Chemistry:Chromium trioxide

From HandWiki
Chromium trioxide
Ball-and-stick model of chromium trioxide
  Chromium, Cr
  Oxygen, O
Powder of chromium trioxide
Names
IUPAC name
Chromium trioxide
Other names
Chromic anhydride, Chromium(VI) oxide, Chromic acid (misnomer)
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
RTECS number
  • GB6650000
UNII
UN number 1463
Properties
CrO3
Molar mass 99.993 g·mol−1
Appearance Dark red granular solid, deliquescent
Odor Odorless
Density 2.7 g/cm3 (20 °C)[1]
Melting point 197 °C (387 °F; 470 K)[1]
Boiling point 250 °C (482 °F; 523 K)
decomposes[1]
  • 164.8 g/(100 mL) (0 °C)
  • 169 g/(100 mL) (25 °C)[1]
  • 172.6 g/(100 mL) (40 °C)
  • 198.1 g/(100 mL) (100 °C)[2]
Solubility Soluble in H
2SO
4, HNO
3, (CH
3CH
2)
2O, CH
3COOH, (CH
3)
2CO
+40·10−6 cm3/mol[1]
Thermochemistry
73.2 J/(mol·K)[3]
−589.3 kJ/mol[4]
Hazards
Safety data sheet ICSC 1194
GHS pictograms GHS03: OxidizingGHS05: CorrosiveGHS06: ToxicGHS08: Health hazardGHS09: Environmental hazard[5]
GHS Signal word Danger
H271, H301+311Script error: No such module "Preview warning".Category:GHS errors, H314, H317, H330, H334, H335, H340, H350, H361f, H372, H410[5]
P210, P260, P280, P303+361+353, P304+340+310, P305+351+338[5]
NFPA 704 (fire diamond)
Lethal dose or concentration (LD, LC):
80 mg/kg (rats, oral)[6]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
Infobox references
Tracking categories (test):

Chromium trioxide (also known as chromium(VI) oxide or chromic anhydride) is an inorganic compound with the formula CrO
3. It is the acidic anhydride of chromic acid, and is sometimes marketed under the same name.[6] This compound is a dark-purple solid under anhydrous conditions and bright orange when wet. The substance dissolves in water concomitant with hydrolysis.[clarification needed] Millions of kilograms are produced annually, mainly for electroplating.[7] Chromium trioxide is a powerful oxidiser, a mutagen, and a carcinogen.[8]

Production, structure, and basic reactions

Chromium trioxide is generated by treating sodium dichromate with sulfuric acid:[6]

H
2SO
4 + Na
2Cr
2O
7 → 2 CrO
3 + Na
2SO
4 + H
2O

Approximately 100,000 tonnes are produced annually by this or similar routes.[7]

The solid consists of chains of tetrahedrally coordinated chromium atoms that share vertices. Each chromium center therefore shares two oxygen centers with neighbors. Two oxygen atoms are not shared, giving an overall stoichiometry of 1:3.[9][10]

Ball-and-stick model of chains in the crystal structure of CrO
3
  Chromium, Cr
  Oxygen, O

The structure of monomeric CrO
3 has been calculated using density functional theory, and is predicted to be pyramidal (point group C3v) rather than planar (point group D3h).[11]

Ball-and-stick model of the DFT-calculated structure of the CrO3 monomer

Chromium trioxide decomposes above 197 °C, liberating oxygen and eventually giving Cr
2O
3:

4 CrO
3 → 2 Cr
2O
3 + 3 O
2

It is used in organic synthesis as an oxidant, often as a solution in acetic acid,[9] or acetone in the case of the Jones oxidation. In these oxidations, the Cr(VI) converts primary alcohols to the corresponding carboxylic acids and secondary alcohols to ketones. The reactions are shown below:

  • Primary alcohols to carboxylic acids
    4 CrO
    3     + 3 RCH
    2    OH + 12 H+
     → 3 RCOOH + 4 Cr3+ + 9 H
    2    O
  • Secondary alcohols to ketones
    2 CrO
    3     + 3 R
    2    CHOH + 6 H+
     → 3 R
    2    C=O + 2 Cr3+ + 6 H
    2    O

Applications

Chromium trioxide is mainly used in chrome plating. It is typically employed with additives that affect the plating process but do not react with the trioxide. The trioxide reacts with cadmium, zinc, and other metals to generate passivating chromate films that resist corrosion. It is also used in the production of synthetic rubies. Chromic acid solution is also used in applying types of anodic coating to aluminium, which are primarily used in aerospace applications. On the International Space Station, it is used to control bacteria growth in the wastewater storage tank. A chromic acid/phosphoric acid solution is also the preferred stripping agent of anodic coatings of all types.

Safety

Chromium trioxide is highly toxic, corrosive, and carcinogenic.[12] It is the main example of hexavalent chromium, an environmental hazard.[13] The related chromium(III) derivatives are not particularly dangerous; thus, reductants are used to destroy chromium(VI) samples.

Chromium trioxide, being a powerful oxidizer, will ignite organic materials such as alcohols on contact.

Images

  • A concentrated solution of potassium dichromate in water.

  • Addition of sulfuric acid to the solution.

  • Crystallization of chromium trioxide from the reaction.

  • Reaction between chromium trioxide and ethanol

  • Reaction between chromium(VI) oxide and ethanol (2).JPG
  • Reaction between chromium(VI) oxide and ethanol (3).JPG

References

  1. ↑ 1.0 1.1 1.2 1.3 1.4 Lide, David R., ed (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0. 
  2. ↑ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). D. Van Nostrand Company. p. 250. https://archive.org/details/solubilitiesino01seidgoog. 
  3. ↑ "chromium(VI) oxide". http://chemister.ru/Database/properties-en.php?dbid=1&id=3425. 
  4. ↑ Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc.. ISBN 0-07-049439-8. 
  5. ↑ 5.0 5.1 5.2 Sigma-Aldrich Co., Chromium(VI) oxide. Retrieved on 2021-11-22.
  6. ↑ 6.0 6.1 6.2 6.3 "Chromium trioxide". AroKor Holdings Inc.. http://www.chemicalland21.com/industrialchem/inorganic/CHROMIUM%20TRIOXIDE.htm. 
  7. ↑ 7.0 7.1 Anger, G.; Halstenberg, J.; Hochgeschwender, K.; Scherhag, C.; Korallus, U.; Knopf, H.; Schmidt, P.; Ohlinger, M. (2000). "Chromium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a07_067. ISBN 3527306730. 
  8. ↑ Mamyrbaev, Arstan Abdramanovich; Dzharkenov, Timur Agataevich; Imangazina, Zina Amangalievna; Satybaldieva, Umit Abulkhairovna (2015-04-16). "Mutagenic and carcinogenic actions of chromium and its compounds". Environmental Health and Preventive Medicine (Springer Science and Business Media LLC) 20 (3): 159–167. doi:10.1007/s12199-015-0458-2. ISSN 1342-078X. PMID 25877777. 
  9. ↑ 9.0 9.1 Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5 
  10. ↑ Stephens, J. S.; Cruickshank, D. W. J. (1970). "The crystal structure of (CrO3)∞". Acta Crystallographica Section B 26 (3): 222. doi:10.1107/S0567740870002182. 
  11. ↑ Zhai, H. J.; Li, S.; Dixon, D. A.; Wang, L. S. (2008). "Probing the Electronic and Structural Properties of Chromium Oxide Clusters (CrO3)−n and (CrO3)n (n = 1–5): Photoelectron Spectroscopy and Density Functional Calculations". Journal of the American Chemical Society 130 (15): 5167–77. doi:10.1021/ja077984d. PMID 18327905. 
  12. ↑ "Chromium Trioxide (MSDS)". J. T. Baker. http://hazard.com/msds/mf/baker/baker/files/c4400.htm. 
  13. ↑ The environmental impact of hexavalent chromium inspired the 2000 biographical Hollywood movie Erin Brockovich.

External links



Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Chromium_trioxide&oldid=3332342"