Periodic trends can be stated as the as the patters that helps in present in the periodic table and helps in describing the different aspects of the element, which includes the size and the different properties of the electrons. The different properties of the electrons can be termed ass electronic properties. The major and important periodic properties are electronegativity, electron affinity, ionization potential, the melting point, atomic size and the characteristics of metals. The periodic table is one of the helpful source for the chemists as it helps them by providing them with an individual tool that can easily predicts the properties of the elements. This periodic trends exists due to the presence of similarity in the atomic structure of the elements with respect to their group of families and it also exists due to the periodic nature of the different elements. However, it can be stated that periodic trend is the variation in the properties of an element when the atomic number is increased. Periodic trend is related with the regular change in the atomic structure of all the elements present in the periodic table. However, while moving from left to right across the periodic table it is observed that the physical properties of all the elements changes. The changes are also due to the changes in the physical properties and due to the interactions of the bond with the elements.

    Electronegativity can be stated as the ability of the atom to attract and combine with other electrons. Electronegativity is the atoms tendency to attract the electrons and form different bond with different electrons. While moving from left to right across the period it is observed that the electronegativity increases. While moving down the group the electronegativity decreases. Ionization energy is the energy which is required to eliminate an electron from its outermost shell in order to attain the stability. While moving left to right across the periodic table it is observed that the ionization energy of the elements increases. Electron affinity can be termed as the ability of an atom to accept an electron in order to attain the stability. It is observed that the more negative is the electron affinity, greater is the chance of atoms affinity for electrons. While moving left to right in the periodic table it is observed that the electron affinity increases. While moving down the group the electron affinity decreases. Atomic radius can be easily observed throughout the periodic table. It is the distance from the nucleus of the atoms to the electrons present in the outermost valence shell.  It is observed that while moving left to righ