Periodic trends of the properties of the elements in the periodic table

Periodic trends of the properties of the elements in the periodic table The properties of the elements that show trends and these trends can be predicted using the periodic table. It could also be explained by analyzing the electron configurations of elements. This is because the elements of the standard, win or lose valence electrons to achieve the stable octet formation.The property of the elements that show trends and these trends can be predicted using the periodic table. It could also be explained by analyzing the electron configurations of elements. This is because the elements of the standard, win or lose valence electrons to achieve the stable octet formation.In In addition to these activities, there are two other important trends. First, the electrons are added one after the other, from left to right during a period. And, as is the case, the electrons of the outer shell experience increasingly strong nuclear attraction. As a result, the electrons are closer to the center and near. The second trend is the movement of a column of the periodic table, where the outer electrons are less firmly attached to the center. Explain these trends and periodicity of the basic properties of atomic radius, ionization energy, electronic affinity, and electronegativity.But before achieved, we need to know a little 'more of these words: atomic radius   The atomic radius of an element is half the distance between the centers of two atoms of an element that is in contact with each other. In general, the atomic radius is about a period that goes from left to right and get off after a certain group. Therefore, the atoms with the largest atomic radii are in Group I and in the lower half energy groups.Ionization   Ionization energy or ionization potential is the energy required to completely remove an electron from an atom of gas or ions. And, closer and an electron is bound in the center, the more difficult it is to be removed and its higher ionization energy. Ionization energy is also needed for a second valence electron from the univalent ions to divalent ions, and so on.Electron AffinityElectron affinity is the energy change that occurs when an electron is added to an atom of gas. It reflects the ability of an atom of an electron. And the atom with effective nuclear charge have a greater affinity for electrons. Therefore, some generalizations can be found on the electron affinity of some groups in the periodic table. The alkaline earths low electron affinity values. This is due to the fact that they are under-filled tanks. However, the halogens have high electron affinity, because the addition of an electron in an atom in a completely filled shell. Noble gases have zero affinity for electrons, since each atom possesses a stable octet, and not accept an electron readily.Electro negativityAn atom more electro negativity has a great ability to attract electrons bond. Therefore, electro negativity is a measure of attraction of an atom for electrons in a chemical bond. It is linked to the ionization energy. Thus, electrons with low IONIZATION ENERGIES low electro negativity, because their nuclei do not exert a strong attraction for electrons. And the elements with high electro negativity IONIZATION ENERGIES high. This is due to the strong drag electrons from nucleus.Therefore, electro-negativity depends on the atomic number. Since the atomic number increases, the negativity from electro, as a consequence of the increasing gap between the valence electron and nucleus. An example of an electro-positive element, ie one with low electro negativity is cesium. And an example of a very negative electro fluorine.Dr.George Grant is an expert researcher in bio-chemistry. He has extensive research and field trials. He is a teacher to visit some of the most renowned science college. For more information about the chemical instruments and definitions, see below --