The sulfur trioxide is usually colorless and oily but is highly corrosive in nature. Also, it is called battery acid and is used to manufacture acids, fertilizers, lead-acid batteries, in the pickling of metal, purification of petroleum, and others. The lewis structure is also called an electron dot structure which determines the number of valence electrons present in an atom. Moreover, they also describe how these valence electrons are participating in the bond formation to form a molecule.
Also, the Lewis structure helps with figuring out the number and nature single, double, and triple of the bond shown with the help of lines. To understand these diagrams, it is essential to know how the number of valence electrons has been calculated.
The atomic number of the sulfur is 16 which makes its electronic configuration 1s2 2s2 2p6 3s2 3p4. As the p shell needs to accommodate 6 electrons, there is a need for two more electrons to complete the 3p shell. On the other hand, the atomic number of oxygen is eight that make its electronic configuration 1s2 2s2 2p4.
Again, there is a need for two more electrons to stabilize the 2p shell. Now, the Lewis structure needs to be drawn in such a manner that 3p and all 2p shells are filled. The electrons that lie in the outermost shell of an atom that readily takes part in the bond formation are called valence electrons. The hold of the nucleus on these electrons is less along with a dearth in number makes these electrons participate in the bond formation.
So, in the case of sulfur trioxide, six valence electrons in every single atom of sulfur and three atoms of oxygen participate to form one molecule. As per the octet rule, the maximum number of electrons that can be filled within a valence shell is eight.
Sulfur can expand its octet and can accommodate up to 12 electrons because of which, it does not follow the octet rule. As there is a small energy difference between 3p and 3d shells, with the help of a little excitation, an unpaired electron can move from the 3p shell to the 3d shell easily. In case when all the valence electrons are in the 3s and 3p shell, sulfur can produce up to two shared covalent bonds and two lone pairs.
But, when one valence electron reaches 3d shell, sulfur can produce four shared covalent bonds and one lone pair. It is essential to understand that the sulfur can expand its octet to incorporate a maximum of ten to twelve electrons. Moreover, when one more valence electron reaches the 3d shell, the total number of unpaired electrons becomes six in the sulfur. With this condition, sulfur can now form six covalent bonds allowing twelve electrons around its valence shell. The formation of more covalent bonds means the release of more energy, allowing the final configuration to be much more stable.
These electrons are negative and repel each other. Moreover, as there are three oxygen, it will be X3. That means we have AX3 for the SO 3 molecule. By the way, that is the reason why SO 3 is having the shape of Trigonal Planar. The bond angle of SO 3 is degrees. Valence: Here, sulfur in the center because of its lowest electron capability, and three oxygen around it. Sulfur brings 6, and oxygen brings 3 each. That means; SO 3 has 24 valence electrons.
When we draw it, firstly we get the three structures at the top. Sulfur in the center and Oxygen around it is making a connection each to the central atom. There should be single bonds initially. There are 6 electrons in the structure which we have made, and there are 24 in total.
So we need to put 18 electrons down. Now fill the outer atoms so that it satisfies the octet rule. Tip: When you put them, start counting from 7 to Then take a decision regarding the formal charge. If you want to find out, use this formula to make it simple;. The sulfur can handle 12 electrons per atom. Now, take out 2 dots from each of the oxygen and put one more bond connection to each. So, as you can see, now there are 10 electrons around it. Sulfur trioxide gas is produced due to oxidation of sulfur dioxide gas in air.
There are three double bonds around sulfur atom with oxygen atoms in SO molecule. Each oxygen atom has two lone pairs in SO 3 lewis structure.
But, there is no lone pair on sulfur atom in SO 3 lewis structure as lewis structure of SO 2. All atoms have sp 2 hybridization. Each oxygen atom has one sigma bond and two lone pairs.
Therefore, oxygen atoms' hybridization should be sp 2. For sulfur atom, there are three sigma bonds and no lone pair and it's hybridization is also sp 2.
Following steps are the main guidelines we have to use for drawing the lewis structure of SO 3. Each step is explained in detail in next sections.
If you are a beginner to lewis structure drawing, follow these sections slowly and properly to understand it completely. Look the figures to understand each step. Both sulfur and oxygen belongs to the group VIA elements' series. Therefore, they have six electrons in their valence shell. To find number of valence electron, these valence electrons of each element should be multiplied with their respective number of atoms in the molecule. Below, That step are done. There are no charges in SO 3 molecule.
Therefore, no addition or reduction of valence electrons due to charges. Total electron pairs are determined by dividing the number total valence electrons by two.
There are several requirements to be the center atom in a molecule. We have to think whether center atom is sulfur or oxygen.
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