Sulfur is an abundant non-metal which is multivalent and is of great emphasis. Let us gain more insight into this element in this article.
Sulfur is usually obtained in the form of sulfate and sulfide ores and exists in cyclic octameric forms. In appearance, it is a yellow hard stone and is odorless due to which it is designated as brimstone or burning stone.
Sulfur is a very vast element in terms of its properties and applications. It is ubiquitous with its presence in chemicals, environment, and living systems in various allotropic forms and complexes. Let us discuss various periodic characteristics related to it like atomic number and weight, electronegativity, block, radius, etc.
Sulfur symbol
The symbol of sulfur according to atomic theory is the first letter of the element which is S.
Sulfur group in the periodic table
Sulfur belongs to group 16 of the periodic table which is called popularly as chalcogen family or oxygen family.
Sulfur period in the periodic table
Sulfur is situated in the 3rd period of the periodic table.
Sulfur block in the periodic table
Sulfur is present in the p block of the periodic table where non-metals are present.
Sulfur atomic number
The atomic number of sulfur is 16.
Sulfur atomic weight
The atomic weight of sulfur is 32.065 u.
Sulfur electronegativity according to Pauling
The electronegativity of sulfur according to the Pauling scale is 2.58 which is quite low compared to its group counterpart oxygen because it can form an expanded octet.
Sulfur atomic density
Monoclinic form of sulfur has an atomic density of 1.96 g/cm3 and the atomic density of rhombic sulfur is 2.07 g/cm3 which differs because of the difference in the arrangements of the solid.
Sulfur melting point
The melting point of sulfur is 115.21-degree Celsius which is low, and it can easily show sublimation at 20 to 50 degrees Celsius range.
Sulfur boiling point
The boiling point of sulfur is 444.7-degree Celsius which is again not high because of the presence of weak van der Waals forces which are easy to overcome.
Sulfur van der Waals radius
The van der Waals radius of sulfur is 1.8 angstroms.
Sulfur ionic/covalent radius
Sulfur being a non-metal has a very high covalent radius of 1.04 angstrom which in molecular form shows angular distortions.
Sulfur isotopes
Isotopes are formed when there is a difference in the sub-atomic particles of an element. Let us find out the no. of isotopes in the case of sulfur.
There are 23 isotopes of sulfur which have various atomic masses ranging from 27 to 49. The stable isotopes of sulfur and their abundance on earth’s crust are:
- 32S (95.02%)
- 33S (0.75%)
- 34S (4.21%)
- 36S (0.02%)
Sulfur electronic shells
Electronic shells are a broader way to understand the arrangement of electrons which follows the concept of principal quantum number. Let us check it for sulfur.
There are 3 electronic shells in sulfur according to the division of electrons. The electrons in the 3 electronic shells are divided according to the octet rule as 2, 8, 6.
Sulfur energy of first ionization
The first ionization energy of sulfur is 999.6 KJ/mol which is quite low because of the large size of sulfur which decreases the nuclear attraction and electron removal becomes easier.
Sulfur energy of second ionization
The second ionization energy of sulfur is 2252 KJ/mol which is higher than the first one due to increased nuclear attraction.
Sulfur energy of third ionization
The third ionization energy of sulfur is 3357 KJ/mol which is the highest because after the removal of 2 electrons the unpaired electrons are removed, and much energy is required to remove the 3rd electron.
Sulfur oxidation states
Sulfur can have many oxidation states which solely depends on the compound formed. It can exhibit a -2, +2, +4, and +6 oxidation state due to empty d orbitals which help in the expansion of valences.
Sulfur electron configuration
The electron configuration of sulfur is [Ne]3s23p4 where Ne is the noble gas neon.
Sulfur CAS number
The CAS number of sulfur is 7704-34-9.
Sulfur ChemSpider ID
The ChemSpider ID of sulfur in its atomic S form is 4515054.
Sulfur allotropic forms
Allotropism is the existence of a single compound in many forms generally due to differences in the physical arrangement. Let us analyze it for sulfur.
Sulfur has many allotropic forms but some of them are stable and can exist. These allotropic forms are:
- Rhombic Sulfur
- Monoclinic Sulfur
- Colloidal Sulfur
- Milk of Sulfur
Sulfur chemical classification
Sulfur is quite reactive which makes it suitable for its versatility. The chemical properties associated with it are:
- Sulfur can exhibit many chemical reactions like hydrogenation, electron transfer reaction, and combustion.
- Sulfur has a significant contribution in organic chemistry as organosulfur compounds like thiols, sulfonium ions, thioethers, etc.
- Sulfur has usages in many scientific fields like pharma, agriculture, metallurgy, etc.
- The elemental form of sulfur is not a hazard but its complexation with other elements is the cause of environmental and health issues.
Sulfur state at room temperature
Sulfur exists in octameric form under room temperature or normal conditions, and is a bright yellow crystalline solid.
Is Sulfur paramagnetic?
Paramagnetism in elements is highly influenced by the azimuthal quantum number. Let us judge magnetism in sulfur on similar criteria.
Sulfur as an atom is paramagnetic as it has 2 unpaired electrons in its ground state, a characteristic unique to paramagnetism. But the same theory cannot be applied in its molecular S8 state.
Conclusion
In a nutshell, sulfur is a crystalline non-metal that like other members of its family is an element of importance. It is quite evident from its characteristics and properties which makes it worthy in various industries and sectors.
Hello, I am Mansi Sharma, I have completed my master’s in Chemistry. I personally believe that learning is more enthusiastic when learnt with creativity. I am a Subject Matter Expert in Chemistry.
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