![]() The formal charges being 0 for all of the atoms in the CoCl 2 molecule tells us that the Lewis dot structure presented above is stable. In this case, Element V N B/2 FC Co 2 0 4/2 0 Cl 6 6 2/2 0 CL 6 6 2/2 0 It is determined such that the elemental charge on each atom is closest to zero.įC = Valence Electrons – Non-bonding electrons – (Bonding electrons ÷ 2) To check if this structure is indeed stable, we must calculate its formal charges.įormal charges for an element/structure help determine its most stable Lewis Structure state. However, we must first check for stability. The temptation here would be to establish a double bond on either side to obtain a Cobalt octet. It can be observed above that Cobalt does not fulfill its octet requirements. All 12 valence electrons are used in this process. These are then used to fulfill the octets for the outer atoms, i.e., the two Chlorine atoms. Having used four valence electrons for bond formation, we now have 12 valence electrons available to us. Two valence electrons are used to create a Co-Cl bond. We then use the valence electrons to form covalent bonds between the atoms. The two Chlorine atoms flank the Cobalt atom on either side. In this case, Cobalt acts as the central atom due to its relatively electropositive nature. The next step is to determine the central atom and arrange the remaining elements around the central atom. The Cobalt and Chlorine atoms present contribute 16 valence electrons by virtue of their electronic configuration. As discussed in the previous section, valence electrons are integral and act as the building blocks of the structure. The first step to obtaining the Lewis structure is to calculate the number of valence electrons available. Its molecular geometry, polarity, and reactivity can be determined by observing the corresponding Lewis structure. The Lewis structure of a compound helps predict many of its properties. ![]() ![]() ![]() Thus, the total number of valence electrons in Cobalt Dichloride is given by:Ģ + 14 = 16 valence electrons. Therefore, the two Chlorine atoms present in CoCl 2 contribute 7 x 2 = 14 valence electrons. The possibility of electrons in its d shell makes it hypervalent. Chlorine’s electronic configuration is given by 3s 2 3p 5. Therefore, a single Cobalt atom contributes 2 x 1 = 2 Valence electrons.īeing in group 7 of the periodic table, Chlorine has seven valence electrons with a valency of -1. This allows the electrons to break free of the atom during exchanges.ĬoCl 2 comprises a Cobalt atom flanked by two Chlorine atoms on either side.īeing in group 9 (transition metals) of the periodic table, Cobalt has an electronic configuration of 3d 7 4s 2. These electrons are present in the outermost shell, where the force of attraction from the nucleus is the weakest. Valence electrons are those electrons that are available to be used during bond formation. These building blocks are the valence electrons contributed by the constituent atoms. To form Lewis structures, we need to know more about the building blocks that help make them.
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