In what manner is the long form of periodic table better than Mendeleev's periodic table? Explain with examples.
In what manner is the long form of periodic table better than Mendeleev's periodic table? Explain with examples.
The long form of the periodic table is better than Mendeleef's periodic table because it classifies the elements on the basis of electronic configurations of their atoms.
The characteristics of this table are
(i) The table consists of 18 vertical columns, called the groups and 7 horizontal rows, called the periods. The groups are marked I to VIII out of which group I to VII are subdivided into subgroups A and B
(ii) This table is based on a more fundamental property, i. e atomic number. It correlates the position of the elements with its electronic configuration more clearly.
(iii) The completion of each period is more logical. In a period as the atomic number increases, the energy shells are gradually filled up until an inert gas configuration is reached. It eliminates the even and odd series of IV, V, VI and VII periods of Mendeleev's periodic table.
(iv) The group I-A elements (Li, Na, K, Rb, Cs, and Fr) are known as alkali metals and the group II-A elements (Be, Mg, Ca, Sr, Ba, and Ra) are known as alkaline earth metals. Elements in group VII-A (F, Cl, Br, I and At ) are called halogens and elements in group VIII-A (He, Ne, Ar, Kr Xe, and Rn) are called noble gases or rare gases.
(v) The group VIII has there similar elements placed together in one place. These are called transition triads, e.g., Fe, Co, and Ni, Ru, Rh and Pd; Os, Ir, and Pt etc. In the 6th and 7th period, 14 elements present called as Lanthanide Series and Actinide Series respectively.
(vi) Based on their electronic configuration elements have been grouped into s- p-, d- and f - blocks, This has helped us to understand their properties more easily. All the transition elements have been brought in the middle as the properties of transition elements are intermediate between s- and p-block elements.
(vii) In this table, a complete separation between metals and non-metals has been achieved. The non-metals are present in the upper right comer of the periodic table.
(viii) There is a gradual change in the properties of the elements with an increase in their atomic numbers, i.e., the periodicity of properties can be easily visualised. The same properties of recurrence in properties occur after the intervals of 2, 8, 8, 18, 18 and 32 elements which indicates the capacity of various periods of the table. This arrangement of elements is easy to remember and reproduce.
The long form of the periodic table is better than Mendeleef's periodic table because it classifies the elements on the basis of electronic configurations of their atoms.
The characteristics of this table are
(i) The table consists of 18 vertical columns, called the groups and 7 horizontal rows, called the periods. The groups are marked I to VIII out of which group I to VII are subdivided into subgroups A and B
(ii) This table is based on a more fundamental property, i. e atomic number. It correlates the position of the elements with its electronic configuration more clearly.
(iii) The completion of each period is more logical. In a period as the atomic number increases, the energy shells are gradually filled up until an inert gas configuration is reached. It eliminates the even and odd series of IV, V, VI and VII periods of Mendeleev's periodic table.
(iv) The group I-A elements (Li, Na, K, Rb, Cs, and Fr) are known as alkali metals and the group II-A elements (Be, Mg, Ca, Sr, Ba, and Ra) are known as alkaline earth metals. Elements in group VII-A (F, Cl, Br, I and At ) are called halogens and elements in group VIII-A (He, Ne, Ar, Kr Xe, and Rn) are called noble gases or rare gases.
(v) The group VIII has there similar elements placed together in one place. These are called transition triads, e.g., Fe, Co, and Ni, Ru, Rh and Pd; Os, Ir, and Pt etc. In the 6th and 7th period, 14 elements present called as Lanthanide Series and Actinide Series respectively.
(vi) Based on their electronic configuration elements have been grouped into s- p-, d- and f - blocks, This has helped us to understand their properties more easily. All the transition elements have been brought in the middle as the properties of transition elements are intermediate between s- and p-block elements.
(vii) In this table, a complete separation between metals and non-metals has been achieved. The non-metals are present in the upper right comer of the periodic table.
(viii) There is a gradual change in the properties of the elements with an increase in their atomic numbers, i.e., the periodicity of properties can be easily visualised. The same properties of recurrence in properties occur after the intervals of 2, 8, 8, 18, 18 and 32 elements which indicates the capacity of various periods of the table. This arrangement of elements is easy to remember and reproduce.
