Nickel anode - 152 mm x 25 mm x 1 mm, 99.6% pure nickel electrode sheet for DIY nickel plating and nickel electroplating, high-purity nickel electrode

HIGH PURITY NICKEL ---- This nickel anode has a 99.6% nickel content, giving it a pure nickel rating that can prevent corrosion, increase wear resistance, shine and beauty.
SIZE: 1 "X 6" X 0.04 "---- 6 inches long, 1 inch wide and 0.04 inches thick, refer to the picture for the detailed parameters.
IDEAL MATERIAL FOR THE COATING ---- When used as a sacrificial nickel anode, this electrode guarantees constant regeneration of the pure nickel content in the solution. A constant and permanent deposition of the metal is guaranteed on the cathode side.
COMMONLY USED ---- This nickel electrode is suitable for almost all galvanic requirements that require a very high level of purity. .
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 nickel : crucible    wire   mesh   foam    foil  strip  Nickel powder

copper     aluminum     lead    Zinc   tin    nickel   iron

   magnesium    bismuth   manganese   chromium    cobalt    titanium

    Tungsten    vanadium   niobium   indium     molybdenum     antimony

      rhenium    germanium    zirconium     cadmium     hafnium

      barium   lithium     beryllium     strontium     calcium

      Tantalum    gadolinium    samarium      yttrium   ytterbium

       Lutetium    praseodymium   holmium     erbium   thulium     dysprosium

       terbium   europium  lanthanum   cerium   neodymium  scandium 

         rubidium    cesium    silicon     carbon

In chemistry, metals are materials whose atoms are united by metallic bonds. They are simple bodies or alloys which are generally hard, opaque, shiny, good conductors of heat and electricity. They are generally malleable, i.e. they can be hammered or pressed to make them change shape without cracking or breaking them. Many substances which are not classified as metallic at atmospheric pressure can acquire metallic properties when subjected to high pressures. Metals have many common applications, and their consumption has increased significantly since the 1980s, to the point that some of them have become critical mineral raw materials.

In astrophysics, and in particular in stellar physics, any chemical element other than hydrogen and helium is called metal. These elements are produced by stellar nucleosynthesis from hydrogen and helium by nuclear fusion, the process at the origin of the energy released by the stars. From this point of view, the metallicity of a star is the proportion of elements other than hydrogen and helium which constitute it.

The electrons of pure or alloyed metallic materials are distributed in energy levels forming a continuum between the valence band, occupied by the valence electrons, and the conduction band, occupied by the free electrons thermally injected from the valence band beyond the Fermi level. These free electrons form a delocalized metallic bond throughout the volume of the material. We can imagine a metal as a three-dimensional network of metal cations bathed in a fluid of very mobile electrons. The free electron model calculates the electrical conductivity and the contribution of electrons to the heat capacity and thermal conductivity of metals, although this model does not take into account the structure of the crystal lattice of the metal. Some materials, such as intermetallic, have partially metallic bonds and are therefore at the limit of ceramics.

The particular electronic nature of a metal bond is responsible for several macroscopic properties of metals: the free electron fluid ensures both high electrical conductivity and thermal conductivity by allowing the circulation of an electric current and promoting propagation phonons in the material; it accounts for the ductility, malleability and plasticity of metals while maintaining their cohesion in the event of deformation breaking the other interatomic bonds; it gives metals their particular absorbance and luster by its interaction with electromagnetic waves, as well as their higher melting point and boiling point than non-metals by strengthening the other types of interatomic bonds. The latter, in particular the covalent coordination bonds, are responsible for the different crystal structures formed by solid metals: the most frequent is the centered cubic structure, followed by the compact hexagonal structure and the centered faces cubic structure.

In a centered cubic structure, each atom is located in the center of a cube formed by its eight neighboring atoms. In cubic structures with centered faces and compact hexagonal, each atom is surrounded by twelve other atoms, but the stacking of these atoms differs between these two structures. Some metals can adopt different crystal structures depending on the temperature and pressure to which they are subjected.