sensorial-concept-Mcs (mtrlSysMols)

McsHitp-creation:: {2020-04-02},

overview of mtrlSysMols

* McsEngl.filMcsMtrlSysMols.last.html!⇒mtrlSysMols,
* McsEngl.dirNtr/filMcsMtrlSysMols.last.html!⇒mtrlSysMols,
* McsEngl.material.006-system-of-molecules!⇒mtrlSysMols,
* McsEngl.material.system-of-molecules!⇒mtrlSysMols,
* McsEngl.mtrlSysMols,
* McsEngl.mtrlSysMls!⇒mtrlSysMols,
* McsEngl.mtrlSysMolecules!⇒mtrlSysMols,
* McsEngl.mtrlSysMols'(material.system-of-molecules)!⇒mtrlSysMols,
* McsEngl.sysMols-material!⇒mtrlSysMols,
* McsEngl.sysMolecules!⇒mtrlSysMols,
* McsEngl.system-of-molecules!⇒mtrlSysMols,

· mtrlSysMols is ANY system of molecules or system of atoms if there is no molecules BUT not to the-level of cellOgm.

01_molecule of mtrlSysMols

* McsEngl.mtrlSysMols'01_molecule,
* McsEngl.mtrlSysMols'att001-molecule,
* McsEngl.mtrlSysMols'molecule-att001,
* McsEngl.molecule-of-mtrlSysMols-att001,

· a-moleculeMtrl of a-mtrlSysMols.

02_atom of mtrlSysMols

* McsEngl.mtrlSysMols'02_atom,
* McsEngl.mtrlSysMols'att002-atom,
* McsEngl.mtrlSysMols'atom-att002,
* McsEngl.atom-of-mtrlSysMols-att002,


03_intermolecular-force (link) of mtrlSysMols

04_physical-property of mtrlSysMols

* McsEngl.mtrlSysMols'04_physical-property,
* McsEngl.mtrlSysMols'att004-physical-property,
* McsEngl.mtrlSysMols'physical-property,
* McsEngl.physical-property,

"A physical property is any property that is measurable, whose value describes a state of a physical system.[1] The changes in the physical properties of a system can be used to describe its changes between momentary states. Physical properties are often referred to as observables. They are not modal properties. Quantifiable physical property is called physical quantity.
Physical properties are often characterized as intensive and extensive properties. An intensive property does not depend on the size or extent of the system, nor on the amount of matter in the object, while an extensive property shows an additive relationship. These classifications are in general only valid in cases when smaller subdivisions of the sample do not interact in some physical or chemical process when combined.
Properties may also be classified with respect to the directionality of their nature. For example, isotropic properties do not change with the direction of observation, and anisotropic properties do have spatial variance.
It may be difficult to determine whether a given property is a material property or not. Color, for example, can be seen and measured; however, what one perceives as color is really an interpretation of the reflective properties of a surface and the light used to illuminate it. In this sense, many ostensibly physical properties are called supervenient. A supervenient property is one which is actual, but is secondary to some underlying reality. This is similar to the way in which objects are supervenient on atomic structure. A cup might have the physical properties of mass, shape, color, temperature, etc., but these properties are supervenient on the underlying atomic structure, which may in turn be supervenient on an underlying quantum structure.
Physical properties are contrasted with chemical properties which determine the way a material behaves in a chemical reaction."

GENERIC-SPECIFIC-TREE of physical-property

* McsEngl.physical-property'generic-specific-tree,

GENERIC-TREE of physical-property

* attribute-of-mtrlSysMols,

* ,

· :
* ,

* ,

SPECIFIC-TREE of physical-property

* generic-property-(quantity),
* genericNo-(quality),
* electrical-property,
* mechanical-property,
* optical-property,
* intensive-(eg temperature),
* extensive-(eg mass),
* space,
* shape,
* weight,
* absorption-(physical),
* absorption-(electromagnetic),
* albedo,
* angular-momentum,
* area,
* brittleness,
* boiling-point,
* capacitance,
* color,
* concentration,
* density,
* dielectric,
* ductility,
* distribution,
* efficacy,
* elasticity,
* electric-charge,
* electrical-conductivity,
* electrical-impedance,
* electric-field,
* electric-potential,
* emission,
* flow-rate-(mass),
* flow-rate-(volume),
* fluidity,
* frequency,
* hardness,
* inductance,
* Intrinsic-impedance,
* intensity,
* irradiance,
* length,
* location,
* luminance,
* luminescence,
* luster,
* malleability,
* magnetic-field,
* magnetic-flux,
* mass,
* melting-point,
* moment,
* momentum,
* opacity,
* permeability,
* permittivity,
* plasticity,
* pressure,
* radiance,
* resistivity,
* reflectivity,
* refractive-index,
* spin,
* solubility,
* specific-heat,
* strength,
* stiffness,
* temperature,
* tension,
* thermal-conductivity-(and-resistance),
* velocity,
* viscosity,
* volume,
* wave-impedance,

05_chemical-property of mtrlSysMols

* McsEngl.mtrlSysMols'05_chemical-property,
* McsEngl.mtrlSysMols'att005-chemical-property,
* McsEngl.mtrlSysMols'chemical-property-att005,

· as material, has chemical-properties.


trivial-name of mtrlSysMols

* McsEngl.mtrlSysMols'trivial-name,
* McsEngl.mtrlSysMols'att006-trivial-name,
* McsEngl.trivial-name--of-mtrlSysMols,

"In chemistry, a trivial name is a nonsystematic name for a chemical substance. That is, the name is not recognized according to the rules of any formal system of chemical nomenclature such as IUPAC inorganic or IUPAC organic nomenclature. A trivial name is not a formal name and is usually a common name.
Generally, trivial names are not useful in describing the essential properties of the thing being named. Properties such as the molecular structure of a chemical compound are not indicated. And, in some cases, trivial names can be ambiguous or will carry different meanings in different industries or in different geographic regions. (For example, a trivial name such as white metal can mean various things.) On the other hand, systematic names can be so convoluted and difficult to parse that their trivial names are preferred. As a result, a limited number of trivial chemical names are retained names, an accepted part of the nomenclature.
Trivial names often arise in the common language; they may come from historic usages in, for example, alchemy. Many trivial names pre-date the institution of formal naming conventions. Names can be based on a property of the chemical, including appearance (color, taste or smell), consistency, and crystal structure; a place where it was found or where the discoverer comes from; the name of a scientist; a mythological figure; an astronomical body; the shape of the molecule; and even fictional figures. All elements that have been isolated have trivial names."

systematic-name of mtrlSysMols

* McsEngl.mtrlSysMols'systematic-name,
* McsEngl.mtrlSysMols'att007-systematic-name,
* McsEngl.IUPAC-name--of-mtrlSysMols,
* McsEngl.systematic-name--of-mtrlSysMols,

"Systematic names (or IUPAC names) derive from the standard IUPAC Rules for the Nomenclature of Organic Chemistry, published in 1979,[15] along with a recommendation published specifically for lipids in 1977.[16] Carbon atom numbering begins from the carboxylic end of the molecule backbone. Double bonds are labelled with cis-/trans- notation or E-/Z- notation, where appropriate. This notation is generally more verbose than common nomenclature, but has the advantage of being more technically clear and descriptive."

Infrsc of mtrlSysMols

* McsEngl.mtrlSysMols'Infrsc,


structure of mtrlSysMols

* McsEngl.mtrlSysMols'structure,


DOING of mtrlSysMols

* McsEngl.mtrlSysMols'doing,


EVOLUTING of mtrlSysMols

* McsEngl.mtrlSysMols'evoluting,

=== McsHitp-creation:
· creation of current concept.

WHOLE-PART-TREE of mtrlSysMols

* McsEngl.mtrlSysMols'whole-part-tree,

* ... Sympan.



* McsEngl.mtrlSysMols'generic-specific-tree,

* ,
* ... entity.

* chemical,
* material-object,
* material-substance,
* mixture,

mtrlSysMols.organism-001 (link)

mtrlSysMols.human-002 (link)


* McsEngl.mtrlSysMols.003-solid!⇒solid,
* McsEngl.mtrlSysMols.solid-003!⇒solid,
* McsEngl.solid--sysMols-material,

"Solid is one of the four fundamental states of matter (the others being liquid, gas, and plasma). The atoms in a solid are closely packed together and contain the least amount of kinetic energy. A solid is characterized by structural rigidity and resistance to a force applied to the surface. Unlike a liquid, a solid object does not flow to take on the shape of its container, nor does it expand to fill the entire available volume like a gas. The atoms in a solid are 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). Solids cannot be compressed with little pressure whereas gases can be compressed with little pressure because the molecules in a gas are loosely packed.
The branch of physics that deals with solids is called solid-state physics, and is the main branch of condensed matter physics (which also includes liquids). Materials science is primarily concerned with the physical and chemical properties of solids. Solid-state chemistry is especially concerned with the synthesis of novel materials, as well as the science of identification and chemical composition."

* system-of-molecules,
* material-object,


* McsEngl.mtrlSysMols.012-fluid!⇒mtrlFluid,
* McsEngl.mtrlSysMols.fluid-012!⇒mtrlFluid,
* McsEngl.mtrlFluid,
* McsEngl.mtrlSysMols.solidNo-012!⇒mtrlFluid,
* McsEngl.fluid-mtrlSysMols-012!⇒mtrlFluid,
====== langoGreek:
* McsElln.ρευστό!=mtrlFluid,

"In physics, a fluid is a substance that continually deforms (flows) under an applied shear stress, or external force. Fluids are a phase of matter and include liquids, gases and plasmas. They are substances with zero shear modulus, or, in simpler terms, substances which cannot resist any shear force applied to them.
Although the term "fluid" includes both the liquid and gas phases, in common usage, "fluid" is often used as a synonym for "liquid", with no implication that gas could also be present. This colloquial usage of the term is also common in medicine and in nutrition ("take plenty of fluids").
Liquids form a free surface (that is, a surface not created by the container) while gases do not. Viscoelastic fluids like Silly Putty appear to behave similar to a solid when a sudden force is applied. Also substances with a very high viscosity such as pitch appear to behave like a solid (see pitch drop experiment)."


* McsEngl.mtrlSysMols.004-liquid!⇒fluidLiquid,
* McsEngl.mtrlSysMols.liquid-004!⇒fluidLiquid,
* McsEngl.fluidLiquid,
* McsEngl.mtrlFluid.liquid!⇒fluidLiquid,
* McsEngl.liquid!⇒fluidLiquid,
* McsEngl.liquid--sysMols-material!⇒fluidLiquid,
====== langoGreek:
* McsElln.υγρό!=fluidLiquid,

"A liquid is a nearly incompressible fluid that conforms to the shape of its container but retains a (nearly) constant volume independent of pressure. As such, it is one of the four fundamental states of matter (the others being solid, gas, and plasma), and is the only state with a definite volume but no fixed shape. A liquid is made up of tiny vibrating particles of matter, such as atoms, held together by intermolecular bonds. Like a gas, a liquid is able to flow and take the shape of a container. Most liquids resist compression, although others can be compressed. Unlike a gas, a liquid does not disperse to fill every space of a container, and maintains a fairly constant density. A distinctive property of the liquid state is surface tension, leading to wetting phenomena. Water is, by far, the most common liquid on Earth.
The density of a liquid is usually close to that of a solid, and much higher than in a gas. Therefore, liquid and solid are both termed condensed matter. On the other hand, as liquids and gases share the ability to flow, they are both called fluids. Although liquid water is abundant on Earth, this state of matter is actually the least common in the known universe, because liquids require a relatively narrow temperature/pressure range to exist. Most known matter in the universe is in gaseous form (with traces of detectable solid matter) as interstellar clouds or in plasma from within stars."


* McsEngl.mtrlSysMols.005-gas!⇒fluidGas,
* McsEngl.mtrlSysMols.gas-005!⇒fluidGas,
* McsEngl.fluidGas,
* McsEngl.gas!⇒fluidGas,
* McsEngl.mtrlFluid.gas!⇒fluidGas,
====== langoGreek:
* McsElln.αέριο!=fluidGas,

"Gas is one of the four fundamental states of matter (the others being solid, liquid, and plasma). A pure gas may be made up of individual atoms (e.g. a noble gas like neon), elemental molecules made from one type of atom (e.g. oxygen), or compound molecules made from a variety of atoms (e.g. carbon dioxide). A gas mixture, such as air, contains a variety of pure gases. What distinguishes a gas from liquids and solids is the vast separation of the individual gas particles. This separation usually makes a colorless gas invisible to the human observer. The interaction of gas particles in the presence of electric and gravitational fields are considered[by whom?] negligible, as indicated by the constant velocity vectors in the image.
The gaseous state of matter occurs between the liquid and plasma states,[1] the latter of which provides the upper temperature boundary for gases. Bounding the lower end of the temperature scale lie degenerative quantum gases[2] which are gaining increasing attention.[3] High-density atomic gases super-cooled to very low temperatures are classified by their statistical behavior as either Bose gases or Fermi gases. For a comprehensive listing of these exotic states of matter see list of states of matter."


* McsEngl.mtrlSysMols.006-plasma!⇒fluidPlasma,
* McsEngl.mtrlSysMols.plasma-006!⇒fluidPlasma,
* McsEngl.fluidPlasma,
* McsEngl.mtrlFluid.plasma!⇒fluidPlasma,
* McsEngl.plasma!⇒fluidPlasma,
* McsEngl.plasma--sysMols-material!⇒fluidPlasma,

"Plasma (from Ancient Greek πλάσμα​, meaning 'moldable substance'[1]) is one of the four fundamental states of matter, and was first described by chemist Irving Langmuir[2] in the 1920s.[3] It consists of a gas of ions – atoms which have some of their orbital electrons removed – and free electrons. Plasma can be artificially generated by heating a neutral gas or subjecting it to a strong electromagnetic field to the point where an ionized gaseous substance becomes increasingly electrically conductive. The resulting charged ions and electrons become influenced by long-range electromagnetic fields, making the plasma dynamics more sensitive to these fields than a neutral gas.[4]
Plasma and ionized gases have properties and display behaviours unlike those of the other states, and the transition between them is mostly a matter of nomenclature[2] and subject to interpretation.[5] Based on the temperature and density of the environment that contains a plasma, partially ionized or fully ionized forms of plasma may be produced. Neon signs and lightning are examples of partially ionized plasmas.[6] The Earth's ionosphere is a plasma and the magnetosphere contains plasma in the Earth's surrounding space environment. The interior of the Sun is an example of fully ionized plasma,[7] along with the solar corona[8] and stars.[9]
Positive charges in ions are achieved by stripping away electrons orbiting the atomic nuclei, where the total number of electrons removed is related to either increasing temperature or the local density of other ionized matter. This also can be accompanied by the dissociation of molecular bonds,[10] though this process is distinctly different from chemical processes of ion interactions in liquids or the behaviour of shared ions in metals. The response of plasma to electromagnetic fields is used in many modern technological devices, such as plasma televisions or plasma etching.[11]
Plasma may be the most abundant form of ordinary matter in the universe,[12] although this hypothesis is currently tentative based on the existence and unknown properties of dark matter. Plasma is mostly associated with stars, extending to the rarefied intracluster medium and possibly the intergalactic regions.[13]"


* McsEngl.mtrlSysMols.007-Uom,
* McsEngl.mtrlSysMols.Uom-007,

· a-unit-of-measuremnt for mtrlSysMols.


* McsEngl.mtrlSysMols.Uom.IU,
* McsEngl.IU-international-unit,

"In pharmacology, the international unit is a unit of measurement for the amount of a substance; the mass or volume that constitutes one international unit varies based on which substance is being measured, and the variance is based on the biological activity or effect, for the purpose of easier comparison across substances. International units are used to quantify vitamins, hormones, some medications, vaccines, blood products, and similar biologically active substances.
The name international unit has often been capitalized (in English and other languages), although major English-language dictionaries treat it as a common noun and thus use lower case. The name has several accepted abbreviations. It is usually abbreviated as IU in English, and UI in Romance languages (for example Spanish unidad internacional, French unité internationale, Italian unità internazionale, Romanian unitate internațională), IE in several Germanic languages (for example German internationale Einheit, Dutch internationale eenheid) or as other forms (for example Russian МЕ, международная единица [mezhdunarodnaya yedinitsa], Hungarian NE, nemzetközi egység). In order to remove the possibility of having the letter "I" confused with the digit "1", some hospitals have it as a stated policy to omit the "I", that is, to only use U or E when talking and writing about dosages, while other hospitals require the word "units" (or words "international units") to be written out entirely.[1] (For example, "three international units per litre" may be abbreviated "3 U/l". The fact that in the SI - Système International - convention the abbreviation for 'litre' or 'litres' is lower case 'l' introduces another potential source of confusion in many fonts between the letters "I" and 'l' and the digit "1").
Many biological agents exist in different forms or preparations (e.g. vitamin A in the form of retinol or beta-carotene). The goal of the IU is to be able to compare these, so that different forms or preparations with the same biological effect will contain the same number of IUs. To do so, the WHO Expert Committee on Biological Standardization provides a reference preparation of the agent, arbitrarily sets the number of IUs contained in that preparation, and specifies a biological procedure to compare other preparations of the same agent to the reference preparation. Since the number of IUs contained in a new substance is arbitrarily set, there is no equivalence between IU measurements of different biological agents. For instance, one IU of vitamin E cannot be equated with one IU of vitamin A in any way, including mass or efficacy.
Despite its name, IU is not part of the International System of Units used in physics and chemistry. The IU should not be confused with the enzyme unit, also known as the international unit of enzyme activity and abbreviated as U.
Mass equivalents of 1 IU
For some substances, the precise mass equivalent of one IU has been changed. When that happens, the former IU mass for that substance is officially abandoned in favor of a newly established mass. The unit count will often still remain in use.[clarify] Such a change has happened with the immunoassay standards for prolactin: as one batch of standard (84/500; 53 mIU ≈ 2.5 μg) was running out of stock, a new standard (83/573; 67 mIU ≈ 3.2 μg) was calibrated against the old one (as 67.2 mIU) and replaced the former.[6]
* Vitamin A: 1 IU is the biological equivalent of 0.3 μg retinol, or of 0.6 μg beta-carotene[7][8][a]
* Vitamin C: 1 IU is 50 μg L-ascorbic acid[citation needed]
* Vitamin D: The biological activity of 40 IU is equal to 1 μg[9]
* Vitamin E: 1 IU is the biological equivalent of about 0.667 mg d-alpha-tocopherol (2/3 mg exactly), or of 0.90 mg of dl-alpha-tocopherol[10]
* Insulin: 1 IU is equivalent to 0.0347 mg of human insulin (28.8 IU/mg)[11][12]
* Oxytocin: 1 IU is equivalent to 1.68 μg of pure peptide[13]"


* McsEngl.mtrlSysMols.008-substance!⇒mtrlSubstance,
* McsEngl.mtrlSysMols.substance-008!⇒mtrlSubstance,
* McsEngl.mtrlSubstance,
* McsEngl.bodySbtc!⇒mtrlSubstance,
* McsEngl.material-substance!⇒mtrlSubstance,
* McsEngl.substance!⇒mtrlSubstance,
====== langoGreek:
* McsElln.ουσία!=mtrlSubstance,

"chemical substance
Matter of constant composition best characterized by the entities (molecules, formula units, atoms) it is composed of. Physical properties such as density, refractive index, electric conductivity, melting point etc. characterize the chemical substance.
Source: Physical Chemistry Division, unpublished [Terms]
Cite as: IUPAC. Compendium of Chemical Terminology, 2nd ed. (the "Gold Book"). Compiled by A. D. McNaught and A. Wilkinson. Blackwell Scientific Publications, Oxford (1997). Online version (2019-) created by S. J. Chalk. ISBN 0-9678550-9-8."
· a-material-body without shape or not interesting in its shape, is a-substance.
· a-liquid, a-gas or a-powder is always a-substance.
· a-rock from its shape view, is an-object.
· a-rock from its matter view, is a-substance.
"(n) shape, form (the spatial arrangement of something as distinct from its substance) "geometry is the mathematical science of shape""


* McsEngl.bodyMtrl.substanceNo!⇒mtrlObject,
* McsEngl.bodyObjt!⇒mtrlObject,
* McsEngl.mtrlSysMols.009-substanceNo!⇒mtrlObject,
* McsEngl.mtrlSysMols.substanceNo-009!⇒mtrlObject,
* McsEngl.mtrlObject,
* McsEngl.material-object!⇒mtrlObject,
* McsEngl.object.material!⇒mtrlObject,
====== langoGreek:
* McsElln.υλικό-αντικείμενο!=mtrlObject,

· object is a-material-body with shape.
· a-rock from its shape view, is an-object.
· a-rock from its matter view, is a-substance.

shape of mtrlObject

* McsEngl.mtrlObject'form,
* McsEngl.mtrlObject'shape,
* McsEngl.shape-of-mtrlObject,

"(n) shape, form (the spatial arrangement of something as distinct from its substance) "geometry is the mathematical science of shape""
the external form, contours, or outline of someone or something.
"she liked the shape of his nose"
Similar: form, appearance, configuration, formation, structure, figure, build, physique, body, contours, lines, outline, silhouette, profile, design, format, cut, pattern, mould,
[Google dict]


* McsEngl.mtrlSysMols.010-chemical!⇒mtrlChemical,
* McsEngl.mtrlSysMols.chemical-010!⇒mtrlChemical,
* McsEngl.bodyMtrChm!⇒mtrlChemical,
* McsEngl.bodyMtrl.pure!⇒mtrlChemical,
* McsEngl.chm!⇒mtrlChemical,
* McsEngl.chemical!⇒mtrlChemical,
* McsEngl.chemical-body!⇒mtrlChemical,
* McsEngl.chemical-substance!⇒mtrlChemical,
* McsEngl.materialChemical!⇒mtrlChemical,
* McsEngl.mtrlChemical, {2020-05-14},
* McsEngl.pure-bodyMtrl!⇒mtrlChemical,
* McsEngl.pure-material-body!⇒mtrlChemical,
====== langoSinago:
* McsSngo.kemo!=mtrlChemical,
====== langoGreek:
* McsElln.χημική-ουσία!=mtrlChemical,

· chemical-body or chemical I call an-elementrary-chemical, a-compound-chemical, and an-alloy. {2020-04-06},
· chemical-body or chemical I call a-chemical-elementrary or a-chemical-compound. {2020-04-03},
· chemical-body or chemical is a-material-atom, a-chemical-elementrary and a-chemical-compound. {2020-03-31},
chemical substance
Matter of constant composition best characterized by the entities (molecules, formula units, atoms) it is composed of. Physical properties such as density, refractive index, electric conductivity, melting point etc. characterize the chemical substance.
Source: Physical Chemistry Division, unpublished [Terms]
Cite as: IUPAC. Compendium of Chemical Terminology, 2nd ed. (the "Gold Book"). Compiled by A. D. McNaught and A. Wilkinson. Blackwell Scientific Publications, Oxford (1997). Online version (2019-) created by S. J. Chalk. ISBN 0-9678550-9-8.
"A chemical substance is a form of matter having constant chemical composition and characteristic properties.[1][2] Some references add that chemical substance cannot be separated into its constituent elements by physical separation methods, i.e., without breaking chemical bonds.[3] Chemical substances can be simple substances[4], chemical compounds, or alloys. Chemical elements may or may not be included in the definition, depending on expert viewpoint.[4]"
"In chemistry, a chemical substance is a form of matter that has constant chemical composition and characteristic properties.[1] It cannot be separated into components by physical separation methods, i.e. without breaking chemical bonds. They can be solids, liquids or gases.
Chemical substances are often called 'pure' to set them apart from mixtures. A common example of a chemical substance is pure water; it has the same properties and the same ratio of hydrogen to oxygen whether it is isolated from a river or made in a laboratory. Other chemical substances commonly encountered in pure form are diamond (carbon), gold, table salt (sodium chloride) and refined sugar (sucrose). However, simple or seemingly pure substances found in nature can in fact be mixtures of chemical substances. For example, tap water may contain small amounts of dissolved sodium chloride and compounds containing iron, calcium and many other chemical substances.
Chemical substances exist as solids, liquids, gases, or plasma and may change between these phases of matter with changes in temperature or pressure. Chemical reactions convert one chemical substance into another.
Forms of energy, such as light and heat, are not considered to be matter, and thus they are not "substances" in this regard."

01_molecule of mtrlChemical

* McsEngl.mtrlChemical'01_molecule,
* McsEngl.mtrlChemical'att001-molecule,
* McsEngl.mtrlChemical'molecule-att001,
* McsEngl.molecule-of-chemical-att001,


02_atom of mtrlChemical

* McsEngl.mtrlChemical'02_atom,
* McsEngl.mtrlChemical'att002-atom,
* McsEngl.mtrlChemical'atom-att002,
* McsEngl.atom-of-chemical-att002,


03_intermolecular-bond of mtrlChemical

* McsEngl.mtrlChemical'03_intermolecular-bond,
* McsEngl.mtrlChemical'att003-intermolecular-bond,
* McsEngl.mtrlChemical'intermolecular-bond-att003,
* McsEngl.intermolecular-bond-of-chemical,


04_physical-property of mtrlChemical

* McsEngl.mtrlChemical'04_physical-property,
* McsEngl.mtrlChemical'att004-physical-property,
* McsEngl.mtrlChemical'physical-property-att004,


05_chemical-property of mtrlChemical

* McsEngl.mtrlChemical'05_chemical-property,
* McsEngl.mtrlChemical'att05-chemical-property,
* McsEngl.mtrlChemical'chemical-property-att05,


06_chemical-reaction of mtrlChemical

* McsEngl.mtrlChemical'06_chemical-reaction,
* McsEngl.mtrlChemical'att005-chemical-reaction,
* McsEngl.mtrlChemical'chemical-reaction-att005,



* McsEngl.mtrlChemical'generic-specific-tree,

GENERIC-TREE of mtrlChemical

* mtrlSysMols,

* ,

· :
* ,

* ,

SPECIFIC-TREE of mtrlChemical

* chemical-compound,
* chemical-element,


* McsEngl.mtrlSysMols.011-chemicalNo!⇒mtrlChemicalNo,
* McsEngl.mtrlSysMols.chemicalNo-011!⇒mtrlChemicalNo,
* McsEngl.chemicalNo!⇒mtrlChemicalNo,
* McsEngl.mixture!⇒mtrlChemicalNo,
* McsEngl.mtrlChemicalNo, {2020-05-14},
* McsEngl.pureNo-bodyMtrl!⇒mtrlChemicalNo,
====== langoSinago:
* McsSngo.kemoUgo!=mtrlChemicalNo,

"In chemistry, a mixture is a material made up of two or more different substances which are physically combined.[1]A mixture is the physical combination of two or more substances in which the identities are retained and are mixed in the form of solutions, suspensions and colloids.[2][3]
Mixtures are one product of mechanically blending or mixing chemical substances such as elements and compounds, without chemical bonding or other chemical change, so that each ingredient substance retains its own chemical properties and makeup.[4] Despite the fact that there are no chemical changes to its constituents, the physical properties of a mixture, such as its melting point, may differ from those of the components. Some mixtures can be separated into their components by using physical (mechanical or thermal) means. Azeotropes are one kind of mixture that usually poses considerable difficulties regarding the separation processes required to obtain their constituents (physical or chemical processes or, even a blend of them).[5][6][7]"


* McsEngl.mtrlSysMols.013-hydrocarbon,
* McsEngl.mtrlSysMols.hydrocarbon-013,
====== langoGreek:
* McsElln.υδρογονάνθρακας!=hydrocarbon,

"In organic chemistry, a hydrocarbon is an organic compound consisting entirely of hydrogen and carbon.[1]:620 Hydrocarbons are examples of group 14 hydrides. Hydrocarbons from which one hydrogen atom has been removed are functional groups called hydrocarbyls.[2] Because carbon has 4 electrons in its outermost shell (and because each covalent bond requires a donation of 1 electron, per atom, to the bond) carbon has exactly four bonds to make, and is only stable if all 4 of these bonds are used.
Aromatic hydrocarbons (arenes), alkanes, cycloalkanes and alkyne-based compounds are different types of hydrocarbons.
Most hydrocarbons found on Earth naturally occur in petroleum, where decomposed organic matter provides an abundance of carbon and hydrogen which, when bonded, can catenate to form seemingly limitless chains.[3][4]"


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