Solid

Solid is one of the <a href="/facts/State_of_matter/ojlIA1UF">four fundamental states of matter</a> (along with liquid, gas, and plasma), and is a way in which all matter can be arranged on a microscopic scale under certain conditions. <a href="/facts/Molecules/N9ljSfFq">Molecules</a> in a solid are closely packed and do not slide past each other as is the case for <a href="/facts/Fluid/tMQ46Tmz">fluids</a>. Solids resist compression, expansion, or external forces that would alter its shape, with the degree to which they are resisted dependent upon the specific material under consideration. Solids also always possess the least amount of kinetic energy per atom/molecule relative to other phases or, equivalently stated, solids are formed when matter in the liquid / gas phase is cooled below a certain temperature. This temperature is called the <a href="/facts/Melting_point/MY0w0h0k">melting point</a> of that substance and is an <a href="/facts/Intrinsic/5WJ1zN7q">intrinsic</a> property, i.e. independent of how much of the matter there is.
Solids are characterized by <a href="/facts/Structural_rigidity/QN30Aq69">structural rigidity</a> and resistance to applied external forces and pressure. Unlike liquids, solids do not flow to take on the shape of its container, nor does it expand to fill the entire available volume like a gas. Much like the other three fundamental phases, solids also <a href="/facts/Thermal_expansion/BP2vjX0N">expand when heated</a>, the thermal energy put into increasing the distance and reducing the <a href="/facts/Potential_energy/I03KLbmn">potential energy</a> between atoms. However, solids do this to a much lesser extent. When heated to its melting point or <a href="/facts/Sublimation_(phase_transition)/KDoKokMn">sublimation point</a>, solids melt into a liquid or <a href="/facts/Sublimation_(phase_transition)/KDoKokMn">sublimate</a> directly into a gas, respectively. For solids that directly <a href="/facts/Sublimation_(phase_transition)/KDoKokMn">sublimate</a> into a gas, the melting point is replaced by the sublimation point. As a rule of thumb, melting will occur if the subjected pressure is higher than the substance's <a href="/facts/Triple_point/Npary634">triple point</a>'s pressure, and sublimation will occur otherwise. Melting and melting points refer exclusively to transitions between solids and liquids. Melting occurs across a great extent of temperatures, ranging from 0.10 K for <a href="/facts/Helium-3/SmPC5oT3">helium-3</a> under 30 bars (3 MPa) of pressure, to around 4,200 K at 1 atm for the composite <a href="/facts/Refractory/LoKrzGkR">refractory</a> material <a href="/facts/Hafnium_carbonitride/D0Vrjwpv">hafnium carbonitride</a>.
The atoms in a solid are tightly bound to each other in one of two ways: regular <a href="/facts/Geometric_lattice/DkCTIQL1">geometric lattices</a> called <a href="/facts/Crystal/e2R2mk3E">crystalline solids</a> (e.g. metals, <a href="/facts/Ice/BGvkKFjD">water ice</a>), or irregular arrangements called <a href="/facts/Amorphous_solid/YTIzmrR0">amorphous solids</a> (e.g. glass, plastic). Molecules and atoms forming crystalline lattices usually organize themselves in a few well-characterized packing structures, such as body-centered cubic. The adopted structure can and will vary between various pressures and temperatures, as can be seen in <a href="/facts/Phase_diagram/rcemFgW0">phase diagrams</a> of the material (e.g. <a href="/facts/Phase_diagram/rcemFgW0">that of water</a>, see left and upper). When the material is composed of a single species of atom/molecule, the phases are designated as <a href="/facts/Allotropy/2WUdHWxg">allotropes</a> for atoms (e.g. <a href="/facts/Diamond/IBUdnd1y">diamond</a> / <a href="/facts/Graphite/sSf3KMXr">graphite</a> for <a href="/facts/Carbon/ukrgQexo">carbon</a>), and as <a href="/facts/Crystal_polymorphism/bu2tqsB9">polymorphs</a> (e.g. calcite / aragonite for <a href="/facts/Calcium_carbonate/UQ1wLFna">calcium carbonate</a>) for molecules.
Non-<a href="/facts/Porosity/UoyAJU8X">porous</a> solids invariably strongly resist any amount of <a href="/facts/Compression_(physics)/2wwcVmM0">compression</a> that would otherwise result in a decrease of total <a href="/facts/Volume/aeAXCBUd">volume</a> regardless of temperature, owing to the <a href="/facts/Electron_degeneracy_pressure/fupuyb5c">mutual-repulsion</a> of neighboring electron clouds among its constituent atoms. In contrast to solids, gases are <a href="/facts/Ideal_gas_law/Pphokwhf">very easily compressed</a> as the molecules in a gas are far apart with few intermolecular interactions. Some solids, especially metallic alloys, can be <a href="/facts/Deformation_(physics)/xK7R59oI">deformed</a> or pulled apart with enough force. The degree to which this solid resists deformation in differing directions and axes are quantified by the <a href="/facts/Elastic_modulus/Et73KjbT">elastic modulus</a>, <a href="/facts/Ultimate_tensile_strength/Cv2jPplR">tensile strength</a>, <a href="/facts/Specific_strength/D3nbocax">specific strength</a>, as well as other measurable quantities.
For the vast majority of substances, the solid phases have the highest <a href="/facts/Density/92p6hh9I">density</a>, moderately higher than that of the liquid phase (if there exists one), and solid blocks of these materials will sink below their liquids. Exceptions include water (<a href="/facts/Iceberg/2xFa1Xb2">icebergs</a>), <a href="/facts/Gallium/EucevDs9">gallium</a>, and <a href="/facts/Plutonium/4bUw9zH3">plutonium</a>. All naturally occurring elements on the periodic table has a melting point at standard atmospheric pressure, with three exceptions: the <a href="/facts/Noble_gas/j0yHMEAE">noble gas</a> <a href="/facts/Helium/yRul93TG">helium</a>, which remains a liquid even at absolute zero owing to <a href="/facts/Zero-point_energy/Kuusl57a">zero-point energy</a>; the <a href="/facts/Metalloid/uMFVXuTq">metalloid</a> <a href="/facts/Arsenic/k1c4f44D">arsenic</a>, sublimating around 900 K; and the life-forming element carbon, which sublimates around 3,950 K.
When applied pressure is released, solids will (very) rapidly re-expand and release the stored energy in the process in a manner somewhat similar to those of gases. An example of this is the (oft-attempted) confinement of freezing water in an inflexible container (of steel, for example). The gradual freezing results in an increase in volume, as ice is less dense than water. With no additional volume to expand into, <a href="/facts/Ice/BGvkKFjD">water ice</a> subjects the interior to intense pressures, causing the container to explode with great force.
Solids' properties on a macroscopic scale can also depend on whether it is contiguous or not. Contiguous (non-aggregate) solids are characterized by <a href="/facts/Structural_rigidity/QN30Aq69">structural rigidity</a> (as in <a href="/facts/Rigid_body/THezBlq2">rigid bodies</a>) and strong resistance to applied forces. For solids aggregates (e.g. gravel, sand, dust on lunar surface), solid particles can easily slip past one another, though changes of individual particles (<a href="/facts/Quartz/4n86tE2G">quartz</a> particles for sand) will still be greatly hindered. This leads to a perceived softness and ease of compression by operators. An illustrating example is the non-firmness of coastal sandand of the lunar regolith.
The branch of <a href="/facts/Physics/a7aH2y08">physics</a> that deals with solids is called <a href="/facts/Solid-state_physics/Cmc6hvyR">solid-state physics</a>, and is a major branch of <a href="/facts/Condensed_matter_physics/EBVI5nmL">condensed matter physics</a> (which includes liquids). <a href="/facts/Materials_science/N5HrXRYW">Materials science</a>, also one of its numerous branches, is primarily concerned with the way in which a solid's composition and its properties are intertwined.

Solid open-in-new

Solid