Introduction
The periodic table of elements is table used to display the important information about elements in accordance to their chemical and physical properties. The first physical property that was used to arrange the periodic table is the different boiling points of elements. The second property is the melting point of element. They differ according to their atomic number due to the distance between the energy level and that of the outer electrons. Thirdly the density and viscosity of the element played a major role in determining the arrangement of the elements in the periodic table. The other property is the heat combustion of the elements. This is simply whether the elements are combustible when subjected to heat. Finally, it is very crucial to establish the reaction of the elements with PH and water (base or acid).
The melting point of group 1 elements decreases down the periodic table that is, from lithium 80.5°C (453K) to Francium 27°C (300.15K) at the same time the boiling points decrease from Lithium: 1342°C (1615K) down the periodic table Francium: 677°C (950.15K). This is because there is a weak attraction force as you go down the table due to the free electrons. The elements of the same group react with highly with water and are base to the litmus paper (Ham, 2008 p 23).
Period 3 element has complex melting and boiling points. That is the boiling point of elements of this period increases across the table from Sodium to Silicon then they start to decreases as you move toward argon. Similarly the melting point of these elements increases across the table but starts to decrease from Aluminum to Argon (Ham, 2008 p 31). The elements of the period 3 are combustible in heat across the table and had a PH value of 6 across the table and highly react when it gets in conduct with water.
The fact that C and Si are in the same in group qualifies them as the most chemically similar element compared to those of the same period C and Si has the similar chemical properties because they compose of same number of those electron in the outer energy level (outer electrons). The outer electrons are responsible in determining the chemical properties of an element hence giving the Si and C the similar properties due to the equal numbers of electrons (Ham, 2008 p 36). Whereas elements of the same periods (C and N), have different chemical properties due to the increase of electron across the table hence a change in the outer electrons. It would therefore result to elements with different chemical properties.
Mendeleev predicated that the future discovery of Ekasilicon which was discovered in 1886 by Winkler and name it Germanium. Mendeleev predicted that the unknown element (Ekasilicon) would have at atomic weight of about 72 which come to pass after the discovery of Germanium with the weight of 72.59. Ekasilicon was predicted to be dark gray metal and Winkler discovers a similar metal with a gray appearance (Ham, 2008 p 51). Mendeleev predicted were a perfect match for he predicted a density of 5.5 g/cm3 and Germanium was discovered to have a density of 5.47 g/cm3. Ekasilicon was predicted to have a high melting which turn out to Germanium 9580C.
The chemical properties of Ekasilicon were predicted to slightly attract to hydrochloric acid and would not have any reaction with the sulphuric acid. On the contrary the Germanium did not dissolved with hydrochloric acid neither did it have any reaction with sulphuric acid as predicted. These and other chemical properties indicate that Mendeleev made a perfect and an intelligence prediction of the elements (Ham, 2008 p 77).
Works Cited
Ham, Becky. The periodic table. New York: Chelsea House, 2008. Print.
