Chemistry:4-Nitroaniline

From HandWiki
Revision as of 01:42, 16 March 2024 by Jworkorg (talk | contribs) (link)
(diff) ← Older revision | Latest revision (diff) | Newer revision → (diff)
4-Nitroaniline
Skeletal formula of p-nitroaniline
Ball-and-stick model of the p-nitroaniline molecule
P-nitroanilin.jpg
Names
Preferred IUPAC name
4-Nitroaniline
Systematic IUPAC name
4-Nitrobenzenamine
Other names
p-Nitroaniline
1-Amino-4-nitrobenzene
p-Nitrophenylamine
Identifiers
3D model (JSmol)
508690
ChEBI
ChEMBL
ChemSpider
EC Number
  • 202-810-1
27331
KEGG
RTECS number
  • BY7000000
UNII
UN number 1661
Properties
C6H6N2O2
Molar mass 138.12 g/mol
Appearance yellow or brown powder
Odor faint, ammonia-like
Density 1.437 g/ml, solid
Melting point 146 to 149 °C (295 to 300 °F; 419 to 422 K) (lit.)
Boiling point 332 °C (630 °F; 605 K)
0.8 mg/ml at 18.5 °C (IPCS)
Vapor pressure 0.00002 mmHg (20°C)[1]
-66.43·10−6 cm3/mol
Hazards
Main hazards Toxic
Safety data sheet JT Baker
GHS pictograms GHS06: ToxicGHS08: Health hazard
GHS Signal word Warning
H301, H311, H331, H373, H412
P260, P261, P264, P270, P271, P273, P280, P301+310, P302+352, P304+340, P311, P312, P314, P321, P322, P330, P361, P363, P403+233, P405, P501
NFPA 704 (fire diamond)
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
1
2
0
Flash point 199 °C (390 °F; 472 K)
Lethal dose or concentration (LD, LC):
3249 mg/kg (rat, oral)
750 mg/kg (rat, oral)
450 mg/kg (guinea pig, oral)
810 mg/kg (mouse, oral)[2]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 6 mg/m3 (1 ppm) [skin][1]
REL (Recommended)
 TWA 3 mg/m3 [skin][1]
IDLH (Immediate danger)
 300 mg/m3[1]
Related compounds
Related compounds
 2-Nitroaniline, 3-Nitroaniline
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is ☑Y☒N ?)
Infobox references
Tracking categories (test):

4-Nitroaniline, p-nitroaniline or 1-amino-4-nitrobenzene is an organic compound with the formula C6H6N2O2. A yellow solid, it is one of three isomers of nitroaniline. It is an intermediate in the production of dyes, antioxidants, pharmaceuticals, gasoline, gum inhibitors, poultry medicines, and as a corrosion inhibitor.[3]

Synthesis

4-Nitroaniline is produced industrially via the amination of 4-nitrochlorobenzene:[3]

ClC6H4NO2 + 2 NH3 → H2NC6H4NO2 + NH4Cl

Below is a laboratory synthesis of 4-nitroaniline from aniline. The key step in this reaction sequence is an electrophilic aromatic substitution to install the nitro group para to the amino group. The amino group can be easily protonated and become a meta director. Therefore, a protection of the acetyl group is required. After this reaction, a separation must be performed to remove 2-nitroaniline, which is also formed in a small amount during the reaction.[4]
Synthesis of nitroaniline.svg

Applications

4-Nitroaniline is mainly consumed industrially as a precursor to p-phenylenediamine, an important dye component. The reduction is effected using iron metal and by catalytic hydrogenation.[3]

It is a starting material for the synthesis of Para Red, the first azo dye:[5]

Synthesis of Para Red

Laboratory use

Nitroaniline undergoes diazotization, which allows access to 1,4-dinitrobenzene[6] and nitrophenylarsonic acid.[7] With phosgene, it converts to 4-nitrophenylisocyanate.[8] [9]

Carbon snake demonstration

When heated with sulfuric acid, it dehydrates and polymerizes explosively into a rigid foam.[10]

In Carbon snake demo, paranitroaniline can be used instead of sugar, if the experiment is allowed to proceed under an obligatory fumehood.[11] With this method the reaction phase prior to the black snake's appearance is longer, but once complete, the black snake itself rises from the container very rapidly.[12] This reaction may cause an explosion if too much sulfuric acid is used.[13]

Toxicity

The compound is toxic by way of inhalation, ingestion, and absorption, and should be handled with care. Its -1">50 in rats is 750.0 mg/kg when administered orally. 4-Nitroaniline is particularly harmful to all aquatic organisms, and can cause long-term damage to the environment if released as a pollutant.[14]

See also

References

  1. ↑ 1.0 1.1 1.2 1.3 NIOSH Pocket Guide to Chemical Hazards. "#0449". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0449.html. 
  2. ↑ "p-Nitroaniline". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/100016.html. 
  3. ↑ 3.0 3.1 3.2 Booth, Gerald (2003-03-11). "Nitro Compounds, Aromatic". in Wiley-VCH (in en). Ullmann's Encyclopedia of Industrial Chemistry (1 ed.). Wiley. doi:10.1002/14356007.a17_411. ISBN 978-3-527-30385-4. https://onlinelibrary.wiley.com/doi/abs/10.1002/14356007.a17_411. ]
  4. ↑ Mohrig, J.R.; Morrill, T.C.; Hammond, C.N.; Neckers, D.C. (1997). "Synthesis 5: Synthesis of the Dye Para Red from Aniline". Experimental Organic Chemistry. New York, NY: Freeman. pp. 456–467. http://web.centre.edu/muzyka/organic/lab/paraRed05.htm. Retrieved 2007-07-18. 
  5. ↑ Williamson, Kenneth L. (2002). Macroscale and Microscale Organic Experiments, Fourth Edition. Houghton-Mifflin. ISBN 0-618-19702-8. https://archive.org/details/macroscalemicros00will_0. 
  6. ↑ Starkey, E. B. (1939). "p-DINITROBENZENE". Organic Syntheses 19: 40. doi:10.15227/orgsyn.019.0040. http://orgsyn.org/demo.aspx?prep=CV2P0225. 
  7. ↑ "p-NITROPHENYLARSONIC ACID". Organic Syntheses 26: 60. 1946. doi:10.15227/orgsyn.026.0060. http://orgsyn.org/demo.aspx?prep=CV3P0665. 
  8. ↑ Shriner, R. L.; Horne, W. H.; Cox, R. F. B. (1934). "p-NITROPHENYL ISOCYANATE". Organic Syntheses 14: 72. doi:10.15227/orgsyn.014.0072. http://orgsyn.org/demo.aspx?prep=CV2P0453. 
  9. ↑ "2,6-DIIODO-p-NITROANILINE". Organic Syntheses 12: 28. 1932. doi:10.15227/orgsyn.012.0028. http://orgsyn.org/demo.aspx?prep=CV2P0196. 
  10. ↑ Poshkus, A. C.; Parker, J. A. (1970). "Studies on nitroaniline–sulfuric acid compositions: Aphrogenic pyrostats". Journal of Applied Polymer Science 14 (8): 2049–2064. doi:10.1002/app.1970.070140813. https://onlinelibrary.wiley.com/doi/10.1002/app.1970.070140813. 
  11. ↑ Summerlin, Lee R.; Ealy, James L. (1988). "Experiment 100: Dehydration of p-Nitroaniline: Sanke and Puff". Chemical Demonstrations: A Sourcebook for Teachers Volume 1 (2nd ed.). American Chemical Society. pp. 171. ISBN 978-0-841-21481-1. https://eric.ed.gov/?id=ED286722. 
  12. ↑ "Carbon Snake: demonstrating the dehydration power of concentrated sulfuric acid" (in en). 2013-06-06. https://communities.acs.org/t5/Educators-and-Students/Carbon-Snake-demonstrating-the-dehydration-power-of-concentrated/td-p/7732. 
  13. ↑ (in en) Making a carbon snake with P-Nitroaniline, https://www.youtube.com/watch?v=YKHUnHDphTc, retrieved 2022-01-31 
  14. ↑ "4-Nitroaniline". St. Louis, Missouri: Sigma-Aldrich. December 18, 2020. https://www.sigmaaldrich.com/SG/en/sds/aldrich/185310. 

External links



Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:4-Nitroaniline&oldid=3719497"