10025-85-1

Basic information

• Product Name: Trichlorine nitride
• Synonyms: Trichlorine nitride;Nitrogen chloride;nitrogen trichloride;TRICHLORAMINE;Trichloramine: (Nitrogen chloride);Nitrogen chloride(NCl3) (6CI,7CI,8CI,9CI)
• CAS NO: 10025-85-1
• Molecular Formula: Cl₃N
• Molecular Weight: 120.3657
• EINECS: 233-045-1
• Mol File: 10025-85-1.mol
• Article Data: 16

Chemical Properties

• Melting Point: -27°C
• Boiling Point: 71°C (estimate)
• Flash Point: °C
• Appearance: /yellow oily liquid
• Density: 1.653
• Vapor Pressure: 131mmHg at 25°C
• Refractive Index: 1.492
• PKA: -22.67±0.70(Predicted)
• Water Solubility: insoluble H2O, decomposes in H2O after 24h; soluble CS2, phosphorus trichloride, benzene, CCl4, CHCl3 [MER06]
• CAS DataBase Reference: Trichlorine nitride(CAS DataBase Reference)
• NIST Chemistry Reference: Trichlorine nitride(10025-85-1)
• EPA Substance Registry System: Trichlorine nitride(10025-85-1)

Safety Data

• RIDADR: 3099
• HazardClass: 5.1
• PackingGroup: II
• Hazardous Substances Data: 10025-85-1(Hazardous Substances Data)

Usage

Chemical Properties

Yellow oil or rhombic crystals.Insoluble in cold water; decomposes in hot water; soluble in chloroform, phosphorus trichloride, and carbon disulfide.

Physical properties

Yellow, oily, heavy liquid; pungent odor; density 1.653 g/mL; freezes to rhombohedral crystalline solid below -40°C; evaporates in air rapidly; vaporpressure 150 torr at 20°C; explodes when heated at 93°C; highly unstable, decomposes explosively in light; insoluble in water, decomposes slowly in cold water after several hours; decomposes in hot water; soluble in benzene, chloroform, carbon tetrachloride, carbon disulfide and phosphorus trichloride.

Uses

Bleaching of flour; wastage control of citrus fruit.

Preparation

Nitrogen trichloride is prepared by passing chlorine gas into slightly acid solution of ammonium chloride. The product is continuously extracted with carbon tetrachloride: NH4Cl + 3Cl2 → NCl3 + 4HCl Hypochlorous acid, HOCl, also may be used instead of chlorine in such preparation. Nitrogen trichloride can be prepared by the action of anhydrous chlorine with anhydrous ammonia: 3Cl2 + NH3 → NCl3 + 3HCl Nitrogen trichloride is made commercially by electrolyzing an acidified solution of ammonium chloride.

Hazard

Explodes when heated to approximately 200F (93C) or when exposed to direct sunlight. Toxic by ingestion and inhalation, strong irritant.

Safety Profile

Moderately toxic by inhalation. An irritant to the eyes, skin, mucous membranes, and a systemic central nervous system irritant. An explosive sensitive to impact, light, and ultrasound. The solid explodes on melting. The liquid explodes above 60°C. Concentrated solutions are also explosive. Explosive decomposition is initiated by contact with: concentrated ammonia, arsenic, dinitrogen tetraoxide, hydrogen sulfide, hydrogen trisulfide, nitrogen oxide, organic matter, ozone, phosphine, phosphorus, potassium cyanide, potassium hydroxide solutions, selenium, hydrogen chloride, hydrogen fluoride, hydrogen bromide, hydrogen iodide. mxtures with chlorine + hydrogen are potentially explosive. Upon decomposition it emits toxic fumes of Cl- and NOx. See also CHLORIDES.

InChI:InChI=1/Cl3N/c1-4(2)3

Synthetic route

calcium hypochlorite (7778-54-3) + ammonium chloride (12125-02-9) → nitrogen trichloride (10025-85-1)

Conditions	Yield
With hydrogenchloride In dichloromethane; water at 4℃; for 0.75h;

ammonium chloride → nitrogen trichloride (10025-85-1) + perchlorate(1-) (14797-73-0)

Conditions	Yield
In water Electrolysis;

nitrosylchloride (2696-92-6) → nitrosoamine (81390-26-3, 35576-91-1, 81407-93-4) + nitrogen trichloride (10025-85-1)

Conditions	Yield
With ammonia In neat (no solvent) reaction of NOCl with melted NH3;;

phosphorus pentachloride (10026-13-8, 874483-75-7) + nitrosylchloride (2696-92-6) → nitrogen trichloride (10025-85-1) + trichlorophosphate (10025-87-3, 12599-09-6, 63736-95-8)

Conditions	Yield
In not given react. with NOCl;;
In not given educts are passed through a porcelain tube heated at 1000 to 1100.degreeC;; very poor yield;;
In not given heating;;
In not given educts are passed through a porcelain tube heated at 1000 to 1100.degreeC;; very poor yield;;

nitrogen (7727-37-9) + nitrogen(II) oxide (10102-43-9) + boron trichloride (10294-34-5) → nitrogen trichloride (10025-85-1) + boron monoxide (12505-77-0)

Conditions	Yield
with "active N" in presence of traces of O2;
with "active N" in presence of traces of O2;

hydrazine (302-01-2) → nitrogen trichloride (10025-85-1)

Conditions	Yield
With chlorine with chlorine excess, in presence of CCl4;
With Cl2 with chlorine excess, in presence of CCl4;

ammonia (7664-41-7) + chlorine (7782-50-5) → nitrogen trichloride (10025-85-1) + ammonium chloride

Conditions	Yield
with dried gases at ambient temp., under 25 Torr; at higher pressure no NCl3 formed;
In tetrachloromethane at -90 and -180°C;;
In pentane at -90 and -180°C;;

ammonia (7664-41-7) → nitrogen trichloride (10025-85-1) + hypochlorite (14380-61-1)

Conditions	Yield
In water; sodium chloride Electrolysis; the anode is graphite, cathode is platimun wire;

ammonium chloride → nitrogen trichloride (10025-85-1)

Conditions	Yield
In not given Electrolysis; a cold satd. soln. is used;;
In water Electrolysis; NCl3 is formed at a platinum anode and explodes at touching of both poles;;
In water Electrolysis; electrolysis of concd. NH4Cl soln. at 35 - 40°C; don't stirring soln.;;

calcium hypochlorite (7778-54-3) + ammonium chloride → nitrogen trichloride (10025-85-1)

Conditions	Yield
In water reaction of acidified NH4Cl soln. with calcd. amount of Ca(ClO)2;; chloride free NCl3;;
In water reaction of acidified NH4Cl soln. with calcd. amount of Ca(ClO)2;; chloride free NCl3;;

ammonium chloride + chlorine (7782-50-5) + sodium hydroxide (1310-73-2) → nitrogen trichloride (10025-85-1)

Conditions	Yield
In water 5% NaOH satd. with Cl2 reacts with NH4Cl soln. in excess;; NCl3 is extracted with benzene;;
In water 5% NaOH satd. with Cl2 reacts with NH4Cl soln. in excess;; NCl3 is extracted with benzene;;

hydrogenchloride (7647-01-0) + Chlorkalk (15944-13-5) + ammonium chloride → nitrogen trichloride (10025-85-1)

Conditions	Yield
In not given formation of NCl3 at ambient temp. is only succesful at addn. of HCl;;
In water NCl3 is extracted with CCl4;;
In water NCl3 is extracted with benzene;;

Chlorkalk (15944-13-5) + ammonium chloride → nitrogen trichloride (10025-85-1) + nitrogen (7727-37-9)

Conditions	Yield
In water without addn. of acid;;	A 0% B n/a

Chlorkalk (15944-13-5) + ammonium chloride → nitrogen trichloride (10025-85-1)

Conditions	Yield
In not given to a soln. of bleaching powder cooled to 0°C is added a satd. soln. of NH4Cl; formed NCl3 can explode by addn. of rosin oil;;
In not given to a soln. of bleaching powder cooled to 0°C is added a satd. soln. of NH4Cl; formed NCl3 can explode by addn. of rosin oil;;

chloroamine (12190-75-9) + ammonium chloride → nitrogen trichloride (10025-85-1)

Conditions	Yield
In water explosion;;
In water
In water

Upstream product

• 2696-92-6 nitrosylchloride 
• 10026-13-8 phosphorus pentachloride 
• 7727-37-9 nitrogen 
• 10102-43-9 nitrogen(II) oxide 
• 10294-34-5 boron trichloride 
• 302-01-2 hydrazine 
• 7664-41-7 ammonia 
• 7782-50-5 chlorine 
• 7778-54-3 calcium hypochlorite 
• 1310-73-2 sodium hydroxide 
• 7647-01-0 hydrogenchloride 
• 15944-13-5 Chlorkalk 
• 12190-75-9 chloroamine 
• 14989-30-1 hypochloric acid 

Downstream Products

• 7782-68-5 iodic acid 
• 865-44-1 iodine trichloride 
• 7553-56-2 iodine 
• 2696-92-6 nitrosylchloride 
• 108-77-0 1,3,5-trichloro-2,4,6-triazine 
• 33121-27-6 Dichlormethyl-bis(isocyaniddichlorid) 
• 33142-86-8 Monochlormethyl-tris(isocyaniddichlorid) 
• 7782-50-5 chlorine 
• 29164-55-4 perchloro-2-aza-1-propene 
• 10025-78-2 trichlorosilane 
• 13966-57-9 chlorosilane 
• 10024-97-2 dinitrogen monoxide 
• 7727-37-9 nitrogen 
• 13444-90-1 Nitryl chloride 

Relevant articles and documents

Electrochemical behavior of chloramines on the rotating platinum and gold electrodes

Electroreduction of chloramines (mono-, di-, and trichloramine) in 1 M NH4Cl solutions of different pH was investigated at the rotating platinum and gold electrodes. It was found that all chloramines are present in the solution in nonprotonated forms and give well-formed one-step or two-step current-potential waves. The final products of reduction are ammonium (or ammonia) and chloride ions. Monochloramine is reduced in a single two-electron irreversible wave. Hydrazine is not an intermediate in monochloramine reduction. Dichloramine reduction generally proceeds in two two-electron steps (via monochloramine). Below pH 4.3 a kinetic current due to the protonated dichloramine reduction (single four-electron wave) is in force, appearing as an increase of the height of the first step on lowering pH. Due to this process below pH 2.5 only one four-electron reduction wave is observed. Trichloramine reduction occurs in two steps: two-electron trichloramine to dichloramine reduction and four-electron dichloramine reduction. In strong acidic solutions the kinetic current due to the protonated trichloramine reduction has to be taken into account. A reaction mechanism common for all chloramines was proposed with [NXCl·] as an intermediate (X = H2, HCl, and Cl2 for mono-, di-, and trichloramine, respectively). The rate-determining step does not involve proton transfer.

The role of cobalt oxide or magnesium oxide in ozonation of ammonia nitrogen in water

In this study, the reaction mechanisms for ozonation of ammonia nitrogen in the presence of Co3O4 or MgO were investigated. For the reaction over Co3O4, Cl– in the reaction solution was indispensable and ClO– was formed by a non-catalytic oxidation of Cl–. Co3O4 promoted the reaction of NH4+ with ClO– to give the products including NO3–, chloramines and gaseous products. In contrast, Cl– was unnecessary for the reaction with MgO. pH of the reaction solution was maintained at around 9 throughout the reaction owing to partial dissolution of MgO. Ammonia nitrogen was decomposed to mainly NO3– by non-catalytic radical reaction involving OH·, which was formed by the reaction of OH– with O3 in weakly basic solution. To keep the reaction solution weakly basic, H+ formed with the decomposition of NH4+ was neutralized. As a result, about the same amount of Mg2+ as that of decomposed ammonia nitrogen was dissolved.