Download Periodic Table of Elements

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Introduction:
Periodic Table of Elements
Science Links
2013-2014
Introduction:
• Each row is called a period.
• Elements within periods do NOT show
similarities.
• The periodic table arranges
information in a logical
way.
• The columns of elements
are called groups or
families.
• Elements in the same
family have similar
properties
Valence Electrons:
• In chemistry, valence electrons are the
electrons contained in the outermost, or
valence, electron shell of an atom.
Helium atom model
This helium (He) model displays two valence
electrons located in its outermost energy level.
Helium is a member of the noble gases and
contains two protons, neutrons, and electrons.
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Metals:
• Metals are found on the LEFT side of the
periodic table.
Metals Physical Properties:
• The physical properties of metals make them easy
to identify.
• Metals:
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Conduct Heat
Conduct Electricity
Have a Bright Metallic Luster
Are Malleable
Have High Melting Points
• Give everyday examples of the above in your
notes!
Metals Chemical Properties:
• Metal atoms can have 1, 2, 3, or 4 electrons
in their outer shell. (Valence)
• This means they commonly share their
electrons in chemical bonding.
Non-Metals:
• Non- Metals are found on right side of the
periodic table.
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Non-Metal Physical Properties:
• Non-Metals have no luster and are dull in
appearance.
• They do NOT conduct heat or electricity
very well.
• Non-Metals are often brittle and have lower
densities and lower melting points than
metals.
Metalloids:
Non-Metal Chemical Properties:
• Atoms of non-metals have 5, 6, 7, or 8
electrons in their outer energy level.
• This means that they tend to accept
electrons when they combine chemically.
• Those with 8 valence electrons are stable
and non-reactive.
Zig Zag Stairstep – divides metals and non-metals
metaloids are on the border
• These elements have properties of
both metals and non-metals.
• Metalloid means “sort of metal”
• Metalloids can be shiny or dull;
they conduct heat and electricity
better than non-metals, but not as
well as metals.
• They are ductile and malleable.
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The Families
Family 1:
• The elements in family 1 (except hydrogen)
are alkali metals.
• These atoms have 1 valence electron.
• They are the most reactive metals
• Alkali Metals: Li, Na, K, Rb, Cs, and Fr
Families 3-12:
• The elements in columns 3 to 12 are the transition
metals.
• Transition metals are good conductors of heat and
electricity, and are often highly colored.
• Examples: Zn, Hg, and Pt
Family 2:
• Elements in family 2 are the Alkaline
Metals (or alkali Earth metals).
• They have 2 valance electrons.
• Alkaline Metals: Be, Mg, Ca, Sr, Ba, and
Ra
Family 13:
• Family 13 is the Boron family.
• These elements have 3 valence electrons;
Boron is the only non-metal, the other are
metals.
• Aluminum is the most abundant metal on
Earth.
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Family 14:
• Family 14 is the Carbon family.
• These atoms have 4 valence electrons.
• The metalloids include Silicon and
Germanium, and the metals are Tin and
Lead.
Family 16:
• Family 16 is the Oxygen family, and these
atoms have 6 valance electrons.
• These atoms also tend to share electrons
when forming compounds.
• Oxygen is the most abundant element in the
earth’s crust and the 2nd most in the
atmosphere.
• Examples: S, Te, and Po
Family 15:
• Family 15 is the Nitrogen Family.
• These atoms have 5 valence electrons and
tend to share electrons when they bond.
• Nitrogen is the most abundant element in
the Earth’s atmosphere.
Family 17:
• Family 17 is known as the Halogen family.
• They have 7 valence electrons and are the most
reactive non-metals.
• They only need to gain 1 electron and are not
found as free atoms in nature.
• They often combine with the transition metals.
• Examples: Cl, I, and Br
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Family 18:
Periods
• In the periodic table, elements
have something in common if
they are in the same row.
• The last family is known
as the Noble Gasses.
• These elements are
typically stable because
their outer shell is full with
8 valance electrons.
• Most atoms strive to be
like the Noble Gases.
• Examples: Ne, Ar, and Kr
• All of the elements in a period
have the same number of
atomic orbitals. Every element
in the top row (the first period)
has one orbital for its electrons.
Periods
• All of the elements in the
second row (the second period)
have two orbitals for their
electrons. It goes down the
periodic table like that.
• At this time, the maximum
number of electron orbitals or
electron shells for any element
is seven.
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