hydrogen
Properties
• Non-Lusterous
• Poor conductors of heat and electricity
• Not malleable or ductile
• Many are gases at room temperature
Semi-metals
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Found on the stairstep
B, Si, As, Te, At, Ge, Sb
Also known as metalloids
May have properties similar to either
metals or non-metals
All are solid at room temperature
Alkali Metals
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Group 1 on the PT
Has one valence
electron.
Highly reactive
Never found in
elemental form in
nature.
Must be stored in
mineral oil to avoid
reacting with
water.
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Mostly soft and
silvery.
React with
halogens to form
salts.
More reactive the
farther down the
list you go.
Alkaline Earth Metals
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Group 2 on the PT
Has two valence
electrons.
Soft and silver
colored.
React with water,
but not as strongly
as the alkali
metals.
Also react with
halogens to form
salts.
Boron Family
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Group 3 on the PT
Has 3 valence electrons
Aluminum: 3rd most abundant
element in the earth’s crust
Carbon Family
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Group 4 on the PT
Has 4 valence
electrons
Carbon:
• Most on earth is
found in limestone
• Important because
it is found in every
living cell
• Can also be in the
form of diamonds
and graphite
• Combines with
hydrogen to form
hydrocarbons (fuels
such as methane,
propane, butane)
• Hydrocarbons make
up the majority of
the atmosphere of
Saturn’s moon,
Titan
Carbon Family, cont.
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Silicon
• 2nd most abundant
element in earth’s
crust
• Like carbon, can
form many
compounds
• Silica (silicon
dioxide) is the main
component in glass
• In its pure form, is
used to make
transistors and
solar cells
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Germanium: not
common, but is
used in electronics
Tin: coating on
“tin” cans
Lead: used to be
used in plumbing;
today it is used to
make automobile
batteries
Nitrogen Family
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Group 5 on the PT
Has 5 valence electrons
Nitrogen: makes up 78% of Earth’s
atmosphere; essential to living
organisms
Phosphorus: also found in living
things; phosphoric acid (H3PO4) is
widely used in manufacturing; also
found in soft drinks!
Oxygen Family
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Group 6 on the PT
Has 6 valence electrons
Oxygen Family, cont.
Oxygen
 Most abundant
element on Earth (2nd
most in atmosphere)
 Required for
respiration and
combustion
 Used in the steelmaking process
 Found in air as O2 and
ozone as O3
Sulfur
 Known since ancient
times as brimstone
 A main component of
“fools gold”
 Most compounds with
sulfur have unpleasant
odors (rotten eggs,
even skunks!)
 Largest use is in
sulfuric acid (H2SO4)
in manufacturing
Halogen Family
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Group 7 on the PT
Has 7 valence
electrons
Highly reactive
Only family to have
at least one solid,
one liquid and one
gas at room temp.
Fluorine is one of
the most reactive
elements in
existence
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Teflon is made of
fluorine bonded to
carbon
Noble Gas Family
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Group 8 on the PT
Most have 8 valence electrons
(helium only 2)
Odorless, colorless
Extremely low chemical reactivity
Also called inert gases
Transition Metals
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Have a variety of charge possibilities.
Many of them can have more than
one charge (ex: iron can be +2 or
+3).
They include chromium (makes
chrome), iron (structural material),
the coinage metals (copper, silver,
gold) and many others.
Inner Transition Metals
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Lanthanides:
• Form +3 ions
• Soft, silvery metals
• Most have little commercial use
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Actinides:
• All are radioactive
• Only thorium and uranium occur to any
large amount in nature