Tin element periodic table

Tin was one of the first metals used by humans. Until 5,000 years ago, tin was mixed with copper to produce bronze, an alloy that was stronger than either of the pure metals. The cassiterite mineral, SnO2, is the main source of pure tin. Tin is used in a wide range of applications, for example, plated steel objects, such as cans, to prevent them from corroding. Tin chloride is used to dye silks. This metal continues to be used in a variety of resistant alloys, such as pewter, soft solder and bronze.

Tin element periodic table

Electron configuration

The electron configuration of an element describes the arrangement of electrons in the atoms of that element, and be used to predict its chemical properties and reactivity.

In the electron configuration notation, the letters "s", "p", "d", and "f" represent the different types of atomic orbitals, and the superscripts indicate the number of electrons in each orbital. The orbitals are filled in a specific order, starting with the lowest energy orbital and working up.

electron configuration of element Sn

Emission spectra

Each element in the periodic table presents its own unique emission spectra, which is determined by the energy levels of its electrons. When an electron in an atom is excited to a higher energy level, it can de-excite by emitting a photon of light with an energy equal to the difference between the two levels. This results in a characteristic emission line in the spectra (which corresponds to specific wavelengths of light). These spectra are usefull to identify the elements present in a sample.

emmision spectra of element Sn

Symmary of properties (Sn)

Atomic weight118.710(7)
Discoverer (year)unknown (ancient)
Natural formmetallic solid (tetragonal)
Electron configuration[Kr] 4d10 5s2 5p2
M.p. (ºC)232
B.p. (ºC)2270
Earth's crust abundance (ppm)2.3
Isotope (abundance %)112Sn (0.97), 114Sn (0.66), 115Sn (0.34), 116Sn (14.54), 117Sn (7.68), 118Sn (24.22), 119Sn (8.59), 120Sn (32.58), 122Sn (4.63), 124Sn (5.79)
Density (g/cm3)7.31
vdW radius (pm)217
Covalent radius (pm)140
Electronegativity (Pauling)1.96
Vaporisation enthalpy (Kj/mol)290.40
Fusion enthalpy (kJ/mol)7.03
Specific heat capacity (J/g·K) at 25ºC and 1 at0.23
Thermal conductivity (W/cm·K) at 25 ºC and 1 at0.670
Oxidation number+4, +2
Electronic affinity (eV)1.11
1st Ionization energy (eV)7.3439

Definition of terms in the previous table

  • Atomic weight: The average mass of an element's atoms, typically given in atomic mass units (amu).
  • Natural form: The most stable and abundant form of an element that occurs naturally in the environment.
  • Electron configuration: The arrangement of electrons in an atom or molecule.
  • Melting point: The temperature at which a solid substance turns into a liquid.
  • Boiling point: The temperature at which a liquid substance turns into a gas.
  • Earth's crust abundance (ppm): The concentration of an element in the Earth's crust, typically given in parts per million (ppm).
  • Isotope (abundance %): A variant of an element that has the same number of protons in the nucleus, but a different number of neutrons. The abundance of an isotope is the percentage of the isotope in a sample of the element.
  • Density (g/cm3): The mass of a substance per unit volume.
  • vdW radius (pm): The radius of an atom or molecule as predicted by the van der Waals model, typically given in picometers (pm).
  • Covalent radius (pm): The distance from the center of an atom to the center of another atom with which it is bonded covalently, typically given in picometers (pm).
  • Electronegativity (Pauling): A measure of an atom's ability to attract electrons in a chemical bond, based on the Pauling scale.
  • Vaporisation enthalpy (kJ/mol): The amount of energy required to convert a substance from a liquid to a gas at a constant temperature.
  • Fusion enthalpy (kJ/mol): The amount of energy required to convert a substance from a solid to a liquid at a constant temperature.
  • Specific heat capacity (J/g·K) at 25ºC and 1 at: The amount of heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius at a constant pressure.
  • Thermal conductivity (W/cm·K) at 25 ºC and 1 at: The ability of a substance to conduct heat, typically given in watts per centimeter per kelvin.
  • Oxidation number: A positive or negative integer that represents the number of electrons that an atom has gained or lost in a chemical compound.
  • Electronic affinity: The energy change associated with adding an electron to a neutral atom to form a negative ion.
  • 1st Ionization energy: The energy required to remove the most loosely bound electron from a neutral atom.

Back to the Periodic Table of the Elements.