Periodic classification of elements and periodicity

CHAPTER: 1 [Periodic classification of elements and periodicity]

INTRODUCTION

To achieve a thorough understanding of a complex subject like chemistry, it would be Highly desirable to fit all the facts into a simple logical pattern. The periodic table of elements has Served the purpose to systematize the properties of the elements for well over 100 years.

 The Development of periodic table is one of the most significant achievements in the history of Chemical sciences. (The Periodic Table provides a basic framework to study the periodic Behaviour of physical and chemical properties of elements as well a

s their compounds In previous classes, you have learnt about the periodic classification of elements.  This Chapter describes in more detail the periodic table and the periodicity of elements.

Historical Background

The early history of ideas leading up to the Periodic classification of elements is Fascinating but will not be treated in detail. Those who made memorable contributions in this Field are Al-Razi, Dobereiner, Newlands and Mendeleev. Al-Razi’s classifications was based on The physical and chemical properties of substances. Dobereiner, a German chemist in 1829, Arranged then known elements in group called Triads, as each contained three elements with Similar properties. Newlands who was an English chemist, in 1864, classified 62 elements, Known at that time, in increasing order of their atomic masses. 

He noticed that every eighth Element had some properties in common with the first one. The principle on which this Classification is based was called the Law of Octaves.

• In 1871, a Russian Chemist, Dmitri Mendeleev, gave a more useful and comprehensive Scheme for the classification of elements. He presented the first regular periodic table in which  Elements of similar chemical properties were arranged in eight vertical columns called Groups. 

The horizontal rows of the table were called Periods.[Mendeleev also started by arranging the Elements in ascending order of their atomic masses and found that elements having similar Chemical properties appeared at regular intervals. This significant observation was called Periodic Law.

Mendeleev left some gaps in his table for elements, which had not Discovered, and by considering their positions in the periodic table, he predicted properties of These elements. For example, germanium was not known at that time, but Mendeleev was Confident that this element must exist so he predicted its properties. 

A few years later, germanium Was indeed discovered and a remarkable agreement was found with Mendeleev’s predictions.

 Improvements in Mendeleev’s Periodic Table

In order to make the periodic table more useful and accurate, a few improvements were Made in Mendeleev’s periodic table. After the discovery of atomic number by Moseley in 1911, it Was noticed that elements could be classified more satisfactorily by using their atomic numbers, Rather than their atomic masses. Hence, the periodic table was improved by arranging the Elements in ascending order of their atomic numbers instead of their atomic masses.

 This Improvement rectified a number of confusions present in the old periodic table. The modern Periodic Law states that: “if the elements are arranged in ascending order of their atomic Numbers, their chemical properties repeat in a periodic manner”.

Another improvement was the addition of an extra group (group VIIIA) at the extreme Right of the periodic table. This group contains noble gases, which had not been discovered in Mendeleev’s time.

Another confusion in Mendeleev’s table was that elements like Be, Mg, Ca, Sr, Ba and Zn, Cd, Hg were placed in a single vertical group, while according to their properties they

Belonged to two different categories. The same was true for so many other elements placed in the Same vertical group. In modern periodic table, the confusion was removed by dividing the Elements in two types of vertical groups, A and B. In modern periodic table, Be, Mg, Ca, Sr and Ba are placed in group IIA and Zn, Cd, Hg in group IIB.

THE MODERN PERIODIC TABLE

In modern periodic table (see periodic table) all the elements are arranged in ascending Order of their atomic numbers. Followings are the essential features of the periodic table.

Groups and Periods

Elements with similar properties are placed in vertical columns called Groups. There are Eight groups, which are usually numbered by Roman numerals I to VIII. Each group is divided Into two subgroups, designated as A and B subgroup. The subgroups, containing the Representative or normal elements are labelled as A subgroup, whereas B subgroups contain less Typical elements, called transition elements and are arranged in the centre of the periodic table.

The horizontal rows of the periodic table are called Periods. The essential features of periods are As follows: There are 7 periods in the periodic table numbered by Arabic numerals 1 to 7. The period 1 contains only two elements, hydrogen and helium.

The periods 2 and 3 contain eight elements each and are called short periods. All the Elements in these periods are representative elements and belong to A subgroup. In these Periods, every eighth element resembles in properties with the first element. 

As lithium And beryllium in the 2nd period resemble in most of their properties with sodium and Magnesium of the 3rd period, respectively. Similarly, boron and aluminium both show Oxidation state of +3, fluorine in 2nd period has close resemblances with chlorine of 3rd Period.

The periods 4 and 5 are called long periods. Each long period consists of eighteen Elements. Out of these, eight are representative elements belonging to A subgroup Similar to second and third periods. Whereas the other ten elements, placed in the centre Of the table belong to B subgroups and are known as transition elements. In these Periods, the repetition of properties among the elements occurs after 18 elements. 

As After ,,K (having atomic number 19) the next element with similar properties is. Rb. The period 6 is also a long period, which contains thirty two elements. In this period There are eight representative elements, ten transition elements and a new set of fourteen Elements called Lanthanides as they start after ,La. Lanthanides have remarkably Similar properties and are usually shown separately at the bottom of the periodic table.

The period 7 is incomplete so far. It contains only two normal elements Frand Ra, ten Transition elements and fourteen inner transition elements. The inner transition elements Of this period are called Actinides, as they follow ,,Ac. The actinides are also shown at the Bottom of the periodic table under the Lanthanides. Due to their scarcity, the inner Transition elements are also called rare earth elements.

Some More Families in the Periodic Table:

While studying about periods you have noticed that certain rows of elements with Similar properties have assigned common names such as transition elements, Lanthanides, Actinides or Rare Earth elements. Similarly, due to their peculiar characteristics, some typical Elements belonging to sub-group A, have also been assigned family names.

Similarly, due to their presence in Earth’s crust and alkaline character, the elements of Group IIA are known as Alkaline Earth Metals. Another important family in the periodic table is Halogen family. The name “Halogens” is given to the elements of group VIIA, due to their salt Forming properties. As the gases of group VIIIA are least reactive they are called “Noble Gases These family names are useful for a quick recognition of an element in the periodic table.