Sulfur dichloride is a chemical compound having chemical formula SCl2. It exists as a liquid with cherry-red texture at standard conditions of temperature and pressure. Many of you may have a question regarding whether SCl2 is polar or not. In this article, we will answer this question and will cover its properties and applications.
So, Is SCl2 Polar or Nonpolar? SCl2 (Sulfur dichloride) is polar in nature because of bent geometrical shape due to the presence of lone pair present on sulfur atom. The difference between the electronegativity of sulfur and chlorine atoms makes the S-Cl bonds polar and the entire molecule also becomes polar and gives dipole moment of 0.54D.
Sulfur dichloride is a cherry red liquid substance having a pungent smell. Basically, it is produced by the process of chlorination of sulfur.
Below is the chemical reaction of the chlorination of sulfur.
S8 + 4Cl2 ——–> 4S2Cl2 ΔH(Heat enthalphy) = −58.2 kJ/mol
Further chlorination of intermediate compound (S2Cl2).
S2Cl2 + Cl2 ———> 2SCl2 ΔH (Heat enthalphy) = −40.6 kJ/mol
The molecular mass of the SCl2 compound is 102.97 g·mol−1, calculated as below
Mol mass of SCl2 = 1 * 32 (Mol mass of S) + 2 * 35.4 (Mol mass of Cl) = 102.97 g·mol−1.
If we talk about the chemical composition of the Sulfur dichloride, the molecule consists of 2 atoms of chlorine and 1 sulfur atom.
Sulfur is the central atom surrounded by two chlorine atoms. The valence electrons of Sulfur are 6 ie; it has 6 electrons in its outermost shell and Chlorine has 7 electrons in its outermost shell.
The chlorine atoms need one electron to complete its octet. Therefore, both chlorine atoms get covalently bonded with the sulfur atom leaving behind two lone pairs on the sulfur atom.
The two lone pairs on the sulfur atom cause repulsion with the bond pairs. As per VSEPR theory, due to the electronic repulsion the shape of the molecule gets bent (V-shape) similar to that of the water molecule.
The lone pair pushes both S-Cl bonds in the downward directions and resulting in the bent shaped molecule.
The molecules that have lone pairs have distorted shape because they cause electronic repulsion among the molecule.
If we talk about the electronegativity of its atoms. The electronegativity of chlorine is 3.16 and that of sulfur is 2.58.
Due to this difference between their electronegativity, the S-Cl bond becomes polar in nature.
Electronegativity of an atom is its strength with which it can attract the bonded electron pairs towards its side.
As a result, the dipole moment of the S-Cl bond also turns out to non zero and due to V-shaped structure the dipole of both bonds does not get canceled.
The net dipole moment of the entire SCl2 molecule turns out to be 0.54D. The sulfur gains partial positive charge whereas the chlorine atoms gain partial negative charge.
What are Polar and Nonpolar Molecules?
The molecules are held by the interatomic forces like ionic, covalent, metallic, and hydrogen bonds. These bonds are found in many chemical compounds.
Out of these bonds, covalent and ionic bonds are the strongest. Covalent bonds can be polar and nonpolar depending upon several parameters discussed in the sub-topic.
Polar Molecules: The molecules that have non zero value fo their dipole moment are polar in nature. These molecules have two poles (positive and negative) inside the molecule.
The atoms in these molecules share an unequal proportion of charge because they differ in their electronegativity.
More electronegative atom attracts the bonded electron pair slightly more towards its side and gains partial negative charge and other atom gains relatively positive charge.
In this way, two poles generate across a polar molecule. Few examples of such molecules are IF5, H2O, etc.
You can check out the reason for the polarity of IF5.
Nonpolar Molecule: The molecules that have zero dipole moment are nonpolar in nature. No poles are generated in such molecules.
The atoms in these molecules have a uniform distribution of charge. Two atoms that are covalently bonded form a nonpolar bond if they both have equal electronegativity.
Few examples of such molecules are XeF2, Hexane, etc. You can check out the reason for then non-polarity of XeF2.
Why is SCl2 a polar molecule?
Sulfur dichloride molecule is a bent shaped molecule due to the presence of two lone pairs on Sulfur atom.
As per the VSEPR theory, the lone pair and bond pairs cause repulsion among them as a result, the S-Cl bonds get in the downward directions resulting in the V-shape molecule.
Unlike asymmetric molecules, the dipole moment of S-Cl bonds does not get canceled by each other.
The dipole moment of the entire molecule SCl2 comes out to be 0.54D. The geometrical structure and the difference between the electronegativity results in the formation of a polar molecule.
Because the asymmetric shape of molecule disperses the charge non-uniformly among the atoms of the molecule resulting in the positive and negative poles to be created across the molecule.
Factors affecting polarity of a molecule
Electronegativity: The electronegativity of atoms forming a covalent bond is one of the crucial parameters to check whether a molecule is polar or not.
If there exists a difference between the electronegativity of two atoms forming a molecule, the molecule tends to be polar due to an imbalance in charge distribution.
Therefore, the polarity of a molecule is directly proportional to the difference between the electronegativity of atoms.
Geometrical Structure: The shape of a molecule also depicts the polarity of a molecule by simply viewing its shape.
The asymmetrically shaped molecules tend to be polar because of some non zero dipole value.
Whereas the symmetrically shaped molecules are nonpolar as they get dipoles canceled by each other in case a molecule consists of a polar bond within it.
Dipole moment: The dipole moment of a molecule is the measure of the polarity of a molecule. Greater the value of the dipole of a molecule more is its polarity.
Mathematically, it is the product of the charge on the atoms and the distance between them.
D = Q * R
SCl2 Lewis and Geometrical Structure
The lewis structure of a molecule is also known as its electron dot structure. It determines the number of valence electrons and the electrons taking participation in forming the bonds of the molecule.
If we talk about the lewis structure of SCl2, we need to know about the valence electrons of SCl2.
Here, sulfur is the central atom having 6 electrons in its outermost shell, and chlorine atom has 7 electrons in its outermost shell and needs one electron to complete its octet.
Therefore, we have a total of 20 valence electrons present in the SCl2 molecule.
Both chlorine atoms form covalent bonds with the sulfur atom leaving behind the two lone pairs on sulfur atom.
The lone pairs cause repulsion with bond pairs due to which the S-Cl bonds face force in the downward direction and the shape of molecules becomes bent like that H2O (water) molecule.
The bond angle of the Cl-S-Cl bond is around 103 degrees. And the bond length of S-Cl is 201 pm.
Properties of SCl2
- It appears as a red liquid with a pungent odor.
- The melting point of sulfur dichloride is around −121.0 °C or −185.8 °F and its boiling point is 59 °C or 138 °F.
- It undergoes hydrolysis in water.
- The SCl2 molecule has sp3 hybridization of their orbitals.
- The density of this liquid is around 1.621 g·cm−3.
- The autoignition temperature of this compound is 234 °C.
Uses of SCl2
- It is used as a chlorinating agent for chlorination purposes.
- It is also used for the manufacturing of insecticides, synthetic rubbers.
- It is also used in the wood industry for hardening the softwoods.
Sulfur dichloride is a bent shaped molecule due to the presence of 2 lone pairs on the sulfur atom.
The sulfur atom is the central atom surrounded by two chlorine atoms with a bond angle of around 103 degrees.
The difference between the electronegativity of sulfur and chlorine atoms make the S-Cl bond polar and entire molecule results in the dipole moment 0.54 D.
Due to asymmetric geometrical shape and unequal electronegativity of atoms, the SCl2 molecule is polar.
Guys, if you have any doubts regarding the polarity of SCl2, you can ask them in the comment section. We will answer you as soon as possible.