The melting point is the temperature at which the disruptive vibrations of the particles of the solid overcome the attractive forces operating within the solid. At some point, the amplitude of vibration becomes so large that the atoms start to invade the space of their nearest neighbors and disturb them, and the melting process initiates. As a solid is heated, its particles vibrate more rapidly as the solid absorbs kinetic energy. The motion of individual atoms, ions, or molecules in a solid is restricted to vibrational motion about a fixed point. The atoms in a solid are tightly bound to each other, either in a regular geometric lattice (crystalline solids, which include metals and ordinary ice) or irregularly (an amorphous solid such as common window glass), and are typically low in energy. Solids are similar to liquids in that both are condensed states, with particles that are far closer together than those of a gas. The first theory explaining the mechanism of melting in bulk was proposed by Lindemann, who used the vibration of atoms in the crystal to explain the melting transition. When considered as the temperature of the reverse change from liquid to solid, it is called the freezing point or crystallization point. The melting point of a substance depends on pressure and is usually specified at standard pressure. Adding heat will convert the solid into a liquid with no temperature change. In thermodynamics, the melting point defines a condition where the solid and liquid can exist in equilibrium. When considered as the temperature of the reverse change from vapor to liquid, it is called the condensation point. The pressure at which vaporization (boiling) starts to occur for a given temperature is called the saturation pressure. The temperature at which vaporization (boiling) starts to occur for a given pressure is called the saturation temperature or boiling point. In thermodynamics, saturationdefines a condition in which a mixture of vapor and liquid can exist together at a given temperature and pressure. Weinrich Minerals, Inc.Note that these points are associated with the standard atmospheric pressure. Rock and Mineral Shows Google Search for Iron
McDougall Minerals Google Search for Iron Google Search for IronĮxceptional Minerals Google Search for Iron of Minerals,2nd ed.,1990)ĭakota Matrix Minerals Google Search for IronĮxcalibur Mineral Corp. (01.01)with metallic elements other than the platinum groupĠ1.01.11.01 Kamacite? alpha-(Fe,Ni) F m3m 4/m 3 2/mĠ1.01.11.02 Taenite gamma-(Fe,Ni) F m3m 4/m 3 2/mĠ1.01.11.03 Tetrataenite FeNi P 4/mmm 4/m 2/m 2/mĠ1.01.11.04 Awaruite Ni2FetoNi3Fe P m3m 4/m 3 2/mĠ1.01.11.06 Wairauite CoFe P m3m 4/m 3 2/mĠ1.AE.05 01 - ELEMENTS (Metals and intermetallic alloys metalloids and nonmetals carbides, silicides, nitrides, phosphides)Ġ1.AE.05 Kamacite? alpha-(Fe,Ni) F m3m 4/m 3 2/m GRapi = 0 (Gamma Ray American Petroleum Institute Units) Iron is Not Radioactive PE Iron = 31.03 barns/electron U=PE Iron x rElectron Density= 225.68 barns/cc. Standardized Intensity (100%) Reflection Spectra of Iron in Air λĬalculated Relative Intensity Colors of Iron in Air Relativeīulk Density (Electron Density)=7.27 gm/cc note: Specific Gravity of Iron =7.81 gm/cc. Massive - Uniformly indistinguishable crystals forming large masses. Granular - Generally occurs as anhedral to subhedral crystals in matrix.
fractured metals).ĭisseminated - Occurs in small, distinct particles dispersed in matrix. View Additional jPOWD Structure files for Iron Wilburn D R, Bassett W A, American Mineralogist, 63 (1978) p.591-596, Hydrostatic compression of iron and related compounds: An overview, P = 1 Kbar This locality is one of the very few known localities for terrestrial native iron.Ī = 2.874, Z = 2 V = 23.74 Den(Calc)= 7.81 Link to Location Data.Ĭomments: Specimen of volcanic rock containing dark gray grains of native Iron. Valid Species (Pre IMA) 900 BC (Dana # Added)Īsteroid fragments and in German and Greenland basalts. In meteorites and rarely basalts that have intruded carbon-rich sediments.
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