Hydrogen
14.01 K
Helium
0.95 K
Lithium
453.7 K
Beryllium
1570 K
Boron
2348 K
Carbon
3823 K
Nitrogen
63.1 K
Oxygen
54.8 K
Fluorine
53.5 K
Neon
24.6 K
Sodium
370.9 K
Magnesium
923 K
铝
933.5 K
Silicon
1687 K
Phosphorus
317.3 K
Sulfur
388.4 K
Chlorine
171.6 K
Argon
83.8 K
Potassium
336.5 K
Calcium
1115 K
Scandium
1814 K
Titanium
1941 K
Vanadium
2183 K
Chromium
2180 K
Manganese
1519 K
Iron
1811 K
Cobalt
1768 K
Nickel
1728 K
Copper
1357.8 K
Zinc
692.7 K
Gallium
302.9 K
Germanium
1211.4 K
Arsenic
1090 K
Selenium
494 K
Bromine
265.8 K
Krypton
115.8 K
Rubidium
312.5 K
Strontium
1050 K
Yttrium
1799 K
Zirconium
2128 K
Niobium
2750 K
Molybdenum
2896 K
Technetium
2430 K
钌
2607 K
Rhodium
2237 K
Palladium
1828.1 K
Silver
1234.9 K
Cadmium
594.2 K
Indium
429.8 K
Tin
505.1 K
Antimony
903.8 K
Tellurium
722.6 K
Iodine
386.9 K
Xenon
161.3 K
Caesium
301.6 K
Lanthanoids
Hafnium
2506 K
Tantalum
3290 K
Tungsten
3695 K
Rhenium
3459 K
Osmium
3306 K
Iridium
2739 K
Platinum
2041.4 K
Gold
1337.3 K
Mercury
234.3 K
Thallium
577 K
Lead
600.6 K
Bismuth
544.4 K
Polonium
527 K
Astatine
575 K
Radon
202 K
Francium
300 K
Radium
973 K
Actinoids
Rutherfordium
Dubnium
Seaborgium
Bohrium
Hassium
Meitnerium
Darmstadtium
Roentgenium
Copernicium
Nihonium
Flerovium
Moscovium
Livermorium
Tennessine
Oganesson
Lanthanum
1193 K
Cerium
1071 K
Praseodymium
1204 K
Neodymium
1294 K
Promethium
1373 K
Samarium
1345 K
Europium
1095 K
Gadolinium
1568 K
Terbium
1629 K
Dysprosium
1685 K
Holmium
1747 K
Erbium
1770 K
Thulium
1818 K
Ytterbium
1092 K
Lutetium
1936 K
Actinium
1323 K
Thorium
2023 K
Protactinium
1845 K
Uranium
1408 K
Neptunium
917 K
Plutonium
913 K
Americium
1449 K
Curium
1618 K
Berkelium
1323 K
Californium
1173 K
Einsteinium
1133 K
Fermium
1800 K
Mendelevium
1100 K
Nobelium
1100 K
Lawrencium
1900 K
Melting Point of Chemical Elements
In general,meltingis aphase changeof a substance from the solid to the liquid phase. Themelting pointof a substance is the temperature at which this phase change occurs. Themelting pointalso defines a condition in which the solid and liquid can exist in equilibrium. Adding a heat will convert the solid into a liquid with no temperature change. At the melting point the two phases of a substance, liquid and vapor, have identical free energies and therefore are equally likely to exist. Below the melting point, the solid is the more stable state of the two, whereas above the liquid form is preferred. The melting point of a substance depends on pressure and is usually specified at standard pressure. When considered as the temperature of the reverse change from liquid to solid, it is referred to as the freezing point or crystallization point.
See also:Melting Point Depression
The first theory explaining mechanism of melting in the bulk was proposed by Lindemann, who used vibration of atoms in the crystal to explain the melting transition. Solids are similar to liquids in that both are condensed states, with particles that are far closer together than those of a gas. 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. Themotion of individual atoms, ions, or molecules in a solid is restricted to vibrational motion about a fixed point. As a solid is heated, itsparticles vibrate more rapidlyas the solid absorbs kinetic energy. 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. Themelting pointis the temperature at which the disruptive vibrations of the particles of the solid overcome the attractive forces operating within the solid.
As with boiling points, the melting point of a solid is dependent on the strength of those attractive forces. For example, sodium chloride (NaCl) is an ionic compound that consists of a multitude of strong ionic bonds. Sodium chloride melts at 801°C. On the other hand, ice (solid H2O) is a molecular compound whose molecules are held together by hydrogen bonds, which is effectively a strong example of an interaction between two permanent dipoles. Though hydrogen bonds are the strongest of the intermolecular forces, the strength of hydrogen bonds is much less than that of ionic bonds. The melting point of ice is 0 °C.
Covalent bonds often result in the formation of small collections of better-connected atoms called molecules, which in solids and liquids are bound to other molecules by forces that are often much weaker than the covalent bonds that hold the molecules internally together. Such weak intermolecular bonds give organic molecular substances, such as waxes and oils, their soft bulk character, and their low melting points (in liquids, molecules must cease most structured or oriented contact with each other).