Neptunium Compounds

Neptunium compounds are compounds containg the element neptunium (Np). Neptunium has five ionic oxidation states ranging from +3 to +7 when forming chemical compounds, which can be simultaneously observed in solutions. It is the heaviest actinide that can lose all its valence electrons in a stable compound. The most stable state in solution is +5, but the valence +4 is preferred in solid neptunium compounds. Neptunium metal is very reactive. Ions of neptunium are prone to hydrolysis and formation of coordination compounds.^[1]

Solution chemistry

When it is in an aqueous solution, neptunium can exist in any of its five possible oxidation states (+3 to +7) and each of these show a characteristic color.^[2] The stability of each oxidation state is strongly dependent on various factors, such as the presence of oxidizing or reducing agents, pH of the solution, presence of coordination complex-forming ligands, and even the concentration of neptunium in the solution.^[3]

Oxidation state	Representative compound
2	[K(2.2.2-crypt)][NpCp'3]
3	Neptunium(III) chloride, K[NpCp4]
4	Neptunium(IV) oxide, NpCp4
5	Neptunium(V) fluoride
6	Neptunium(VI) fluoride, NpO2+2
7	Neptunium(VII) oxide-hydroxide, NpO3+2

In acidic solutions, the neptunium(III) to neptunium(VII) ions exist as Np³⁺, Np⁴⁺, NpO+2, NpO2+2, and NpO+3. In basic solutions, they exist as the oxides and hydroxides Np(OH)₃, NpO₂, NpO₂OH, NpO₂(OH)₂, and NpO3−5. Not as much work has been done to characterize neptunium in basic solutions.^[3] Np³⁺ and Np⁴⁺ can easily be reduced and oxidized to each other, as can NpO+2 and NpO2+2.^[4]

Neptunium(III)

Np(III) or Np³⁺ exists as hydrated complexes in acidic solutions, Np(H₂O)3+n.^[5] It is a dark blue-purple and is analogous to its lighter congener, the pink rare-earth ion Pm³⁺.^[5][6] In the presence of oxygen, it is quickly oxidized to Np(IV) unless strong reducing agents are also present. Nevertheless, it is the second-least easily hydrolyzed neptunium ion in water, forming the NpOH²⁺ ion.^[7] Np³⁺ is the predominant neptunium ion in solutions of pH 4–5.^[7]

Neptunium(IV)

Np(IV) or Np⁴⁺ is pale yellow-green in acidic solutions,^[5] where it exists as hydrated complexes (Np(H₂O)4+n). It is quite unstable to hydrolysis in acidic aqueous solutions at pH 1 and above, forming NpOH³⁺.^[7] In basic solutions, Np⁴⁺ tends to hydrolyze to form the neutral neptunium(IV) hydroxide (Np(OH)₄) and neptunium(IV) oxide (NpO₂).^[7]

Neptunium(V)

Np(V) or NpO+2 is green-blue in aqueous solution,^[5] in which it behaves as a strong Lewis acid.^[3] It is a stable ion^[3] and is the most common form of neptunium in aqueous solutions. Unlike its neighboring homologues UO+2 and PuO+2, NpO+2 does not spontaneously disproportionate except at very low pH and high concentration:^[4]

2 NpO+2 + 4 H⁺ ⇌ Np⁴⁺ + NpO2+2 + 2 H₂O

It hydrolyzes in basic solutions to form NpO₂OH and NpO₂(OH)−2.^[7]

Neptunium(VI)

Np(VI) or NpO2+2, the neptunyl ion, shows a light pink or reddish color in an acidic solution and yellow-green otherwise.^[5] It is a strong Lewis acid^[3] and is the main neptunium ion encountered in solutions of pH 3–4.^[7] Though stable in acidic solutions, it is quite easily reduced to the Np(V) ion,^[3] and it is not as stable as the homologous hexavalent ions of its neighbours uranium and plutonium (the uranyl and plutonyl ions). It hydrolyzes in basic solutions to form the oxo and hydroxo ions NpO₂OH⁺, (NpO₂)₂(OH)2+2, and (NpO₂)₃(OH)+5.^[7]

Neptunium(VII)

Np(VII) is dark green in a strongly basic solution. Though its chemical formula in basic solution is frequently cited as NpO3−5, this is a simplification and the real structure is probably closer to a hydroxo species like [NpO₄(OH)₂]³⁻.^[5][6] Np(VII) was first prepared in basic solution in 1967.^[3] In strongly acidic solution, Np(VII) is found as NpO+3; water quickly reduces this to Np(VI).^[3] Its hydrolysis products are uncharacterized.^[7]

Hydroxides

The oxides and hydroxides of neptunium are closely related to its ions. In general, Np hydroxides at various oxidation levels are less stable than the actinides before it on the periodic table such as thorium and uranium and more stable than those after it such as plutonium and americium. This phenomenon is because the stability of an ion increases as the ratio of atomic number to the radius of the ion increases. Thus actinides higher on the periodic table will more readily undergo hydrolysis.^[3][7]

Neptunium(III) hydroxide is quite stable in acidic solutions and in environments that lack oxygen, but it will rapidly oxidize to the IV state in the presence of air. It is not soluble in water.^[8] Np(IV) hydroxides exist mainly as the electrically neutral Np(OH)₄ and its mild solubility in water is not affected at all by the pH of the solution. This suggests that the other Np(IV) hydroxide, Np(OH)−5, does not have a significant presence.^[7][9]

Because the Np(V) ion NpO+2 is very stable, it can only form a hydroxide in high acidity levels. When placed in a 0.1 M sodium perchlorate solution, it does not react significantly for a period of months, although a higher molar concentration of 3.0 M will result in it reacting to the solid hydroxide NpO₂OH almost immediately. Np(VI) hydroxide is more reactive but it is still fairly stable in acidic solutions. It will form the compound NpO₃· H₂O in the presence of ozone under various carbon dioxide pressures. Np(VII) has not been well-studied and no neutral hydroxides have been reported. It probably exists mostly as [NpO₄(OH)₂]³⁻.^{[7][10][11][12]}

Oxides

Three anhydrous neptunium oxides have been reported, NpO₂, Np₂O₅, and Np₅O₈, though some studies^[13] have stated that only the first two of these exist, suggesting that claims of Np₅O₈ are actually the result of mistaken analysis of Np₂O₅. However, as the full extent of the reactions that occur between neptunium and oxygen has yet to be researched, it is not certain which of these claims is accurate. Although neptunium oxides have not been produced with neptunium in oxidation states as high as those possible with the adjacent actinide uranium, neptunium oxides are more stable at lower oxidation states. This behavior is illustrated by the fact that NpO₂ can be produced by simply burning neptunium salts of oxyacids in air.^{[5][14][15][16]}

The greenish-brown NpO₂ is very stable over a large range of pressures and temperatures and does not undergo phase transitions at low temperatures. It does show a phase transition from face-centered cubic to orthorhombic at around 33-37GPa, although it returns to is original phase when pressure is released. It remains stable under oxygen pressures up to 2.84 MPa and temperatures up to 400 °C. Np₂O₅ is black-brown in color and monoclinic with a lattice size of 418×658×409 picometres. It is relatively unstable and decomposes to NpO₂ and O₂ at 420-695 °C. Although Np₂O₅ was initially subject to several studies that claimed to produce it with mutually contradictory methods, it was eventually prepared successfully by heating neptunium peroxide to 300-350 °C for 2–3 hours or by heating it under a layer of water in an ampoule at 180 °C.^{[14][16][17][18]}

Neptunium also forms a large number of oxide compounds with a wide variety of elements, although the neptunate oxides formed with alkali metals and alkaline earth metals have been by far the most studied. Ternary neptunium oxides are generally formed by reacting NpO₂ with the oxide of another element or by precipitating from an alkaline solution. Li₅NpO₆ has been prepared by reacting Li₂O and NpO₂ at 400 °C for 16 hours or by reacting Li₂O₂ with NpO₃ · H₂O at 400 °C for 16 hours in a quartz tube and flowing oxygen. Alkali neptunate compounds K₃NpO₅, Cs₃NpO₅, and Rb₃NpO₅ are all created by a similar reaction:

NpO₂ + 3 MO₂ → M₃NpO₅ (M = K, Cs, Rb)

The oxide compounds KNpO₄, CsNpO₄, and RbNpO₄ are formed by reacting Np(VII) ([NpO₄(OH)₂]³⁻) with a compound of the alkali metal nitrate and ozone. Additional compounds have been produced by reacting NpO₃ and water with solid alkali and alkaline peroxides at temperatures of 400 - 600 °C for 15–30 hours. Some of these include Ba₃(NpO₅)₂, Ba₂NaNpO₆, and Ba₂LiNpO₆. Also, a considerable number of hexavalent neptunium oxides are formed by reacting solid-state NpO₂ with various alkali or alkaline earth oxides in an environment of flowing oxygen. Many of the resulting compounds also have an equivalent compound that substitutes uranium for neptunium. Some compounds that have been characterized include Na₂Np₂O₇, Na₄NpO₅, Na₆NpO₆, and Na₂NpO₄. These can be obtained by heating different combinations of NpO₂ and Na₂O to various temperature thresholds and further heating will also cause these compounds to exhibit different neptunium allotropes. The lithium neptunate oxides Li₆NpO₆ and Li₄NpO₅ can be obtained with similar reactions of NpO₂ and Li₂O.^{[19][20][21][22][23][24][25][26]}

A large number of additional alkali and alkaline neptunium oxide compounds such as Cs₄Np₅O₁₇ and Cs₂Np₃O₁₀ have been characterized with various production methods. Neptunium has also been observed to form ternary oxides with many additional elements in groups 3 through 7, although these compounds are much less well studied.^[19][27][28]

Halides

Although neptunium halide compounds have not been nearly as well studied as its oxides, a fairly large number have been successfully characterized. Of these, neptunium fluorides have been the most extensively researched, largely because of their potential use in separating the element from nuclear waste products. Four binary neptunium fluoride compounds, NpF₃, NpF₄, NpF₅, and NpF₆, have been reported. The first two are fairly stable and were first prepared in 1947 through the following reactions:

NpO₂ + ​¹⁄₂ H₂ + 3 HF → NpF₃ + 2 H₂O   (400°C)

NpF₃ + ​¹⁄₂ O₂ + HF → NpF₄ + ​¹⁄₂ H₂O  (400°C)

Later, NpF₄ was obtained directly by heating NpO₂ to various temperatures in mixtures of either hydrogen fluoride or pure fluorine gas. NpF₅ is much more difficult to create and most known preparation methods involve reacting NpF₄ or NpF₆ compounds with various other fluoride compounds. NpF₅ will decompose into NpF₄ and NpF₆ when heated to around 320 °C.^{[29][30][31][32]}

NpF₆ or neptunium hexafluoride is extremely volatile, as are its adjacent actinide compounds uranium hexafluoride (UF₆) and plutonium hexafluoride (PuF₆). This volatility has attracted a large amount of interest to the compound in an attempt to devise a simple method for extracting neptunium from spent nuclear power station fuel rods. NpF₆ was first prepared in 1943 by reacting NpF₃ and gaseous fluorine at very high temperatures and the first bulk quantities were obtained in 1958 by heating NpF₄ and dripping pure fluorine on it in a specially prepared apparatus. Additional methods that have successfully produced neptunium hexafluoride include reacting BrF₃ and BrF₅ with NpF₄ and by reacting several different neptunium oxide and fluoride compounds with anhydrous hydrogen fluorides.^{[30][33][34][35]}

Four neptunium oxyfluoride compounds, NpO₂F, NpOF₃, NpO₂F₂, and NpOF₄, have been reported, although none of them have been extensively studied. NpO₂F₂ is a pinkish solid and can be prepared by reacting NpO₃ · H₂O and Np₂F₅ with pure fluorine at around 330 °C. NpOF₃ and NpOF₄ can be produced by reacting neptunium oxides with anhydrous hydrogen fluoride at various temperatures. Neptunium also forms a wide variety of fluoride compounds with various elements. Some of these that have been characterized include CsNpF₆, Rb₂NpF₇, Na₃NpF₈, and K₃NpO₂F₅.^{[30][32][36][37][38][39][40]}

Two neptunium chlorides, NpCl₃ and NpCl₄, have been characterized. Although several attempts to create NpCl₅ have been made, they have not been successful. NpCl₃ is created by reducing neptunium dioxide with hydrogen and carbon tetrachloride (CCl₄) and NpCl₄ by reacting a neptunium oxide with CCl₄ at around 500 °C. Other neptunium chloride compounds have also been reported, including NpOCl₂, Cs₂NpCl₆, Cs₃NpO₂Cl₄, and Cs₂NaNpCl₆. Neptunium bromides NpBr₃ and NpBr₄ have also been created; the latter by reacting aluminium bromide with NpO₂ at 350 °C and the former in an almost identical procedure but with zinc present. The neptunium iodide NpI₃ has also been prepared by the same method as NpBr₃.^[41][42][43]

Chalcogenides, pnictides, and carbides

Neptunium chalcogen and pnictogen compounds have been well studied primarily as part of research into their electronic and magnetic properties and their interactions in the natural environment. Pnictide and carbide compounds have also attracted interest because of their presence in the fuel of several advanced nuclear reactor designs, although the latter group has not had nearly as much research as the former.^[44]

Chalcogenides

A wide variety of neptunium sulfide compounds have been characterized, including the pure sulfide compounds NpS, NpS₃, Np₂S₅, Np₃S₅, Np₂S₃, and Np₃S₄. Of these, Np₂S₃, prepared by reacting NpO₂ with hydrogen sulfide and carbon disulfide at around 1000 °C, is the most well-studied and three allotropic forms are known. The α form exists up to around 1230 °C, the β up to 1530 °C, and the γ form, which can also exist as Np₃S₄, at higher temperatures. NpS can be created by reacting Np₂S₃ and neptunium metal at 1600 °C and Np₃S₅ can be prepared by the decomposition of Np₂S₃ at 500 °C or by reacting sulfur and neptunium hydride at 650 °C. Np₂S₅ is made by heating a mixture of Np₃S₅ and pure sulfur to 500 °C. All of the neptunium sulfides except for the β and γ forms of Np₂S₃ are isostructural with the equivalent uranium sulfide and several, including NpS, α−Np₂S₃, and β−Np₂S₃ are also isostructural with the equivalent plutonium sulfide. The oxysulfides NpOS, Np₄O₄S, and Np₂O₂S have also been created, although the latter three have not been well studied. NpOS was first prepared in 1985 by vacuum sealing NpO₂, Np₃S₅, and pure sulfur in a quartz tube and heating it to 900 °C for one week.^{[44][45][46][47][48][49][50]}

Neptunium selenide compounds that have been reported include NpSe, NpSe₃, Np₂Se₃, Np₂Se₅, Np₃Se₄, and Np₃Se₅. All of these have only been obtained by heating neptunium hydride and selenium metal to various temperatures in a vacuum for an extended period of time and Np₂Se₃ is only known to exist in the γ allotrope at relatively high temperatures. Two neptunium oxyselenide compounds are known, NpOSe and Np₂O₂Se, are formed with similar methods by replacing the neptunium hydride with neptunium dioxide. The known neptunium telluride compounds NpTe, NpTe₃, Np₃Te₄, Np₂Te₃, and Np₂O₂Te are formed by similar procedures to the selenides and Np₂O₂Te is isostructural to the equivalent uranium and plutonium compounds. No neptunium−polonium compounds have been reported.^{[44][50][51][52][53]}

Pnictides and carbides

Neptunium nitride (NpN) was first prepared in 1953 by reacting neptunium hydride and ammonia gas at around 750 °C in a quartz capillary tube. Later, it was produced by reacting different mixtures of nitrogen and hydrogen with neptunium metal at various temperatures. It has also been created by the reduction of neptunium dioxide with diatomic nitrogen gas at 1550 °C. NpN is isomorphous with uranium mononitride (UN) and plutonium mononitride (PuN) and has a melting point of 2830 °C under a nitrogen pressure of around 1 MPa. Two neptunium phosphide compounds have been reported, NpP and Np₃P₄. The first has a face centered cubic structure and is prepared by converting neptunium metal to a powder and then reacting it with phosphine gas at 350 °C. Np₃P₄ can be created by reacting neptunium metal with red phosphorus at 740 °C in a vacuum and then allowing any extra phosphorus to sublimate away. The compound is non-reactive with water but will react with nitric acid to produce Np(IV) solution.^[54][55][56]

Three neptunium arsenide compounds have been prepared, NpAs, NpAs₂, and Np₃As₄. The first two were first created by heating arsenic and neptunium hydride in a vacuum-sealed tube for about a week. Later, NpAs was also made by confining neptunium metal and arsenic in a vacuum tube, separating them with a quartz membrane, and heating them to just below neptunium's melting point of 639 °C, which is slightly higher than the arsenic's sublimation point of 615 °C. Np₃As₄ is prepared by a similar procedure using iodine as a transporting agent. NpAs₂ crystals are brownish gold and Np₃As₄ is black. The neptunium antimonide compound NpSb was created in 1971 by placing equal quantities of both elements in a vacuum tube, heating them to the melting point of antimony, and then heating it further to 1000 °C for sixteen days. This procedure also created trace amounts of an additional antimonide compound Np₃Sb₄. One neptunium-bismuth compound, NpBi, has also been reported.^{[54][55][57][58][59][60]}

The neptunium carbides NpC, Np₂C₃, and NpC₂ (tentative) have been reported, but have not characterized in detail despite the high importance and utility of actinide carbides as advanced nuclear reactor fuel. NpC is a non-stoichiometric compound, and could be better labelled as NpC_x (0.82 ≤ x ≤ 0.96). It may be obtained from the reaction of neptunium hydride with graphite at 1400 °C or by heating the constituent elements together in an electric arc furnace using a tungsten electrode. It reacts with excess carbon to form pure Np₂C₃. NpC₂ is formed from heating NpO₂ in a graphite crucible at 2660–2800 °C.^{[54][55][61][62]}

Other inorganic compounds

Hydrides

Neptunium reacts with hydrogen in a similar manner to its neighbor plutonium, forming the hydrides NpH_2+x (face-centered cubic) and NpH₃ (hexagonal). These are isostructural with the corresponding plutonium hydrides, although unlike PuH_2+x, the lattice parameters of NpH_2+x become greater as the hydrogen content (x) increases. The hydrides require extreme care in handling as they decompose in a vacuum at 300 °C to form finely divided neptunium metal, which is pyrophoric.^[63]

Phosphates, sulfates, and carbonates

Being chemically stable, neptunium phosphates have been investigated for potential use in immobilizing nuclear waste. Neptunium pyrophosphate (α-NpP₂O₇), a green solid, has been produced in the reaction between neptunium dioxide and boron phosphate at 1100 °C, though neptunium(IV) phosphate has so far remained elusive. The series of compounds NpM₂(PO₄)₃, where M is an alkali metal (Li, Na, K, Rb, or Cs), are all known. Some neptunium sulfates have been characterized, both aqueous and solid and at various oxidation states of neptunium (IV through VI have been observed). Additionally, neptunium carbonates have been investigated to achieve a better understanding of the behavior of neptunium in geological repositories and the environment, where it may come into contact with carbonate and bicarbonate aqueous solutions and form soluble complexes.^[64][65]

Organometallic compounds

A few organoneptunium compounds are known and chemically characterized, although not as many as for uranium due to neptunium's scarcity and radioactivity. The most well known organoneptunium compounds are the cyclopentadienyl and cyclooctatetraenyl compounds and their derivatives.^[66] The trivalent cyclopentadienyl compound Np(C₅H₅)₃·THF was obtained in 1972 from reacting Np(C₅H₅)₃Cl with sodium, although the simpler Np(C₅H₅) could not be obtained.^[66] Tetravalent neptunium cyclopentadienyl, a reddish-brown complex, was synthesized in 1968 by reacting neptunium(IV) chloride with potassium cyclopentadienide:^[66]

NpCl₄ + 4 KC₅H₅ → Np(C₅H₅)₄ + 4 KCl

It is soluble in benzene and THF, and is less sensitive to oxygen and water than Pu(C₅H₅)₃ and Am(C₅H₅)₃.^[66] Other Np(IV) cyclopentadienyl compounds are known for many ligands: they have the general formula (C₅H₅)₃NpL, where L represents a ligand.^[66] Neptunocene, Np(C₈H₈)₂, was synthesized in 1970 by reacting neptunium(IV) chloride with K₂(C₈H₈). It is isomorphous to uranocene and plutonocene, and they behave chemically identically: all three compounds are insensitive to water or dilute bases but are sensitive to air, reacting quickly to form oxides, and are only slightly soluble in benzene and toluene.^[66] Other known neptunium cyclooctatetraenyl derivatives include Np(RC₈H₇)₂ (R = ethanol, butanol) and KNp(C₈H₈)·2THF, which is isostructural to the corresponding plutonium compound.^[66] In addition, neptunium hydrocarbyls have been prepared, and solvated triiodide complexes of neptunium are a precursor to many organoneptunium and inorganic neptunium compounds.^[66]

Coordination complexes

There is much interest in the coordination chemistry of neptunium, because its five oxidation states all exhibit their own distinctive chemical behavior, and the coordination chemistry of the actinides is heavily influenced by the actinide contraction (the greater-than-expected decrease in ionic radii across the actinide series, analogous to the lanthanide contraction).^[67]

Solid state

Few neptunium(III) coordination compounds are known, because Np(III) is readily oxidized by atmospheric oxygen while in aqueous solution. However, sodium formaldehyde sulfoxylate can reduce Np(IV) to Np(III), stabilizing the lower oxidation state and forming various sparingly soluble Np(III) coordination complexes, such as Np₂(C₂O₄)₃·11H₂O, Np₂(C₆H₅AsO₃)₃·H₂O, and Np₂[C₆H₄(OH)COO]₃.^[67]

Many neptunium(IV) coordination compounds have been reported, the first one being (Et₄N)Np(NCS)₈, which is isostructural with the analogous uranium(IV) coordination compound.^[67] Other Np(IV) coordination compounds are known, some involving other metals such as cobalt (CoNp₂F₁₀·8H₂O, formed at 400 K) and copper (CuNp₂F₁₀·6H₂O, formed at 600 K).^[67] Complex nitrate compounds are also known: the experimenters who produced them in 1986 and 1987 produced single crystals by slow evaporation of the Np(IV) solution at ambient temperature in concentrated nitric acid and excess 2,2′-pyrimidine.^[67]

The coordination chemistry of neptunium(V) has been extensively researched due to the presence of cation–cation interactions in the solid state, which had been already known for actinyl ions.^[67] Some known such compounds include the neptunyl dimer Na₄(NpO₄)₂C₁₂O₁₂·8H₂O and neptunium glycolate, both of which form green crystals.^[67]

Neptunium(VI) compounds range from the simple oxalate NpO₂C₂O₄ (which is unstable, usually becoming Np(IV)) to such complicated compounds as the green (NH₄)₄NpO₂(CO₃)₃.^[67] Extensive study has been performed on compounds of the form M₄AnO₂(CO₃)₃, where M represents a monovalent cation and An is either uranium, neptunium, or plutonium.^[67]

Since 1967, when neptunium(VII) was discovered, some coordination compounds with neptunium in the +7 oxidation state have been prepared and studied. The first reported such compound was initially characterized as Co(NH₃)₆NpO₅·nH₂O in 1968, but was suggested in 1973 to actually have the formula [Co(NH₃)₆][NpO₄(OH)₂]·2H₂O based on the fact that Np(VII) occurs as [NpO₄(OH)₂]³⁻ in aqueous solution.^[67] This compound forms dark green prismatic crystals with maximum edge length 0.15–0.4 mm.^[67]

In aqueous solution

Most neptunium coordination complexes known in solution involve the element in the +4, +5, and +6 oxidation states: only a few studies have been done on neptunium(III) and (VII) coordination complexes.^[68] For the former, NpX²⁺ and NpX+2 (X = Cl, Br) were obtained in 1966 in concentrated LiCl and LiBr solutions, respectively: for the latter, 1970 experiments discovered that the NpO3+2 ion could form sulfate complexes in acidic solutions, such as NpO₂SO+4 and NpO₂(SO₄)−2; these were found to have higher stability constants than the neptunyl ion (NpO2+2).^[68] A great many complexes for the other neptunium oxidation states are known: the inorganic ligands involved are the halides, iodate, azide, nitride, nitrate, thiocyanate, sulfate, carbonate, chromate, and phosphate. Many organic ligands are known to be able to be used in neptunium coordination complexes: they include acetate, propionate, glycolate, lactate, oxalate, malonate, phthalate, mellitate, and citrate.^[68]

Analogously to its neighbours, uranium and plutonium, the order of the neptunium ions in terms of complex formation ability is Np⁴⁺ > NpO2+2 ≥ Np³⁺ > NpO+2. (The relative order of the middle two neptunium ions depends on the ligands and solvents used.)^[68] The stability sequence for Np(IV), Np(V), and Np(VI) complexes with monovalent inorganic ligands is F⁻ > H₂PO−4 > SCN⁻ > NO−3 > Cl⁻ > ClO−4; the order for divalent inorganic ligands is CO2−3 > HPO2−4 > SO2−4. These follow the strengths of the corresponding acids. The divalent ligands are more strongly complexing than the monovalent ones.^[68] NpO+2 can also form the complex ions [NpO+2M³⁺] (M = Al, Ga, Sc, In, Fe, Cr, Rh) in perchloric acid solution: the strength of interaction between the two cations follows the order Fe > In > Sc > Ga > Al.^[68] The neptunyl and uranyl ions can also form a complex together.^[68]

See also

• Protactinium compounds
• Promethium compounds

References

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