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PERIODIC TABLE OF
THE ELEMENTS
Click Below &
Enjoy a Periodic Table Tune!
periodic table song
WRITE
Founding Scientists
• Mendeleev:
proposed 1st periodic table where
elements were arranged according to
ATOMIC MASS.
• Moseley:
revised periodic table and arranged
elements according to ATOMIC NUMBER.
Elements are arranged:
Vertically into Families
Horizontally Into Periods
Why?
If you looked at one
atom of every element
in a group or family
you would see…
Each atom has the same number of
electrons in it’s outermost shell, the
same number of valence electrons.
• An example…
The group 2 atoms all have 2 electrons
in their outer shells
Be (Beryllium)
Atom
Mg (Magnesium) Atom
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Families
• 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 family usually
have similar properties, both chemical and
physical.
If you looked at an atom from each
element in a period
you would see…
Each atom has the same number of
electron holding shells.
An example…
The period 4 atoms each have 4 electron
containing shells
4th Shell
K (Potassium)
Kr (Krypton)
Atom
Atom
Fe (Iron) Atom
ACTIVITY
TO GET A BETTER UNDERSTANDING
AND APPRECIATION FOR THE
STRUGGLES AND METHODOLOGY
EARLY SCIENTISTS USED TO
ARRANGE THE ELEMENTS AND FIND
TRENDS IN THEIR PROPERTIES, YOU
WILL NOW COMPLETE THE INDEX
CARD ACTIVITY.
Each FAMILY has distinct PHYSICAL
AND CHEMICAL properties
The periodic table is divided into several
FAMILIES based on the properties of
different atoms.
Label your periodic table with the following
families of elements, color coding them if
you want:
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Alkali Metals
Soft, silvery colored
metals
Very reactive!!!
CLICK ON THE LINK BELOW TO
VIEW A VIDEO:
reactions of alkali metals
Alkali Metals reacting with water:
•
•
•
•
•
Li (Lithium)
Na (Sodium)
K (Potassium)
Rb (Rubidium)
Cs (Cesium)
What would you expect
from Francium?!?!
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Reactivity of Metals
• As observed on the video, lithium is reactive,
sodium is more reactive, potassium is even
more reactive!
• Cesium blows out the wall of the glass
container!!!
• Label your periodic table with the following:
• Most reactive metals are in the bottom left of
the periodic table!
Alkaline Earth Metals
Silvery-White Metals
Fairly reactive
Many are found in rocks in
the earth’s crust
Click on the link below
to view a video
reactions of the alkaline earth
metals
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Reactivity of Metals
• Once again, as seen on the video, the
reactivity of the alkaline earth metals
increases as we go down the family!
• However, these metals are not as reactive as
the alkali metals in the same period!
• So Mg is less reactive than Na, but more
reactive than Be!!!
• Location allows prediction of reactivity!
Transition Metals
Most are good
conductors of
electricity
Malleable (easily
bent/hammered into
wires or sheets)
Click on the link below
to view a video:
properties of transition metals
How many things can you think
of that have transition metals in
them?
Metalloids
elements highlighted in pink
These elements have properties of both metals and non-metals
Highlight these on your periodic table
What are semiconductors (metalloids)
used in?
Si (Silicon) and Ge (Germanium) are very important “semi-conductors”
Halogens
Most are
Poisonous
Fairly reactive
Chlorine Gas was used as a
chemical weapon during World
War I.
It was used by the Nazis in World
War II.
CLICK BELOW TO VIEW A
VIDEO OF THE HALOGENS
REACTIVITY OF THE
HALOGENS
Reactivity of the Nonmetals
• As observed on the video, fluorine is the
most reactive of all of the nonmetals!
• Most reactive nonmetals are at the top
right of the periodic table (excluding the
noble gases of course)!
• Label your periodic table accordingly!!
• Most reactive nonmetal
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Noble Gases
Unreactive
Gases at room
temperature
Jellyfish lamps made with noble
gases artist- Eric Ehlenberger
Colors Noble Gases
produce in lamp tubes:
• Ne (Neon): orange-red
• Ar (Argon): pale lavender
• He (Helium): pale peach
• Kr (Krypton): pale silver
• Xe (Xenon): pale, deep blue
Lanthanide Series
Actinide Series
Periodic Table & Trends
repeating or cyclical patterns
WRITE
on the table
Atomic Radius (pm)
250
200
150
100
50
0
0
5
10
Atomic Number
15
20
Periodic Law
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When elements are arranged in order of
increasing atomic #, elements with similar
properties appear at regular intervals.
250
K
Atomic Radius (pm)
Na
200
Li
150
100
Ar
50
Ne
0
0
5
10
Atomic Number
15
20
ATOMIC RADIUS TRENDS
LARGEST ONES ARE THE ALKALI METALS IN THE ROW
SMALLEST ONES ARE THE NOBLE GASES IN THE ROW
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Atomic Radius
Increases DOWN
Decreases ACROSS
1
2
3
4
5
6
7
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Atomic Radius
Down a Family: Atomic Radius INCREASES
WHY? More energy levels with each
consecutive period.
Across a Period: Atomic Radius DECREASES
WHY? Effective nuclear force increases
because the attraction of the nucleus for the
electron cloud increases.
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Ionization Energy
the energy required to remove an
electron from an atom.
• Across a Period: Ionization Energy INCREASES
WHY? It becomes increasingly more difficult to
remove an electron from an atom.
• Down a Group: Ionization Energy DECREASES
WHY? It becomes increasingly less difficult to
remove an electron from an atom.
IONIZATION ENERGY
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TRENDS
HIGHEST I.E. BELONG TO THE NOBLE GASES
LOWEST I.E. BELONG TO THE ALKALI METALS
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Ionization Energy
First Ionization Energy
Increases to the RIGHT
Decreases DOWN a family
1
2
3
4
5
6
7
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Ionic Radius
Cations (+)
atoms lose eget smaller
Anions (–)
atoms gain eget larger
© 2002 Prentice-Hall, Inc.
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Electronegativity
the tendency for an atom to attract
electrons to itself when it is chemically
combined with another element
ECl > ENa
Example: NaCl Cl takes e- away from Na
ELECTRONEGATIVITY
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TRENDS
HIGHEST ELECTRONEGATIV ITY IS FLUORINE
fluorine
chlorine
bromine
LOWEST ELECTRONEGATITIES BELONG TO THE NOBLE GASES
ELECTRONEGATIVITY
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Electronegativity
Across a Period: Electronegativity INCREASES
WHY? Fluorine has a very high tendency to
attract electrons within a bond due to a high
effective nuclear force.
Down a Group: Electronegativity DECREASES
WHY? Elements in a group have
decreasing effective nuclear force. Atoms
tend to give up electrons more easily the
lower you go on the periodic table.
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Summary of Trends
Put these directly on
your periodic table
as a summary of the
trends
Increasing Ionization Energy
Increasing Electronegativity
Decreasing Size
Decreasing Ionization Energy
Decreasing Electronegativity
Increasing Size
Examples
• Which atom has the larger radius?
Be
or Ba
Ba
Ca
or Br
Ca
Examples
• Which atom has the higher 1st I.E.?
N
or Bi
N
Ba
or Ne
Ne
Examples
• Which particle has the larger radius?
S
Al
or
2S
2S
or
3+
Al
Al
COMPARISON OF METALS
WRITE AND NONMETALS
METALS
NONMETALS
•
•
•
•
Lose electrons easily
Low ionization energies
Low electronegativities
Form positive ions that
are smaller than the
atoms from which they
come
•
•
•
•
Gain electrons easily
High ionization energies
High electronegativities
Form negative ions that
are larger than the
atoms from which they
come
For the Test, know the following
• The people and vocabulary
• The families and periods
• The trends in reactivity,
electronegativity, ionization
energy, and size (explanations)
• Metal/nonmetal differences