The Modern Periodic Table Chemistry Presentation

7/28/2019 The Modern Periodic Table Chemistry Presentation

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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.




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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_shell


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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_radius


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Attention!

The Modern Periodic Table Chemistry Presentation

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