Periodicity in Properties

Following the systematisation of the knowledge gained by a number of scientists through their observations and experiments, we have the classification of elements into groups, the development of the Periodic Law, and the development of the periodic table itself. Johann Dobereiner, a German chemist who worked in the early 1800s, was the first to consider the idea of trends in the properties of different elements. Since many elements were being discovered in the nineteenth century, it was necessary to classify them in order to study them individually. This was made possible by the classification of elements. A number of classification schemes were proposed, including ‘Dobereiner’s Triads’ and ‘Newland’s Octaves.’

Dobereiner’s Triads

Johann Wolfgang Dobereiner, a German chemist, attempted to classify elements with similar properties into groups of three elements each, based on his observations. Triads were the names given to these groups. Dobereiner predicted that in these triads, the atomic mass of the middle element would be more or less equal to the mean of the atomic masses of the other two elements in the triad, according to his calculations.

A triad containing lithium, sodium, and potassium, for instance, would be an example of this type. Lithium has an atomic mass of 6.94 and potassium has an atomic mass of 39.10. The atomic mass of sodium, the middle element in this triad, is 22.99, which is more or less the same as the mean of the atomic masses of lithium and potassium combined (which is 23.02).

The following are the limitations of Dobereiner’s Triads:

• All of the elements that were known at the time couldn’t be grouped together into triads.
• Only four triads were mentioned: (Li, Na, K), (Ca, Sr, Ba), (Cl, Br, I), and (Cl, Br, I), and (S,Se,Te).

Newland’s Octaves

In the year 1866, the English scientist John Newlands arranged the 56 known elements in increasing order of atomic mass, a method known as the Newlands classification. He noticed a trend in which every eighth element exhibited properties that were similar to the first element he discovered.

Newland’s Law of Octaves states that when the elements are arranged in increasing order of atomic mass, the periodicity in properties of two elements with an interval of seven elements between them will be similar if the elements are arranged in increasing order of atomic mass.

The following are the limitations of Newland’s octaves:

• With the exception of calcium, Newland’s Octaves were used to classify the elements until that element.
• In addition, the discovery of noble gases increased the limitations of this method because they could not be included in this arrangement without causing it to be completely disrupted.

Mendeleev’s Periodic Table 

In 1869, Russian chemist Dmitri Ivanovich Mendeleev published his periodic table, which is still in use today.

It is stated in the Periodic Law (also known as Mendeleev’s Law) that the chemical properties of elements are a periodic function of their atomic weights, and this is known as Mendeleev’s Law.

The following are some of the advantages of Mendeleev’s Periodic Table:

• The addition of these newly discovered elements to the periodic table had no effect on the structure of the table. Germanium, gallium, and scandium are examples of such elements.
• It was employed to correct the incorrect atomic weights that were in use at the time.
• Mendeleev’s table allowed for a deviation from the atomic weight order to be observed.

The following are some of the limitations of Mendeleev’s Periodic Table:

• Although hydrogen belonged to the group of alkali metals, it also possessed properties similar to those of a halogen atom.
• Because this type of classification of elements was done by taking the atomic weight of the element into consideration, isotopes were positioned in different places. In Mendeleev’s table, protium, deuterium, and tritium would all occupy different positions as a result of this.
• The anomalous positioning of a few elements revealed that the atomic masses of the elements did not increase in a predictable manner from one to the next. An example of this would be the placement of cobalt (atomic mass 58.9) before nickel (atomic mass 58.2). (atomic mass of 58.7).

These techniques served as the foundation for the development of the modern periodic table. Mendeleev, however, was the most important contributor to the development of the modern periodic table. Mendeleev is also known as the “Father of the Modern Periodic Table,” for his contributions to the development of the modern periodic table. In honour of Mendeleev, the modern periodic law is also known as Mendeleev’s Law.

Modern periodic table

Henry Moseley, an English physicist, conducted research into the wavelength of the characteristic x-rays in the year 1913. We demonstrated that the square root of the frequency of the line is related to the atomic number by employing a variety of metals as anti cathode materials. Moseley devised the modern periodic law, which is based on the observations made above and states as follows:

“The periodic function of the atomic numbers of the elements determines the physical and chemical properties of the elements.”

Atomic mass is determined by the number of protons and neutrons present in the nucleus of an atom. It is not very closely associated with the properties of the element, particularly the chemical properties, because the nucleus is contained within the atom. In addition to the number of electrons in the system, these are also related to the distributions of electrons in the different energy shells. The chemical properties of the elements with different electronic arrangements of the atoms are different from one another. Mendeleev predicted that, because the atomic number, rather than the mass number, determines the total number of electrons in an atom, it should be atomic number that is used to classify elements in the periodic table rather than atomic mass to classify elements in the periodic table.

Periodicity is defined as the occurrence of repeated occurrences of similar properties of elements placed in a group and separated by a specific definite gap in atomic number.

On the modern periodic table, elements are classified according to their properties.

There are 18 vertical columns, which are referred to as groups (1-18), and 7 horizontal rows, which are referred to as periods in the modern periodic table.

• Hydrogen and Helium are both found in the first period of the periodic table.
• The second period contains eight elements ranging from Lithium to Neon in their composition.
• The third period contains eight elements, ranging from Sodium to Argon.
• The fourth period contains eighteen elements, ranging from Potassium to Krypton.
• The fifth period contains eighteen elements ranging from Rubidium to Xenon.
• The sixth period consists of thirty-two different elements.
• The seventh period is incomplete.

Conclusion

From time to time, new and improved versions of the Periodic Table are developed. The emphasis is on chemical reactions and valence in some forms, whereas the electronic configuration of elements is emphasised in other forms. The most convenient and widely used version of the Periodic Table of the elements today is the so-called “long form,” which is a modern version. The horizontal rows (which Mendeleev referred to as series) are referred to as periods, and the vertical columns are referred to as groups.