Some nature of the periodic elements

Periodic properties of elements are properties that change uniformly in accordance with the increase of atomic number elements. Periodic properties of elements associated with the electron structure of elements. Periodic properties of elements including the atomic radius, ionization energy, electron affinity, and electronegativity.

1. Atomic Radius
atomic radius is the distance from the center core to the outermost electron. Atomic radius is determined by measuring the bond length (distance between the nuclei) in covalent compounds, such as the Cl-Cl or H-H and then dividing by two. Therefore, the radius of an atom is often called the covalent radius.
Atomic radius varies depending on the size terikan between nucleus and electrons. The bigger the attraction, the smaller the atomic radius. Factors affecting the attraction of this is the number of protons in the nucleus and the amount of skin that contains the electrons.
Core with a lot of larger numbers of protons have a greater attraction for electrons, including the outermost electron. So, in a period from left to right, the radius of the smaller atoms. When we move from top to bottom in a class of periodic structure, the number of electron shells increases and, therefore, atomic radius increases as well.

2. Ionization Energy
Ionization energy is the minimum energy required to remove one electron from a neutral atom or an ion in the form of gas. Factors influencing the ionization energy, among others, the core charge, the distance from the core electrons, and the number of electrons that is between the outer and core electrons. In one group, atomic radius increases so that the core appeal of the smaller outer electrons, electrons are easily removed, the energy needed to remove more small. From left to right in one period, as described in the previous section, the core attraction of the greater electron, electrons are more difficult to be released, the greater ionization energy. It can be seen in this picture.












3. Electron Affinity
Electron affinity is the energy that accompanies the process of adding one electron on sati in the form of neutral gas atoms to form negative ions.










4. Electronegativity
Electronegativity is a number that states the tendency of an element to attract electrons in a chemical bond side. An atom's electronegativity is its atomic Affected by both weight and the distance That its valence electrons from the charged nucleus reside. The higher the electronegativity associated number, the more the element or compound Towards it attracts electrons.