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Why is Mendeleev's choice of formulae of compounds as the basis of deciding the position of an element in his periodic table a good one?how does this result in elements having similar chemical properties being placed in the same group?

Asked by 17th March 2013, 11:38 AM
Answered by Expert
Answer:
  • Mendeleev developed a Periodic Table of elements wherein the elements were arranged on the basis of their atomic mass and also on the similarity on chemical properties. 
  • Among chemical properties, he took the formulae of the hydrides and oxides formed by an element as one of the basic properties of an element for classification.
  • He selected oxygen and hydrogen as they are very reactive and formed compounds with most elements.
  • He then took 63 cards (as 63 elements were discovered during his time) and wrote properties of each element on one card. 
  • He arranged them in increasing order of atomic masses, and observed periodic reoccurance of elements with similar properties. 
  • On this basis he formulated a Periodic Law, which states that the properties of elements are the periodic function of their atomic masses.

Hence, Mendeleev's choice of formulae of compounds as the basis for deciding the position of an element in his table was good. This lead to elements with similar chemical properties being placed in the same group. 

There were a few instances where Mendeleev placed an element of greater atomic mass before the element of lower atomic mass so that elements with similar properties could be grouped together.

Answered by Expert 18th March 2013, 5:40 AM
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