User:Double sharp/Tin

Tin, ₅₀Sn

Tin
Allotropes	silvery-white, β (beta); gray, α (alpha)
Standard atomic weight Ar°(Sn)
	118.710±0.007 118.71±0.01 (abridged)
Tin in the periodic table
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson Ge ↑ Sn ↓ Pb indium ← tin → antimony
Atomic number (Z)	50
Group	group 14 (carbon group)
Period	period 5
Block	p-block
Electron configuration	[Kr] 4d10 5s2 5p2
Electrons per shell	2, 8, 18, 18, 4
Physical properties
Phase at STP	solid
Melting point	505.08 K ​(231.93 °C, ​449.47 °F)
Boiling point	2875 K ​(2602 °C, ​4716 °F)
Density (at 20° C)	white (β): 7.289 g/cm3 gray (α): 5.770 g/cm3
when liquid (at m.p.)	6.99 g/cm3
Heat of fusion	white (β): 7.03 kJ/mol
Heat of vaporization	white (β): 296.1 kJ/mol
Molar heat capacity	white (β): 27.112 J/(mol·K)
Vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 1497 1657 1855 2107 2438 2893
Atomic properties
Oxidation states	common: −4, +2, +4 −3,? −2,? −1,? 0, +1, +3
Electronegativity	Pauling scale: 1.96
Ionization energies	1st: 708.6 kJ/mol 2nd: 1411.8 kJ/mol 3rd: 2943.0 kJ/mol
Atomic radius	empirical: 140 pm
Covalent radius	139±4 pm
Van der Waals radius	217 pm
Spectral lines of tin
Other properties
Natural occurrence	primordial
Crystal structure	white (β): ​body-centered tetragonal (tI4)
Lattice constants	white (β): a = 583.13 pm c = 318.11 pm (at 20 °C)
Crystal structure	gray (α): ​face-centered diamond-cubic (cF8)
Lattice constant	gray (α): a = 648.96 pm (at 20 °C)
Thermal expansion	white (β): 21.76×10−6/K (at 20 °C) gray (α): 5.20×10−6/K (at 20 °C)
Thermal conductivity	66.8 W/(m⋅K)
Electrical resistivity	115 nΩ⋅m (at 0 °C)
Magnetic ordering	white (β): paramagnetic gray (α): diamagnetic
Molar magnetic susceptibility	white (β): +3.1×10−6 cm3/mol (298 K)
Young's modulus	50 GPa
Shear modulus	18 GPa
Bulk modulus	58 GPa
Speed of sound thin rod	2730 m/s (at r.t.) (rolled)
Poisson ratio	0.36
Mohs hardness	1.5
Brinell hardness	50–440 MPa
CAS Number	7440-31-5
History
Discovery	protohistoric, around 35th century BC
Symbol	"Sn": from Latin stannum
Isotopes of tin
Main isotopes Decay abun­dance half-life (t1/2) mode pro­duct 112Sn 0.970% stable 114Sn 0.66% stable 115Sn 0.34% stable 116Sn 14.5% stable 117Sn 7.68% stable 118Sn 24.2% stable 119Sn 8.59% stable 120Sn 32.6% stable 122Sn 4.63% stable 124Sn 5.79% stable 126Sn trace 2.3×105 y β− 126Sb

Tin is a chemical element with symbol Sn (from Latin: stannum) and atomic number 50. It is a post-transition metal in group 14 of the periodic table whose chemistry is intermediate between those of its vertical neighbours, germanium and lead. Tin is obtained chiefly from the mineral cassiterite, which contains tin dioxide, SnO₂. Tin shows a chemical similarity to both of its neighbors in group 14, germanium and lead, and has two main oxidation states, +2 and the slightly more stable +4. Tin is the 49th most abundant element and has, with 10 stable isotopes, the largest number of stable isotopes in the periodic table, thanks to its magic number of protons. It has two main allotropes: at room temperature, the stable allotrope is β-tin, a silvery-white, malleable metal, but at low temperatures it transforms into the less dense grey α-tin, which has the diamond cubic structure. Metallic tin is not easily oxidized in air or water at room temperature, though it does react with steam and with air on heating.

The first alloy used on a large scale was bronze, made of tin and copper, from as early as 3000 BC. After 600 BC, pure metallic tin was produced. Pewter, which is an alloy of 85–90% tin with the remainder commonly consisting of copper, antimony, and lead, was used for flatware from the Bronze Age until the 20th century. In modern times, tin is used in many alloys, most notably tin/lead soft solders, which are typically 60% or more tin and in the manufacture of transparent, electrically conducting films of indium tin oxide in optoelectronic applications. Another large application for tin is corrosion-resistant tin plating of steel. Because of the low toxicity of inorganic tin, tin-plated steel is widely used for food packaging as tin cans. However, some organotin compounds (compounds formed from tin and hydrocarbons) can be almost as toxic as cyanide.

Characteristics

Physical and atomic

A tin atom has fifty electrons, arranged in the electron configuration [Kr]4d¹⁰5s²5p². Of these, four are valence electrons, occupying the 5s and 5p subshells. Like the other stable members of group 14, carbon, silicon, germanium, and lead, tin has the same number of valence electrons as valence orbitals: hence, it can complete its octet and obtain the stable noble gas configuration of xenon by forming sp³ hybrid orbitals, forming tetrahedral tetravalent SnX₄ derivatives where the central tin atom shares an electron pair with each of the four atoms it is bonded to. Nevertheless, tin also shows significant chemistry in the divalent state, in which only the 5p electrons are involved in bonding: the trend down the group favours the lower +2 oxidation state over the higher +4 for the heavier elements, as bond energy decreases with size from silicon to lead so that the energy needed to use the 5s electrons to form bonds is not compensated by the energy released in forming these bonds, particularly when highly electronegative substituents are involved. The first four ionisation energies of tin are 708.4, 1411.4, 2942.2, and 3929.3 kJ/mol respectively, which are close to the values for lead due to the lanthanide contraction. These values are less than those for carbon, silicon, and germanium and accordingly tin is the first element in group 14 to show significant cationic chemstry. Tin has an electronegativity of about 1.96 on the Pauling scale; this is intermediate between the values for germanium (2.01) and lead(II) (1.87), greater than the value for silicon (1.90), and significantly less than the value for lead(IV) (2.33).

Tin forms two allotropes

Chemistry

Oxoacid derivatives

and are they really salts? really Sn is a lame metal chemically

Bibliography

• Clayden, Jonathan; Greeves, Nick; Warren, Stuart (2012). Organic Chemistry (2nd ed.). Oxford University Press. ISBN 978-0-19-927029-3.
• Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
• King, R. Bruce (1995). Inorganic Chemistry of Main Group Elements. Wiley-VCH. ISBN 0-471-18602-3.