Periodic Table

The periodic table is an arrangement of all known elements in order of increasing atomic number and recurring chemical properties. 

• To facilitate the study of elements, all known elements must be arranged according to their properties, with related elements falling into the same groups and dissimilar elements being separated. This process is known as element classification.
• The Mendeleev periodic table, an earlier version of the periodic table, was based on the law that “Physical and chemical properties of elements are the periodic function of their atomic masses”.
• Mendeleev’s (1861) scientific classification of chemical elements based on their masses or atomic weights has been disproved, leading to the development of the modern periodic table law.
• The Modern periodic table, long form of the periodic table, is based on the law that “Physical and chemical properties of elements are the periodic function of their atomic numbers”.
• The classification of elements in the long version of the periodic table is based on the order of increasing atomic numbers or Periodicity (i.e., periodic repetition of attributes).
• Periodicity is the recurrence of similar-behaving elements at regular intervals when these elements are grouped in ascending order of their atomic numbers.
• There are 18 vertical columns of elements known as groups and seven horizontal rows of elements known as seven periods. The modern periodic table, therefore, contains 18 groups, which are numbered from 1 to 18.
• The periodic table contains interesting facts that clearly illustrate the relationship between electronic structure and periodic accommodation capacity as the purpose of chemical elements.
• The atomic structure or the electrical arrangement of an element determines its periodicity.
• As a result, the recurrence of comparable features results from repeated electrical configurations or atomic structures. Thus, the repetition of an analogous electrical arrangement is the cause of periodicity.
• The many kinds of metals and non-metals in chemistry are arranged into the s, p, d, and f-block on the periodic table by the modern periodic law, which is based on the atomic number and valence shell electron configuration of elements.
• s- block elements: The arrangement of electrons in the periodic table gives rise to the designation “s-block element” in which the valence electron enters the ns-orbital and gradually fills it by the configuration rules. S-block elements are the 1st and 2nd group elements.
• p-block elements: The last electron in a P block element enters one of the three p-orbitals of its corresponding shell. As a p-subshell has three degenerate p-orbitals, each of which may hold two electrons, there are six groups of p-block elements. P-block elements are those that belong to groups 13 to 18. ns² np^1-6 is the general electrical configuration for these elements.
• d-block elements: d-block elements are those that are found from Group 3 to Group 12 in the middle of the periodic table. Because the final electron gets to the d-orbital of the penultimate shell, they are known as a “d-block” element.
• f-block elements: The f-block elements, also known as inner transition elements, are those whose final electron to enter the f-orbital is known. In addition to having electrons in the outermost orbital, these elements also have electrons (0 to 1) in the penultimate energy level’s d orbital and (1 to 14) in the f orbital. In the f-block, there are mainly two series that correspond to the filling of the 4f and 5f orbitals.