Zinc

Symbol

Zn

Atomic number

30

Atomic mass	65.38		Thermal conductivity	1.16
Atomic radius	1.53		Covalent radius	1.25
Density	7.14		Atomic volume	9.2
Melting point	692.73		Oxidation states	2
Boiling point	1180		Stable isotopes	5
Heat of vapor.	115.3		Electronegativity	1.65
Heat of fusion	7.322		First ionization	9.394
Specific heat	0.39		Electrical conduct.	...

Electron configuration

Zinc

Zinc is a bluish-white, moderately hard metal. It is brittle at room temperature and at temperatures above 150°C, being workable only in the range between 100°C and 150°C. It is an active metal and will displace hydrogen even from dilute acids.

The principal use of zinc is for the galvanizing of iron sheets or wires. In moist air zinc oxidizes and becomes coated with a tough film of zinc carbonate which protects it from further corrosion. Galvanizing is done by dipping the iron into molten zinc. Zinc can also be electroplated onto iron pieces, giving a smoother galvanized surface. Sherardized iron is formed by coating the iron with and iron-zinc alloy and then baking at 800°C. The zinc coating on iron offers protection even if the zinc coating is broken by means of cathodic protection. The zinc has a more negative reduction potential (-.76V) than iron (-.04V) and therefore acts as an anode and oxidizes in preference to the iron.

Zinc is used in making alloys such as brass (the alloy with copper). Zinc is used as the outside electrode in dry cell batteries It was used in early voltaic cells such as the Daniell cell.

Zinc sulfate is used as a disinfectant and as a white pigment in paints.

Zinc oxide (ZnO) is also used as pigment called zinc white, and is used in antiseptics (zinc oxide ointment for burns). Zinc oxide is used in making rubber to improve the mechanical characteristics of the product. It is used as a constituent of the photoconductive surfaces in photocopiers.

The most common zinc ore is sphalerite, ZnS. Zinc metal is produced by first roasting the ore in air to form its oxide

The zinc oxide is then reduced by heating it with coke (carbon) which produces the metal vapor. The vapor is condensed to the liquid form and cooled to form the solid metal

The fact that the temperature required for reduction is above the boiling point for zinc (907°C) delayed the discovery of zinc. Similar reductions were used to prepare copper, lead and iron even in ancient Rome. Zinc was probably also produced, but was lost to vaporization. Brass was formed several centuries before the discovery of zinc as a pure metal (brass is a mixture of copper and zinc).

In addition to the sphalerite, zinc joins with iron to form the sulfide wurtzite, (Zn,Fe)S. Another naturally occuring ore of zinc is a carbonate mineral called Smithsonite. A striking green color is exhibited by the mineral bayldonite which combines copper, zinc and lead with an arsenate group. Another green zinc mineral is the zinc arsenate adamite, Zn₂AsO₄(OH). The zinc arsenate mineral reinerite, Zn₃(AsO₃)₂, lacks the dramatic color. Zinc forms the silicate willemite, Zn₂SiO₄ which can also produce green crystals.

Zinc Nuclear Data