Zinc

Copper - Zinc - Gallium
Zn Cd
	Full table

General

Name, Symbol, Number

Zinc, Zn, 30

Chemical series

Transition metals

Group, Period, Block

12 , 4 , d

Density, Hardness

7140 kg/m³, 2.5

Appearance

blueish pale grey

Atomic Properties

Atomic weight

65.409 amu

Atomic radius (calc.)

135 (142) pm

Covalent radius

131 pm

van der Waals radius

139 pm

Electron configuration

[Ar]3d3d¹⁰4s²

e^- 's per energy level

2, 8, 18, 2

Oxidation states (Oxide)

2 (amphoteric)

Crystal structure

hexagonal

Physical Properties

State of matter

solid (diamagnetic)

Melting point

692.68 K (787.15 �F)

Boiling point

1180 K (1665 �F)

Molar volume

9.16 ×1010^-3 m³/mol

Heat of vaporization

115.3 kJ/mol

Heat of fusion

7.322 kJ/mol

Vapor pressure

192.2 Pa at 692.73 K

Velocity of sound

3700 m/s at 293.15 K

Miscellaneous

Electronegativity

1.65 (Pauling scale)

Specific heat capacity

390 J/(kg*K)

Electrical conductivity

16.6 10⁶/m ohm

Thermal conductivity

116 W/(m*K)

1^st ionization potential

906.4 kJ/mol

2^nd ionization potential

1733.3 kJ/mol

3^rd ionization potential

3833 kJ/mol

4^th ionization potential

5731 kJ/mol

Most Stable Isotopes

iso	NA	half-life	DM	DE M eV	DP
⁶⁴Zn	48.6%	Zn is stable with 34 neutrons
⁶⁵Zn	{syn.}	244.26 days	&epsilon	1.352	⁶⁵Cu
⁶⁶Zn	27.9%	Zn is stable with 36 neutrons
⁶⁷Zn	4.1%	Zn is stable with 37 neutrons
⁶⁸Zn	18.8%	Zn is stable with 38 neutrons
⁷²Zn	{syn.}	46.5 hours	&beta	0.458	⁷²Ga

SI units & STP are used except where noted.

Zinc is a chemical element in the periodic table that has the symbol Zn and atomic number 30.

Table of contents

1 Notable characteristics
2 Applications
3 History
4 Biological role
5 Occurrence
6 Compounds
7 Isotopes
8 Precautions
9 External links

Notable characteristics

Zinc is a metal, mined in Vieille Montagne and Zinkgruvan, used in the process of galvanizing steel. It is moderately reactive as metals go, will combine with oxygen and other non-metals, and will react with dilute acids to release hydrogen. It is the fourth most common metal in use, trailing only iron, aluminum, and copper in tons of metal produced per year.

The one common oxidation state of zinc is +2.

Applications

Zinc is used to galvanize metals to prevent their corrosion.
Zinc is used in alloys such as brass, nickel silver, typewriter metal, various solder formulas, German silver, etc.
Brass, in turn, has wide application because of its strength and corrosion resistance.
Zinc is used in die castings, especially by the automobile industry.
Rolled zinc is used as part of the containers of batteries.
Zinc oxide is used as a white pigment in watercolors and paints, and as an activator in the rubber industry. As an over-the-counter ointment, it is applied as a thin coating on the exposed skin of the face and nose to prevent dehydration and thereby protect against sunburn in the summer and windburn in the winter. Applied thinly to a baby's diaper area (perineum) with each diaper change, it protects against rash.
Zinc chloride is used as a deodorant and as a wood preservative.
Zinc sulfide is used in luminescent pigments, for making the hands of clocks and other items that glow in the dark.
Zinc methyl (Zn(CH₃)₂) is used in a number of organic syntheses.
Lotions made of calamine, a mix of Zn-(hydroxy-)carbonates and silicates, are used to treat skin rash.
Zinc metal is included in most proprietary over-the-counter daily vitamin and mineral preparations. Along with some other metals, it is commonly believed to possess anti-oxidant properties, which protect against premature ageing of the skin and muscles of the body. In larger amounts, taken as zinc alone in other proprietaries, it is believed to speed up the healing process after an injury.
Zinc gluconate glycine is taken in lozenge form as a remedy for the common cold.

History

Zinc alloys have been used for centuries, as brass goods dating to 1000-1400 BCE have been found in Palestine and zinc objects with 87% zinc have been found in prehistoric Transylvania. Because of the low boiling point and chemical reactivity of this metal (isolated zinc would tend to go up the chimney rather than be captured), the true nature of this metal was not understood in ancient times.

The manufacture of brass was known to the Romans by about 30 BCE, using a technique where calamine and copper were heated together in a crucible. The zinc oxides in calamine were reduced, and the free zinc metal was trapped by the copper, forming an alloy. The resulting brass was either cast or hammered into shape.

Smelting and extraction of impure forms of zinc was being accomplished as early as 1000 AD in India and China. By the end of the 14th century, the Hindus were aware of the existence of zinc as a metal separate from the seven known to the ancients. In the West, the discovery of pure metallic zinc is most often credited to the German Andreas Marggraf, in the year 1746, though the whole story is considerably more involved.

Descriptions of brass manufacture are found in Western Europe in the writings of Albertus Magnus, ca 1248, and by the 16th century, the understanding and awareness of the new metal broadened considerably. Agricola observed, in 1546, that a white metal could be condensed and scraped off the walls of a furnace when zinc ores were smelted. He added in his notes that a similar metal called "zincum" was being produced in Silesia. Paracelsus (died 1541) was the first in the West to say that that "zincum" was a new metal and that it had a separate set of chemical properties from other known metals.

The upshot is that zinc was known by the time Margraaf made his discoveries and in fact zinc had been isolated two years earlier by another chemist, Anton von Swab. However, Margraaf's reports were exhaustive and methodical and the quality of his research cemented his reputation as the discoverer of zinc.

The word "zink", as a term, was originally used by L�hneyes in 1697.

Before the discovery of the zinc sulfide flotation technique, calamine was the mineral source of zinc metal.

Biological role

Zinc is an essential element in human beings, necessary for sustaining life. Deficiencies of zinc have marked effects on weight gain in animals. Zinc is found in insulin, zinc finger proteins, and such enzymes as superoxide dismutase.

According to some sources, taking zinc tablets may provide some immunity against colds and flu, although this is disputed.

Occurrence

Zinc is the 23rd most abundant element in the earth's crust. The most heavily mined ores tend to contain roughly 10% iron as well as 40-50% zinc. Minerals from which zinc is extracted include sphalerite, zinc blende, smithsonite, calamine, and franklinite.

Compounds

Zinc oxide is perhaps the best known and most widely used zinc compound, as it makes a good base for white pigments in paint. It also finds industrial use in the rubber industry, and is sold as opaque sunscreen. A variety of other zinc compounds find use industrially, such as zinc chloride (in deodorants), zinc sulfide (in luminescent paints), and zinc methyl in the organic laboratory. Roughly one quarter of all zinc output is consumed in the form of zinc compounds.

Isotopes

Naturally occurring zinc is composed of the 4 stable isotopes Zn-64, Zn-66, Zn-67, and Zn-68 with 64 being the most abundant (48.6% natural abundance). 22 radioisotopes have been characterized with the most {abundant and/or stable} being Zn-65 with a half-life of 244.26 days, and Zn-72 with a half-life of 46.5 hours. All of the remaining radioactive isotopes have half-lives that are less than 14 hours and the majority of these have half lives that are less than 1 second. This element also has 4 meta states.

Precautions

Metallic zinc is not considered to be toxic, but there is a condition called zinc shakes or zinc chills that can be induced by the inhalation of freshly formed zinc oxide.