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Periodic Table of Elements
chlorine
nitrogen
gold
silver
mercury
oxygen
hydrogen
helium
sodium
niobium
neodymium
carbon
Elements


Science has come
along way since
Aristotle’s theory of
Air, Water, Fire, and
Earth.
Scientists have
identified 90 naturally
occurring elements,
and created about 28
others.
Periodic Table

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The periodic table organizes the elements in a
particular way. A great deal of information about an
element can be gathered from its position in the
period table.
For example, you can predict with reasonably good
accuracy the physical and chemical properties of
the element. You can also predict what other
elements a particular element will react with
chemically.
Understanding the organization and plan of the
periodic table will help you obtain basic information
about each of the 118 known elements.
Mendeleev

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
In 1869, Dmitri Ivanovitch
Mendeléev created the first accepted
version of the periodic table.
He grouped elements according to
their atomic mass, and as he did, he
found that the families had similar
chemical properties.
Blank spaces were left open to add
the new elements he predicted
would occur.
In
1869 Mendeleev and Lothar Meyer (Germany)
published nearly identical classification schemes
for elements known to date. The periodic table is
base on the similarity of properties and reactivities
exhibited by certain elements. Later, Henri
Moseley ( England,1887-1915) established that
each elements has a unique atomic number, which
is how the current periodic table is organized.
Properties of Metals

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Metals are good conductors
of heat and electricity.
Metals are shiny.
Metals are ductile (can be
stretched into thin wires).
Metals are malleable (can
be pounded into thin
sheets).
A chemical property of
metal is its reaction with
water which results in
corrosion.
Properties of Non-Metals


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Sulfur
Non-metals are poor
conductors of heat and
electricity.
Non-metals are not
ductile or malleable.
Solid non-metals are
brittle and break
easily.
They are dull.
Many non-metals are
gases.
Properties of Metalloids




Silicon
Metalloids (metal-like)
have properties of both
metals and non-metals.
They are solids that can
be shiny or dull.
They conduct heat and
electricity better than nonmetals but not as well as
metals.
They are ductile and
malleable.
Families

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Columns of elements are
called groups or families.
Elements in each family
have similar but not
identical properties.
For example, lithium (Li),
sodium (Na), potassium
(K), and other members of
family IA are all soft,
white, shiny metals.
Periods

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Each horizontal row of
elements is called a
period.
The elements in a period
are not alike in properties.
In fact, the properties
change greatly across
even given row.
Families on the Periodic Table

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Elements on the periodic table can be
grouped into families (also known as
groups or columns) bases on their
chemical properties.
Each family has a specific name to
differentiate it from the other families in
the periodic table.
Elements in each family react differently
with other elements.
ALKALI METALS
Group 1
 Hydrogen is not a member, it is
a non-metal
 Soft and silvery metals
 Very reactive, esp. with water
 Conduct electricity
Alkali Metals


The alkali family is found in
the first column of the
periodic table.
They are shiny, have the
consistency of clay, and are
easily cut with a knife.
Alkali Metals


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They are the most
reactive metals.
They react violently
with water.
Alkali metals are
never found as free
elements in nature.
They are always
bonded with
another element.
Alkaline Earth Metals


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They are never found uncombined in nature.
They have two valence electrons.
Alkaline earth metals include magnesium
and calcium, among others.
ALKALINE EARTH METALS
Group 2
 White and
malleable
 Reactive, but
less than
Alkali metals
 Conduct
electricity
TRANSITION METALS
Groups in the middle


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
Good conductors of
heat and electricity.
Some are used for
jewelry.
The transition metals
are able to put up to
32 electrons in their
second to last shell.
Can bond with many
elements in a variety
of shapes.
Transition Metals

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Transition Elements
include those elements
in the B families.
These are the metals
you are probably most
familiar: copper, tin,
zinc, iron, nickel, gold,
and silver.
They are good
conductors of heat and
electricity.
Transition Metals

The compounds of transition metals are usually
brightly colored and are often used to color paints.
Boron Family

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The Boron Family is
named after the first
element in the family.
This family includes a
metalloid (boron), and the
rest are metals.
This family includes the
most abundant metal in the
earth’s crust (aluminum).
BORON FAMILY
Group 3
 Most are
metals
 Boron is a
metalloid
Carbon Family


This family includes a
non-metal (carbon),
metalloids, and metals.
The element carbon is
called the “basis of life.”
There is an entire branch
of chemistry devoted to
carbon compounds called
organic chemistry.
CARBON FAMILY
Group 4
 Contains
metals,
metalloids,
and a nonmetal Carbon
(C)
Nitrogen Family
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The nitrogen family is named
after the element that makes
up 78% of our atmosphere.
This family includes nonmetals, metalloids, and
metals.
Other elements in this family
are phosphorus, arsenic,
antimony, and bismuth.
NITROGEN FAMILY
Group 5
 Can share
electrons to
form
compounds
 Contains
metals,
metalloids,
and nonmetals
Oxygen Family


Most elements in this family
share electrons when
forming compounds.
Oxygen is the most
abundant element in the
earth’s crust. It is extremely
active and combines with
almost all elements.
OXYGEN FAMILY
Group 6
 Contains
metals,
metalloids,
and nonmetals
 Reactive
Halogen Family


The elements in this
family are fluorine,
chlorine, bromine,
iodine, and astatine.
Halogens are the most
active non-metals. They
are never found free in
nature.
Halogens
Group 7
 Used as
disinfectants
 All are nonmetals
 Very reactive
are often
bonded with
elements from
Group 1
Noble Gases
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Noble Gases are colorless gases that are extremely unreactive.
One important property of the noble gases is their inactivity.
They are inactive because their outermost energy level is full.
Because they do not readily combine with other elements to
form compounds, the noble gases are called inert.
The family of noble gases includes helium, neon, argon,
krypton, xenon, and radon.
All the noble gases are found in small amounts in the earth's
atmosphere.
Noble Gases
Group 8
 Exist as gases
 Non-metals
 Not reactive
with other
elements
Rare Earth Elements
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The thirty rare earth
elements are composed
of the lanthanide and
actinide series.
One element of the
lanthanide series and
most of the elements in
the actinide series are
called trans-uranium,
which means synthetic or
man-made.
Rare Earth Metals
 Some
are
Radioactive
 The rare
earths are
silver,
silverywhite, or
gray
metals.
 Conduct
electricity
Periods
•Each
row is called a “period” or
“series”
•The period or row number tells
you how many energy levels an
atom has -
Group
Groups
Group
8 = 8 electrons
1 = 1 electron
Group
Except
for
He, it has 2
electrons
2 = 2 electrons
•Each
column is called a
“group”
•The
group number tells us
the number of electrons an
atom has in its outermost
energy level -
•The
electrons in the outer
energy level are called
“valence electrons”
Transition Metals
•
How many
valence
electrons do
the transition
metals have?
Determine the number of energy
levels and the number of valence
electrons for:

2nd
Period = 2 shells
4th
Group =
4 valence
electrons
Determine the number of energy
levels and the number of valence
electrons for:

3rd
Period = 3 shells
1st
Group =
1 valence
electron

Name
the element.
Number of energy
levels ?
Valence electrons ?

Name
the element.
Number of energy
levels ?
Valence electrons ?
Neon
2nd
Period = 2 energy levels
8th

Group = 8 valence
electrons

Name
the element.
Number of shells ?
Valence electrons ?

Name
the element.
Number of energy
levels ?
Valence electrons ?
Hydrogen
1st
Period = 1 energy level
1st

Group = 1 valence
electron

Name
the element.
Number of shells ?
Valence electrons ?
Potassium
4th
1st

Period = 4 shells
Group = 1 valence
electron