In this article, we are going to analyze the SBr4 lewis structure and various facts about it.
SBr4 or sulfur bromide is an inorganic compound which form by covalent bonding. So the bonding in sulfur bromide can be explained by the concept of lewis dot structure. So we will study SBr4 lewis structure in detail and various facts related to it in the following sections.
Some facts about SBr4
The observed molar mass of sulfur bromide or sulfur tetrabromide is around351.681 g/mol. It is observed to exist as a gas (colorless) having an odor similar to sulfur. It is a very hazardous gas, that can be threat to the skin. Hence one should be very careful while handling it. Talking about its reactivity, it’s seen to react very vigorously with H2O.
How to draw lewis structure for SBr4?
We must know the number of valence electrons in order to draw the structure. So the number of valence electrons in sulfur tetrabromide: According to the formula there is one sulfur atom and 4 bromine atoms in the structure.
The number of valence electrons in sulfur are 6 and in bromine, there are 7 (as there are four bromine atoms in the molecule, the number of valence electrons will be 7×4=28 electrons). So total number of valence electrons in the molecule will be 6+28=34 electrons. Now we have to identify the atom that has to be placed in the center, so the central atom is the one that has the least electronegativity. In this molecule, sulfur will be the central atom, and the rest(bromine) atoms will be the surrounding ones.
As we can see, the dots around the atoms represent the number of valence electrons. So the dots are placed in a manner that it satisfies the valency of the bonding atoms. Hence in each bond fluorine and antimony both contribute one electron each and thus satisfy each others valency. As only one pair of electrons is involved in the formation of the bond the resulting bond is a single bond. We can see that one electron pair does not participate in bonding.
SBr4 Lewis Structure shape
Taking into account the SBr4 lewis structure shape, it has a trigonal bipyramidal shape.
In the molecule, we can notice that it is little tilted at an angle less then 102 degrees and at a angle of 173 degrees. Due to the presence of one lone pair on sulfur, it leads to trigonal bipyramidal kind of geometry.
SBr4 Lewis structure formal charge
A formal charge on any atom is the difference in between number of valence electrons (includes every atom) and associated number of electrons. It is assumed by formal charge that any electrons that are shared are shared equally between two bonding atoms. Formal charge is calculated by using the below formula:
Where, the term V means number of valence electrons contributed by the atom (as though isolated from a molecule).
The term N means number of unbound (valence electrons) on atom that is being considered of molecule.
The term B means the total number of electrons that are shared by bonds with the other atoms in molecule.
So, considering the molecule of SBr4, the formal charge on the sulfur atom at the center is zero. Hence the formal charge on the entire molecule will be zero.
SBr4 Lewis structure lone pairs
A lone pair means pair of valence electrons which are not shared during the process of bonding.
They are meant to be found in outermost (electron) shell of the atoms. We can say that the number of lone pairs around any atom when added to the number of electrons participating in bonding equals to the number of valence electrons in the atom. The concept of lone pair is of VSEPR (valence shell electron repulsion theory). Coming to the molecule of SBr4 there is one lone pair present.
Hybridization is the concept/process of mixing the atomic orbitals in order to form new orbitals (hybrid) which have much different shape, energy. (Hybrid orbital formation is possible when the atomic orbitals have comparable kind of energies). This formed (hybrid) orbitals can be used to explain properties like atomic bonding and geometry (molecular). The hybridization in SBr4 molecule is sp3d.
SBr4 lewis structure resonance
SBr4 Lewis structure octet rule
According to octet rule, an atom wants to obtain completely filled octet. Meaning there should be total 8 electrons present in the outermost shell. This is the reason Sulfur forms single bonds by sharing one electron pair each with 4 bromine atoms. But we can see there is one extra electron pair with sulfur which is responsible for the trigonal bipyramidal geometry of the molecule.