Atomic Properties of S
- Atomic Number of S
- 16
- Atomic Mass of S
- 32.0600 u
- Electron Configuration
- [Ne] 3s2 3p4
- Electronegativity
- 2.58
- Block
- p-block
- Group
- 16
- Period
- 3
A pile of elemental sulfur is bright yellow and nearly odorless. The famous rotten-egg smell belongs mainly to hydrogen sulfide, while other sulfur compounds help create the aromas of garlic, onions, skunks, and hot springs. Sulfur receives the reputation; its compounds provide the evidence.
Life uses sulfur with greater precision. The amino acids cysteine and methionine place it inside proteins. Bonds between pairs of cysteine sulfur atoms can tie distant parts of a protein together, helping stabilize shapes in materials such as hair and keratin. Plants absorb sulfur chiefly as sulfate from soil, then living systems convert it into the reduced forms needed for biochemistry.
Industry handles sulfur on a vast scale, largely to manufacture sulfuric acid. That acid supports fertilizer production, mineral processing, petroleum refining, batteries, and many chemical syntheses. Production and consumption of sulfuric acid are so broad that they have long served as a rough indicator of industrial activity. Sulfur also cross-links polymer chains during rubber vulcanization, turning sticky natural rubber into a stronger and more durable material.
The element occurs near volcanic vents and in underground deposits, but much modern sulfur is recovered while removing sulfur compounds from oil and natural gas. Pollution control transforms an unwanted contaminant into industrial feedstock.
Sulfur's Sustainer story corrects its own first impression. The pure element is not the smell. It is a biochemical connector, a rubber-strengthening bridge, and the starting point for one of industry’s most widely used chemicals. The dramatic odors are only one branch of a much larger chemistry.