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Periodic Properties of the Elements: Trends in the Periodic Table

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Ionization Energy
Ionization energy or ionization potential is the energy required to completely remove an electron from a gaseous atom or ion. Ionization energy is also required to remove a second valence electron from the univalent ion to fo

The properties of the elements exhibit trends and these trends can be predicted with the help of the periodic table. They can also be explained and understood by analyzing the electron configurations of the elements. This is because, elements tend to gain or lose valence electrons to bring into being the stable octet formation.

The properties of the elements exhibit trends and these trends can be predicted with the help of the periodic table. They can also be explained and understood by analyzing the electron configurations of the elements. This is because, elements tend to gain or lose valence electrons to do the job the stable octet formation.

In build-up to this activity, there are two other important trends. First, electrons are added, one at a time, moving from left to right biased a period. And, as this happens, the electrons of the outermost shell experience increasingly strong nuclear attraction. As a result, the electrons naturalize closer to the nucleus and more tightly bound. The second trend is the moving down a wing in the periodic table, where the outermost electrons assimilate to less tightly trim to the nucleus. And these trends explain the periodicity observed in the elemental properties of subatomic radius, ionization energy, electron affinity, and electronegativity.

But, early going into that we need to know a bit more in all directions the topping mentioned terms:

Atomic Radius
The indivisible radius of an element is half of the distance the centers of two building block of an element that are in contact with each other. Generally, the microscopic radius decreases obliquely a period, from left to right and increases down a given group. Therefore, the with the largest microscopic radii are located in Group I and at the lower half of groups.

Ionization Energy
Ionization energy or ionization potential is the energy required to completely remove an electron from a gaseous atom or ion. And, the closer and more tightly an electron is division line to the nucleus, the more difficult it is to remove and the higher its ionization energy. Ionization energy is also required to remove a second valence electron from the univalent ion to form the divalent ion, and so on.

Electron Affinity

Electron liability is the energy be converted into that occurs when an electron is another to a gaseous atom. It reflects the know-how of an atom to fall into an electron. And the matter with stronger effective nuclear governance have a greater electron affinity. Therefore, some generalizations can be made within call the electron affinities of warranted groups in the periodic table. The alkaline earths have low electron predilection values. This is they have filled sub shells. But, the halogens have high electron affinities as things go of the adding of an electron to an atom results in a completely filled shell. Noble gases have zero electron affinities, since each atom possesses a stable octet and will not catch an electron readily.

Electro negativity

An atom with higher electro negativity has a great facility for pulling bonding electrons. Therefore, electro negativity is a measure of the captivation of an atom for the electrons in a chemical bond. It’s related to ionization energy. So, electrons with low ionization energies have low electro negativities for their nuclei do not exert a strong lovely force on electrons. And, elements with high ionization energies have high electro negativities. This is as of the strong pull exerted on electrons by the nucleus.

Therefore, electro negativity is dependant on the isotopic number. As the an number increases, the electro negativity decreases, as a result of increased distance the valence electron and nucleus. An example of an electropositive element, i.e. one with low electro negativity, is cesium. And an example of a highly electronegative element is fluorine.

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