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{{Short description|Anion with formula OCN and charge –1}} | |||
The '''cyanate''' ] is an ] consisting of one ] ], one ] atom, and one ] atom (OCN<sup>−</sup>), in that order, and possesses 1 unit of negative ], borne mainly by the nitrogen atom. In ]s the '''cyanate group''' is a ]. | |||
{{Distinguish|fulminate}} | |||
] of the cyanate anion]] | |||
The structure of cyanate is resonant between these two structures: | |||
:O<sup>−</sup> − C ≡ N and O = C = N<sup>−</sup> | |||
The cyanate ion is isoelectronic with ], and so shares its linear shape. | |||
The '''cyanate ion''' is an ] with the ] {{chem2|OCN-}}. It is a ] of three forms: {{chem2|}} (61%) ↔ {{chem2|}} (30%) ↔ {{chem2|}} (4%). | |||
The cyanate ion is an ] in ] because it can react to form an alkyl cyanate R-OCN (exception) or an alkyl ] R-NCO (rule). ] cyanates (C<sub>6</sub>H<sub>5</sub>OCN) can be formed by a reaction of ] with ] (ClCN) in the presence of a base. | |||
Cyanate is the derived anion of ], H−N=C=O, and its lesser ] cyanic acid (a.k.a. cyanol), H−O−C≡N. | |||
'''Cyanates''' are salts of ] for example ] (KNCO). | |||
Any salt containing the ion, such as ], is called a cyanate. | |||
The ''cyanate'' ion is relatively non-toxic in comparison to cyanides. Use of this fact is made in cyanide decontamination processes where a permanganate oxidation converts toxic cyanide to cyanate. | |||
The cyanate ion is an ] of the much-less-stable ] anion, {{chem2|CNO-}} or {{chem2|}}.<ref name=mart2019>William R. Martin and David W. Ball (2019): "Small organic fulminates as high-energy materials. Fulminates of acetylene, ethylene, and allene". ''Journal of Energetic Materials'', volume 31, issue 7, pages 70-79. {{doi|10.1080/07370652.2018.1531089}}</ref> | |||
The ] ion has the same formula but different structure. | |||
The cyanate ion is an ], forming ] with a metal ion in which either the nitrogen or oxygen atom may be the ]. It can also act as a ]. | |||
{{Functional Groups}} | |||
Compounds that contain the '''cyanate ]''', −O−C≡N, are known as cyanates or ]s. The cyanate functional group is distinct from the ] functional group, −N=C=O; the ] functional group, {{chem2|\sO\sN+\tC-}}; and the ] functional group, {{chem2|\sCNO}} or {{chem2|\sC\tN+\sO-}}. | |||
{{inorganic-compound-stub}} | |||
==Cyanate ion== | |||
] | |||
The three atoms in a cyanate ion lie on a straight line, giving the ion a linear structure. The ] is described most simply as | |||
] | |||
: :Ö̤−C≡N: | |||
] | |||
with a single C−O bond and a triple C≡N bond. (Or more completely as :Ö̤−C≡N: ↔ Ö̤=C=N̤̈ ↔ :O≡C−N̤̈:) The ] of a cyanate salt has a band at ca. 2096 cm<sup>−1</sup>; such a high frequency is characteristic of a ].<ref>Nakamoto, Part A, p171</ref> | |||
The cyanate ion is a ]. Both the oxygen and nitrogen atoms carry a ] of electrons and either one, the other, or both can be donated to ] acceptors. It can be described as an ]. | |||
] | |||
==Cyanate salts== | |||
] is ] with sodium ], confirming the linear structure of the cyanate ion.<ref>Wells, p722.</ref> It is made industrially by heating a mixture of ] and ].<ref>Greenwood, p324</ref> | |||
:{{chem2|Na2CO3 + 2 OC(NH2)2 -> 2 NaNCO + CO2 + 2 NH3 + H2O}} | |||
A similar reaction is used to make ]. Cyanates are produced when ]s are oxidized. Use of this fact is made in cyanide decontamination processes where oxidants such as ] and ] are used to convert toxic cyanide into less-toxic cyanate. | |||
{|class="wikitable" | |||
!Name | |||
!formula | |||
!Crystal system | |||
!Space group | |||
!Unit cell (Å) | |||
!volume (Å<sup>3</sup>) | |||
!Density (g/cm<sup>3</sup>) | |||
!Comment | |||
!Reference | |||
|- | |||
|] | |||
|NH<sub>4</sub>OCN | |||
|tetragonal | |||
|P4/nmm | |||
|''a''=5.082 ''b''=5.082 ''c''=5.551 | |||
| | |||
| | |||
|decomposes when heated to ] | |||
|<ref>{{cite journal|title=Ammonium cyanate shows N-H···N hydrogen bonding, not N-H···O|author1=MacLean, Elizabeth J. |author2=Harris, Kenneth D. M. |author3=Kariuki, Benson M. |author4=Kitchin, Simon J. |author5=Tykwinski, Rik R. |author6=Swainson, Ian P. |author7=] |author8=Jack D.|journal= Journal of the American Chemical Society|year=2003|volume=125|pages=14449–14451|doi=10.1021/ja021156x|pmid=14624593 }}</ref> | |||
|- | |||
|] | |||
|LiOCN | |||
|trigonal | |||
|''R''{{overline|3}}''m'' | |||
|''a'' = 3.230 ''b'' = 14.268 Z=3 | |||
|128.90 | |||
|1.895 | |||
|melts at 475 °C | |||
|<ref>{{cite journal |author1=Erik Hennings |author2=Horst Schmidt |author3=Wolfgang Voigt |title=Structure and Thermal Properties of Lithium Cyanate |journal=Zeitschrift für anorganische und allgemeine Chemie |date=2011 |volume=637 |issue=9 |pages=1199–1202 |doi=10.1002/zaac.201100081 |language=en}}</ref> | |||
|- | |||
|] | |||
|NaOCN | |||
|hexagonal | |||
|''R''{{overline|3}}''m'' | |||
|''a'' = 3.568 ''c'' = 15.123 | |||
|166.72 | |||
|1.94 | |||
|melts at 550 °C | |||
|<ref>{{cite journal |author1=Olaf Reckeweg |author2=Armin Schulz |author3=Brian Leonard |author4=Francis J. DiSalvo |title=Single-Crystal X-Ray Diffraction Study of Na at 170 K and its Vibrational Spectra |journal=Zeitschrift für Naturforschung B |date=2010 |volume=65 |issue=4 |pages=528–532 |doi=10.1515/znb-2010-0416 |language=en|doi-access=free }}</ref> | |||
|- | |||
|] | |||
|KOCN | |||
|tetragonal | |||
|''I''4/''mcm'' | |||
|''a'' = 6.091 ''c'' = 7.052 | |||
|261.6 | |||
|2.056 | |||
|melts at 315 °C | |||
|<ref>{{cite journal |author1=Hiroki Nambu |author2=Mizuhiko Ichikawa |author3=Torbjörn Gustafsson |author4=Ivar Olovsson |title=X-ray diffraction study of KOCN at room temperature |journal=Journal of Physics and Chemistry of Solids |date=2003 |volume=64 |issue=11 |pages=2269–2272 |doi=10.1016/S0022-3697(03)00258-0 |language=en}}</ref> | |||
|- | |||
|] | |||
|RbOCN | |||
|tetragonal | |||
|''I''4/''mcm'' | |||
|''a'' = 6.35 ''c'' = 7.38 | |||
|297.58 | |||
|2.85 | |||
| | |||
|<ref name=inorg>T. C. Waddington "Lattice parameters and infrared spectra of some inorganic cyanates" J. Chem. Soc., 1959, 2499-2502. {{doi|10.1039/JR9590002499}}</ref> | |||
|- | |||
|] | |||
|CsOCN | |||
|tetragonal | |||
|''I''4''mcm'' | |||
|''a'' = 6.519 ''c'' = 7.994 | |||
|339.68 | |||
|3.42 | |||
| | |||
|<ref>{{cite journal |author1=Olaf Reckeweg |author2=Armin Schulz |author3=Francis J. DiSalvo |title=Structural characterization and Raman spectrum of Cs |journal=Zeitschrift für Naturforschung B |date=2020 |volume=75 |issue=1–2 |pages=129–133 |doi=10.1515/znb-2019-0168 |language=en|doi-access=free }}</ref> | |||
|- | |||
|] | |||
|TlOCN | |||
|tetragonal | |||
|''I''4''mcm'' | |||
|''a'' = 6.23 ''c'' = 7.32 | |||
|284.3 | |||
|5.76 | |||
| | |||
|<ref name="inorg" /> | |||
|- | |||
|] | |||
|AgOCN | |||
|monoclinic | |||
|''P''2<sub>1</sub>/''m'' | |||
|''a'' = 5.474 ''b'' = 6.378 ''c'' = 3.417 ''β'' = 90.931° | |||
|119.29 | |||
|4.173 | |||
|melts at 652 °C | |||
|<ref>{{cite journal |author1=D.J. Williams |author2=S.C. Vogel |author3=L.L. Daemen |title=Neutron diffraction study of cyanate ligand order/disorder in AgNCO at 300–50K |journal=Physica B: Condensed Matter |date=2006 |volume=385-386 |issue=1 |pages=228–230 |doi=10.1016/j.physb.2006.05.197 |language=en}}</ref> | |||
|- | |||
|] | |||
|Sr(OCN)<sub>2</sub> | |||
|orthorhombic | |||
|''Fddd'' | |||
|''a'' = 6.151 ''b'' = 11.268 ''c'' = 11.848 Z = 8 | |||
|821.1 | |||
|2.78 | |||
| | |||
|<ref name="Sreu">{{cite journal |author1=Sandro Pagano |author2=Giuseppe Montana |author3=Claudia Wickleder |author4=Wolfgang Schnick |title=Urea Route to Homoleptic Cyanates—Characterization and Luminescence Properties of and M(OCN)2 with M=Sr, Eu |journal=Chemistry: A European Journal |date=2009 |volume=15 |issue=25 |pages=6186–6193 |doi=10.1002/chem.200900053 |language=en|doi-access=free |pmid=19444832 }}</ref> | |||
|- | |||
|} | |||
==Complexes with the cyanate ion== | |||
Cyanate is an ] which can donate the pair of electrons on the nitrogen atom or the oxygen atom, or both. Structurally the isomers can be distinguished by the geometry of the complex. In ''N''-bonded cyanate complexes the M−NCO unit sometimes has a linear structure, but with ''O''-bonded cyanate the M−O−C unit is bent. Thus, the silver cyanato complex, {{chem2|−}}, has a linear structure as shown by ].<ref name=ChemicalElements>{{Greenwood&Earnshaw2nd|page=325}} (click )</ref> However, the crystal structure of ] shows zigzag chains of nitrogen atoms and silver atoms.<ref>{{cite journal |url=https://scripts.iucr.org/cgi-bin/paper?a04540 |first1=D. |last1=Britton |first2=J. D. |last2=Dunitz |title=The crystal structure of silver cyanate |journal=Acta Crystallographica |date=1965 |volume=18 |issue=3 |pages=424–428 |doi=10.1107/S0365110X65000944 |doi-access=free}}</ref> There also exists a structure | |||
NCO | |||
/ \ | |||
Ni Ni | |||
\ / | |||
OCN | |||
in which the Ni-N-C group is bent.<ref name=ChemicalElements/> | |||
] has been used extensively to distinguish between isomers. Many complexes of ] metals are ''N''-bonded. ''O''-Bonding has been suggested for complexes of the type {{chem2|^{''n''−}|}}, M = Mo(III), Re(IV), and Re(V). The yellow complex {{chem2|Rh(])3(NCO)}} and orange complex {{chem2|Rh(])3(OCN)}} are ] and show differences in their infrared spectra which can be used for diagnosis.<ref name=cno>Nakamoto, Part B, pp 121–123.</ref> | |||
The cyanate ion can bridge between two metal atoms by using both its donor atoms. For example, this structure is found in the compound {{chem2|])2](])2}}. In this compound both the Ni−N−C unit and Ni−O−C unit are bent, even though in the first case donation is through the nitrogen atom.<ref>Greenwood, Table 8.9</ref> | |||
==Cyanate functional group== | |||
Compounds that contain the cyanate ], −O−C≡N, are known as cyanates or ]s. ] cyanates such are phenyl cyanate, {{chem2|C6H5OCN}} can be formed by a reaction of ] with ], ClCN, in the presence of a base. | |||
]s that contain the isocyanate ] −N=C=O are known as ]s. It is conventional in ] to write isocyanates with two double bonds, which accords with a simplistic ] of the bonding. In ] reactions cyanate usually forms an isocyanate. Isocyanates are widely used in the manufacture of ]<ref name=Seymour>{{cite journal |last1=Seymour |first1=Raymond B. |author-link2=George B. Kauffman |last2=Kauffman |first2=George B. |year=1992 |title=Polyurethanes: A Class of Modern Versatile Materials |journal=] |volume=69 |issue=11 |page=909 |doi=10.1021/ed069p909 |bibcode=1992JChEd..69..909S}}</ref> products and ]s; ], used to make pesticides, was a major factor in the ]. | |||
==See also== | |||
* ], {{chem2|CN-}} and ] group, −C≡N | |||
* ] or isonitrile group, −N≡C | |||
* ], {{chem2|SCN-}}, −S−C≡N | |||
* ], {{chem2|SeCN-}}, −Se−C≡N | |||
* ], {{chem2|TeCN-}}, −Te−C≡N | |||
* ] group, −N=C=O | |||
* ] group, −N=C=S | |||
* ] group, −N=C=Se | |||
==References== | |||
{{Reflist}} | |||
==External links== | |||
* | |||
==Bibliography== | |||
*{{Greenwood&Earnshaw2nd}} | |||
*{{cite book|last=Nakamoto|first=K.|title=Infrared and Raman spectra of Inorganic and Coordination compounds|edition=5th|series=Part A|year=1997|publisher=Wiley|isbn=0-471-16394-5}} | |||
*{{cite book|last=Nakamoto|first=K.|title=Infrared and Raman spectra of Inorganic and Coordination compounds|edition=5th|series=Part B|year=1997|publisher=Wiley|isbn=0-471-16392-9}} | |||
*{{cite book|last=Wells|first=A.F|title=Structural Inorganic Chemistry|edition=3rd.|year=1962|publisher=Clarendon Press|location=Oxford|isbn=0-19-855125-8}} | |||
{{Cyanates}} | |||
{{Inorganic compounds of carbon}} | |||
{{Nitrogen compounds}} | |||
{{Functional groups}} | |||
] | |||
] | |||
] |
Latest revision as of 08:48, 15 December 2024
Anion with formula OCN and charge –1 Not to be confused with fulminate.The cyanate ion is an anion with the chemical formula OCN. It is a resonance of three forms: [O−C≡N] (61%) ↔ [O=C=N] (30%) ↔ [O≡C−N] (4%).
Cyanate is the derived anion of isocyanic acid, H−N=C=O, and its lesser tautomer cyanic acid (a.k.a. cyanol), H−O−C≡N.
Any salt containing the ion, such as ammonium cyanate, is called a cyanate.
The cyanate ion is an isomer of the much-less-stable fulminate anion, CNO or [C≡N−O].
The cyanate ion is an ambidentate ligand, forming complexes with a metal ion in which either the nitrogen or oxygen atom may be the electron-pair donor. It can also act as a bridging ligand.
Compounds that contain the cyanate functional group, −O−C≡N, are known as cyanates or cyanate esters. The cyanate functional group is distinct from the isocyanate functional group, −N=C=O; the fulminate functional group, −O−N≡C; and the nitrile oxide functional group, −CNO or −C≡N−O.
Cyanate ion
The three atoms in a cyanate ion lie on a straight line, giving the ion a linear structure. The electronic structure is described most simply as
- :Ö̤−C≡N:
with a single C−O bond and a triple C≡N bond. (Or more completely as :Ö̤−C≡N: ↔ Ö̤=C=N̤̈ ↔ :O≡C−N̤̈:) The infrared spectrum of a cyanate salt has a band at ca. 2096 cm; such a high frequency is characteristic of a triple bond.
The cyanate ion is a Lewis base. Both the oxygen and nitrogen atoms carry a lone pair of electrons and either one, the other, or both can be donated to Lewis acid acceptors. It can be described as an ambidentate ligand.
Cyanate salts
Sodium cyanate is isostructural with sodium fulminate, confirming the linear structure of the cyanate ion. It is made industrially by heating a mixture of sodium carbonate and urea.
- Na2CO3 + 2 OC(NH2)2 → 2 NaNCO + CO2 + 2 NH3 + H2O
A similar reaction is used to make potassium cyanate. Cyanates are produced when cyanides are oxidized. Use of this fact is made in cyanide decontamination processes where oxidants such as permanganate and hydrogen peroxide are used to convert toxic cyanide into less-toxic cyanate.
Name | formula | Crystal system | Space group | Unit cell (Å) | volume (Å) | Density (g/cm) | Comment | Reference |
---|---|---|---|---|---|---|---|---|
Ammonium cyanate | NH4OCN | tetragonal | P4/nmm | a=5.082 b=5.082 c=5.551 | decomposes when heated to urea | |||
Lithium cyanate | LiOCN | trigonal | R3m | a = 3.230 b = 14.268 Z=3 | 128.90 | 1.895 | melts at 475 °C | |
Sodium cyanate | NaOCN | hexagonal | R3m | a = 3.568 c = 15.123 | 166.72 | 1.94 | melts at 550 °C | |
Potassium cyanate | KOCN | tetragonal | I4/mcm | a = 6.091 c = 7.052 | 261.6 | 2.056 | melts at 315 °C | |
Rubidium cyanate | RbOCN | tetragonal | I4/mcm | a = 6.35 c = 7.38 | 297.58 | 2.85 | ||
Cesium cyanate | CsOCN | tetragonal | I4mcm | a = 6.519 c = 7.994 | 339.68 | 3.42 | ||
Thallium cyanate | TlOCN | tetragonal | I4mcm | a = 6.23 c = 7.32 | 284.3 | 5.76 | ||
Silver cyanate | AgOCN | monoclinic | P21/m | a = 5.474 b = 6.378 c = 3.417 β = 90.931° | 119.29 | 4.173 | melts at 652 °C | |
Strontium cyanate | Sr(OCN)2 | orthorhombic | Fddd | a = 6.151 b = 11.268 c = 11.848 Z = 8 | 821.1 | 2.78 |
Complexes with the cyanate ion
Cyanate is an ambidentate ligand which can donate the pair of electrons on the nitrogen atom or the oxygen atom, or both. Structurally the isomers can be distinguished by the geometry of the complex. In N-bonded cyanate complexes the M−NCO unit sometimes has a linear structure, but with O-bonded cyanate the M−O−C unit is bent. Thus, the silver cyanato complex, [Ag(NCO)2], has a linear structure as shown by X-ray crystallography. However, the crystal structure of silver cyanate shows zigzag chains of nitrogen atoms and silver atoms. There also exists a structure
NCO / \ Ni Ni \ / OCN
in which the Ni-N-C group is bent.
Infrared spectroscopy has been used extensively to distinguish between isomers. Many complexes of divalent metals are N-bonded. O-Bonding has been suggested for complexes of the type [M(OCN)6], M = Mo(III), Re(IV), and Re(V). The yellow complex Rh(PPh3)3(NCO) and orange complex Rh(PPh3)3(OCN) are linkage isomers and show differences in their infrared spectra which can be used for diagnosis.
The cyanate ion can bridge between two metal atoms by using both its donor atoms. For example, this structure is found in the compound [Ni2(NCO)2(En)2](BPh4)2. In this compound both the Ni−N−C unit and Ni−O−C unit are bent, even though in the first case donation is through the nitrogen atom.
Cyanate functional group
Compounds that contain the cyanate functional group, −O−C≡N, are known as cyanates or cyanate esters. Aryl cyanates such are phenyl cyanate, C6H5OCN can be formed by a reaction of phenol with cyanogen chloride, ClCN, in the presence of a base.
Organic compounds that contain the isocyanate functional group −N=C=O are known as isocyanates. It is conventional in organic chemistry to write isocyanates with two double bonds, which accords with a simplistic valence bond theory of the bonding. In nucleophilic substitution reactions cyanate usually forms an isocyanate. Isocyanates are widely used in the manufacture of polyurethane products and pesticides; methyl isocyanate, used to make pesticides, was a major factor in the Bhopal disaster.
See also
- Cyanide, CN and nitrile group, −C≡N
- Isocyanide or isonitrile group, −N≡C
- Thiocyanate, SCN, −S−C≡N
- Selenocyanate, SeCN, −Se−C≡N
- Tellurocyanate, TeCN, −Te−C≡N
- Isocyanate group, −N=C=O
- Isothiocyanate group, −N=C=S
- Isoselenocyanate group, −N=C=Se
References
- William R. Martin and David W. Ball (2019): "Small organic fulminates as high-energy materials. Fulminates of acetylene, ethylene, and allene". Journal of Energetic Materials, volume 31, issue 7, pages 70-79. doi:10.1080/07370652.2018.1531089
- Nakamoto, Part A, p171
- Wells, p722.
- Greenwood, p324
- MacLean, Elizabeth J.; Harris, Kenneth D. M.; Kariuki, Benson M.; Kitchin, Simon J.; Tykwinski, Rik R.; Swainson, Ian P.; Dunitz; Jack D. (2003). "Ammonium cyanate shows N-H···N hydrogen bonding, not N-H···O". Journal of the American Chemical Society. 125: 14449–14451. doi:10.1021/ja021156x. PMID 14624593.
- Erik Hennings; Horst Schmidt; Wolfgang Voigt (2011). "Structure and Thermal Properties of Lithium Cyanate". Zeitschrift für anorganische und allgemeine Chemie. 637 (9): 1199–1202. doi:10.1002/zaac.201100081.
- Olaf Reckeweg; Armin Schulz; Brian Leonard; Francis J. DiSalvo (2010). "Single-Crystal X-Ray Diffraction Study of Na[OCN] at 170 K and its Vibrational Spectra". Zeitschrift für Naturforschung B. 65 (4): 528–532. doi:10.1515/znb-2010-0416.
- Hiroki Nambu; Mizuhiko Ichikawa; Torbjörn Gustafsson; Ivar Olovsson (2003). "X-ray diffraction study of KOCN at room temperature". Journal of Physics and Chemistry of Solids. 64 (11): 2269–2272. doi:10.1016/S0022-3697(03)00258-0.
- ^ T. C. Waddington "Lattice parameters and infrared spectra of some inorganic cyanates" J. Chem. Soc., 1959, 2499-2502. doi:10.1039/JR9590002499
- Olaf Reckeweg; Armin Schulz; Francis J. DiSalvo (2020). "Structural characterization and Raman spectrum of Cs[OCN]". Zeitschrift für Naturforschung B. 75 (1–2): 129–133. doi:10.1515/znb-2019-0168.
- D.J. Williams; S.C. Vogel; L.L. Daemen (2006). "Neutron diffraction study of cyanate ligand order/disorder in AgNCO at 300–50K". Physica B: Condensed Matter. 385–386 (1): 228–230. doi:10.1016/j.physb.2006.05.197.
- Sandro Pagano; Giuseppe Montana; Claudia Wickleder; Wolfgang Schnick (2009). "Urea Route to Homoleptic Cyanates—Characterization and Luminescence Properties of [M(OCN)2(urea)] and M(OCN)2 with M=Sr, Eu". Chemistry: A European Journal. 15 (25): 6186–6193. doi:10.1002/chem.200900053. PMID 19444832.
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 325. ISBN 978-0-08-037941-8. (click here)
- Britton, D.; Dunitz, J. D. (1965). "The crystal structure of silver cyanate". Acta Crystallographica. 18 (3): 424–428. doi:10.1107/S0365110X65000944.
- Nakamoto, Part B, pp 121–123.
- Greenwood, Table 8.9
- Seymour, Raymond B.; Kauffman, George B. (1992). "Polyurethanes: A Class of Modern Versatile Materials". J. Chem. Educ. 69 (11): 909. Bibcode:1992JChEd..69..909S. doi:10.1021/ed069p909.
External links
Bibliography
- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- Nakamoto, K. (1997). Infrared and Raman spectra of Inorganic and Coordination compounds. Part A (5th ed.). Wiley. ISBN 0-471-16394-5.
- Nakamoto, K. (1997). Infrared and Raman spectra of Inorganic and Coordination compounds. Part B (5th ed.). Wiley. ISBN 0-471-16392-9.
- Wells, A.F (1962). Structural Inorganic Chemistry (3rd. ed.). Oxford: Clarendon Press. ISBN 0-19-855125-8.
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Inorganic compounds of carbon and related ions | |
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Compounds | |
Carbon ions | |
Nanostructures | |
Oxides and related |
Nitrogen species | |
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Hydrides | |
Organic | |
Oxides | |
Halides | |
Oxidation states | −3, −2, −1, 0, +1, +2, +3, +4, +5 (a strongly acidic oxide) |
Functional groups | |||||||||||||||
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Hydrocarbons (only C and H) | |||||||||||||||
Only carbon, hydrogen, and oxygen (only C, H and O) |
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Only one element, not being carbon, hydrogen, or oxygen (one element, not C, H or O) |
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Other | |||||||||||||||