Stable isotopes of zinc available from ISOFLEX
|Isotope||Z(p)||N(n)||Atomic Mass||Natural Abundance||Enrichment Level||Chemical Form|
Request a Quote
Zinc was discovered in 1746 by Andreas Marggraf. It takes its name from the German word zink, which means “point” or “tine” and refers to the form of zinc crystals after smelting. Centuries earlier, zinc ores were used for making brass, a mixture of copper and zinc.
Zinc is a shining white metal with a bluish-gray luster (called “spelter”) and is brittle at room temperature. It is a good conductor of electricity, is soluble in acids and alkalis, and is insoluble in water. It has a hexagonal close-packed structure. Zinc is diamagnetic and is also highly electropositive, replacing less electropositive metals from their aqueous salt solutions or melts. The metal is attacked by mineral acids. Reactions with sulfuric and hydrochloric acids produce hydrogen.
Zinc is attacked by moist air at room temperatures. Dry air causes no reaction at ambient temperatures, but the metal combines with dry oxygen rapidly above 225 ºC. Zinc reacts with carbon dioxide in the presence of moisture at ordinary temperatures, forming a hydrated basic carbonate. The metal, on heating with dry halogen gases, yields zinc halides. However, in the presence of moisture, the reaction occurs rapidly at ambient temperatures. The metal dissolves in hot solutions of caustic alkalis to form zincates and to evolve hydrogen.
Some important applications of zinc include galvanizing steel, producing die castings, as a chemical addition to rubber and paints, in dry cells, in making electrodes, and as a reducing agent. Zinc forms numerous alloys, including brass, nickel silver, German silver, commercial bronze, soft solder, aluminum solder and spring brass. Zinc is also an essential nutrient element required for the growth of animals.
As an essential nutrient, zinc is not regarded as toxic. However, the metal fumes, oxide fumes and chloride fumes can produce adverse inhalation effects. Ingestion of soluble salts can cause nausea.
Properties of Zinc
|Standard state||Solid at 298 °K|
|CAS Registry ID||7440-66-6|
|Group in periodic table||12|
|Period in periodic table||4|
|Block in periodic table||d-block|
|Color||Bluish pale gray|
|Melting point||419.6 °C|
|Boiling point||907 °C|
|Vaporization point||907 ºC|
|Thermal conductivity||116 W/(m·K) at 298.2 °K|
|Electrical resistivity||5.92 µΩ·cm at 20 °C|
|Specific heat||0.39 kJ/kg K|
|Heat of vaporization||119 kJ·mol-1|
|Heat of fusion||7.35 kJ·mol-1|
|Density of solid||7.14 g/cm3|
|Atomic radius||1.34 Å|
|Ionic radius||0.60 Å (coordination number 4) and 0.74 Å (coordination number 6)|
- Zn isotope fractionation during sorption onto kaolinite
- Copper and zinc isotope compositions in human bone and enamel
- Zn speciation and stable isotope fractionation in a contaminated urban wetland soil Typha latifolia system
- Evaporative fractionation of zinc during the first nuclear detonation
- Insights into Trace Metal Metabolism in Health and Disease from PET: “PET Metallomics”
- Assessment of coupled Zn concentration and natural stable isotope analyses of urine as a novel probe of Zn status