Modern periodic law and the present form of periodic table

The periodic table is a cornerstone of chemistry, serving as a visual representation of the elements and their properties. From Dmitri Mendeleev’s first attempts in 1869 to organize the elements to the modern periodic table we use today, the table has undergone significant changes. This article explores the modern periodic law and its present form, shedding light on the evolution and importance of this fundamental scientific tool.

The Modern Periodic Law

The modern periodic law is a fundamental concept in chemistry that states: “The properties of elements are a periodic function of their atomic numbers.” This law replaced the earlier periodic law, formulated by Mendeleev, which was based on atomic mass. The switch to atomic number as the organizing principle was a pivotal moment in the history of chemistry and revolutionized our understanding of the elements.

Atomic number is a unique property of each element, representing the number of protons in an atom’s nucleus. Elements are arranged in ascending order of their atomic numbers in the modern periodic table. This arrangement ensures that elements with similar properties appear in the same column or group.

The Present Form of the Periodic Table

The modern periodic table has evolved from the initial version proposed by Mendeleev. It consists of 118 confirmed elements, organized into seven rows, or periods, and 18 columns, or groups. Here is an overview of the key features of the present form of the periodic table:

  1. Periods: There are seven horizontal rows in the periodic table, numbered from 1 to 7. Elements in the same period have the same number of electron shells.
  2. Groups: The periodic table is divided into 18 vertical columns, known as groups. Elements within the same group share similar chemical properties. Some of the most important groups include the alkali metals (Group 1), the noble gases (Group 18), and the transition metals (Groups 3-12).
  3. Block Classification: Elements are classified into four main blocks: s-block, p-block, d-block, and f-block. This classification is based on the subshell in which the last electron resides.
  4. Lanthanides and Actinides: The lanthanide and actinide series are placed below the main body of the periodic table. These elements are typically removed to keep the table more compact.
  5. Color-Coding: To make it easier to identify the different blocks, groups, and the classifications of elements, the periodic table often uses various colors.

Now, let’s take a closer look at a condensed representation of the periodic table, showcasing some key elements and their properties:


The modern periodic law and its manifestation in the present form of the periodic table have transformed our understanding of the elements and their relationships. This table, with its rows, columns, and blocks, is a visual masterpiece that not only organizes elements but also provides insights into their properties and behaviors. As science continues to advance, the periodic table remains an invaluable tool for researchers and students alike, offering a foundation for exploring the world of chemistry.

As our knowledge of the elements expands, so too will the periodic table evolve, ensuring that it remains a dynamic and essential resource in the realm of science.

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