Sulphur: Origin, Symbol, Chemical Properties & Uses

Sulphur: Sulphur is the tenth most abundant element the universe has known since ancient times. The name Sulphur is derived from the Sanskrit word sulvere and also from the Latin name sulphurium. In ancient times, Sulphur was used as medicine, fumigants, incense and bleaching agents. People used to treat many kinds of skin disorders using Sulphur.

After calcium and phosphorus, Sulphur is the third most important mineral in our body. It helps in fixing DNA and prevents cell damage in the human body. You can find Sulphur in the food that we eat. Turkey, beef, eggs, fish, chicken, nuts, seeds, grains, legumes, chickpeas, couscous, lentils, oats, turkey, walnuts, leafy green vegetables, allium vegetables, cruciferous vegetables are all high in Sulphur. In this article, we will know more about Sulphur and its importance.

What is Sulphur?

Sulphur is a chemical element with the symbol S and atomic number 16. It is a non-metal which is present in the \({\rm{1}}{{\rm{6}}^{{\rm{th}}}}\)   group and \({{\rm{3}}^{{\rm{rd}}}}\) period of the periodic table. Sulphur is the tenth most abundant element in the universe. Antoine Lavoisier discovered it in \(1777.\)

Occurrence of Sulphur

Sulphur occurs in nature both in the state and in the combined form. In the state, it is found around volcanoes. In the combined state, it occurs in the following forms:

Sulphides: Sulphur is widely available as sulphides of metals. For example, Galena \(\left( {{\rm{PbS}}} \right){\rm{,}}\) Cinnabar \(\left( {{\rm{HgS}}} \right){\rm{,}}\) iron pyrite \(\left( {{\rm{Fe}}{{\rm{S}}_{\rm{2}}}} \right){\rm{,}}\) chalcopyrite \(\left( {{\rm{CuFe}}{{\rm{S}}_{\rm{2}}}} \right){\rm{,}}\) sphalerite \(\left( {{\rm{ZnS}}} \right){\rm{,}}\) etc.

Sulphates: In nature, a large amount of Sulphur is distributed as sulphate. For example, Gypsum \(\left( {{\rm{CaS}}{{\rm{O}}_{\rm{4}}}{\rm{.2}}{{\rm{H}}_{\rm{2}}}{\rm{O}}} \right){\rm{,}}\) Epsom salt \(\left( {{\rm{MgS}}{{\rm{O}}_{\rm{4}}}} \right){\rm{,}}\) Barite \(\left( {{\rm{BaS}}{{\rm{O}}_{\rm{4}}}} \right){\rm{,}}\) Glauberite \(\left( {{\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}} \right){\rm{,}}\) etc.

Sulphur also occurs in petroleum gases like hydrogen sulphide.

Study About Modern Periodic Table

Sulphur Element

Sulphur is a non-metallic element with atomic number 16, and symbol S. Group 16 is also known as Chalcogen group. In molecular form, it exists as a molecule. The atomic number of Sulphur is \(16,\) which means Sulphur contains \(16\) protons and \(16\) electrons.

Therefore, the electronic configuration of the Sulphur is \(\left[ {{\rm{Ne}}} \right]{\rm{\;3}}{{\rm{s}}^{\rm{2}}}{\rm{\;3}}{{\rm{p}}^{\rm{4}}}\) (Electronic configuration is the distribution of electrons of an atom in atomic orbitals).

From the electronic configuration of the Sulphur, we can identify the valency of Sulphur. The combining capacity of an element is known as valency. Sulphur has six valence electrons, so two more electrons are required to achieve the electronic configuration of a noble gas. Hence, the valency of the Sulphur is \(2.\) Similarly, the valency of group \(16\) elements is \(2.\)

Atomic Mass of Sulphur

The atomic mass of an element indicates the number of times one atom of the element under consideration is heavier than \({\frac{{\rm{1}}}{{{\rm{12}}}}^{{\rm{th}}}}\) of the \({\rm{C – 12}}\) atom. Thus, if we say that the atomic mass of Sulphur is \(32,\) it means that a Sulphur atom is \(32\) times heavier than \({\frac{{\rm{1}}}{{{\rm{12}}}}^{{\rm{th}}}}\) of the \({\rm{C – 12}}\) atom. In other words, the atomic mass of Sulphur is \({\rm{32u}}{\rm{.}}\)

Allotropes of Sulphur

Sulphur exists in numerous allotropic forms, of which three forms are the most important. These three primary allotropic forms are:

(i) Rhombic Sulphur or α-Sulphur: It is the common form of Sulphur and is formed by slowly evaporating the solution of roll Sulphur in \({\rm{C}}{{\rm{S}}_{\rm{2}}}\) until octahedral Sulphur crystals appear.

Structure: Rhombic Sulphur exists as \({{\rm{S}}_{\rm{8}}}\) molecules. In this structure, Sulphur atoms are arranged in a puckered ring.

(ii) Monoclinic Sulphur or β -Sulphur: This Sulphur is made by melting rhombic Sulphur in a dish and cooling it until a crust appears. The remaining liquid is poured out through two holes in the crust. When the crust is removed, colourless needle-shaped monoclinic Sulphur crystals develop.

Structure: Monoclinic Sulphur have \({{\rm{S}}_{\rm{8}}}\) molecules. These \({{\rm{S}}_{\rm{8}}}\) molecules are packed to one another to give different crystal structures. The \({{\rm{S}}_{\rm{8}}}\) ring in this form is puckered and has a crown shape.

(iii) Plastic Sulphur or δ-Sulphur: Plastic Sulphur is formed when molten Sulphur is poured into cold water and forms a soft rubber-like mass.

Extraction of Sulphur: Frasch Process

This process is particularly suited when the Sulphur deposits are found at a depth of \(600-1000\) feet covered with hard layers of rocks, clay and quicksand, preventing ordinary mining operations.

In the extraction of Sulphur, a \({\rm{30 cm}}\) diameter pipe is first drawn through the quicksand to the Sulphur bed. This pipe serves as the casing. The Frasch Sulphur pump is subsequently installed in this casing, consisting of three concentric pipes with diameters of \({\rm{15}}\,{\rm{cm}},{\rm{7}}.{\rm{5}}\,{\rm{cm}},\) and \({\rm{2}}.{\rm{5}}\,{\rm{cm}},\) respectively. Superheated water at \({\rm{445 – 455}}\,{\rm{K}}\) is forced down through the \({\rm{15}}\,{\rm{cm}}\) pipe. The water melts the Sulphur bed and makes an emulsion with Sulphur.

A blast of hot air under a pressure of about \(35\) atmospheres passes through the \({\rm{2}}.{\rm{5}}\,{\rm{cm}}\) pipe. The blast of air causes the emulsion and foam to rise through the middle \({\rm{7}}.{\rm{5}}\,{\rm{cm}}\) pipe to the surface. The emulsion that rises to the surface is collected in massive wooden vats where Sulphur solidifies. The huge blocks of Sulphur thus obtained are about \(99.5%\) pure. The distillation process may further purify it.

Study Periodic Classification of Elements

Properties of Sulphur

Physical Properties

1. The ordinary Sulphur is pale yellow, brittle and solid crystalline in nature.
2. It has a faint smell and a marked taste. 
3. It is a poor conductor of heat but a bad conductor of electricity.    
4. It is insoluble in water but dissolves readily in carbon disulphide and turpentine oil. It is only slightly soluble in alcohol and ether.
5. It has no physiological effect on humans but is toxic to lower forms of life.
6. It exhibits the allotropic phenomenon and exists in a variety of allotropic modifications.
7. The different allotropic forms of Sulphur possess different physical characteristics.

Chemical Properties

1. Burning property of Sulphur: Sulphur burns in air with a pale blue flame and forms Sulphur dioxide with traces of Sulphur trioxide.

\({\rm{S + \;}}{{\rm{O}}_{\rm{2}}} \to {\rm{S}}{{\rm{O}}_{\rm{2}}}\)

\({\rm{2S}}{{\rm{O}}_{\rm{2}}}{\rm{ + \;}}{{\rm{O}}_{\rm{2}}} \to {\rm{2S}}{{\rm{O}}_{\rm{3}}}\)

2. Reaction of Sulphur with acids: Sulphur is not affected by dilute and cold acids. However, it reduces hot and concentrated Sulphuric and nitric acids.

3. Reaction of Sulphur with alkalis: Sulphur dissolves in alkalis and gives sulphides and thiosulphates.

4. Reaction of Sulphur with metals: Sulphur combines with almost all the metals on heating, forming their sulphides, but it does not react with noble metals such as gold and platinum.

5. Reaction of Sulphur with non-metals: Sulphur combines heating with non-metals like carbon, phosphorus, etc.
For example,

Uses of Sulphur

1. It is primarily used in the production of Sulphur dioxide, which is then used in fumigation, bleaching and the manufacture of Sulphuric acid.
2. It is used to make a Na/S battery, which can store five times more electricity than a lead storage battery.
3. It is used in the manufacture of Sulphur dyes, which are cheap and very fast.
4. It is used in medicines, primarily for skin diseases, internally as sulpha drugs and externally as Sulphur ointments.
5. It is used in the vulcanization of rubber, gun powder, fireworks, and matches.
6. It is used to destroy bacteria, fungi, insects, etc., like fungicides and insecticides.

Summary

From this article, we can conclude that Sulphur is the 10th most abundant element on the earth’s crust, and it occurs in nature both in the state and in a combined state. Its dual nature makes it more important as well as it has various uses in our day to day life, in agricultural, industrial and commercial fields.

PRACTICE QUESTIONS RELATED TO SULPHUR

Frequently Asked Questions on Sulphur

Q.1. What foods contain Sulphur?
Ans: Turkey, beef, eggs, fish, chicken, nuts, seeds, grains, and legumes, chickpeas, couscous, eggs, lentils, oats, turkey and walnuts, leafy green vegetables, allium vegetables, cruciferous vegetables are all high in Sulphur. 

Q.2 Is Sulphur harmful to humans?
Ans: No, It has no physiological effect on humans but is toxic to lower forms of life. Ingesting too much Sulphur, on the other hand, may cause a burning sensation or diarrhoea.

Q.3. What does Sulphur do to the human body?
Ans: Sulphur is required by the human body to build and repair DNA and protect the cells from damage that can lead to severe diseases such as cancer.

Q.4. Is there Sulphur in sugar?
Ans: Yes, Sulphur is present in sugar. This is because Sulphur is an additive used by manufacturers to purify sugar.  

Q.5. What is the use of Sulphur in homoeopathy?
Ans: It’s used to treat acne, hay fever, skin redness, dandruff, scaly and red skin patches, and itchy skin infection caused by mites, lice, cold sores, warts, and poison oak, ivy, and sumac diseases, as well as other health issues.

Q.6. Is Sulphur good for the skin?
Ans: Sulphur appears to have antibacterial properties against acne-causing bacteria. It can also assist in the loosening and shedding of skin.

Hope this article was helpful. If you face any issue do let us know about it in the comments section below and we will get back to you soon.