And due to this vast difference in electronegativity, there will be a dipole moment between Sulphur and Fluorine atoms. So here the difference of the electronegativities of both these atoms is much higher than 0.5, which makes the S-F bonds polar. When we compare Sulphur and Fluorine atoms’ electronegativities, the value of electronegativity of Sulphur is 2.58 and for Fluorine is 3.98. And as a result, the charges will not be evenly distributed, increasing the chances of the polarity in the molecule.
As these lone pairs try to keep their repulsive forces minimal, they push down the Fluorine atoms.ĭue to the presence of the lone pairs, there is symmetry in the molecule. These lone pairs of electrons distort the shape of the molecule, and hence it is non-linear. Sulfur Difluoride has a bent molecule geometry having two single bonds and two lone pairs of electrons.
So in the Lewis Structure of SF2, there are single bonds between Sulphur and Fluorine atoms with two lone pairs of electrons on the central Sulphur atom. So a total of 16 valence electrons are used.Īnd Sulfur atom has four valence electrons that do not participate in bond formation and hence it is called lone pair or nonbonding pair of electrons. As octets of Fluorine atoms are complete, put six valence electrons around each Fluorine atom. So both the Fluorine atoms form a single bond with the Sulphur atom by sharing one valence electron of the Sulphur atom.Įach bond uses up two valence electrons so here four valence electrons are used from 20 valence electrons. So it will be in the central position with both these Fluorine atoms on the terminal ends.įluorine atoms need one valence electron to complete its octet so it will share one valence electron of the Sulphur atom. And now that we know the total valence electrons of SF2, we will start making the Lewis Dot Structure for this molecule.įirstly, place the Sulphur atom in the centre as it is less electronegative than Fluorine. Lewis Structure is the pictorial representation of the arrangement of valence electrons around the individual atoms in the molecule. So, Sulphur Difluoride has a total of 20 valence electrons. Total number of valence electrons for SF 2 – 6 + 7*2 ( as there are two atoms of Fluorine, we will multiply the number by 2) Sulfur has six valence electrons in its outer shell. Total number of valence electrons for SF 2 – Valence electrons of Sulphur + Valence electrons of Fluorine So we will first find out the total valence electrons for Sulphur Difluoride. For drawing the Lewis structure for any molecule, we first need to know the total number of valence electrons.