A CCL4 Lewis structure illustrates the formation of covalent bonds between the atoms of a certain molecule, according to the University of California, Davis. The formation of these bonds involves sharing of electrons in the outermost shells of the atoms involved.
Besides showing the bonds between a molecule's atom, a Lewis structure shows the number of the lone pairs of electrons. For carbon tetrachloride (CCL4), carbon is placed at the center. The carbon atom then forms a single bond with each of the four chlorine atoms.
The three pairs of each of the chlorine’s atoms that are not involved in bonding are placed around the atoms. However, they should be drawn in a way that depicts that they are grouped in pairs. According to Socratic, each of the atoms must have a total of eight electrons in the outer shell in accordance with the octet rule. However, this rule does not apply where a hydrogen atom is involved because it only has the first shell which can only hold a maximum of two electrons. A VSEPR model of the carbon tetrachloride shows that the free atoms that surround an atom of chlorine are placed in regions. The regions are also known as clouds. The regions containing certain electrons should be as far as possible from each other.