Tin

Tin is known from ancient times. Its alloy, bronze, containing 10 to 15% tin has been in use in weapons and tools for millennia.
The most important mineral of tin is cassiterite, SnO2. It occurs in the form of alluvial sand. Also, it is found embedded in granite rocks. Other tin-bearing minerals are stannite and tealite. Abundance of tin in the earth’s crust is estimated to be 2.3 mg/kg. Tin is used for plating steel to make “tin cans” for preserving food. Also, tin is coated over other metals to prevent corrosion. An important application of tin is to produce float glass, made by floating molten glass on molten tin which is used for windows. A number of tin alloys have wide industrial applications and include bronze, solder, Babbit metal, White metal, type metal, fusible metal, and phosphor bronze. A tin-niobium alloy that is superconducting at low temperatures is used in constructing super magnets. Tin also is in wrapping foil and collapsible tube.

Tin is a ductile, malleable, lustrous solid with a gray to almost silver-white color. Tin forms covalent bonds with carbon forming a variety of organometallic or organotin compounds, and the physical and chemical properties differ for various compounds such as Tin II (SnO) and Tin IV (SnO2), organotins, and inorganic tin compounds. Tin compounds are generally insoluble in water and have vapor pressures of approximately 0mmHg. Tin is not easily oxidized and resists corrosion; however, powdered tin has a tendency to oxidize, especially at high humidity.

Silvery-white metal at ordinary temperature; slowly changes to gray below 13.2°C; soft, malleable, and somewhat ductile; Brinell hardness 2.9. Tin has two allotropic forms: (1) white tin, the beta form, and (2) gray tin, the alpha form. The white tin (beta form) has a tetragonal structure. When cooled below 13.2°C, its color slowly changes from white to gray, the beta allotrope converting to alpha (gray tin). The presence of small amounts of antimony or bismuth prevents this transformation from white to gray tin. Other impurities such as zinc or aluminum promote change from white to gray tin.
Some other physical properties are: density 7.28 g/cm3 (white), 5.75 g/cm3 (gray) and 6.97 g/cm3 (liquid at the melting point); melts at 231.9°C; vaporizes at 2,602°C; electrical resistivity 11.0 and 15.5 microhm-cm at 0 and 100°C, respectively; viscosity 1.91 and 1.38 centipoise at 240 and 400°C, respectively; surface tension 5.26 and 5.18 dynes/cm at 300 and 400°C, respectively; modulus of elasticity 6 – 6.5x106 cgs psi; magnetic suspectibility 0.027x10–6 cgs units; thermal neutron absorption cross section 0.625 barns; insoluble in water; soluble in HCl, H2SO4, aqua regia, and alkalies; slightly soluble in dilute nitric acid.

Tin is primarily produced from the ore cassiterite (SnO2). It has a variety of industrial and domestic uses; its usefulness stems from its pliability and ability to readily form compounds and alloys with other metals, inorganic compounds, and organic compounds. Tin metal is used to line cans for storing and transporting food, beverages, and aerosols. Bronze is an alloy of tin and copper; pewter is an alloy of tin with various amounts of antimony, copper, bismuth, and sometimes lead. Soldering compounds are made with tin alloys. Inorganic tin is used in making toothpaste, perfumes, soaps, coloring agents, food additives, dyes, and in the glass industry.
Tributyltin is used as a slime control in paper mills, for disinfection of circulating industrial cooling waters, as antifouling agents, and in the preservation of wood. Tributyltin, triphenyltin, and tricyclohexyltin are used in agriculture as fungicides, anti-helminthics, miticides, herbicides, nematocides, ovicides, molluscicides, ascaricides, pesticides, in industry as biocides, and as antifouling agents for large ship bottoms and fishery farm nets. In the past, several organometallic metallocene complexes of tin have been identified as having antitumor activity. Tin protoporphyrin has been used to treat acute hepatic porphyria. Niobium– tin compounds are used to build superconducting magnets.

Tin is produced commercially from mineral cassiterite, SnO2. The mineral is mined from alluvial sand deposits by different techniques, such as various dredging (usually applied to low-grade deposits), gravel-pump mining (on level ground), and open-pit mining. The ore is broken up mechanically by blasting and drilling. It then is crushed and ground to produce finely divided material that can be separated by gravity concentration and froth flotation. Tin concentrates so obtained require removal of sulfide before smelting. This is done by roasting concentrates at high temperatures which removes both sulfur and arsenic. Lead sulfide is converted to lead sulfate but all other associated metal sulfides, such as those of iron, copper, zinc, and bismuth, are converted to oxides.
Tin is produced from oxide by heating at high temperatures with carbon. Small amounts of limestone and sand are added to coal for this reduction and to promote removal of impurities. Primary smelting is carried out in a reverbaratory furnace at a temperature between 1,200 to 1,300°C. Electric arc furnaces also are used. The molten tin collected at the bottom is cast into slabs. The slags are resmelted at a higher temperature, up to 1,480°, in the same type of furnaces to recover more tin that is combined as silicates.
Tin obtained above contains small amounts of impurities. It is purified by resmelting in a small reverberatory furnace at a temperature just above the melting point of tin. The molten tin is drawn out, separating iron, copper, arsenic, antimony, and other metals. Purified tin is further refined by boiling or polling processes to remove traces of impurity metals, such as lead and bismuth.

At ordinary temperatures tin is stable in air. It actually forms a very thin protective oxide film. In powder form, and especially in the presence of moisture, it oxidizes. When heated with oxygen it forms tin(IV) oxide, SnO2.Tin reacts with all halogens forming their halides. Reaction with fluorine is slow at ordinary temperatures; however, chlorine, bromine and iodine readily react with the metal.
Tin is attacked by concentrated acids. With dilute acids the reaction may be slow or very slow. The metal readily reacts with hot concentrated hydrochloric acid and aqua regia but slowly with cold dilute hydrochloric acid. The reaction also is slow with hot dilute sulfuric acid, which dissolves the metal, particularly in the presence of an oxidizing agent. The reaction with nitric acid is generally slow. Hot concentrated acid converts the metal to an insoluble hydrated tin(IV) oxide. The reaction is rapid with moist sulfur dioxide or sulfurous acid, chlorosulfonic, and pyrosulfuric acids. Organic acids such as, acetic, oxalic, and citric acids react slowly with the metal, particularly in the presence of air or an oxidizing agent.
Strong alkaline solutions of caustic soda or caustic potash dissolve tin forming the stannate, Na2SnO3, or K2SnO3. The metal is stable in dilute solutions of ammonia or sodium carbonate.
Tin dissolves in solutions of oxidizing salts such as potassium chlorate or potassium persulfate. The metal does not react with neutral salts in aqueous solutions. In air, tin reacts slowly with neutral salts.
The metal does not combine directly with hydrogen, nitrogen or ammonia gas.

Tin has a long, colorful history. The extraction and use of tin began during the Bronze Age around 3000 BC when early craftsmen discovered that bronze – a noncorrosive metal that is extremely hard and strong enough to be used for spears, swords, arrows, and other especially important objects at that time – could be produced by smelting tin with copper. Tin is also the primary constituent of pewter. Long ago, people developed the belief that trace amounts of tin seemed to help prevent fatigue and depression, and that drinking out of tin cups could help combat these ailments. Tin toys, tin coated cans, and tin roofs have also enjoyed great popularity in the past.

Tin is a gray to almost silver-white, ductile, malleable, lustrous metal.

Tin is a soft, silvery-white metal located in the carbon group, similar in appearance to freshcutaluminum. When polished, it takes on a bluish tint caused by a thin protective coatingof oxidized tin. This property makes it useful as a coating for other metals. It is malleable andductile, meaning it can be pounded, rolled, and formed into many shapes, as well as “pulled”into wires through a die.
There are two allotropes of tin. One is known as gray or alpha (α) tin, which is not verystable. The other is known as white tin or beta (β), which is the most common allotrope. Thetwo forms (allotropes) of tin are dependent on temperature and crystalline structure. Whitetin is stable at about 13.2°C. Below this temperature, it turns into the unstable gray alphaform. There is also a lesser-known third allotrope of tin called “brittle tin,” which exists above161°C. Its name is derived from its main property.
Tin’s melting point is 231.93°C, its boiling point is 2,602°C, and the density is 5.75 g/cm3for the gray allotrope (alpha) and 7.287 g/cm3 for the white allotrope (beta).

There are 49 isotopes of tin, 10 of which are stable and range from Sn-112to Sn-124. Taken together, all 10 stable isotopes make up the natural abundance of tinfound on Earth. The remaining 39 isotopes are radioactive and are produced artificially innuclear reactors. Their half-lives range from 190 milliseconds to 1×10⁺⁵ years.

The name “tin” is thought to be related to the pre-Roman Etruscan god Tinia, and the chemical symbol (Sn) comes from stannum, the Latin word for tin.

Tin is the 49th most abundant element found in the Earth’s crust. Although tin is nota rare element, it accounts for about 0.001% of the Earth’s crust. It is found in deposits inMalaysia, Thailand, Indonesia, Bolivia, Congo, Nigeria, and China. Today, most tin is minedas the mineral ore cassiterite (SnO₂), also known as tinstone, in Malaysia. Cassiterite is tin’smain ore. There are no significant deposits found in the United States, but small deposits arefound on the southeast coast of England. To extract tin from cassiterite, the ore is “roasted” ina furnace in the presence of carbon, thereby reducing the metal from the slag.

Although tin is located in group 14 as a metalloid, it retains one of the main characteristicsof metals: in reacting with other elements, it gives up electrons, forming positive ions just asdo all metals.
Tin has a relatively low melting point (about 231°C or 4,715°F), and it reacts with someacids and strong alkalis, but not with hot water. Its resistance to corrosion is the main characteristicthat makes it a useful metal.
There is an interesting historical event related to the two main allotropes of tin. At temperaturesbelow 13 degrees centigrade, “white” tin is slowly transformed into “gray” tin, whichis unstable at low temperatures, and during the brutally cold winter of 1850 in Russia, thetin buttons sewn on soldiers’ uniforms crumbled as the tin changed forms. In the 1800s, tinwas also widely used for pots, pans, drinking cups, and dinner flatware. However, at very lowtemperatures, these implements also disintegrated as their chemical structure was altered.

Known to the ancients. Tin is found chiefly in cassiterite (SnO2). Most of the world’s supply comes from China, Indonesia, Peru, Brazil, and Bolivia. The U.S. produces almost none, although occurrences have been found in Alaska and Colorado. Tin is obtained by reducing the ore with coal in a reverberatory furnace. Ordinary tin is composed of ten stable isotopes; thirty-six unstable isotopes and isomers are also known. Ordinary tin is a silver-white metal, is malleable, somewhat ductile, and has a highly crystalline structure. Due to the breaking of these crystals, a “tin cry” is heard when a bar is bent. The element has two allotropic forms at normal pressure. On warming, gray, or α tin, with a cubic structure, changes at 13.2°C into white, or β tin, the ordinary form of the metal. White tin has a tetragonal structure. When tin is cooled below 13.2°C, it changes slowly from white to gray. This change is affected by impurities such as aluminum and zinc, and can be prevented by small additions of antimony or bismuth. This change from the α to β form is called the tin pest. Tin–lead alloys are used to make organ pipes. There are few if any uses for gray tin. Tin takes a high polish and is used to coat other metals to prevent corrosion or other chemical action. Such tin plate over steel is used in the so-called tin can for preserving food. Alloys of tin are very important. Soft solder, type metal, fusible metal, pewter, bronze, bell metal, Babbitt metal, white metal, die casting alloy, and phosphor bronze are some of the important alloys using tin. Tin resists distilled sea and soft tap water, but is attacked by strong acids, alkalis, and acid salts. Oxygen in solution accelerates the attack. When heated in air, tin forms SnO2, which is feebly acid, forming stannate salts with basic oxides. The most important salt is the chloride (SnCl2 · H2O), which is used as a reducing agent and as a mordant in calico printing. Tin salts sprayed onto glass are used to produce electrically conductive coatings. These have been used for panel lighting and for frost-free windshields. Most window glass is now made by floating molten glass on molten tin (float glass) to produce a flat surface (Pilkington process). Of recent interest is a crystalline tin–niobium alloy that is superconductive at very low temperatures. This promises to be important in the construction of superconductive magnets that generate enormous field strengths but use practically no power. Such magnets, made of tin–niobium wire, weigh but a few pounds and produce magnetic fields that, when started with a small battery, are comparable to that of a 100 ton electromagnet operated continuously with a large power supply. The small amount of tin found in canned foods is quite harmless. The agreed limit of tin content in U.S. foods is 300 mg/kg. The trialkyl and triaryl tin compounds are used as biocides and must be handled carefully. Over the past 25 years the price of commercial tin has varied from 50￠/lb ($1.10/kg) to about $6/kg. Tin (99.99% pure) costs about $260/kg.

Tin is used in tin plating; soldering; dental alloys; collapsible tubes; in the production of tin salts.

One of the most important uses of tin is in the coating of thin steel sheets to make “tinplate,” which in turn is used to make what is known as the “tin can.” The tin coating is thin,inexpensive to apply, and resistant to most foods for extended periods of time. Other inertcoatings are sometimes used on the inside of the can to further protect the foods for longerperiods of time.
Tin is alloyed with many metals. It is added to lead to make low-melting alloys for firepreventionsprinkler systems and easy-melting solder.
It is used for bearings, to plate electrodes, and to make pewter, Babbitt metal, and dentalamalgams.
Tin also has been mixed with other metals for making castings for letter type used in printingpresses.
Some compounds of tin are used as fungicides and insecticides. Tin is also used for “weighting”silk, to give the fabric more body and heft.
Molten glass is poured over a pool of molten tin to produce smooth, solid, flat plate andwindow glass.

Chiefly for tin-plating and manufacture of food, beverage and aerosol containers, soldering alloys, babbitt and type metals, manufacture of tin salts, collapsible tubes, coating for copper wire. Principle component in pewter. Alloys as dental materials (silver-tin-mercury), nuclear reactor components (tin-zirconium), aircraft components (tin-titanium), bronze (copper-tin), brass.

Metallic element of atomic number 50, group IVA of the periodic system, aw 118.69, valences of 2, 4; 10 isotopes.

A white lustrous metal of low melting point; the fourth member of group 14 of the periodic table. Tin itself is the first distinctly metallic element of the group even though it retains some amphoteric properties. Its electronic structure has outer s²p² electrons ([Kr]4d¹⁰5s²5p²). The element is of low abundance in the Earth’s crust (0.004%) but is widely distributed, largely as cassiterite (SnOsub>2). The metal has been known since early bronze age civilizations when the ores used were relatively rich but currently worked ores are as low as 1–2% and considerable concentration must be carried out before roasting. The metal itself is obtained by reduction using carbon,
SnOsub>2 + C → Sn + COsub>2
Tin is an expensive metal and several processes are used for recovering tin from scrap tin-plate. These may involve chlorination (dry) to the volatile SnCl4, or electrolytic methods using an alkaline electrolyte:
Sn+ 4OH^-→ Sn(OH)₄^2-+ 2e^-(anode)
Sn(OH)₄^2- → Sn²⁺ + 4OH^- (cathode)
Sn²⁺ + 2e → Sn (cathode)
Tin does not react directly with hydrogen but an unstable hydride, SnH4, can be prepared by reduction of SnCl4. The low stability is due to the rather poor overlap of the diffuse orbitals of the tin atom with the small H-orbitals. Tin forms both tin(II) oxide and tin(IV) oxide. Both are amphoteric, dissolving in acids to give tin(II) and tin(IV) salts, and in bases to form stannites and stannates,
SnO + 4OH^- → [SnO₃]^4-+2H₂O
stannite (relatively unstable)
SnO₂ + 4OH^- → [SnO₄]^4–+ 2H₂O
stannate
The halides, SnX₂, may be prepared by dissolving tin metal in the hydrogen halide or by the action of heat on SnO plus the hydrogen halide. Tin(IV) halides may be prepared by direct reaction of halogen with the metal. Although tin(II) halides are ionized in solution their melting points are all low suggesting considerable covalence in all but the fluoride. The tin(IV) halides are volatile and essentially covalent with slight polarization of the bonds. Tin(II) compounds are readily oxidized to tin(IV) compounds and are therefore good reducing agents for general laboratory use.
Tin has three crystalline modifications or allotropes, α-tin or ‘gray tin’ (diamond structure), β-tin or ‘white tin’, and γ-tin; the latter two are metallic with close packed structures. Tin also has several isotopes. It is used in a large number of alloys including Babbit metal, bell metal, Britannia metal, bronze, gun metal, and pewter as well as several special solders.
Symbol: Sn; m.p. 232°C; b.p. 2270°C; r.d. 7.31 (20°C); p.n. 50; r.a.m. 118.710.

Tin is relatively rare, composing only about 0.0006% in the earth’s crust. The major tin ore is cassiterite, a naturally occurring tin (IV) oxide (SnO2). The other major tin-containing minerals are stannate, teallite, cylindrite, and canfieldite that are sulfides of tin.

White TIN is an almost silver-white, ductile, malleable, lustrous solid. Mp 232°C; bp: 2507°C. Density: 7.3 g cm-3. Pure white TIN becomes non-metallic powdery gray TIN if held for a sustained period at temperatures less than 13°C.

TIN is a reducing agent. Stable in massive form in air, but oxidizes (corrodes) in air as a powder, especially in the presence of water. Dissolve slowly in dilute strong acids in the cold. Dissolves in hot aqueous KOH and other strongly basic solutions. Incompatible with acids and base. Incompatible with chlorine and turpenTINe.

Tin, as the elemental metal, is nontoxic. Most, but not all of tin’s inorganic salts and compoundsare also nontoxic.
In contrast, almost all organic tin compounds (tin compounds composed of carbon andhydrocarbons) are very toxic and should be avoided. If they are used, special equipment andcare must be taken in handling.
(Note: When chemical formulas use the letter “R” preceding an element’s symbol, it designatessome form of organic compound—for example, R4Sn. If the letter “X” follows theelement’s symbol in a formula, it designates some form of inorganic compound—for example,SnX₂. Thus, a whole series of tin compounds could be designated as R₄Sn₂, R₂Sn, or SnX₄,SnX₂, and so forth.)

Inorganic tin salts are irritants of the eyes and skin. No systemic effects have been reported from industrial exposure. Some inorganic tin compounds can cause skin or eye irritation because of acid or alkaline reaction produced with water. Tin tetrachloride, stannous chloride, and stannous sulfate are strong acids; sodium and potassium stannate are strong alkalies.

Non flammable

Hot-dip coatings can be applied to fabricatedparts made of mild and alloy steels, cast iron,and copper and copper alloys to improveappearance and corrosion resistance. Like zinc,the coatings consist of two layers — a relativelypure outer layer and an intermediate alloy layer.
An invisible surface film of stannic oxideis formed during exposure, which helps toretard, but does not completely prevent, corrosion.The coatings have good resistance to tarnishingand staining indoors, and in most rural,marine, and industrial atmospheres. They alsoresist foods. Corrosion resistance in all casescan be markedly improved by increasing thicknessand controlling porosity. Typical applicationswhere they can be used are milk cans,condenser and transformer cans, food and beveragecontainers, and various items of sanitaryequipment such as cast iron mincing machinesand grinders.

An inhalation hazard. Questionable carcinogen with experimental tumorigenic data by implant route. Combustible in the form of dust when exposed to heat or by spontaneous chemical reaction with Br2, BrF3, Cl2, ClF3, Cu(NO3), K2O2, S. See also POWDERED METALS and TIN COMPOUNDS.

The most important use of tin is as a protective coating for other metals, such as in the food and beverage canning industry; in roofing tiles; silverware, coated wire; household utensils; electronic components; and pistons. Common tin alloys are phosphor bronze; light brass; gun metal; high tensile brass; manganese bronze; die-casting alloys; bearing metals; type metal; and pewter. These are used as soft solders, fillers in automobile bodies; and as coatings for hydraulic brake parts; aircraft landing gear and engine parts. Metallic tin is used in the manufacture of collapsible tubes and foil for packaging. Exposures to tin may occur in mining, smelting, and refining; and in the production and use of tin alloys and solders. Inorganic tin compounds are important industrially in the production of ceramics; porcelain, enamel, glass; and inks; in the production of fungicides; anthelmintics, insecticides; as a stabilizer it is used in polyvinyl plastics and chlorinated rubber paints; and it is used in plating baths.

Limited animal testing with stannous chloride has not revealed evidence of carcinogenic potential. Mixed results have been observed in genotoxic assays.

Tin is a naturally occurring element in the earth’s crust with ~2–3 ppm in concentration and found in environmental media in both organic and inorganic forms. Tin may be released to the environment from natural and anthropogenic sources. The most significant releases of tin are from burning of fossil fuels and industrial production and use of tin. Tin compounds are generally only sparingly soluble in water and are likely to partition to soils, sediments, and possibly to aquatic organisms. Inorganic tin cannot be degraded in the environment, but may undergo redox reaction, ligand exchange, and precipitation reactions. Inorganic tin can be transformed into organometallic forms through the microbial methylation process. Degradation of organotin compounds involves the breaking of the tin–carbon bond through UV irradiation or biological and chemical cleavage. The speciation of organotin compounds is pH-dependent. In sediment, organotins are generally persistent. Photodegradation of organotins may occur at relatively slow rates. Hydrolysis is considered insignificant. Organotin compounds may be significantly bioconcentrated by aquatic organisms. Tin has been historically used in antifouling paints and coatings for the bottom of boats, but this has been discontinued because of its extreme toxicity to marine organisms.
A bioconcentration factor (BCF) relates the concentration of a chemical in plants and animals to the concentration of the chemical in the medium in which they live. It was estimated that the BCFs of inorganic tin were 100, 1000, and 3000 for marine and freshwater plants, invertebrates, and fish. Marine algae can bioconcentrate stannic tin by a factor of 1900. The BCF of tributyltin was estimated to be 473, but measured BCFs were always higher. Bioconcentration factors for bis(tributyltin)oxide with marine oysters were measured as 2300–11 400. Seven-day BCFs were derived for seven organotin compounds for muscle, liver, kidney, and vertebra tissue of carp. The BCFs ranged from 12 to 5012; the highest factors were found for tributyltins. However, these factors were not based on steady-state conditions, and may be low estimates. No information was obtained on the food chain and biomagnification of inorganic or organic tin.

UN3089 Metal powders, flammable, n.o.s., Hazard Class: 4.1; Labels: 4.1-Flammable solid.

Tin powder is purified by adding it to about twice its weight of 10% aqueousNaOH and shaking vigorously for 10minutes. (This removes oxide film and stearic acid or similar material that is sometimes added for pulverisation.) It is then filtered, washed with water until the washings are no longer alkaline to litmus, rinsed with MeOH and dried in air. [Sisido et al. J Am Chem Soc 83 538 1961.]

All organic tin compounds, including trimethyltin, triethyltin, and tributyltin compounds, have the ability to cause damages to the structure of Vitamin B12 depletion of methyl group necessary for DNA and RNA reactions. Due to lipophilicity, organotin compounds may affect lipid bilayers by altering membrane fluidity where it is an initial site of activation. Thus, these compounds can bind to proteins and inhibit mitochondrial oxidative phosphorylation (hydrolysis of adenosine triphosphate) and brain glucose oxidation and are toxic. Very little data are available on inorganic tin.

TIN is a reducing agent. Stable in bulk form in air, but as powder it corrodes (oxidizes) in air, especially in the presence of moisture. Keep away from strong oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause fires or explosions. Incompatible with acids, alkalies, bases, chlorine, turpentine; reacts violently with acetic aldehyde, ammonium nitrate, ammonium perchlorate, hexachloroethane. Strong reducing agents may react violently with halogens, bromine fluoride, chlorine trifluoride, copper nitrate, disulfur dichloride, nitrosyl fluoride, potassium dioxide, sodium peroxide, sulfur, and other chemicals. May form explosive compounds with hexachloroethane, pentachloroethane, picric acid, potassium iodate, potassium peroxide, 2,4,6-trinitrobenzene-1,3,5-triol.