Metals
Metals are on the left side of the Periodic Table
Metals have 1, 2, 3, or 4 electrons in their
outermost energy level
Most metals have only 1 or 2 electrons in the
outermost energy level.
These valence electrons are loosely (weakly)
held the physical and chemical properties of
metals.
They behave rather like positive nuclei in a “sea”
of loosely held electrons
Physical Properties
Luster (shiny)= light reflecting off the electrons.
Very good conductors of heat and electricity
The loosely held electrons are able to move
an electric current (movement of electrons)
Silver (Ag) is the best conductor: Copper (Cu)
is the second best.
Malleable and ductile the (+) nuclei can slip
through the loosely held electrons
High density and high melting points
Chemical Properties
Metals tend to lose their outermost electrons
8 electrons in the outer shell= a stable
configuration.
The more loosely held the electrons, the more
easily they are lost, the more reactive the
metal.
Metals with 1 outer electron are the most weakly
held the most reactive metals (Group 1A, 1).
Those with 2 outer electrons (Group IIA, 2) are
slightly less reactive e
As you move down a group, the elements
become more reactive because the outer
electrons are further from the nucleus
Chemical Properties
Francium (Fr) is the most reactive metal.
Metals tend to react with air and water 
Corrosion= a gradual chemical reaction
which wears away a metal.
Rust is the corrosion of iron.
Tarnish is the corrosion of Silver (Ag)
Nonmetals
On the right side of the Periodic Table
Nonmetals have 4, 5, 6, 7, or 8 electrons in the
outermost energy level
These valence electrons are tightly held the
physical and chemical properties of nonmetals
The positive nuclei are “locked” between the
tightly held electrons which are unable to move
The number of electrons in the outer shell
determines the chemical and physical properties
of an element
Physical Properties
Usually opposite to the physical properties
of metals
Dull
Nonconductors or poor conductors of
heat and electricity
Brittle
Generally lower densities and melting
points
Chemical Properties
Nonmetals tend to gain electrons 8 electrons
in the outer shell= a stable configuration
Nonmetals that need 1 electron(s)
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Group VIIA, 17
Or 2 electrons (Group VIA, 16) to fill their outer
energy level are the most reactive
The Noble Gases are nonreactive= inert
because the outer shell is full (complete) and
thus stable
Metalloids
Solids between the metals and nonmetals
They will conduct, but not as well as metals
They are ductile and malleable, but not as much
as metals because they have 3, 4, 5, 6, or 7
electrons in the outer shell
Metalloids with 6 or 7 electrons in the outer shell
are large atoms
The outer shell is far from the nucleus and the
atom isn’t as tightly held to the nucleus.
Active Metals
Group 1A (1) = the Alkali metals
Lithium (Li), Sodium (Na), Potassium (k),
Rubidium (Rb), Cesium (Cs), and Francium
(Fr)
Hydrogen is not an alkali metal it is actually a
nonmetal
This group easily loses its 1 outer electron so it
is the most reactive group of metals
It is never found in the free or uncombined state
in nature
It must be stored under oil to protect it from
oxygen and water
It reacts violently with oxygen and water
Active Metals
The Alkali metals form important
compounds such as NaCl
They are soft, silvery, and have lower
melting and boiling points than other
metals
Sodium (Na) and Potassium (K) are the
most important to plants and animals
Active Metals
Group IIA (2) = the Alkaline Earth metals
Beryllium (Be), Magnesium (Mg), Calcium
(Ca), Strontium (Sr), Barium (Ba), Radium
(Ra)
This is the second most reactive group of
metals.
They are also never found free in nature
because their 2 outer electrons are easily lost
They are harder, denser, and have higher
melting and boiling points than Group 1
Calcium and Magnesium are the most
important both in biology and industry
Magnesium is used in fireworks, cars, planes,
spacecraft, baseball/softball bats, and old
fashioned flashbulbs
Transition Metals
Rows 3-12 (in middle of periodic table)
Often occur as uncombined elements
Often form colored compounds
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Paints—cadmium=yellow, cobalt=blue
Toxic– limited use
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Iron triad– Iron, cobalt, nickel
Used to create steel
Iron most widely used of all metals
Nickel used to give added strength and shiny,
protective coating
Transition Metals
Coinage metals– copper, silver, gold
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Most coins now made of nickel and copper
Copper used in electrical wiring
Zinc, cadmium, mercury
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Zinc and cadmium used to coat other metals
Cadmium used in rechargeable batteries
Mercury– only metal that is liquid at room temperature
Used in thermometers (not much now), thermostats,
switches, and batteries
poisonous
Lanthanides
Elements from 57-71
Commonly referred to as the rare earth metals
(along with scandium and yttrium)
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Most are not that rare though
Many more common than gold
Uses:
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catalysts
Deflect UV and Infrared rays so are often used in the
production of sunglasses
lasers
Actinides
Actinides– 89-103
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Thorium and Uranium only
ones occur in substantial
amounts in nature
Small amounts of
plutonium have been found
The rest are synthetic
Nuclear weapons have
released six others into
nature
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Bomb on Nagasaki had a
plutonium charge
Halogens
Group 17 (VIIA)
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Very reactive
Found only in nature in compounds or ions
Exists as diatomic molecules
Only periodic group exhibiting all 3 states of matter at
room temp.
If gains an electron from a metal it forms a salt
Fluorine is most reactive
Added to toothpaste and water to stop
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Chlorine disinfects water (most abundant)
Bromine is only nonmetal liquid at room temp.
Noble Gases
Stable
Eight electrons in outer
shell (except He)
All are odorless and
colorless
He used to ease
breathing for asthma
patients
Xenon is used as an
anesthetic