Transcript The Periodic Table of the Elements

The Periodic Table of the
Elements
History of the Periodic Table
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Antoine Lavoisier
(1790)
23 Element List
Lost his head
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John Newlands –
1864
Forms periodic table
called octaves.
Realizes properties
repeat every 8th
element.
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Lothar Meyer, Dmitri
Mendeleev – 1869
First Periodic Table
Based upon masses
Left spaces for
missing elements
believing they would
be discovered at later
time.
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Henry Moseley –
1913
Learned that each
element has a
specific number of
protons
Developed modern
periodic table
Based upon Protons
Modern Periodic Table
Columns are called groups or families
 Rows are called periods
 Those with an “A” are called the
representative elements
 Those with a “B” are called the transition
elements
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Parts of the Periodic Table
Metals – Those that are shiny, usually
solid at room temperature, good
conductors, malleable and ductile.
 Metalloids – have physical/chemical
properties of both metals and nonmetals.
 Nonmetals – usually gas or brittle, dull
solids. Poor conductors of heat/electricity.
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Parts of the Metals
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Column 1 – Alkali Metals – All have one electron
in their outermost energy level, all react violently
with water, must be stored under oil or kerosene.
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Hydrogen is placed in the first column because of it
having one electron in its outermost level, and the
theory that on Jupiter, Hydrogen might actually be a
metal
Column 2 -Alkaline Earth Metals – Have 2
electrons in their outermost energy level, react
violently, but not as violent as Column 1.
Transitional Metals – Those metals that
exist on the middle of the periodic table.
 Inner transitional Metals – Those that exist
at the bottom of the periodic table. Are
either in the Lanthanide or Actinide Series.
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Parts of the Nonmetals
Halogens – 7A – A very reactive group of
elements. So much that they will never be
found alone in nature.
 Noble Gases – 8A – An extremely
unreactive group of elements
 Diatomic Elements - BrINClHOF
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Bohr and Lewis
Bohr Model – A planetary model of the
atom with electrons orbiting the nucleus
 Lewis Dot Structure 
Valence Electrons
First Column – 1 Valence electron
 Second Column – 2 Valence electrons
 Third Column – 3 Valence Electrons
 Fourth Column – 4 Valence electrons
 Fifth Column – 5 Valence electrons
 Sixth Column – 6 Valence Electrons
 Seventh Column – 7 Valence Electrons
 Eighth Column – 8 Valence/Except Helium
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Ionization Energy
Electronegativity
Indicates the ability of an atom to attract
electrons in a chemical bond.
 Elements that want to get rid of electrons
to complete the octet rule have low
electronegativity
 Elements that have almost 8 electrons
have a high electronegativity
 Noble gases don’t have an
electronegativity
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Bell Work 10/20/14
Show me your colored periodic table for a
grade and then keep it to study for test.
 Log on to the textbook Chapter 6
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Periodic Trends
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What trends do we know already?
Atomic Radii - today
 Ionic Radii – Today
 Electronegativity – Tomorrow
 Ionization Energy - Tomorrow
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Review
Representative Elements?
 Transitional Elements?
 Innertransitional Elements?
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Periodic Table
Russian, Dmitri Mendeleev
 when he arranged them by ___________,
he found similar properties at certain
intervals
 published the first periodic table in 1869
 left empty________ where he predicted
undiscovered _________ should be
 confirmed his predictions and
persuaded other chemists
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Periodic Table
In 1911, Henry Moseley (English) found
that the pattern worked best if arranged by
number of_________
 Our current periodic tables use this
method or arrangement
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Review
How many liquids?
 How many gases?
 How many solids?
 How many metals?
 How many metalloids?
 How many nonmetals?
 BrINCLHOF = 7th Heaven
 Coinage Metals?
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Group/Family names going across
are…
Column1 - __________ Metals
Column 2 -___________ Metals
Columns 3 -12 - ___________ Metals
Column 13 – Boron Group
Column 14 – Carbon Group
Column 15 – Nitrogen Group
Column 16 – Oxygen Group
Chalcogen Group
Column 17 - ________
Column 18 - _____ Gases
_____ Gases
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Atomic Radii
Defined by the edge of its
orbital but since the
edges are fuzzy, difficult
to determine
 Atomic Radii – half the
distance between the
nuclei of identical atoms
that are bonded together
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Atomic Radius
Atomic Radii
Which is bigger?
 Na
or Rb?
 Rb
 Na
or S?
 Na
S
or Te?
 Te
Octet Rule
In order for an element to be happy, the
outermost energy level must be full. Either
2, or 8 electrons.
 In order to reach this state, elements will
give, take, or share electrons
 Rule of Column and Charge
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Ionic Radius
Metallic Bonds
Ions slide past each other.
 Outer electrons weakly held, making good
conductor.
 Sea of Electrons
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