Transcript Coloring the Periodic Table - Families

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Dmitri Mendeleev, a Russian
scientist born in Tobolsk, Siberia in
1834, is known as the father of the
periodic table of the elements.
The periodic table of the elements
is an important tool used by
students and chemists around the
world to help them understand and
simplify the often complex world of
chemical reactions.
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Mendeleev set out to find a pattern in the
elements.
He wrote facts on paper cards for each
element.
Melting Point
 Density
 Colors
 Atomic Masses
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After laying all of his cards out he noticed
that by arranging them according to their
properties they were arranged in order of
increasing atomic mass.
Mendeleev was even able to use the
patterns in his table to predict the
properties of undiscovered elements.
The first periodic table was published in
1869.
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Arrangement of the known elements based on
atomic number and chemical and physical
properties
Divided into three basic categories:
 Metals
 Non-Metals
 Metalloids
The periodic table is useful in
predicting:
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Chemical behavior of the elements
Trends
Properties of the elements
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Atoms are made of protons, electrons, and
neutrons.
Elements are atoms of only one type.
Elements are identified by the atomic
number (# of protons in the nucleus).
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Electrons are arranged in a region around the
nucleus called an electron cloud. Energy levels
are located within the cloud.
At least one energy level and as many as seven
energy levels exist in atoms.
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Electrons in levels farther away from the
nucleus have more energy.
Inner levels will fill first before outer
levels.
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Energy levels hold a specific amount
of electrons:
 1st
level = up to 2
 2nd level = up to 8
 3rd level = up to 8 (first 18 elements only)
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The electrons in the outermost level are
called valence electrons.
Determine reactivity - how elements will react
with others to form compounds
 The outermost level does not usually fill
completely with electrons.
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Elements are grouped into vertical columns
because they have similar properties.
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These are called groups or families.
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Groups are numbered 1–18.
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Group numbers can help you determine the
number of valence electrons:
Group 1 has 1 valence electron.
 Group 2 has 2 valence electrons.
 Groups 3–12 are transition metals and
commonly have 1 or 2 valence electrons, but
may have more.
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Groups 13–18 have 10 fewer than the group
number. For example:
Group 13 has 3 valence electrons.
 Group 15 has 5 valence electrons.
 Group 18 has 8 valence electrons.
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Reactivity is a chemical property that
determines how elements will react
with others to form compounds.
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What makes an element reactive?
● Number
of valence electrons each atom
has
● When outer levels are full, atoms are
stable.
● When they are not full, they react:
●Gain, lose, or share electrons
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The most reactive metals are the elements
in Groups 1 and 2.
Elements in Group 1 need seven more electrons
to fill their outer level.
 Elements in Group 2 need six more electrons to
fill their outer level.
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These groups are known as the “givers”
because they easily give up their valence
electrons to make a compound.
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The most reactive nonmetals are the elements in
Groups 16 and 17.
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Elements in Group 16 only need two more electrons to fill
their outer level.
Elements in Group 17 only need one more electron to fill
their outer level.
These groups are known as the “takers” because
they easily receive valence electrons to make a
compound.
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Groups run vertically in the periodic table.
They are numbered from 1–18.
Elements in the same groups have the same
number of valence electrons in the outer
energy level with the exception of some
transition metals.
Grouped elements behave chemically in
similar ways.
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The Periodic table is designed to help you predict
what an element's physical and chemical properties
are.
You can also predict what elements will bond with
each other.
Vertically into Groups
Horizontally Into Periods
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An example…
Be (Beryllium)
Atom
Mg (Magnesium) Atom
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The number of outer or “valence” electrons
in an atom effects the way an atom bonds.
The way an atom bonds determines many
properties of the element.
This is why elements within a group usually
have similar properties.
you would see…
An example…
4th Shell
K (Potassium)
Kr (Krypton)
Atom
Atom
Fe (Iron) Atom
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The periodic Table is divided into several
groups based on the properties of
different atoms.
Families/Groups
on the Periodic Table
 Elements on the periodic table can be organized into
families or groups based on their physical and
chemical properties.
 Each family/group has a specific name to
differentiate it from the other families/groups in
the periodic table.
 Elements in each
family/group react
differently with
other elements.
Fill in the notes as we go thru….
Color code each small section so that
you will know how to color/label the
‘big’ Periodic table.
HYDROGEN
 Stands alone
 1 valence electron
 Very reactive
 Reacts violently with Oxygen under right conditions
ALKALI METALS
Group 1
 Hydrogen is not a member, it is a
non-metal.
 1 valence electron in its
outermost shell
 Soft and silvery metals
 Very reactive, esp. with water
and the halogens (group 17 with
7 valence electrons)
 Conduct electricity
Image: http://www.learner.org/interactives/periodic/groups2.html
ALKALINE EARTH METALS
Group 2
 2 valence electrons in
the outermost shell
 White and malleable
metals
 Reactive, but less
than Alkali metals
 Conduct electricity
TRANSITION METALS
Groups 3-12 in the middle
 The number of valence
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electrons is varied in the
transition metal groups.
Less reactive than the first
two groups.
Can bond with many elements
in a variety of shapes.
Good conductors of heat and
electricity.
Some are used for jewelry.
METALLOIDS
 A zig-zag line that separates metals from
metalloids—Outline the metalloid element
boxes darkly
 Elements from Groups 13–17 contain some
metalloids.
 These elements have characteristics of
metals and non-metals.
BORON FAMILY
Group 13
 3 valence electrons in the
outermost shell
 Most are metals
 Boron is a metalloid
 Mildly reactive; need to
lose three electrons or
gain five electrons to be
stable.
 Aluminum is the 3rd most
common element in the
Earth’s crust
 Increase in reactivity as
the atomic number
increases (move down).
CARBON FAMILY
Group 14
 4 valence electrons in
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the outermost shell
Contains metals (Sn, Pb),
metalloids (Si, Ge), and a
non-metal Carbon (C)
Mildly reactive; need to
lose or gain four
electrons to be stable.
Sometimes found bound
to itself such as in
diamonds, tin cans, lead
pipes.
Carbon is found in all
organic matter.
NITROGEN FAMILY
Group 15
 5 valence electrons in
the outermost shell
 Mildly reactive Can
share electrons to
form compounds.
Needs to lose five
electrons or gain
three electrons to be
stable.
 Contains one metal
(Bi), metalloids (As,
Sb), and non-metals
(N).
OXYGEN FAMILY
Group 16
 6 valence electrons in the
outermost shell
 Contains metalloids (Te,
Po) and non-metals (O, S,
Se)
 Reactive, but less than
the Halogens (group 17)
 Oxygen is the most
common element found in
the Earth’s crust and as
O2 is needed for us to
breathe.
HALOGENS
Group 17
 7 valence electrons in
the outermost shell
 All are non-metals
 Very reactive and are
often bonded with
elements from the
Alkali Metals (Group 1)
 Also known as ‘saltformers’ because they
form salts when they
react with metals.
NOBLE GASES
Group 18
 Non-metals
 8 valence electrons in
the outer shell =
Stable
 Helium (He) has only
2 electrons in the
outer shell = Stable
 Not reactive with
other elements
 Exist as gases
Lanthanides and Actinides
(Rare Earth Metals)
 Some are
Radioactive (give
off radiation)
 Some rare
earths are
silver, silverywhite, or gray
metals.
 Conduct
electricity