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The Periodic Table of elements
mercutio F.4D(6)
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Section 1ltPeriodic Table of elements and
history
gtSection 2ltMain Group and who was

discovery and when gtSection
3ltR.A.M and date of discovery gtSection
4ltHow to use Periodic Table gt
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Section 1ltPeriodic Table of elements and
historygt
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D. I. Mendeleyev(Right Picture) was the first to
state the periodic law close to its present form.
He proposed in 1869 that the properties of
elements are periodic(Left Picture) functions of
the atomic weight and grouped the elements
accordingly in a periodic system. Working
independently and not aware of Mendeleyev's work,
Lothar Meyer arrived at a similar system,
publishing his results about a year after
Mendeleyev's. When Mendeleyev devised his
periodic table a number of positions could not be
fitted by any of the then known elements.
Mendeleyev suggested that these empty spaces
represented undiscovered elements and by means of
his system accurately predicted their general
properties and atomic weights.
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Mendeleevs periodic table of 1869 seems all the
more remarkable when we consider his relative
isolation from the main centres of chemical
research in Western Europe,and the rather naive
attempts made by scientists in those centres to
bring some sort of order to the growing list of
chemical elements. The concept that Mendeleyev
found most helpful in laying out his table was
the notion of valences, proposed in 1852 by the
English chemist Sir Edward Frankland. The idea
was this almost all the elements known at the
time would combine with either hydrogen or
oxygen, so the valence of an element was related
to the number of atoms of hydrogen or oxygen that
combined with that element.
A modern version of the Table appears below.
Atoms are ordered by their atomic number in the
Periodic Table. The Table is set up so as to
indicate the number of electron shells in each
atom and the number of valence electrons
(electrons in the outermost shell) in the atom.
As you descend rows in the Table, the number of
electron shells in the atom increases.
In 1869, the Russian chemist Mendeleyev noted
that the repeating patterns of behavior could be
arranged in a sequence of elements giving rise to
the "Periodic Table" of the elements.
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The alkali metals, found in group 1 of the
periodic table, are very reactive metals that do
not occur freely in nature. These metals have
only one electron in their outer shell.
Therefore, they are ready to lose that one
electron in ionic bonding with other elements. As
with all metals, the alkali metals are malleable,
ductile, and are good conductors of heat and
electricity. The alkali metals are softer than
most other metals. Caesium and francium are the
most reactive elements in this group. Alkali
metals can explode if they are exposed to water.

The Alkali Metals are Lithium
,Sodium ,Potassium ,Rubidium ,Caesium ,Francium
Section 2ltMain Groupgt

• The alkaline earth elements are metallic elements
  found in the second group of the periodic table.
  All alkaline earth elements have an oxidation
  number of 2, making them very reactive. Because
  of their reactivity, the alkaline metals are not
  found free in nature.
• The Alkaline Earth Metals are
• Beryllium,Magnesium,Calcium,Strontium ,Barium
  ,Radium

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The 37 elements in groups 3 through 12 of the
periodic table are called "transition metals". As
with all metals, the transition elements are both
ductile and malleable, and conduct electricity
and heat. The interesting thing about transition
metals is that their valence electrons, or the
electrons they use to combine with other
elements, are present in more than one shell.
This is the reason why they often exhibit several
common oxidation states. There are three
noteworthy elements in the transition metals
family. These elements are iron, cobalt, and
nickel, and they are the only elements known to
produce a magnetic field.
The Transition
Metals areScandium,Titanium,Vanadium,Chromium,Ma
nganese,Iron,Cobalt,Nickel,Copper,Zinc,Yttrium,
Zirconium,Niobium,Molybdenum,Technetium,Ruthenium,
Rhodium,Palladium,Silver,Cadmium,Lanthanum,Hafniu
m,Tantalum,Tungsten,Rhenium,Osmium,Iridium,Platinu
m,Gold,Mercury,Actinium,Unnilquadium,Unnilpentium
,Unnilhexium,Unnilseptium,Unniloctium,Unnilennium

• The 7 elements classified as "other metals" are
  located in groups 13, 14, and 15. While these
  elements are ductile and malleable, they are not
  the same as the transition elements. These
  elements, unlike the transition elements, do not
  exhibit variable oxidation states, and their
  valence electrons are only present in their outer
  shell. All of these elements are solid, have a
  relatively high density, and are opaque. They
  have oxidation numbers of3,4,and3.
• The "Other Metals" are
• Aluminium,Gallium,Indium,Tin,Thallium,Lead
  ,Bismuth

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Non-metals are the elements in groups 14-16 of
the periodic table. Non-metals are not able to
conduct electricity or heat very well. As opposed
to metals, non-metallic elements are very
brittle, and cannot be rolled into wires or
pounded into sheets. The non-metals exist in two
of the three states of matter at room
temperature gases (such as oxygen) and solids
(such as carbon). The non-metals have no metallic
luster, and do not reflect light. They have
oxidation numbers of 4, -3, and -2.
The
Non-Metal elements are
Hydrogen,Carbon,Nitrogen,Oxygen,Phosphorus,Sulph
ur,Selenium

• The halogens are five non-metallic elements found
  in group 7 of the periodic table. The
  term"halogen" means "salt-former" and compounds
  containing halogens are called "salts". All
  halogens have 7 electrons in their outer shells,
  giving them an oxidation number of -1. The
  halogens exist, at room temperature, in all three
  states of matter
• Solid- Iodine, Astatine Liquid- Bromine Gas-
  Fluorine, Chlorine
• The Halogens are
• Fluorine,Chlorine,Bromine,Iodine,Astatine

The six noble gases are found in group 18 of the
periodic table. These elements were considered to
be inert gases until the 1960's, because their
oxidation number of 0 prevents the noble gases
from forming compounds readily. All noble gases
have the maximum number of electrons possible in
their outer shell (2 for Helium, 8 for all
others), making them stable.
Helium,Neon,Argon,Krypton,Xenon,Ra
don
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Section 3ltR.A.M and date of discoverygt
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Someone do not know the elements were date of
discovery and Relative Atomic Mass(R.A.M),so I
scanned some information (have 103 elements) to
give they.The small picture is a scientists
note for elements.
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The easiest way to locate elements on the table
is by their atomic numbers. The Table of the
elements gives the atomic number of each element.
Chemists place the elements into classes that
have some similar properties. These classes are
shown in color on the periodic table.Uses of the
periodic table include comparing the chemical
behavior of the elements. For example, group 8A
contains the elements helium, neon, argon,
krypton, xenon, and radon. These elements,
called the noble gases, are gases at ordinary
temperatures and pressures. None of them
combines easily with other elements to form
compounds. This behavior is especially
interesting when compared to that of the elements
one atomic number higher and one atomic number
lower than each noble gas. These neighboring
elements are among the most easily combined
elements. The atoms of the neighboring elements
often change their electronic structure to that
of the nearest noble gas atom.One way to change
an atom's electronic structure is for it to
combine with other atoms and gain or lose
electrons. When atoms or groups of atoms gain or
lose electrons, they become ions and take on an
electric charge. For example, when sodium metal
reacts with chlorine gas, each sodium atom loses
one electron and each chlorine atom gains one.
The sodium ion then has the same electronic
structure as an atom of the noble gas neon. The
chlorine ion has the same electronic structure as
an atom of the noble gas argon.
Section 4ltHow to use Periodic Table
gt
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Developed by awareness of repetitions in the
property similarities of the known elements, it
was charted by Dmitri Mendeleyev for his students
(see at right) , and first published in 1869 with
his "periodic law" presenting that the sequence
of elements depended on their weights (later
changed to atomic number).Atomic MassAtomic
NumberThe number of protons in an atom defines
what element it is. For example carbon atoms
have six protons, hydrogen atoms have one, and
oxygen atoms have eight. The number of protons
in an atom is referred to as the atomic number of
that element. The number of protons in an atom
also determines the chemical behavior of the
element. Atomic SymbolThe atomic symbol is
one or two letters chosen to represent an element
("H" for "hydrogen," etc.). These symbols are
used internationally. Typically, a symbol is the
truncated name of the element or the truncated
Latin name of the element. Click here for a list
of the elements and their symbols.
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Atomic MassThe atomic mass is the average mass
of an element in atomic mass units ("amu").
Though individual atoms always have an integer
number of amus, the atomic mass on the periodic
table is stated as a decimal number because it is
an average of the various isotopes of an
element. Isotopes can have a weight either more
or less than the average. The average number of
neutrons for an element can be found by
subtracting the number of protons (atomic number)
from the atomic mass. Electron
ConfigurationThe electron configuration is the
orbital description of the locations of the
electrons in an unexcited atom. Using principles
of physics, chemists can predict how atoms will
react based upon the electron configuration. They
can predict properties such as stability, boiling
point, and conductivity. Typically, only the
outermost electron shells matter in chemistry, so
we truncate the inner electron shell notation by
replacing the long-hand orbital description with
the symbol for a noble gas in brackets. This
method of notation vastly simplifies the
description for large molecules. Example The
electron configuration for Be is 1s22s,2 but we
write He2s2 where He is equivalent to all the
electron orbitals in the helium atom. The
Letters, s, p, d, and f designate the shape of
the orbitals and the superscript gives the number
of electrons in that orbital.
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The End