describe the formation of electron dot structure of the chlorine Cl2
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Answer:
Lewis Dot Structures
During chemical bonding it is the valence electrons which move amongst different atoms. In order to keep track of the valence electrons for each atom and how they may be shared in bonding we use the Lewis Dot Structure for atoms and molecules. In this approach we represent the valence electrons as dots around the element symbol. For example, oxygen has 6 valence electrons, so we write the symbol O for oxygen and surround it with 6 dots:


The unpaired electrons are represented as single dots, and the paired electrons as double dots. The placement of the single or double dots around the symbol is not critical. Alternatively, we can represent the paired electrons as a line. That is, we replace the double dots as shown below:

Let's consider other examples. A sodium atom has 11 electrons, but only one is a valence electron. The other 10 are inside a closed shell with a Neon electron configuration. Thus, we draw the Lewis structure for a sodium atom as the symbol Na with a single dot:

A chlorine atom has 17 electrons, but only 7 of these are valence electrons. Thus, we draw the Lewis structure as:

In Ionic Bonds valence electrons are completely transferred (not shared). Thus, we write the Lewis structure for NaCl as:

As you can see Chlorine is now surrounded by 8 electrons in the n=3 shell and Sodium has lost its one valence electron in the n=3 shell. Of course, Sodium, is still surrounded by the 8 electrons of the n=2 shell, but we do not show electrons in the inner closed shells.
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