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What is Sulfur

Sulfur (pronunciation: SUL-fer) is a yellowish powdery or crystalline element belonging to the family of Chalcogen and nonmetals in the periodic table and is represented by the chemical symbol S [1, 2, 3]. Although pure sulfur is odorless, the bad smell linked with the element comes from some of its compounds, including hydrogen sulfide (H2S) that produces the “rotten egg” smell and mercaptans (an organic compound) that gives the defensive odor in skunks [4].


There are about 24 isotopes of sulfur, ranging from 26S to 49S out of which four are stable, including 32S, 33S, 34S, and 36S with natural abundances of 94.99%, 0.75%, 4.25%, and 0.01% respectively [5]. Most of its radioactive isotopes are short-lived, except 35S that has a half-life period of 87 days [5].


Where is Sulfur Found

Sulfur naturally occurs as an element in volcanic areas and is also present in several minerals like galena, Epsom salts, gypsum, and iron pyrites [1].

Earlier it was commercially obtained by using the Frasch process, which involved passing super-heated steam and melting the underground deposits of sulfur so that it could be collected on the surface in its liquid state [1].

It is now produced during the purification processes of oil, tar sands, and natural gas wherein sulfur is separated [1]. While sulfur is present in all living things, it remains in them after fossilization, like in fossil fuels [1, 4].

Sulfur Cycle


Origin of its Name: It is not known from where its name exactly originated, but it is believed to have been derived either from the Sanskrit word ‘sulvere’, meaning “enemy of copper”, the Latin word ‘sulfurium’, or the Arabic word ‘sufra’ meaning yellow [1, 4].

Who discovered it: Although its discovery is unclear, the element was known to the ancient humans, as it is mentioned in the Bible and was commonly used in many parts of Asia and Europe [1].

When and How was it Discovered

According to the Bible, the Hebrew God destroyed the ancient cities of Sodom and Gomorrah, as burning sulfur (brimstone) rained from the heaven [1]. The ancient Greeks used it as a fumigant, and in Sicily, it was used for preserving wine and bleaching cloth [1]. For hundreds of years, sulfur, as well as salt and mercury, were believed to have comprised all the metals, forming the foundation of alchemy by which metals could be transmuted into one another [1].

The French chemist Antoine Lavoisier believed that it was a new element, but could not prove it [1]. In 1808, Humphry Davy thought it was a compound containing hydrogen [1]. In the following year, Joseph Louis Gay-Lussac and Louis Jacques Thénard studied its characteristics and proved it to be a new element [1].

Element 16

Sulfur Identification

Atomic number 16 [1]
CAS number 7704-34-9 [1]
Position in the periodic table Group Period Block
  16 [1] 3 [1] p [1]

Properties and Characteristics of Sulfur

General Properties

Relative atomic mass 32.06 [1]
Atomic mass 32.06 amu [1]
Molar mass 32.0650 g/mol [6]
Molecular weight  32.06 g/mol [3]
Allotropes α-S, β-S, S2, S3, octasulfur (cyclo-S8) [1]

Physical Properties

Color Most common is yellow [1, 7]
Melting point/freezing point 115.21 °C, 239.38 °F [1]
Boiling point 444.61 °C, 832.3 °F [1]
Density 2.07 g cm-3 [1]
State of matter at room temperature (solid/liquid/gas) Solid [1, 7]
– Mohs 2 [8]
Electrical Conductivity 1 X 10-15 S/m [8]
Charge 2- [9]
Thermal (heat) conductivity 0.205 W/(m K) [8]
Specific heat 708 J kg-1 K-1 [1]
Bulk modulus 7.7 [1]
Shear modulus Unknown [1]
Young’s modulus Unknown [1]
Vapor pressure
– Temperature (K) 400 600 800 1000 1200 1400 1600 1800 2000 2200 2400
– Pressure (Pa)

Chemical Properties

Oxidation states 6, 4, 2, -2 [1]
Isotopes Isotope Mass Abundance (%) Half-life Mode of decay
  32S 34.972 94.99
  33S 32.971 0.75
  34S 33.968 4.25
  36S 35.967 0.01

Sulfur Lewis Dot Structure

Atomic Data of Sulfur (Element 16)

Valence electrons 6 [10]
Quantum numbers
– n 3 [10]
– ℓ 1 [10]
– m -1 [10]
– ms -1/2 [10]
Electron configuration (noble gas configuration) [Ne] 3s23p4 [1]
Atomic structure
– Number of electrons 16 [7]
– Number of neutrons 16 [7]
– Number of protons 16 [7]
Radius of Atom
– Atomic radius 1.80 Å [1]
– Covalent radius 1.04 Å [1]
Electronegativity (Pauling-scale) 2.58 [1]
Electron affinity 200.41 kJ mol-1 [1]
Ionization energy (kJ mol-1) 1st 2nd 3rd 4th 5th 6th 7th 8th
  999.589 2251.763 3356.72 4556.231 7004.305 8495.824 27107.363 31719.56

Sulfur Electron Configuration (Bohr Model)

What is Sulfur Used for

  • Sulfur is commonly used for the production of an essential chemical compound, sulfuric acid, which has many uses including the production of phosphoric acid for making fertilizers [1, 7].
  • It is used in the vulcanization process for making black rubber more durable [1, 7].
  • Sulfur is an important component in black gunpowder and fungicides [1, 7].
  • Because of its distinctive odor, sulfur is used in natural gas supplies for detecting gas leaks easily [1].
  • Its compound, calcium sulfate, is mined for using it in plaster of paris and cement [1].
  • Its sulfites are used as food preservatives and in bleaching paper [1].
  • Many sulfate derivatives are commonly used as detergents and surfactants [1].

Is Sulfur Toxic

While sulfur and sulfate are not toxic to humans, sulfur dioxide, hydrogen sulfide, and carbon disulfide are all considered to be poisonous [1]. Hydrogen sulfide, in particular, is dangerous because it can cause respiratory paralysis, resulting in death [1].

Sulfur dioxide, produced through the combustion of unpurified oil and coal and released into the air, causes acid rain, which can result in the death of living things in and around water bodies [1, 4].

The element itself is vital for all living organisms, as the plants and algae use sulfate from soil or water [1]. An average human has 140 g sulfur in his body, obtaining it from the protein he takes (about 1 g/day) [1].

Sulfuric Acid

Interesting Facts

  • Sulfur is graphically represented by an alchemical symbol with fire and brimstone in the background [1].
  • The element constitutes approximately 3% of the mass of the Earth which is enough to create two additional moons [4].
  • While it is insoluble in water, it does not easily dissolve in other chemicals [3, 4].
  • Since the large intestine in humans is full of bacteria, sulfur compounds are produced [4]. It is the reason why the intestinal gas has a bad odor [4].
  • Sulfur passes to and from the soil, rocks, waterways, and then through living things, which is collectively called the sulfur cycle [11].

Cost of Sulfur

The price of pure sulfur is about $0.5 per gram, and in bulk, its price is about $0.2-$0.45 per gram [7].



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