Atomic Properties of Sn
- Atomic Number of Sn
- 50
- Atomic Mass of Sn
- 118.7100 u
- Electron Configuration
- [Kr] 4d10 5s2 5p2
- Electronegativity
- 1.96
- Block
- p-block
- Group
- 14
- Period
- 5
Mix copper with enough tin and the result is bronze, generally harder and easier to cast than copper alone. That alloy helped reshape tools, weapons, art, and trade thousands of years ago. Tin remained useful because it melts readily, bonds into alloys, and resists corrosion. Modern steel food cans carry a thin tin coating; the can is not made mainly of tin.
Solder provides another changing story. Traditional electronics used tin-lead alloys, but lead exposure and waste concerns drove broad adoption of lead-free solders based largely on tin with silver, copper, or other additions. The replacement changes melting temperatures and manufacturing behavior, demonstrating that removing a hazardous component can require redesign rather than a simple swap.
Bend a bar of metallic beta-tin and it may make a crackling “tin cry” as crystal grains deform. Cool tin below about 13 degrees Celsius for long enough and a more dramatic transformation can occur: metallic white tin slowly changes to brittle, powdery gray tin. This tin pest is an allotrope change, accelerated by colder conditions and seeding, not an instant curse that destroys every object in winter.
Tin has ten naturally occurring stable isotopes, more than any other element, reflecting unusual nuclear stability around 50 protons. Cassiterite, SnO2, is its principal ore. Tin compounds also appear in glass coatings, catalysts, and stannous fluoride toothpaste.
Tin is a Tinkerer across eras and structures. One alloy opened the Bronze Age, another joins circuits, a surface coating protects steel, and rearranged atoms turn a shiny metal into a crumbling semiconductor.