The Sulfur Dioxide which is also known as Sulphur Dioxide is the entity of a bond between Sulfur and Oxygen atoms. It is known as a formula written as SO2. Here we will provide an explanation of SO2 molecular geometry, SO2 electron geometry, SO2 bond angle, and SO2 Lewis structure.Now, if we want to check the exact molecular shape of SO2, then we should understand the positions and number of electrons distributed between Sulphur and Oxygen. In the outer level, Sulphur has six electrons, and the Oxygen has four of them among which one electron is used for each bond. So total number of ten electrons in five pairs. To make bonds, four pairs are needed, so one pair remains alone. The two double bonds use two pairs each and form as a single unit.As the single alone pair not counted in the shapes description, we can conclude that the molecular shape of SO2 is V-Shaped or Bent. So, our first perception of the original structure does not match with the original one. The electron geometry of SO2 is formed in the shape of a trigonal planner. The three pairs of bonding electrons arranged in the plane at an angle of 120-degree. As the one pair remained alone, two double pairs are bonded and form a bent shape. By analyzing the Lewis structure of SO2, we can see that the SO2 is asymmetrical because it contains a region with different. Though there are so many similarities between electron geometry and molecular geometry, there are some key differences. One of the most notable differences is that the electron geometry can be associated with one or more molecular shapes. It depends on the central atoms structure of electrons of the molecule, while the molecular geometry depends on the other atoms too which are bonded to the central atom or the free pairs of electrons.To create the Lewis structure of SO2, you need to arrange the eight valence electrons on the Sulphur. To design the best Lewis structure, you also need to calculate the formal charge of every atom too. You know that both the Sulphur and Oxygen has six valence electrons each. Here we have two Oxygen atoms, so a total number of valence electrons will be eighteen.The SO2 has a bond angle of 120-degree. One single atom of Sulphur is bonded with two atoms of Oxygen covalently. It causes a repulsion of electron pairs to form the 120-degree angle.
