Information about Immiscibility
Miscibility is a term in chemistry that refers to the property of liquids to mix in all proportions, forming a homogeneous solution. In principle, the term applies also to other phases (solids and gases), but the main focus on the solubility of one liquid in another. For example, water and ethanol are miscible in all proportions.
By contrast, substances are said to be immiscible if in any proportion, they do not form a homogeneous phase. For example, diethyl ether is fairly soluble in water, but these two solvents are not miscible since they are not soluble in all proportions.
In organic compounds, the weight percent of hydrocarbon chain often determines the compounds miscibility with water. For example, among the alcohols, ethanol has two carbon atoms and is miscible with water, whereas octanol with a C8H17 substituent is not. Octanol's immiscibility leads it to be used as a standard for partition equilibria. This is also the case with lipids; the very long carbon chains of lipids cause them to almost always be immiscible with water. Analogous situations occur for other functional groups. Acetic acid is miscible with water, whereas valeric acid (C4H9CO2H) is not. Simple aldehydes and ketones tend to be miscible with water, since a hydrogen bond can form between the hydrogen atom of a water molecule and the unbonded (lone) pair of electrons on the carbonyl oxygen atom.
Immiscible metals are unable to form alloys. Typically, a mixture will be possible in the molten state, but upon freezing the metals separate into layers. This property allows solid precipitates to be formed by rapidly freezing a molten mixture of immiscible metals. One example of immiscibility in metals is copper and cobalt, where rapid freezing to form solid precipitates has been used to create granular GMR materials.
Miscibility is partly a function of entropy, and so is seen more commonly in states of matter that are more entropic. Gases mix quite readily, but solids only rarely display miscibility. Two useful exceptions to this rule are solid solutions of copper with nickel (the cupronickel used in coins and specialty plumbing), and of silicon with germanium (used in electronics). Substances with extremely low configurational entropy, especially polymers, are unlikely to be miscible in one another even in the liquid state. Perdeuteropolyethylene is immiscible in polyethylene.
By contrast, substances are said to be immiscible if in any proportion, they do not form a homogeneous phase. For example, diethyl ether is fairly soluble in water, but these two solvents are not miscible since they are not soluble in all proportions.
In organic compounds, the weight percent of hydrocarbon chain often determines the compounds miscibility with water. For example, among the alcohols, ethanol has two carbon atoms and is miscible with water, whereas octanol with a C8H17 substituent is not. Octanol's immiscibility leads it to be used as a standard for partition equilibria. This is also the case with lipids; the very long carbon chains of lipids cause them to almost always be immiscible with water. Analogous situations occur for other functional groups. Acetic acid is miscible with water, whereas valeric acid (C4H9CO2H) is not. Simple aldehydes and ketones tend to be miscible with water, since a hydrogen bond can form between the hydrogen atom of a water molecule and the unbonded (lone) pair of electrons on the carbonyl oxygen atom.
Immiscible metals are unable to form alloys. Typically, a mixture will be possible in the molten state, but upon freezing the metals separate into layers. This property allows solid precipitates to be formed by rapidly freezing a molten mixture of immiscible metals. One example of immiscibility in metals is copper and cobalt, where rapid freezing to form solid precipitates has been used to create granular GMR materials.
Miscibility is partly a function of entropy, and so is seen more commonly in states of matter that are more entropic. Gases mix quite readily, but solids only rarely display miscibility. Two useful exceptions to this rule are solid solutions of copper with nickel (the cupronickel used in coins and specialty plumbing), and of silicon with germanium (used in electronics). Substances with extremely low configurational entropy, especially polymers, are unlikely to be miscible in one another even in the liquid state. Perdeuteropolyethylene is immiscible in polyethylene.
See also
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Liquid is one of the four principal states of matter. A liquid is a fluid that can freely form a distinct surface at the boundaries of its bulk material.
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Characteristics
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Water is a common chemical substance that is essential to all known forms of life.[1] In typical usage, water refers only to its liquid form or state, but the substance also has a solid state, ice, and a gaseous state, water vapor.
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Ethanol, also known as ethyl alcohol, drinking alcohol or grain alcohol, is a flammable, colorless, slightly toxic chemical compound, and is best known as the alcohol found in alcoholic beverages.
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Diethyl ether, also known as ether and ethoxyethane, is a clear, colorless, and highly flammable liquid with a low boiling point and a characteristic smell. It is the most common member of a class of chemical compounds known generically as ethers.
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organic compounds]] An organic compound is any member of a large class of chemical compounds whose molecules contain carbon; for historical reasons discussed below, a few types of compounds such as carbonates, carbon oxides and cyanides, as well as elemental carbon are
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hydrocarbon is an organic compound consisting entirely of hydrogen and carbon. With relation to chemical terminology, aromatic hydrocarbons or arenes, alkanes, alkenes and alkyne-based compounds composed entirely of carbon or hydrogen are referred to as "Pure" hydrocarbons, whereas
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alcohol is any organic compound in which a hydroxyl group (-OH) is bound to a carbon atom of an alkyl or substituted alkyl group. The general formula for a simple acyclic alcohol is CnH2n+1OH.
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atom (Greek ἄτομος or átomos meaning "indivisible") is the smallest particle still characterizing a chemical element.
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Octanol is a straight chain fatty alcohol with eight carbon atoms and the molecular formula CH3(CH2)7OH. Although the term octanol
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Partition equilibrium chromatography is a type of chromatography that is typically used in GC. The stationary phase is a high boiling liquid bonded to solid surface and the mobile phase is a gas.
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Lipids can be broadly defined as any fat-soluble (hydrophobic), naturally-occurring molecules. The term is more-specifically used to refer to fatty-acids and their derivatives (including tri-, di-, and monoglycerides and phospholipids) as well as other fat-soluble sterol-containing
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aldehyde is an organic compound containing a terminal carbonyl group. This functional group, which consists of a carbon atom which is bonded to a hydrogen atom and double-bonded to an oxygen atom (chemical formula O=CH-), is called the aldehyde group.
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A ketone (pronounced as key tone) is either the functional group characterized by a carbonyl group (O=C) linked to two other carbon atoms or a chemical compound that contains this functional group.
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hydrogen bond is a special type of dipole-dipole bond that exists between an electronegative atom and a hydrogen atom bonded to another electronegative atom. This type of bond always involves a hydrogen atom, thus the name.
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carbonyl group is a functional group composed of a carbon atom double-bonded to an oxygen atom : C=O.
The term carbonyl can also refer to carbon monoxide as a ligand in an inorganic or organometallic complex (a metal carbonyl, e.g.
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The term carbonyl can also refer to carbon monoxide as a ligand in an inorganic or organometallic complex (a metal carbonyl, e.g.
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2, −1
(neutral oxide)
Electronegativity 3.44 (Pauling scale)
Ionization energies
(more) 1st: 1313.9 kJmol−1
2nd: 3388.3 kJmol−1
3rd: 5300.5 kJmol−1
Atomic radius 60 pm
Atomic radius (calc.
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(neutral oxide)
Electronegativity 3.44 (Pauling scale)
Ionization energies
(more) 1st: 1313.9 kJmol−1
2nd: 3388.3 kJmol−1
3rd: 5300.5 kJmol−1
Atomic radius 60 pm
Atomic radius (calc.
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2, 1
(mildly basic oxide)
Electronegativity 1.90 (Pauling scale)
Ionization energies
(more) 1st: 745.5 kJmol−1
2nd: 1957.9 kJmol−1
3rd: 3666 kJmol−1
Atomic radius 135 pm
Atomic radius (calc.
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(mildly basic oxide)
Electronegativity 1.90 (Pauling scale)
Ionization energies
(more) 1st: 745.5 kJmol−1
2nd: 1957.9 kJmol−1
3rd: 3666 kJmol−1
Atomic radius 135 pm
Atomic radius (calc.
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2, 3
(amphoteric oxide)
Electronegativity 1.88 (Pauling scale)
Ionization energies
(more) 1st: 760.4 kJmol−1
2nd: 1648 kJmol−1
3rd: 3232 kJmol−1
Atomic radius 135 pm
Atomic radius (calc.
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(amphoteric oxide)
Electronegativity 1.88 (Pauling scale)
Ionization energies
(more) 1st: 760.4 kJmol−1
2nd: 1648 kJmol−1
3rd: 3232 kJmol−1
Atomic radius 135 pm
Atomic radius (calc.
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Ice melting - a classic example of entropy increasing[1] described in 1862 by Rudolf Clausius as an increase in the disgregation of the molecules of the body of ice.
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2, 3
(mildly basic oxide)
Electronegativity 1.91 (Pauling scale)
Ionization energies
(more) 1st: 737.1 kJmol−1
2nd: 1753.0 kJmol−1
3rd: 3395 kJmol−1
Atomic radius 135 pm
Atomic radius (calc.
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(mildly basic oxide)
Electronegativity 1.91 (Pauling scale)
Ionization energies
(more) 1st: 737.1 kJmol−1
2nd: 1753.0 kJmol−1
3rd: 3395 kJmol−1
Atomic radius 135 pm
Atomic radius (calc.
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Cupronickel is an alloy of copper, nickel and strengthening impurities, such as iron and manganese. Cupronickel does not corrode in seawater, because its electrode potential is adjusted to be neutral with regard to seawater.
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Silicon (IPA: /ˈsɪlɪkən/ or /ˈsɪlɪˌkɑn/, Latin: silicium
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Germanium (IPA: /dʒə(r)ˈmeɪniəm/) is a chemical element in the periodic table that has the symbol Ge and atomic number 32.
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emulsion is a mixture of two immiscible (unblendable) substances. One substance (the dispersed phase) is dispersed in the other (the continuous phase). Examples of emulsions include butter and margarine, espresso, mayonnaise, the photo-sensitive side of photographic film, and
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A multiphasic liquid, also known as a multiphasic liquid-liquid-liquid system, is a mixture consisting of more than two immiscible liquid phases. Biphasic mixtures consisting of two immiscible phases are very common and usually consist of an organic solvent and an aqueous
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A heteroazeotrope is an azeotrope where the vapour phase coexists with two liquid phases.
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Examples of heteroazeotropes
- Benzene - Water NBP 69.2 °C
- Dichloromethane - Water NBP 38.5 °C
See also
- Azeotrope
- Batch distillation
- Distillation
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