Via Lewis Structure, we have realized the type of bond formed and the number of lone or unbonded pairs of valence electrons present in an OF2 molecule. Now, we are going to decipher the 3D molecular shape. We have already found the 2D Lewis Structure diagram of the Oxygen Difluoride molecule. Here, oxygen forms a single bond with each of the fluorine atoms (O-F). Since the elements are present in their least possible formal charge values, we have achieved our suitable Lewis Structure configuration. The same goes for the central oxygen atom.īefore we proceed to confirm any sketch to be the perfect Lewis Structure for a given molecule or ionic structure, we need to check the formal charge values.įor Oxygen: Formal Charge = 6 – 0.5*4 – 4 = 6 – 2 – 4 = 0.įor each Fluorine atom: Formal Charge = 7 – 0.5*2 – 6 = 7 – 1 -6 = 0. Here, if we look at the octet rule, both the fluorine atoms have achieved a valency of eight. This is known as octet fulfillment since the elements want to achieve eight electrons in their valence shells.įor example, Carbon tends to attain a Neon configuration.Įxception: Hydrogen tends to achieve Helium configuration, hence only two electrons in the outer shell. The main group elements ( group 1 to group 17 ) of the periodic table have a tendency to attain the octet configuration of the noble gas elements present in group 18 of the same period.
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