Lewis structure of CS2 (or carbon disulfide) contains two double bonds between the carbon (C) atom and each sulfur (S) atom. The carbon atom (C) is in the middle and is surrounded by 2 sulfur atoms (S). The carbon atom has no lone pairs while both sulfur atoms have 2 lone pairs.
There are 16 valence electrons for the CS2 Lewis structure. Carbon is the least electronegative atom and is at the center of this structure. The Lewis structure for CS2 requires that you have double bonds between the carbon (C) and sulfur atoms to fill the octet of carbon.
There are 16 valence electrons available for the Lewis structure of CS2.
CS2 molecule is non-polar by nature. Due to its linear structure of the molecule. The C-S bond shows a slight dipole moment.
< li>Step 4: Choose a central atom.
The lone pair of electrons in the sulfur atom of the CS2 molecule is four. Two sulfur atoms are attached to the central carbon atom. In the CS2 electron geometry structure, the lone pairs on the central carbon atom are zero, the lone pairs on the sulfur atom have two pairs (4 electrons).
The CS2 molecule has two non-metals (i.e. carbon and sulfur); therefore it is a covalent bond. The sulfur atoms form double bonds with the central atom.
As a result, the carbon atom shares two electrons with each sulfur atom that forms a double bond. Therefore, the sharing of electrons between the atoms involved makes the bond in CS2 a covalent bond.
Here in the CS2 molecule, the number of sigma bonds at the central atom is two, and there are no lone pairs of electrons at the central atom since its octet is complete by sharing the valence electrons. Steric number of CS2 is 2; hence its hybridization has two hybrid orbitals, making it an sp hybridization.
The CS2 molecule has no lone pairs in the central carbon atom. Place the valence electrons in the C-S bond pairs, starting with the core carbon, two sulfur atoms in the CS2 molecule. In the CS2 Lewis structure diagram, we always start by introducing valence electrons from the central carbon atom (in step 1).
If a central atom (here C) is surrounded by two valence electron density regions, then it shows sp hybridization. Just in the section above, when discussing the Lewis structure, we learned that in CS2 two double bonds are formed and eight of the 16 valence electrons are consumed for this purpose.
(d) CS2: electron geometry-linear; molecular geometry-linear; Bond angle = 180° Since there are no lone pairs, the bond angle is 180°. Draw a Lewis structure for the molecule: C$2 has 16 valence electrons. Find the total number of electron groups around the central atom: There are two electron groups on C.