Sulfur mononitride

Sulfur mononitride  | Wireframe model of sulfur mononitride | Spacefill model of sulfur mononitride

|

Names
Preferred IUPAC name

sulfur mononitride

Systematic IUPAC name

Azaniumylsulfanidylidyne

Other names

* Aminiosulfanidylidyne
* Thionitroso radical
* Thionitrosyl radical

Identifiers

CAS Number

* 12033-56-6

3D model (JSmol)

* Interactive image

Abbreviations  | (NS)(.)
ChEBI |

* CHEBI:29451

ChemSpider |

* 4576119

Gmelin Reference

| 660

PubChem CID

* 5463441

CompTox Dashboard (EPA)

* DTXSID50923331

InChI

* InChI=1S/H3NS/c1-2/h1H3

Key: ZGSDJMADBJCNPN-UHFFFAOYSA-N

SMILES

* [N+] [S-]

Properties

Chemical formula

| NS
Molar mass | 46.07 g·mol−1

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Infobox references

Chemical compound

Sulfur mononitride is an inorganic compound with the molecular formula SN. It is the sulfur analogue of and isoelectronic to the radical nitric oxide, NO. It was initially detected in 1975, in outer space in giant molecular clouds and later the coma of comets.[1] This spurred further laboratory studies of the compound. Synthetically, it is produced by electric discharge in mixtures of nitrogen and sulfur compounds, or combustion in the gas phase and by photolysis in solution.[2]

## Synthesis

[edit]

The NS radical is a highly transient species, with a lifetime on the order of milliseconds, but it can be observed spectroscopically over short periods of time through several methods of generation. NS is too reactive to isolate as a solid or liquid, and has only been prepared as a vapor in low pressure or low-temperature matrices due to its tendency to rapidly oligomerize to more stable, diamagnetic species.[3]

### Discharge of nitrogen and sulfur vapor

[edit]

Transmission of electric discharge through a glass tube with quartz windows containing a mixture of nitrogen and sulfur vapor (rigorously free of oxygen) results in the spectrum of emitted light gaining bands consistent with the formation of NS.[4]

Passing a mixture of gaseous N2 and S2Cl2 through the side arm of an absorption cell undergoing microwave discharge produces NS. Infrared diode laser spectroscopy taken using this method allowed for derivation of the equilibrium rotational constant, and therefore calculation of the equilibrium bond length as 1.4940 Å.[5]

With low pressure microwave discharge of elemental nitrogen and sulfur, followed by low temperature trapping in argon matrices, one obtains a mixture of products including NS, NNS, SNS, and NSS. By adding excess sulfur, SSNS is also produced.[6]

### Burning of sulfur and nitrogen doped flames

[edit]

Methane was premixed with fuel in the form of either O2, N2O, or air and burned at ambient pressure. The source of nitrogen was introduced by addition of 1–5 mol% NH3 gas and sulfur by 0.01–0.5 mol% H2S or SF6 gas. A steady state concentration of NS within the flame front is observed by laser-induced fluorescence (LIF) spectrum.[7]

### Flash laser photolysis of tetranitrogen tetrasulfide

[edit]

The NS radical was detected by LIF spectrum as the product of photolysis of tetranitrogen tetrasulfide (N4S4) gas by a 248 nm laser.[8]

### Flash and continuous photolysis of Cr(CH3CN)5(NS)2+

[edit]

Aerated solutions of Cr(CH3CN)5(NS)2+ are highly photoactive and prone to rapid decomposition. Deaerated solutions of Cr(CH3CN)5(NS)2+ in acetonitrile are stable as long as they are kept in the dark. Continuous photolysis using 366 nm light is slow, while using a 355 nm pulsed laser results in faster labilization of NS.[9]

## Reactivity

[edit]

### Oligomerization

[edit]

Evidence suggests that NS can react with itself to reach N2S2, N4S4, and polymers of the form (NS)x. (NS)x forms from polymerization of cyclo-N2S2.[3]

cyclo-N2S2. N4S4. (NS)x polymer.

Trans-NSSN results from direct dimerization of NS.[3]

N3S3 has been observed through photoelectron spectroscopy of vapors of the (SN)x, polymer, but has not yet been characterized further. Attempts to produce N3S3 by oxidation of [PPN] [S3N3] were unsuccessful.[10] Its theorized that rapid dimerization to (N3S3)2 will disproportionate irreversibly to N4S4 and N2S2.[3]

N3S3.

### Products of decay with NO2

[edit]

The radical decay time of NS alone is on the order of 1-3 ms. As evident by no change to this decay time upon addition of NO or O2 at ambient temperatures, the NS radical is unreactive with NO and O2. However, rapid, first-order decay is observed with the addition of NO2. This reaction is proposed to proceed through various intermediates, ultimately reaching final products of N2 and SO2.[8] This rapid reaction occurs with a rate constant of k = (2.54 ± 0.12) × 10−11 cm3 molecules−1 s−1 at 295 K. By use of Density Functional Theory based computational calculations, the minima and transition states of the potential energy surface of this reaction have been predicted.[8]

### Astronomical reactivity

[edit]

Within the inner coma of comets, many reactions are theorized to be relevant to the formation and reactivity of the NS radical.[11]

### Metal-thionitrosyl complexes

[edit]

As a ligand, NS acts as a σ-donor and π-acceptor, forming metal-thionitrosyl complexes. Transition-metal thionitrosyl complexes have been prepared by the following procedures:[12]

* Sulfur transfer to metal nitrido complexes
* Example: Reflux of (Ph4P)[OsNCl4] and (Ph4P)NCS yields green-brown solid [Ph4P]2[Os(NS)(NCS)5] [13]
* Reaction of trithiazyltrichloride with transition metal complexes
* NSCl3 \+ OsCl3 > [Os(NS)Cl3]
* Halide abstraction from coordinated thiazyl complexes
* Abstraction of sulfur-bonded fluorine from [(η5−C5H5)Cr(NO)2(NSF)]-[AsF6] by AsF5 > [(η5-C5H5)Cr(NO)2(NS)]-[AsF6]2
* Reaction of NS+ salts with transition metal complexes
* NS+SbF6− \+ [M(CO)5Br] > [M(CO)5(NS)]2+, M=Mn, Re [14]
* NS+AsF6− \+ [(η5-C5H5)Fe(CO)2(SO2)]+ > [(η5-C5H5)Fe(CO)2(NS)] [AsF6]2
* Reaction of tetrasulfur tetranitride with metal halides or nitrides

From X-ray crystallography of many of such metal-thionitrosyl complexes, one can observe that the M-N-S bond angle is nearly linear, suggesting sp hybridization about N. Short M-N distances and long N-S distances reflect the resonance structure of M=N=S having greater contribution than M-N≡S.[12]

Typical v(NS) IR stretching frequencies are approximately 1065 cm−1 for low-valent transition metal complexes and around 1390 cm−1 in the high valent cases, whereas the free gas-phase radical exhibits a 1204 cm−1 signal.[3]

### Electronic structure of Fe(S2CNMe2)2(NS)

[edit]

The electronic structures of Fe(S2CNMe2)2(NE), where E=O, S, or Se were calculated using Density Functional Theory methods. It was found that the large Mulliken spin density remained concentrated on the Fe(NE) core and Fe-N distances experienced little change from the chalcogen atom used. The HOMO of both nitrosyl and thionitrosyl complexes retained 1a1 (dz2) character. The small changes in the energies of the spin orbitals of the complexes, particularly the decreased energetic gap between 2b2 and 1b1 and 2b1 and 1b1 orbitals is attributed to NS being a weaker π-acceptor than NO.[9]

### Photoinduced NS transfer from chromium to iron

[edit]

When a spin-trapping agent, such as Fe(S2CNEt2)2 is present during the photolysis of Cr(CH3CN)5(NS)2+, new S=1/2 EPR bands are observed, attributed to the formation of Fe(S2CNEt2)2(NS), and the signal from Cr(CH3CN)5(NS)2+ disappears. This suggests that the NS radical has transferred from the chromium complex to the iron complex.[9]

An example of an NS in situ transfer is the following reaction, which needs light to occur:

(Cr(CH3CN)5(NS)2+ \+ Fe(S2CNEt2) + CH3CN → Cr(CH3CN)2+6 \+ Fe(S2CNEt2)2(NS)

This was particularly significant as it was the first controlled and well-characterized reactivity of NS in solution. Further, it showed the potential for similar reactivity in known reactions with NO, such as use of this iron dithiocarbamate complex.[3]

## Bonding

[edit]

Model of bonding in the NS radical

The valence electrons of this compound match those of nitric oxide. Sulfur mononitride can be described as some average of a set of resonance structures. The singly bonded structure (first resonance structure shown) has little contribution. The formal bond order is considered to be 2.5.

Resonance structures of NS. Molecular orbital diagram of NS.

### Versus NO

[edit]

The decreasing electronegativity with increasingly heavy chalcogenides leads to a reversal of the dipole. In NO, oxygen is the more electronegative element. In NS, nitrogen is more electronegative. The NS radical is significantly more unstable and prone to catenation than NO.[3]

Comparison of physical properties of nitrogen chalcogenide radicals  | NO  | NS  | NSe

|
|
|

△fH°, kJ·mol−1 | +90.24  | +283.4  | \-
△fG°, kJ·mol−1 | +86.57  | +217.2  | \-
S° 273, J/deg  | +207.5/273 K  | +222.093/298 K  | \-
B.D.E.  | 627.6  | 463±24  | 370 Cal
d(N-E), Å  | 1.1517  | 1.4938  | 1.6634
Bond order  | 2.5  | 2.5  | 2.5

## In astronomy

[edit]

Molecules in distant astronomical regions can be identified based on their unique rotational transitions, of which the corresponding microwave frequencies are detectable by antennae on Earth. The presence of interstellar sulfur mononitride was first reported in 1975 by back to back letters published in the Astrophysical Journal.

Interstellar NS was first identified in the giant molecular cloud Sagittarius B2 (Sgr B2). Its presence was reported in two concurrent articles. Measurements conducted with the National Radio Astronomy Observatory telescope at Kitt Peak, Arizona, picked up millimeter-wavelength radiation in Sgr B2 attributed to c-state transitions of NS in the 2Π1/2 state from J=5/2 to J=3/2 at 115.16 GHz.[15] This assignment was confirmed by measurements conducted at University of Texas Millimeter Wave Observatory on Mount Locke as well, demonstrating J=5/2 to J=3/2 c-state and d-state transitions at 115.16 GHz and 115.6 GHz, respectively. Hyperfine interactions arise from 14N magnetic and electric-quadrupole moments.[16]

NS has been detected in regions responsible for forming massive stars, such as giant molecular clouds like Sg B2 and cold, dark clouds such as L134N and TMC-1. One survey found NS in 12 out of 14 GMC studied, additionally observing the J=7/2 to J=5/2 and J=3/2 to J=1/2 transitions at 161 and 69 GHz, respectively. The abundance of NS in these regions was approximated based on the ratio of observed to intrinsic hyperfine line strengths as well as modeling using a statistical equilibrium program, finding low abundance in all except the Orion molecular cloud.[17]

NS was also observed in the coma of the comets Hyakutake and Hale-Bopp. It is believed that the observed abundance is higher than gas-phase, ion-molecule models due to an unidentified species X-NS photo-dissociating to release NS.[11]

## Industrial applications

[edit]

Detection of NS at steady state concentration in the reaction zone of the combustion of methane doped with ammonia and a fuel sulfur such as H2S suggests that NS may be an important reactive intermediate in burning of hydrocarbon flames in a reducing atmosphere, which is relevant to coal pyrolysis and combustion.[7]

Fossil fuels contain bound nitrogen, which releases elevated levels of nitric oxide emissions during combustion. NOx emissions can be controlled by denitrification of the fuel source, combustion chamber modification, or both. One developing technique is the reburning of NOx, which is reduced to N2. These fuels also contain variable amounts of sulfur, which is oxidized to SO2. Therefore, understanding the reactivity of NO and SO2 is crucial to the process of reburning. The experimental apparatus to test this involved a primary flame for producing combustion products, which were mixed with NO and SO2 to mimic coal burning byproducts. This mixture was fed into the burner at atmospheric pressure. 1–2% decrease in NOx concentration is observed at various percentages of total fuel inlet (reburn ratio) in the presence of 0.1% SO2, which is attributed to the formation of H2S, HS, and the resulting reaction with NO, giving rise to NS. The reaction is:[18]

HS + NO → NS + OH

## Related compounds

[edit]

* Trithiazyl trichloride (NSCl)3
* Sulfur nitride

## References

[edit]

1. ^ Canaves, M. V.; de Almeida, A. A.; Boice, D. C.; Sanzovo, G. C. (March 2002). "Nitrogen Sulfide in Comets Hyakutake (C/1996 B2) and Hale-Bopp (C/1995 O1)". Earth, Moon, and Planets. 90 (1): 335–347\. Bibcode:2002EM&P...90..335C. doi:10.1023/A:1021582300423. S2CID 189898818.
2. ^ Burr, J. G. (1985). Chemi- and Bioluminescence. Clinical and Biochemical Analysis. Vol. 16\. CRC Press. p. 99\. ISBN 0-8247-7277-6.
3. ^ a b c d e f g Boere, R.T.; Roemmele, T.L. (2013). "Chalcogen-Nitrogen Radicals". Comprehensive Inorganic Chemistry. 1: 375–411\. doi:10.1016/B978-0-08-097774-4.00117-0. ISBN 9780080965291.
4. ^ Fowler, A.; Bakker, C. J. (1932-05-02). "The band spectrum of nitrogen sulphide (NS)". Proceedings of the Royal Society of London. Series A, Containing Papers of a Mathematical and Physical Character. 136 (829): 28–36\. Bibcode:1932RSPSA.136...28F. doi:10.1098/rspa.1932.0064. ISSN 0950-1207. S2CID 94966018.
5. ^ Matsumara, Keiji; Kawaguchi, Kentarou; Jagai, Keijchi; Yamada, Chikashi; Hirota, Eizi (1980). "Infrared Diode Laser Spectroscopy of the NS Radical". Journal of Molecular Spectroscopy. 84 (84): 68–73\. Bibcode:1980JMoSp..84...68M. doi:10.1016/0022-2852(80)90239-8.
6. ^ Hassanzadeh, Parviz; Andrews, Lester (1992). "Infrared Spectra of New Sulfur-Nitrogen Species in Solid Argon". J. Am. Chem. Soc. 114: 83–91\. doi:10.1021/ja00027a012.
7. ^ a b Jeffries, Jay; Crosley, David (1986). "Laser-Induced Fluorescence Detection of the NS Radical in Sulfur and Nitrogen Doped Methane Flames". Combustion and Flame. 64 (64): 55–64\. Bibcode:1986CoFl...64...55J. doi:10.1016/0010-2180(86)90098-2.
8. ^ a b c Blitz, Mark; McKee, Kenneth; Pilling, Michael; Vincent, Mark; Hillier, Ian (2002). "Experimental Rate Measurements for NS + NO, O2 and NO2, and Electronic Structure Calculations of the Reaction Paths for NS + NO2". J. Phys. Chem. 106 (36): 8406–841S. doi:10.1021/jp025508y.
9. ^ a b c Dethlefsen, Johannes; Hedegard, Erik; Rimer, R. Dale; Ford, Peter; Dossing, Anders (2009). "Flash and Continuous Photolysis Studies of the Thionitrosyl Complex Cr(CH3CN)5(NS)2+ and the Nitric Oxide Analogs: Reactions of Nitrogen Monosulfide in Solution". Inorganic Chemistry. 48 (1): 231–238\. doi:10.1021/ic8016936. PMID 19032042.
10. ^ Fritz, H.P.; Bruchhaus, R.; Mews, R.; Hofs, H.U. (1985). "Elektrochemische Synthesen. XXIII. Elektrochemische und EPR-spektroskopische Untersuchung des Redoxverhaltens von (SN)+ und [S3N3]?". Z. Anorg. Allg. Chem. 525 (6): 214–220\. doi:10.1002/zaac.19855250625.
11. ^ a b Canaves, Marcus V.; De Almeida, Amaury A.; Boice, Daniel C.; Sanzovo, Gilberto C. (2002), "Nitrogen Sulfide in Comets Hyakutake (C/1996 B2) and Hale-Bopp (C/1995 O1)", Cometary Science after Hale-Bopp, Dordrecht: Springer Netherlands, pp. 335–347, doi:10.1007/978-94-017-1088-6_33, ISBN 978-90-481-6156-0, retrieved 2022-12-15
12. ^ a b Pandey, Krishna (1992). "Coordination Chemistry of Thionitrosyl (NS), Thiazate (NSO-), Disulfidothionitrate (S3N-), Sulfur Monoxide (SO), and Disulfur Monoxide (S2O) Ligands". Progress in Inorganic Chemistry. 40: 445–502.
13. ^ Wright, Michael; Griffith, William (1982). "Studies on Transition-Metal Nitrido and Oxo Complexes. Part VII (1). Substituted Nitrido Complexes of Osmium and Ruthenium". Transition Met. Chem. 7: 53–58\. doi:10.1007/BF00623810. S2CID 95282271.
14. ^ Hartmann, G.; Mews, R.; Sheldrick, G.M. (16 August 1983). "Kationische übergangsmetallkomplexe von thiazylbis-trifluormethylnitroxid". Journal of Organometallic Chemistry. 252 (2): 195–200\. doi:10.1016/0022-328X(83)80083-7.
15. ^ Kuiper, T. B. H.; Kakar, R. K.; Rodriguez Kuiper, E. N.; Zuckerman, B. (September 1975). "Detection of 2.6-millimeter radiation probably due to nitrogen sulfide". The Astrophysical Journal. 200: L151. Bibcode:1975ApJ...200L.151K. doi:10.1086/181919. ISSN 0004-637X.
16. ^ Gottlieb, C. A.; Ball, J. A.; Gottlieb, E. W.; Lada, C. J.; Penfield, H. (September 1975). "Detection of interstellar nitrogen sulfide". The Astrophysical Journal. 200: L147. Bibcode:1975ApJ...200L.147G. doi:10.1086/181918. ISSN 0004-637X.
17. ^ McGonagle, Douglas; Irvine, William M. (1997-03-10). "Nitrogen Sulfide in Giant Molecular Clouds". The Astrophysical Journal. 477 (2): 711–721\. Bibcode:1997ApJ...477..711M. doi:10.1086/303749. ISSN 0004-637X. PMID 11539871. S2CID 39674849.
18. ^ Chagger, Harnit; Goddard, Philip; Murdoch, Patricia; Williams, Alan (1991). "Effect of SO2 on the reduction of NOx by reburning with methane". Fuel. 70 (10): 1137–1142\. doi:10.1016/0016-2361(91)90233-Z.

* v
* t
* e

Molecules detected in outer space

Molecules|

| Diatomic|

* Aluminium monochloride
* Aluminium monofluoride
* Aluminium(II) oxide
* Argonium
* Carbon cation
* Carbon monophosphide
* Carbon monosulfide
* Carbon monoxide
* Cyano radical
* Diatomic carbon
* Fluoromethylidynium
* Helium hydride ion
* Hydrogen chloride
* Hydrogen fluoride
* Hydrogen (molecular)
* Hydroxyl radical
* Imidogen
* Iron(II) oxide
* Magnesium monohydride
* Methylidyne radical
* Nitric oxide
* Nitrogen (molecular)
* Oxygen (molecular)
* Phosphorus monoxide
* Phosphorus mononitride
* Potassium chloride
* Silicon carbide
* Silicon monoxide
* Silicon monosulfide
* Sodium chloride
* Sodium iodide
* Sulfanyl
* Sulfur mononitride
* Sulfur monoxide
* Titanium(II) oxide

|
|

Triatomic|

* Aluminium(I) hydroxide
* Aluminium isocyanide
* Amino radical
* Carbon dioxide
* Carbonyl sulfide
* CCP radical
* Chloronium
* Diazenylium
* Dicarbon monoxide
* Disilicon carbide
* Ethynyl radical
* Formyl radical
* Hydrogen cyanide (HCN)
* Hydrogen isocyanide (HNC)
* Hydrogen sulfide
* Hydroperoxyl
* Iron cyanide
* Isoformyl
* Magnesium cyanide
* Magnesium isocyanide
* Methylene
* Methylidynephosphane
* N2H+
* Nitrous oxide
* Nitroxyl
* Ozone
* Potassium cyanide
* Sodium cyanide
* Sodium hydroxide
* Silicon carbonitride
* c-Silicon dicarbide
* SiNC
* Sulfur dioxide
* Thioformyl
* Thioxoethenylidene
* Titanium dioxide
* Tricarbon
* Trihydrogen cation
* Water

Four
atoms|

* Acetylene
* Ammonia
* Cyanoethynyl
* Formaldehyde
* Fulminic acid
* HCCN
* Hydrogen peroxide
* Hydromagnesium isocyanide
* Isocyanic acid
* Isothiocyanic acid
* Ketenyl
* Methyl cation
* Methyl radical
* Methylene amidogen
* Propynylidyne
* Protonated carbon dioxide
* Protonated hydrogen cyanide
* Silicon tricarbide
* Thiocyanic acid
* Thioformaldehyde
* Tricarbon monosulfide
* Tricarbon monoxide

Five
atoms|

* Ammonium ion
* Butadiynyl
* Carbodiimide
* Cyanamide
* Cyanoacetylene
* Cyanoformaldehyde
* Cyanomethyl
* Cyclopropenylidene
* Formic acid
* Isocyanoacetylene
* Ketene
* Methane
* Methoxy radical
* Methylenimine
* Propadienylidene
* Protonated formaldehyde
* Silane
* Silicon-carbide cluster

Six
atoms|

* Acetonitrile
* Cyanobutadiynyl radical
* Cyclopropenone
* Diacetylene
* E-Cyanomethanimine
* Ethylene
* Formamide
* HC4N
* Ketenimine
* Methanethiol
* Methanol
* Methyl isocyanide
* Pentynylidyne
* Propynal
* Protonated cyanoacetylene

Seven
atoms|

* Acetaldehyde
* Acrylonitrile
* Vinyl cyanide
* Cyanodiacetylene
* Ethylene oxide
* Glycolonitrile
* Hexatriynyl radical
* Methyl isocyanate
* Methylamine
* Propyne
* Vinyl alcohol

Eight
atoms|

* Acetic acid
* Acrolein
* Aminoacetonitrile
* Cyanoallene
* Ethanimine
* Glycolaldehyde
* Hexapentaenylidene
* Methyl formate
* Methylcyanoacetylene

Nine
atoms|

* Acetamide
* Cyanohexatriyne
* Dimethyl ether
* Ethanethiol
* Ethanol
* Methyldiacetylene
* N-Methylformamide
* Octatetraynyl radical
* Propene
* Propionitrile

Ten
atoms
or more|

* Acetone
* Benzene
* Benzonitrile
* Buckminsterfullerene (C60, C60+, fullerene, buckyball)
* Butyronitrile
* C70 fullerene
* Cyanodecapentayne
* Ethyl formate
* Ethylene glycol
* Heptatrienyl radical
* Methyl acetate
* Methyl-cyano-diacetylene
* Methyltriacetylene
* Propionaldehyde
* Pyrimidine

Deuterated
molecules|

* Ammonia
* Ammonium ion
* Formaldehyde
* Formyl radical
* Heavy water
* Hydrogen cyanide
* Hydrogen deuteride
* Hydrogen isocyanide
* N2D+
* Propyne
* Trihydrogen cation

Unconfirmed|

* Anthracene
* Dihydroxyacetone
* Glycine
* Graphene
* H2NCO+
* Hemolithin
* Linear C5
* Methoxyethane
* Naphthalene cation
* Phosphine
* Pyrene
* Silylidyne

Related|

* Abiogenesis
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* Chemical formula
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* Homochirality
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* Iron–sulfur world theory
* Kerogen
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* Organic compound
* Outer space
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* Photodissociation region
* Polycyclic aromatic hydrocarbon (PAH)
* Pseudo-panspermia
* RNA world hypothesis
* Spectroscopy
* Tholin

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Nitrogen species

Hydrides|

* NH3
* NH4+
* NH2−
* N3−
* NH2OH
* N2H4
* HN3
* N3−
* NH5 (?)

Organic|

* NR3
* >C=NR
* −CONR2
* −CN
* HCN
* CN−
* (CN)2
* H2NCN
* HOCN
* HNCO
* HNCS
* CH2N2
* –NO
* –NO2

Oxides|

* NO / (NO)2
* N2O3
* HNO2 / NO−
2 / NO+
* NO2 / (NO2)2
* N2O5
* HNO3 / NO−
3 / NO+

* NO3
* HNO / (HON)2 / N2O2−
2 / N2O
* H2NNO2
* HO2NO / ONOO−
* HO2NO2 / O2NOO−
* NO3−

* H4N2O4 / N2O2−

Halides|

* NF
* NF2
* NF3
* NF5 (?)
* NCl3
* NBr3
* NI3
* FN3
* ClN3
* BrN3
* IN3
* NH2F
* N2F2
* NH2Cl
* NHF2
* NHCl2
* NHBr2
* NHI2

Oxidation states|

−3, −2, −1, 0, +1, +2, +3, +4, +5 (a strongly acidic oxide)

* v
* t
* e

Salts and covalent derivatives of the nitride ion

| NH3
N2H4

HN2−
H2N− |  |  |  | He(N2)11

|
|
|
|

Li3N
LiN3 | Be3N2
Be(N3)2 | BN
-B | C4N2
C2N2
β-C3N4
g-C3N4
CxNy | N2 | NxOy
+O | N3F
N2F2
N2F4
NF3
+F | Ne
Na3N
NaN3 | Mg3N2
Mg(N3)2 | AlN | Si3N4
-Si | PN
P3N5
-P | SxNy

S2N2
S4N4
SN2H2 | NCl3
ClN3
+Cl | Ar
K3N
KN3 | Ca3N2
Ca(N3)2 |  | ScN | TiN
Ti3N4 | VN | CrN
Cr2N | MnxNy | FexNy | Co3N | Ni3N | Cu3N | Zn3N2 | GaN | Ge3N4
-Ge | AsN
+As | Se4N4 | Br3N
BrN3
+Br | Kr
RbN3 | Sr3N2
Sr(N3)2 |  | YN | ZrN | NbN | β-Mo2N | Tc  | Ru  | Rh  | PdN | Ag3N | Cd3N2 | InN | Sn  | SbN | Te4N4?  | I3N
IN3
+I | Xe
CsN3 | Ba3N2
Ba(N3)2 | *  | LuN | HfN
Hf3N4 | TaN | WN | RexNy | Os  | Ir  | Pt  | Au  | Hg3N2 | Tl3N | (PbNH) | BiN | Po  | At  | Rn
Fr  | Ra3N2 | **  | Lr  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og

*  | LaN | CeN | PrN | NdN | PmN | SmN | EuN | GdN | TbN | DyN | HoN | ErN | TmN | YbN
**  | Ac  | ThxNy | PaN | UxNy | NpN | PuN | AmN | CmN | BkN | Cf  | Es  | Fm  | Md  | No
*[CID]: Compound ID
*[EPA]: U.S. Environmental Protection Agency
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