Transcript The properties of Periodic table of elements.

The properties of Periodic
table of elements.
Under normal conditions each atom is
electrically neutral, since the number of
electrons is equal to that of neutrons.Is
However, administration of energy, remove
one or more electrons. The energy
required by an atom to pull the outer
electron of energy is defined first
ionization. The energy required to remove a
second electron is called the energy of
second ionization. The atom formed after
this process is called cation, or positive
ion.
A + energia => A+ + e• The ionization is a periodic property.Furthermore as you
can see how each period beginning with a low ionization
and concludes with a noble gas at high
ionization.Although energy is growing along the period,
not growing so steadily, which is due to the increased
amount of energy that needs a doublet compared to a
separated electron.
From the table we see that the ionization
energy increases along the period from left
to right, but falls along the group progressing
top to bottom. This trend is downwards due
to the lower energy required to extract an
electron that is in the outer energy levels are
less attracted to the center. While,the
upward trend to the right is due to the
increased amount of energy, as is the larger
the atomic weight and number of neutrons,
then the electron will require more energy.
Another periodic property is electronic affinity. It
represents the amount of energy transferred when
an electron is acquired.
A+e- => A- + energia
Affinity for the electronics the same considerations of
ionization.The electron purchased will fit in the outer
level, so long the group will be less and less attracted,
while a long period with the increase of nuclear charge
will always be attracted.
Therefore, the electronic affinity decreases along the
group progressing from top to bottom, while increases
over the period from left to right.
The ionization energy and
electronic affinity are sizes that
indicate the trend that each
atom has to lose or acquire
electrons.
These properties for a more
immediate reading were linked
together in a single property: the
electronegativity. To measure this,
Pauling proposed an arbitrary scale
that assigns the highest value to
Fluorine (4) and the lowest
Cesium (0.7).
Electronegativities is the ability
that the atom of an element to
attract electrons, which agrees
with the atom of another
element when they are linked.
According to the new classification
of the factors of a metal are those
that have low ionization energy,
electronic affinity and
electronegativity.They are left or
down the periodic table.
Another periodic property :The
atomic radius.It is the distance
between the core and outer
electron and is measured
namometers or angstrom
Proceeding along the group down
there is an increase of atomic
radius and volume.This is
explained by falling into that group,
increases the number of the
“quanto principale”, increasing the
total number of levels, so it is less
the attraction towards the center.
While, over the period from right to
left there is a reduction of the
atomic radius.Infact over the period
is an increase in the number of
atoms and therefore protons for the
same principal quantum number,
and more attractive.
Work created by :
Cirillo Michela,
Loviglio Lucia,
Mastrangelo Antonio,
Moramarco Concetta,
Storsillo Sabrina.