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The Modern PeriodicTable
By:
Dato Liang Ak Seruji
Punitha A/P NagappanShutha A/P Avadiyan
Tan Shee Ying
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During the nineteenth century,
chemists began to categorize theelements according to similarities
in their physical and chemicalproperties.
The end result of these studieswas our modern periodic table.
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Scientists Involved In The
Development Of The Periodic Table In
Use Today
Antoine Lavoisier
(1743-1794)
Johann Dobereiner
(1780
1849 )
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John Newlands(1838 1898)
Dmitri Mendeleev(1834
1907)
Lothar Meyer(1830 1895)
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Henry Moseley(1887
1915)
Glenn T. Seaborg(1912 1999)
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Periodic Table
Geography
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The elements in any groupof the periodic table havesimilar physical and chemical
properties!
The vertical columns of the periodic table
are called GROUPS, or FAMILIES.
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There are 18 vertical columns of
elements in the Periodic Table, known as
Group 1, Group 2 until Group 18
Group 1 elements are known as alkali metals.
Group 2 elements are known as alkaline
earth metals. Group 3 to Group 12 elements are known as
transition elements.
Group 17 elements are known as halogens.
Group 18 elements are known as noble
gases.
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The horizontal rows of the periodic table are
called PERIODS.
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There are 7 horizontal rows of elements
in the Periodic Table, known as Period 1,
Period 2 , until Period 7
Period 1 contains 2 elements.
Periods 2 and 3 contain 8 elements. Period 4 and 5 contain 18 elements.
Period 6 contains 32 elements.
Period 7 contains 27 elements.
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Periodicity of chemical
properties The main value of the periodic table is the
ability to predict the chemical properties of an
element based on its location on the table. It
should be noted that the properties vary
differently when moving vertically along the
columns of the table than when moving
horizontally along the rows.
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Trends of groups Elements within the same group have the same electron configurations in
theirvalence shell, which is the most important factor in accounting for their similarproperties.
Elements in the same group also show patterns in theiratomic radius, ionization
energy, and electronegativity.
From top to bottom in a group, the atomic radii of the elements increase. Since
there are more filled energy levels, valence electrons are found farther from the
nucleus.
From the top, each successive element has a lower ionization energy because it is
easier to remove an electron since the atoms are less tightly bound.
Similarly, a group will also see a top to bottom decrease in electronegativity due to
an increasing distance between valence electrons and the nucleus.
http://en.wikipedia.org/wiki/Electron_shellhttp://en.wikipedia.org/wiki/Atomic_radiushttp://en.wikipedia.org/wiki/Ionization_energyhttp://en.wikipedia.org/wiki/Ionization_energyhttp://en.wikipedia.org/wiki/Electronegativityhttp://en.wikipedia.org/wiki/Electronegativityhttp://en.wikipedia.org/wiki/Ionization_energyhttp://en.wikipedia.org/wiki/Ionization_energyhttp://en.wikipedia.org/wiki/Atomic_radiushttp://en.wikipedia.org/wiki/Electron_shell7/28/2019 The Modern Periodic Table Chemistry Presentation
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Trends of periods
Elements in the same period show trends in atomic radius, ionization
energy, electron affinity, and electronegativity. Moving left to right across a period, atomic radius usually decreases.
This occurs because each successive element has an added proton and
electron which causes the electron to be drawn closer to the nucleus.
This decrease in atomic radius also causes the ionization energy to
increase when moving from left to right across a period.
The more tightly bound an element is, the more energy is required to
remove an electron.
Similarly, electronegativity will increase in the same manner as ionization
energy because of the amount of pull that is exerted on the electrons by
the nucleus.
Electron affinity also shows a slight trend across a period.
Metals (left side of a period) generally have a lower electron affinity than
nonmetals (right side of a period) with the exception of the noble gases.
http://en.wikipedia.org/wiki/Atomic_radiushttp://en.wikipedia.org/wiki/Ionization_energyhttp://en.wikipedia.org/wiki/Ionization_energyhttp://en.wikipedia.org/wiki/Electron_affinityhttp://en.wikipedia.org/wiki/Electronegativityhttp://en.wikipedia.org/wiki/Electron_affinityhttp://en.wikipedia.org/wiki/Electron_affinityhttp://en.wikipedia.org/wiki/Electron_affinityhttp://en.wikipedia.org/wiki/Electronegativityhttp://en.wikipedia.org/wiki/Electron_affinityhttp://en.wikipedia.org/wiki/Ionization_energyhttp://en.wikipedia.org/wiki/Ionization_energyhttp://en.wikipedia.org/wiki/Atomic_radius7/28/2019 The Modern Periodic Table Chemistry Presentation
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Thank You For Your
Attention!
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