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Overview of the Periodic Table of Elements

 

On the other hand, elements having, say, 7 electron in the other shell will tend to acquire the missing electron to reach the configuration of the following noble gas (for example, fluorine will acquire one electron and reach the configuration of neon.
             Another periodic property of elements is the electronegativity. The electronegativity is the tendency of an element to acquire one electron. For the reasons discussed above, the electronegativity of elements increasing from left to right along the periodic table, while, in a given group, it decreases from top to bottom. Every element in the periodic table is represented, besides its chemical symbol, by a series of numbers. The top-left one is called the atomic number. It represents the number of protons in that given element which, by definition, is equal to the number of electron of the same element. There cannot be two elements in the periodic table characterized by the same atomic number. The bottom-left number is the mass number, which is the number of the nucleons, that is, the sum of the protons and neutrons of an element. Quite often this is not a whole number, due to the presence of isotopes. .
             For example, carbon has three naturally occurring isotopes: most of its atoms have six protons and six neutrons as well, but about 1% have seven neutrons, and a very small fraction have eight neutrons. Accordingly the mass number of carbon is 12.011. .
             The periodic table was fundamental for the chemical discoveries in the past, but is also important for the ones which will come, since the table can be used to derive relationships between elements and also predict the properties of some new elements which we have not discovered or synthesized yet. Even if other precursors exist, Dmitri Mendeleev, is generally considered the "inventor" of the periodic table in 1869 or rather the one who formulated this method of organization. He developed his idea based on illustrating the properties and periodic trends of the elements known at that time.


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