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In inorganic chemistry and materials chemistry, a ternary compound or ternary phase is a chemical compound containing three different elements.

While some ternary compounds are molecular, e.g. chloroform (HCCl3), more typically ternary phases refer to extended solids. The perovskites are a famous example.[1]

Binary phases, with only two elements, have lower degrees of complexity than ternary phases. With four elements, quaternary phases are more complex.

The number of isomers of a ternary compound provide a distinction between inorganic and organic chemistry: "In inorganic chemistry one or, at most, only a few compounds composed of any two or three elements were known, whereas in organic chemistry the situation was very different."[2]

Ternary crystalline compounds

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Sodium phosphate, Na3PO4, is a ternary compound.

An example is sodium phosphate, Na3PO4. The sodium ion has a charge of 1+ and the phosphate ion has a charge of 3–. Therefore, three sodium ions are needed to balance the charge of one phosphate ion. Another example of a ternary compound is calcium carbonate, CaCO3. In naming and writing the formulae for ternary compounds, rules are similar to binary compounds.

Classifications of ternary crystals

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According to Rustum Roy and Olaf Müller,[3] "the chemistry of the entire mineral world informs us that chemical complexity can easily be accommodated within structural simplicity." The example of zircon is cited, where various metal atoms are replaced in the same crystal structure. "The structural entity ... remains ternary in character and is able to accommodate an enormous range of chemical elements." The great variety of ternary compounds is therefore reduced to relatively few structures: "By dealing with approximately ten ternary structural groupings we can cover the most important structures of science and technology specific to the non-metallics world. It is a remarkable instance of nature's simplexity."[3]: 3, 4 

Lithium niobate is a famous ternary phase. It features three elements: Li, Nb, and O.

Letting A and B represent cations and X an anion, these ternary groupings are organized by stoichiometric types A2BX4, ABX4, and ABX3.

A ternary compound of type A2BX4 may be in the class of olivine, the spinel group, or phenakite. Examples include K2NiF4, β-K2SO4, and CaFe2O4.

One of type ABX4 may be of the class of zircon, scheelite, barite or an ordered silicon dioxide derivative.

In the ABX3 class of ternary compounds, there are the structures of perovskite (structure), calcium carbonate, pyroxenes, corundum and hexagonal ABX2 types.[3]: figure 1, page 3 

Other ternary compounds are described as crystals of types ABX2, A2B2X7, ABX5, A2BX6, and A3BX5.

Ternary semiconductors

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A particular class of ternary compounds are the ternary semiconductors, particularly within the III-V semiconductor family. In this type of semiconductor, the ternary can be considered to be an alloy of the two binary endpoints. Varying the composition between the endpoints allows both the lattice constant and the energy bandgap to be adjusted to produce the properties desired, for example, in emitting light (for example, as a LED) or absorbing light (as a photodetector or a photovoltaic cell). An example would be the semiconductor indium gallium arsenide (InxGa1−xAs), a material with band gap dependent on In/Ga ratio.

Important examples of ternary semiconductors can also be found in other semiconductor families, such as the II-VI family (e.g., Mercury cadmium telluride, Hg1−xCdxTe), or the I-II-VI2 family, with examples such as CuInSe2.

Organics

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In organic chemistry, the carbohydrates and carboxylic acids are ternary compounds with carbon, oxygen, and hydrogen. Other organic ternary compounds replace oxygen with another atom to form functional groups.

The multiplicity of ternary compounds based on {C, H, O} has been noted. For example, corresponds to more than 60 ternary compounds.[4][2]

See also

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References

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Ternary compound

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A ternary compound is a chemical compound composed of three different elements.[1] These compounds are distinct from binary compounds, which contain only two elements, and are prevalent in inorganic chemistry due to their diverse structures and applications. Ternary compounds can be ionic, molecular, or acidic in nature, with ionic forms typically consisting of a monatomic cation paired with a polyatomic anion to achieve charge balance.[2] Common examples of ternary ionic compounds include sodium nitrate (NaNO₃) and calcium sulfate (CaSO₄).[1] Ternary acids represent another key category, formed by hydrogen, oxygen, and a third element, often exhibiting strong or weak acidic properties depending on the central atom's electronegativity and bond strength.[3] Notable examples are sulfuric acid (H₂SO₄), a strong diprotic acid, and nitric acid (HNO₃).[4] Molecular ternary compounds, such as chloroform (CHCl₃), involve covalent bonds between three nonmetallic elements. Naming ternary compounds follows systematic rules: for ionic types, the cation is named first followed by the anion (e.g., ammonium chloride, NH₄Cl), while acids use prefixes like "hypo-" or "per-" based on oxygen content.[1] The study of ternary compounds is fundamental to understanding chemical bonding, reactivity, and material science, as they form the basis for many minerals, pharmaceuticals, and industrial chemicals.[5]

Fundamentals

Definition

A ternary compound is a chemical substance composed of exactly three distinct elements in its simplest formula.[6] This distinguishes it from binary compounds, which involve only two elements, and quaternary compounds, which incorporate four or more; ternary compounds occur commonly in both discrete molecular structures and extended solid-state forms, such as ionic lattices.[7] Representative examples illustrate this composition: chloroform (CHCl₃), a molecular ternary compound featuring hydrogen, carbon, and chlorine, and sodium phosphate (Na₃PO₄), an ionic ternary compound with sodium, phosphorus, and oxygen.[8] Advances in 19th-century inorganic chemistry, including analyses of salt compositions and stoichiometry, established fixed elemental ratios in chemical substances. Perovskites exemplify a prevalent crystalline structure among ternary compounds.[9]

Nomenclature and Stoichiometry

Ternary compounds follow systematic nomenclature rules established by the International Union of Pure and Applied Chemistry (IUPAC), which distinguish between ionic and covalent types based on bonding character. For ionic ternary compounds, the name begins with the cation, typically a metal ion named as the element (e.g., sodium for Na⁺), followed by the name of the polyatomic anion without a space. The anion name often ends in "-ate" or "-ite" for oxyanions, such as phosphate for PO₄³⁻. If multiple cations are present or stoichiometry requires specification, multiplicative prefixes like "di-" or "tri-" are used, and Roman numerals indicate variable oxidation states for transition metals.[10] In formula notation for ionic ternaries, subscripts denote the stoichiometric ratios needed to achieve charge neutrality, as seen in Na₃PO₄ where three Na⁺ cations balance the 3– charge of one PO₄³⁻ anion. Common generalized stoichiometries in solid-state chemistry include ABX₃ (e.g., LiNbO₃, with A = Li⁺, B = Nb⁵⁺, X = O²⁻), A₂BX₄, and ABX₄, where A and B represent distinct cations and X the anion; these reflect balanced valences, such as +1 for A and +2 for B in ABX₃ with X = –1. For non-stoichiometric ternaries, particularly in alloys or defect-containing solids, variable composition is indicated by fractional subscripts, as in InₓGa₁₋ₓAs, where x denotes the tunable indium fraction affecting properties like bandgap.[10] Covalent or molecular ternary compounds, including oxyacids and simple molecules, employ prefix-based nomenclature to specify atom counts, with the least electronegative element named first followed by prefixes (mono-, di-, tri-, etc.) and the root name of the more electronegative elements ending in "-ide." For example, POCl₃ is phosphoryl chloride, extending the binary convention to ternaries. Oxyacids like HNO₃ are traditionally named based on the central atom's oxidation state, yielding nitric acid, though systematic additive names such as trioxidonitrate(1–) for the anion are also permissible. Stoichiometry in molecular formulas uses subscripts without charge indicators unless ionized, prioritizing the order of decreasing electronegativity.[10]

Inorganic Ternary Compounds

Ionic and Molecular Types

Ionic ternary compounds consist of a single cation paired with a polyatomic anion containing two or more elements, resulting in a formula composed of three distinct elements overall.[1] A representative example is calcium carbonate, CaCO3CaCO_3, where the Ca2+Ca^{2+} cation bonds ionically with the CO32−CO_3^{2-} carbonate anion, which itself comprises carbon and oxygen.[1] These compounds exhibit charge neutrality, with the cation's positive charge balancing the anion's negative charge.[11] In contrast, molecular ternary compounds form discrete covalent molecules involving three elements, often featuring a central atom bonded to others, as seen in oxyacids.[12] Nitric acid, HNO3HNO_3, exemplifies this type, with hydrogen, nitrogen, and oxygen linked covalently; the NO3NO_3 group acts as the anionic portion in its dissociated form.[12] Such molecules typically display intramolecular covalent bonding within the polyatomic unit, distinguishing them from purely ionic structures.[12] Synthesis of these compounds often involves neutralization reactions, where a base reacts with an acid or acidic gas to form the ternary salt and water. For instance, calcium hydroxide neutralizes carbon dioxide to yield calcium carbonate:
Ca(OH)2+CO2→CaCO3+H2O Ca(OH)_2 + CO_2 \rightarrow CaCO_3 + H_2O

This process leverages the proton transfer from the acid to the base, producing the polyatomic anion in situ.[13] Precipitation methods also contribute, such as mixing solutions of soluble precursors to form an insoluble ternary salt; for example, calcium chloride and sodium carbonate react to precipitate calcium carbonate:
CaCl2+Na2CO3→CaCO3↓+2NaCl CaCl_2 + Na_2CO_3 \rightarrow CaCO_3 \downarrow + 2NaCl

These aqueous-based syntheses facilitate control over particle size and purity through reaction conditions like pH and temperature. Unique properties of ionic ternary compounds include varied solubility trends governed by ion pairing and lattice energy. Sodium nitrate, NaNO3NaNO_3, is highly soluble in water due to the weak ion-dipole interactions and low lattice energy of alkali metal salts, dissolving readily to form conductive solutions.[14] Conversely, calcium carbonate exhibits low solubility, with a solubility product constant KspK_{sp} of 3.8×10−93.8 \times 10^{-9} at 25°C, rendering it sparingly soluble and useful in applications requiring minimal dissolution.[15] For molecular ternaries like nitric acid, strong acidity arises from complete dissociation in water, yielding H+H^+ and NO3−NO_3^- ions and enabling it to protonate bases effectively.[16] This full ionization classifies HNO3HNO_3 as a strong acid, with a pKapK_a of approximately -1.3, contrasting with weaker ternary acids.[17]

Crystalline Structures and Classifications

Ternary inorganic compounds display diverse crystalline architectures that underpin their materials properties, with several prototypical structures recurring across different stoichiometries. The perovskite structure, characterized by the general formula ABX₃, consists of a framework where large A cations coordinate twelve X anions, while smaller B cations occupy octahedral sites surrounded by six X anions, often resulting in a cubic lattice that can distort to lower symmetries under certain conditions. Lithium niobate (LiNbO₃), for instance, adopts a trigonal variant of this structure (space group R3c) with a distorted lattice, where the NbO₆ octahedra tilt due to the ionic size mismatch between Li⁺ and Nb⁵⁺, contributing to its ferroelectric behavior.[18] Another prevalent motif is the spinel structure (AB₂X₄), featuring a face-centered cubic array of X anions with A cations in tetrahedral interstices and B cations in half the octahedral sites, as exemplified by oxides like ZnAl₂O₄, which exhibit close-packed anion sublattices for enhanced packing efficiency.[19] The zircon structure, common in silicates and phosphates of formula ATO₄, involves chains of edge-sharing AO₈ polyhedra linked by isolated TO₄ tetrahedra, providing a stable framework resistant to radiation damage, as observed in ZrSiO₄ where Zr⁴⁺ occupies dodecahedral sites and Si⁴⁺ tetrahedral ones.[20] Classifications of these crystalline ternary compounds often proceed by stoichiometry, grouping them into categories such as 1:1:1 (e.g., ABX₃ perovskites), 1:2:4 (e.g., AB₂X₄ spinels), or 1:1:2 (e.g., AX₂BY₂ variants akin to ordered zircon-like arrangements), alongside delineations by dominant bonding character—ionic in many oxides like NaCl-type derivatives, covalent in chalcogenides, or metallic in intermetallics. Stability within these classes is assessed via ternary phase diagrams, which map equilibrium regions under controlled temperature and composition; for example, in the Na₂O-Al₂O₃-SiO₂ system, diagrams delineate fields where spinel or perovskite phases form stably up to 1400 °C, guiding synthesis conditions to avoid metastable intermediates.[21] Such diagrams highlight how compositional deviations can induce phase transitions, with invariant points like ternary eutectics marking boundaries for compound formation. Representative examples illustrate structural polymorphism and associated properties. Sodium phosphate (Na₃PO₄) crystallizes in an orthorhombic form (space group Pnma) at ambient conditions, featuring distorted PO₄ tetrahedra coordinated by Na⁺ ions in irregular polyhedra, which confers moderate thermal stability up to decomposition around 1000 °C. Calcium carbonate (CaCO₃) demonstrates polymorphism with calcite adopting a rhombohedral structure (space group R3̄c) for thermodynamic stability at low pressures and aragonite forming an orthorhombic lattice (space group Pmcn) under higher pressures or biogenic conditions, where the latter's denser packing enhances resistance to dissolution in aqueous environments.[22] These structures often impart desirable properties, or piezoelectricity in LiNbO₃, arising from its polar space group and yielding a direct piezoelectric coefficient d₃₃ of approximately 6 pm/V, with operational stability up to its Curie temperature exceeding 1200 °C for sensor applications.[23]

Ternary Semiconductors

Ternary semiconductors are inorganic compounds composed of three elements, typically from the III-V or II-VI groups, that exhibit tunable electronic properties essential for advanced optoelectronic devices. Prominent examples include InₓGa₁₋ₓAs from the III-V family, involving indium (In), gallium (Ga), and arsenic (As), and Hg₁₋ₓCdₓTe from the II-VI family, incorporating mercury (Hg), cadmium (Cd), and tellurium (Te). These alloys allow precise control over material characteristics by varying the composition ratio x (ranging from 0 to 1), enabling bandgap engineering for specific wavelength responses.[24][25] The key property of these ternary semiconductors is their variable bandgap energy, which directly influences light absorption and emission. For InₓGa₁₋ₓAs, the direct bandgap is given by $ E_g(x) = 1.425 - 1.501x + 0.436x^2 $ eV at room temperature, transitioning from approximately 1.425 eV for GaAs (x=0) to 0.36 eV for InAs (x=1), allowing tunability across near-infrared wavelengths. Similarly, Hg₁₋ₓCdₓTe features a tunable bandgap from about 1.5 eV (CdTe, x=1) to negative values for pure HgTe, enabling mid- to long-wave infrared detection. This compositional flexibility also facilitates lattice matching to substrates like InP or GaAs, minimizing defects during epitaxial growth and enhancing device performance. These materials often adopt the zincblende crystal structure, which supports their direct bandgap nature.[24][26][27] Synthesis of ternary semiconductors for electronic applications typically involves advanced thin-film techniques to achieve high-quality layers with uniform composition. Molecular beam epitaxy (MBE) is widely used, as it enables precise control over alloy ratios in ultrahigh vacuum, producing defect-free films for both InₓGa₁₋ₓAs on InP substrates and Hg₁₋ₓCdₓTe on CdZnTe or GaAs. Chemical vapor deposition (CVD), including metalorganic variants, serves as an alternative for scalable production, particularly for infrared-sensitive layers. These methods ensure the necessary purity and thickness (often 1-10 μm) for device integration.[28][29][30] In optoelectronics, InₓGa₁₋ₓAs is pivotal for infrared detectors, where lattice-matched variants (x≈0.53) enable high-sensitivity photodiodes for telecommunications and imaging up to 1.7 μm. Hg₁₋ₓCdₓTe excels in photovoltaics, particularly for mid-wave infrared solar cells that harvest thermal radiation, achieving efficiencies suitable for space and concentrator systems. Both materials support light-emitting diodes (LEDs) with wavelength tuning via x adjustment, facilitating applications in fiber optics and sensors. Their high absorption coefficients and carrier mobilities underpin these uses, driving innovations in high-speed, low-noise devices.[31][32][33]

Organic Ternary Compounds

Characteristics and Common Elements

Organic ternary compounds are defined as molecules containing exactly three distinct elements, most commonly carbon (C) combined with hydrogen (H) and one additional element, distinguishing them from binary hydrocarbons or more complex quaternary structures.[34] This composition aligns with the broader ternary framework of three total elements but emphasizes carbon's central role in forming the molecular skeleton.[35] The most prevalent elemental combination in organic ternary compounds is C-H-O, found in a wide range of oxygenated hydrocarbons such as alcohols and ethers, which constitute a significant portion of naturally occurring and synthetic organic substances.[34] Another common trio is C-H-N, prevalent in nitrogen-containing compounds like amines and amides, essential for biological and pharmaceutical applications.[34] Less frequent but notable combinations include C-H-S in sulfur-bearing organics and C-H-halogen (where halogen denotes F, Cl, Br, or I) in halogenated derivatives, often introduced for specific reactivity or stability enhancements. Bonding in organic ternary compounds is predominantly covalent, with carbon forming strong sigma bonds to hydrogen and the third element, enabling diverse structural motifs like chains, rings, and branches.[36] Functional groups involving the third element, such as hydroxyl (-OH) in C-H-O systems or amino (-NH₂) in C-H-N systems, dictate much of the chemical reactivity and intermolecular interactions through polar covalent or hydrogen bonding capabilities.[36] These compounds exhibit properties like moderate volatility, influenced by molecular weight and intermolecular forces, with lower-molecular-weight variants boiling at temperatures suitable for distillation processes.[37] Solubility is generally high in nonpolar organic solvents due to compatible hydrophobic carbon frameworks, though polar functional groups can enhance miscibility in protic solvents like water for shorter chains.[37] The flexible carbon chain arrangements also confer potential for isomerism, arising from variations in chain branching or functional group positioning, which can lead to distinct physical and reactive profiles without altering elemental composition.[38]

Examples and Isomerism

Organic ternary compounds, composed primarily of carbon, hydrogen, and oxygen, encompass a wide range of molecules including alcohols, aldehydes, ketones, and carboxylic acids. The simplest example is methanol (CH₃OH), a primary alcohol used as a solvent and fuel additive.[39] More complex instances include acetic acid (CH₃COOH), the primary component of vinegar and a key intermediate in biochemical pathways,[40] and glucose (C₆H₁₂O₆), a monosaccharide central to cellular metabolism.[41] Aspirin (C₉H₈O₄), or acetylsalicylic acid, exemplifies a pharmaceutical ternary compound with anti-inflammatory properties derived from its salicylate structure.[42] Examples from other combinations include acetamide (CH₃CONH₂), a C-H-N compound used as a solvent in plastics manufacturing,[43] and chloroform (CHCl₃), a C-H-Cl solvent in organic synthesis.[44] Isomerism in organic ternary compounds arises from the versatile bonding of carbon, leading to structural diversity that affects physical and biological properties. Structural isomers, such as chain versus ring configurations or different functional group positions, are common; for instance, the molecular formula C₉H₁₀O₃ exhibits numerous constitutional isomers, including various aldehydes like the four dimethoxybenzaldehyde isomers.[45][38] Stereoisomers, including enantiomers and diastereomers, further multiply possibilities, particularly in chiral centers found in sugars like glucose, which has multiple anomeric forms. These variations are cataloged extensively in chemical databases, highlighting the combinatorial richness of C-H-O systems.[46] Synthesis of organic ternary compounds often involves reactions adding oxygen-containing groups to binary hydrocarbon precursors. A representative method is the acid-catalyzed hydration of alkenes, where water adds across the double bond following Markovnikov's rule to form alcohols, such as the production of ethanol from ethene. This electrophilic addition proceeds via a carbocation intermediate, enabling scalable synthesis for industrial applications.[47] In applications, the structural diversity from isomerism is pivotal in pharmaceuticals, where specific isomers optimize efficacy and reduce side effects; for example, the (S)-enantiomer of ibuprofen provides faster pain relief compared to the racemic mixture.[48] In biochemistry, ternary carbohydrates such as glucose serve as primary energy sources, metabolized via glycolysis to generate ATP in cells.[41]

References

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  2. Section 6.2: Naming Compounds
  3. 3.4: Writing Formulas for Ionic Compounds. Polyatomic Ions
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  5. Ternary Acids and Bases - UCalgary Chemistry Textbook
  6. Chemistry Chapter 8 Flashcards - Quizlet
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  16. Acid–Base Reactions - Highland Community College
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  21. Lithium Niobate Single Crystals and Powders Reviewed—Part I
  22. Structure of Spinel
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  25. Controls on CaCO 3 Polymorphism: From Laboratory Precipitation to ...
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