| Identification | More | [Name]
Chlorine | [CAS]
7782-50-5 | [Synonyms]
Cl2
Cloro
Chlor
CIRL2
Cl2aa
Chlore
Chlor8
Chloor
Chlorine
chlorine0
Bertholite
dichlorine
CHLORINEGAS
CHLORINE TS
Chebi:29310
chlorinemol
chlorinemol.
caswellno179
Chlorine mol.
chlore(french)
CHLORINE WATER
CHLORINE, 99.5+%
molekularesChlor
Chloride in Water
molecularchlorine
Chlorine molecule
Chlorine in Water
chlorine,diatomic
Liquefied chlorine
Molecular chlorine
chlorine,highpurity
liquefiedchlorinegas
cloro(italian&spanish)
bertholite/warfaregas/
Dimethyl Sulfide-Chlorine
CHLORINE WATER, SATURATED
CHLORINE, ELECTRONIC GRADE
KZBUYRJDOAKODT-UHFFFAOYSA-N
Chlorine, Quant Test Strips
chlorinecyl.with2l(net~2kg)
epapesticidechemicalcode020501
chlorine cyl. with 5 L (net ~6 kg)
chlorine cyl. with 20 L (net ~25 kg) | [EINECS(EC#)]
231-959-5 | [Molecular Formula]
Cl2 | [MDL Number]
MFCD00010934 | [Molecular Weight]
70.91 | [MOL File]
7782-50-5.mol |
| Chemical Properties | Back Directory | [Definition]
The 15th most abundant element in the earth’s crust,
occurring only in the combined state, mainly in
common salt. A strong corrosive acid. | [Appearance]
Chlorine is a greenish-yellow gas. Pungent,
irritating odor. Shipped as a liquefied compressed gas. It is
the commonest of the four halogens which are among the
most chemically reactive of all the elements. It is not flammable; but it is a strong oxidizer, and contact with other
materials may cause fire. | [Melting point ]
−101 °C(lit.) | [Boiling point ]
−34 °C(lit.) | [density ]
1.468（0℃） | [vapor density ]
2.48 (vs air)
| [vapor pressure ]
4800 mm Hg ( 20 °C)
| [storage temp. ]
-20°C | [solubility ]
slightly soluble in H2O | [form ]
Liquid | [color ]
Clear yellow-green | [Odor]
Highly pungent, bleach-like odor detectable at 0.02 to 3.4 ppm (mean = 0.08 ppm) | [Stability:]
Stable. Incompatible with reducing agents, alcohols. | [Odor Threshold]
0.049ppm | [Resistivity]
1E9 μΩ-cm, 20°C | [Water Solubility ]
0.7 g/100 mL | [Merck ]
13,2112 | [BRN ]
3902968 | [Dielectric constant]
2.1（-46℃） | [Exposure limits]
TLV-TWA 1 ppm (～3 mg/m3) (ACGIH and
MSHA); ceiling 1 ppm (OSHA), 0.5 ppm/
15 min (NIOSH); IDLH 30 ppm (NIOSH). | [History]
Chlorine was discovered in
1774 by Scheele, who thought it contained oxygen; named in
1810 by Davy, who insisted it was an element. In nature it is
found in the combined state only, chiefly with sodium as common
salt (NaCl), carnallite (KMgCl3 · 6H2O), and sylvite (KCl).
It is a member of the halogen (salt-forming) group of elements
and is obtained from chlorides by the action of oxidizing
agents and more often by electrolysis; it is a greenish-yellow
gas, combining directly with nearly all elements. At 10°C one
volume of water dissolves 3.10 volumes of chlorine, at 30°C
only 1.77 volumes. Chlorine is widely used in making many
everyday products. It is used for producing safe drinking water
the world over. Even the smallest water supplies are now
usually chlorinated. It is also extensively used in the production
of paper products, dyestuffs, textiles, petroleum products,
medicines, antiseptics, insecticides, foodstuffs, solvents,
paints, plastics, and many other consumer products. Most of
the chlorine produced is used in the manufacture of chlorinat-
The Elements 4-9
ed compounds for sanitation, pulp bleaching, disinfectants,
and textile processing. Further use is in the manufacture of
chlorates, chloroform, carbon tetrachloride, and in the extraction
of bromine. Organic chemistry demands much from
chlorine, both as an oxidizing agent and in substitution, since
it often brings desired properties in an organic compound
when substituted for hydrogen, as in one form of synthetic
rubber. Chlorine is a respiratory irritant. The gas irritates the
mucous membranes and the liquid burns the skin. As little as
3.5 ppm can be detected as an odor, and 1000 ppm is likely to
be fatal after a few deep breaths. It was used as a war gas in
1915. Natural chlorine contains two isotopes. Twenty other
isotopes and isomers are known. | [LogP]
-0.85 at 20℃ | [Uses]
A greenish yellow, poisonous gas, chlorine is one of the halogens used in silver halide photography. In its elemental form, chlorine was used in the daguerreotype process as an accelerator. See also the various chlorides listed under their compound names, such as Ammonium Chloride. | [CAS DataBase Reference]
7782-50-5(CAS DataBase Reference) | [NIST Chemistry Reference]
Chlorine(7782-50-5) | [EPA Substance Registry System]
7782-50-5(EPA Substance) |
| Hazard Information | Back Directory | [Chemical Properties]
Chlorine is a yellow-green gas that is heavier than air and has a strong irritating odor.
Chlorine is used extensively in the production of paper products, dyestuffs, textiles, petroleum products, medicines, antiseptics, insecticides, food, solvents, paints, plastics, and
many other consumer products. Chlorine is mainly used as a bleach in the manufacture of
paper and cloth and to make a wide variety of products. Most of the chlorine produced is
used in the manufacture of chlorinated compounds for sanitation, pulp bleaching, disinfectants, and textile processing. Further use is in the manufacture of chlorates, chloroform,
carbon tetrachloride, and in the extraction of bromine. Organic chemistry demands much
from chlorine, both as an oxidizing agent and in substitution. In fact, chlorine was used as
a war gas in 1915 as a choking (pulmonary) agent. Chlorine itself is not flammable, but it
can react explosively or form explosive compounds with other chemicals such as turpentine and ammonia.
Chlorine is slightly soluble in water. It reacts with water to form hypochlorous acid and
hydrochloric acid. Hypochlorous acid breaks down rapidly. Chlorine gas is used to synthesize other chemicals and to make bleaches and disinfectants. Chlorine is a powerful
disinfectant, and in small quantities ensures clean drinking water. It is used in swimming
pool water to kill harmful bacteria. Chlorine has a huge variety of uses, i.e., as a disinfectant and purifi er, in plastics and polymers, solvents, agrochemicals and pharmaceuticals,
as well as an intermediate in manufacturing other substances where it is not contained in
the fi nal product. Also, a large percentage of pharmaceuticals contain and are manufactured using chlorine. Thus, chlorine is essential in the manufacture of medicines to treat
illnesses such as allergies, arthritis, and diabetes. | [Reactivity Profile]
CHLORINE reacts explosively with or supports the burning of numerous common materials. Ignites steel at 100°C in the presence of soot, rust, carbon, or other catalysts. Ignites dry steel wool at 50°C. Reacts as either a liquid or gas with alcohols (explosion), molten aluminum (explosion), silane (explosion), bromine pentafluoride, carbon disulfide (explosion catalyzed by iron), 1-chloro-2-propyne (excess chlorine causes an explosion), dibutyl phthalate (explosion at 118°C), diethyl ether (ignition), diethyl zinc (ignition), glycerol (explosion at 70-80°C), methane over yellow mercury oxide (explosion), acetylene (explosion initiated by sunlight or heating), ethylene over mercury, mercury(I) oxide, or silver(I) oxide (explosion initiated by heat or light), gasoline (exothermic reaction then detonation), naphtha-sodium hydroxide mixture (violent explosion), zinc chloride (exothermic reaction), wax (explosion), hydrogen (explosion initiated by light), Reacts as either a liquid or gas with carbides of iron, uranium and zirconium, with hydrides of potassium sodium and copper, with tin, aluminum powder, vanadium powder, aluminum foil, brass foil, copper foil, calcium powder, iron wire, manganese powder, potassium, antimony powder, bismuth, germanium, magnesium, sodium, and zinc. Causes ignition and a mild explosion when bubbled through cold methanol. Explodes or ignites if mixed in excess with ammonia and warmed. Causes ignition in contact with hydrazine, hydroxylamine, and calcium nitride. Forms explosive nitrogen trichloride from biuret contaminated with cyanuric acid. Readily forms an explosive N-chloro derivative with aziridine. Ignites or explodes with arsine, phosphine, silane, diborane, stibine, red phosphorus, white phosphorus, boron, active carbon, silicon, arsenic. Ignites sulfides at ambient temperature. Ignites (as a liquid) synthetic and natural rubber. Ignites trialkylboranes and tungsten dioxide. | [Air & Water Reactions]
Water dissolves about twice its volume of chlorine gas, forming a mixture of hydrochloric acid and hypochlorous acids. Will be corrosive due to acidity and oxidizing potential. | [Hazard]
Moderately toxic; eye and upper respiratory
tract irritant. | [Health Hazard]
Chlorine is a respiratory irritant. It causes irritation to the mucous membranes and the
liquid burns the skin. The poisoning caused by chlorine depends on the amount of chlorine a person or an occupational worker is exposed to, and the length of exposure time.
Prolonged exposures to high concentrations of chlorine cause poisoning with symptoms
that include, but are not limited to, coughing, burning sensation in the nose, throat, and
eyes, blurred vision, nausea, vomiting, pain, redness, and blisters on the skin, chest tightness, and pulmonary edema. | [Health Hazard]
Poisonous; may be fatal if inhaled. Contact may cause burns to skin and eyes. Bronchitis or chronic lung conditions. | [Potential Exposure]
Environmental danger. Chlorine is a
toxic gas with corrosive properties. Gaseous chlorine is
widely used as a bleaching agent in the paper, pulp, and
textile industries for bleaching cellulose for artificial fibers.
It is used in the manufacture of chlorinated lime; inorganic
and organic compounds, such as metallic chlorides; chlorinated solvents; refrigerants, pesticides; and polymers, e.g.,
synthetic rubber and plastics; it is used as a disinfectant,
particularly for water and refuse; and in detinning and
dezincing iron. CL has been used as a warfare choking/pulmonary agent. Note: The lowest level at which humans can
detect chlorine through smell and become alert to its irritant properties generally provides sufficient warning of
exposure. However, chronic exposure to chlorine causes
olfactory fatigue and tolerance to its irritant effects. Those
with a history of prolonged exposure to chlorine, may eventually lose their ability to identify incidents of exposure. | [Fire Hazard]
May ignite other combustible materials (wood, paper, oil, etc.). Mixture with fuels may cause explosion. Container may explode in heat of fire. Vapor explosion and poison hazard indoors, outdoors or in sewers. Hydrogen and chlorine mixtures (5-95%) are exploded by almost any form of energy (heat, sunlight, sparks, etc.). May combine with water or steam to produce toxic and corrosive fumes of hydrochloric acid. Emits highly toxic fumes when heated. Avoid plastics and rubber. Avoid heat and contact with hydrogen gas or powdered metals. | [First aid]
If this chemical gets into the eyes, remove any
contact lenses at once and irrigate immediately for at least
30 minutes, occasionally lifting upper and lower lids. Seek
medical attention immediately. If this chemical contacts the
skin, remove contaminated clothing and wash immediately
with soap and water. Seek medical attention immediately.
If this chemical has been inhaled, remove from exposure,
begin rescue breathing (using universal precautions, including resuscitation mask) if breathing has stopped and CPR if
heart action has stopped. Transfer promptly to a medical
facility. When this chemical has been swallowed, get medical attention. Give large quantities of water and induce
vomiting. Do not make an unconscious person vomit.
Medical observation is recommended for 24 to 48 hours
after breathing overexposure, as pulmonary edema may be
delayed. As first aid for pulmonary edema, a doctor or
authorized paramedic may consider administering a drug or
other inhalation therapy. If frostbite has occurred, seek
medical attention immediately; do NOT rub the affected
areas or flush them with water. In order to prevent further
tissue damage, do NOT attempt to remove frozen clothing
from frostbitten areas. If frostbite has NOT occurred, immediately and thoroughly wash contaminated skin with soap
and water. | [Shipping]
UN1017 Chlorine, Hazard Class: 2.3; Labels:
2.3-Poisonous gas, 5.1-Oxidizer, 8-Corrosive material,
Inhalation Hazard Zone B. Cylinders must be transported
in a secure upright position, in a well-ventilated truck.
Protect cylinder and labels from physical damage. The
owner of the compressed gas cylinder is the only entity
allowed by federal law (49CFR) to transport and refill
them. It is a violation of transportation regulations to refill
compressed gas cylinders without the express written permission of the owner. Military driver shall be given full
and complete information regarding shipment and conditions in case of emergency. AR 50-6 deals specifically with
the shipment of chemical agents. Shipments of agent will
be escorted in accordance with AR 740-32. | [Incompatibilities]
A powerful oxidizer. Reacts explosively
or forms explosive compounds with many organic compounds and common substances, such as acetylene, ether,
turpentine, ammonia, fuel gas, hydrogen, and finely divided
metals. Keep away from combustible substances and reducing agents. Corrosive to some plastic, rubber, and coating
materials. Reacts with water to form hypochlorous acid.
Corrosive to many metals in presence of water. | [Description]
Chlorine is a greenish-yellow, nonflammable
gas with a distinctive, pungent odor. It is almost
two and one-half times as heavy as air. The gas
acts as a severe irritant if inhaled. Chlorine liquid
has the color of clear amber and is about
one and one-half times as heavy as water. It is
shipped as a compressed liquefied gas having a
vapor pressure of 86.767 psig at 70°F (598.26
kPa at 21.1°C). Chlorine is nonflammable in
both gaseous and liquid states. However, like
oxygen, it is capable of supporting the combustion
of certain substances. Many organic chemicals
react readily with chlorine, in some cases
with explosive violence. Chlorine usually forms
univalent compounds, but it can combine with a
valence of 3, 4,5, or 7.
Chlorine is only slightly soluble in water.
When it reacts with pure water, weak solutions
of hydrochloric and hypochlorous acids are
formed. Chlorine hydrate (Cl2·8H20) may crystallize
below 49.3°F (9.61°C). | [Waste Disposal]
Return refillable compressed
gas cylinders to supplier. Introduce into large volume and
solution of reducing agent (bisulfite, ferrous salts, or hypo),
neutralize and flush to sewer with water. Recovery is an
option to disposal for chlorine in the case of gases from
aluminum chloride electrolysis and chlorine in waste
waters. See also “Spill Handling.” Nonrefillable cylindersshould be disposed of in accordance with local, state, and
federal regulations. Allow remaining gas to vent slowly
into atmosphere in an unconfined area or exhaust hood.
Refillable-type cylinders should be returned to original supplier with any valve caps and outlet plugs secured and
valve protection caps in place.
| [Isotopes]
There are a total of 25 isotopes of chlorine. Of these, only two are stable andcontribute to the natural abundance on Earth as follows: Cl-35 = 75.77% and Cl-37 =24.23%. All the other 23 isotopes are produced artificially, are radioactive, and have halflivesranging from 20 nanoseconds to 3.01×10+5 years. | [Origin of Name]
From the Greek word khl?ros, meaning “greenish yellow.” | [Occurrence]
Chlorine is the 20th most abundant element on the Earth. It is not found as a free element(atoms) except as a diatomic gas escaping from very hot active volcanoes. It has been knownfor thousands of years as rock salt (halite). It is also found in sylvite and carnallite and as achloride in seawater. In nature, it is mostly found in dissolved salts in seawater and deposits insalt mines. Its best-known compound is sodium chloride (NaCl), which is common table salt.Chlorine is important for the chemical industry. Numerically, it is the 12th most producedchemical in the United States and ranks ninth in volume of chemicals produced in the UnitedStates.
Chlorine is produced commercially by the electrolysis of a liquid solution of sodium chloride(or seawater), through which process an electric current is passed though the solution(electrolyte). | [Characteristics]
Chlorine’s best-known characteristic is its smell. It can be detected when used as householdbleach or as an antiseptic in swimming pools. As an antiseptic, it is added to municipal drinkingwater supplies. Chlorine gas has a very pungent odor that is suffocating when inhaled. Ina more concentrated form, Cl2 was also a deadly poisonous gas used in combat during WorldWar I. Because it combines with so many other elements, particularly metals, chlorine is fundamentalto many industries, particularly the plastics industry.
Laboratory amounts of chlorine (Cl2) are produced by combining hydrochloric acid (HCl)with manganese dioxide (MnO2). The HCl provides the Cl-1 ion. | [Production Methods]
Chlorine is principally produced by electrolysis of NaCl
or KCl brine in either diaphragm, mercury, or membrane
cathode cells. In these processes, gaseous chlorine is released
at the anode and caustic is a by-product. Chlorine may also be
produced by electrolysis of hydrochloric acid (HCl) [7647-
01-0], by oxidation of HCl in the presence of nitrogen oxide
as a catalyst (Kel-Chlor process), or as a coproduct from
metal production. | [Flammability and Explosibility]
Chlorine is noncombustible but is a strong oxidizer and will support combustion of
most flammable substances. | [Agricultural Uses]
Chlorine (Cl) is a halogen, classified in Group 17 (formerly VII), Period 3 of the Periodic Table of elements. It is a greenish yellow gas and has an atomic weight of 35.5
Chlorine is one of the essential elements for plants, although it is not always listed as a micronutrient. It is absorbed in soil almost entirely as chloride ions ((Cl-) which are very mobile, soluble and mostly non-reactive in soil. The role of chlorine in plants is believed to be biochemical, osmotic and in balancing cell cationic charges.
Plants responding to chloride are tomato, pea, lettuce, cabbage, carrot, sugar beet, barley, corn, berries, vine crops, potato, cotton, woody ornamental plants and fruit trees like coconut.
Chlorine is involved in the splitting of water molecules in photoreactionⅡ of photosynthesis. Several enzymes such as ATPase, alpha-amylase and asparagine synthetase require the chloride ion for activation. As the chloride ion is very mobile and is tolerated at high concentrations, it is ideal for maintaining the charge balance when cations (such as potassium) move across cell membranes. The chloride requirement of plants for biochemical functions is hardly more than 100mg/kg of dry plant matter. However, chloride is usually present at much higher concentrations (2000to 20,000mg/kg), suggesting its involvement in functions other than those of a biochemical nature.
The chloride content in plants ranges from 0.2 to 2.0% but in some salt tolerant plants it can be as high as 10%. Excessive chloride accumulation is harmful to plants, causing the leaves to thicken and roll, lowering the quality of potato tubers and the smoking quality of tobacco. If plants sensitive to chloride receive more than 1 to 2 % chloride ions (Cl') , yields are often reduced.
The environment entertains the chlorine cycle. Air, water and soil are at the receiving end of the cycle. For instance, air gets chloride from volcanoes and sea spray, whereas water receives chloride from sewage, food, water-softener wastes, industrial effluents and de-icing salts used on roads. Soil gets its chloride supply from animal manure, rainfall, irrigation waters and potassium chloride fertilizers.
Chlorine in soil follows water movements and is taken up by plants as the chloride (CT) anion. The greater the chloride concentration in a soil solution, the higher the plant uptake. It may also be taken up aerially as Cl- anion or chlorine gas. Chloride, highly mobile in plants, is required in the splitting of water (Hill reaction) during photosynthesis. It enhances oxygen synthesis and photophosphorylation. The accumulation of excessive chloride ions can be toxic. Foliar sprays with chloride- containing irrigation water, if left to dry on the leaves, may cause salt bum.
Since field plots do not display any chloride deficiency and most fertilizers have some chloride (as contaminant), not much is done for chloride rectification. More studies are required to find out the effect of large additions of chloride ions (30to 50kg/ha).
The symptoms of chloride deficiency are not easily identifiable. In nutrient cultures, it was shown that chlorine deficiency is associated with a reduced root growth. Chlorosis in younger leaves and an overall wilting of the plants are the two most common symptoms of chlorine deficiency. Necrosis in some plant parts and leaf bronzing may also be wimessed. Excessive chlorine can be harmful but crops vary widely in their tolerance. The principal effect of too much chlorine is to increase the osmotic pressure of soil water and thereby lower the availability of water to plants.
Chlorine in fertilizers suppresses many diseases. Adequate quantities of chloride-containing fertilizers can mitigate diseases like 'take all root rot', 'stripe rusts', 'leaf rust', 'tan spot of wheat', etc. A moderately excess quantity of chloride is employed to fight such diseases (many times above the nutritional needs). For example, chloride banding of 40kg/ha is recommended to reduce 'take all root rot' on winter wheat in western countries.
Potassium chloride, which contains large quantities of chloride, is a widely used fertilizer. Ammonium chloride, calcium chloride, magnesium chloride and sodium chloride are other sources of chlorine. | [Materials Uses]
At ordinary temperatures, dly chlorine, either
liquid or gas, does not corrode steel. In the presence
of moisture, however, highly corrosive conditions
exist due to the formation of hydrochloric
and hypochlorous acids. Thus precautions should
be taken to keep chlorine and equipment free of moisture. Piping, valves, and containers should
be closed or capped when not in use to keep atmospheric
moisture out ofthe system. | [Physiological effects]
Chlorine gas is primarily a respiratory irritant.
In sufficient concentration, the gas irritates the
mucous membranes, the respiratory tract and the
eyes. In extreme cases difficulty in breathing
may increase to the point where death can occur
from respiratory collapse or lung failure. The
characteristic, penetrating odor of chlorine gas
usually gives warning of its presence in the air.
Also, at high concentrations, it is visible as a
greenish yellow gas. Liquid chlorine in contact
with skin or eyes will cause chemical bums or
frostbite.
ACGIH recommends a Threshold Limit
Value-Time-Weighted Average (TLV-TWA)
of 0.5 ppm (1.5 mg/m3
) for chlorine. The TLVTWA
is the time-weighted average concentration
for a normal 8-hour workday and a 40-hour
workweek, to which nearly all workers may be
repeatedly exposed, day after day, without adverse
effect. | [Carcinogenicity]
In the chronic inhalation bioassay
with rats and mice exposed to 0, 0.4, 1.0, or 2.5 ppm chlorine
for 2 years, described above, incidence of neoplasia in the
nasal passages was not increased by exposure, even though
there were exposure-dependent lesions in the nasal tissues
(199). Chlorine has not been identified as a carcinogen
(IARC 1999). | [storage]
All work with chlorine should be conducted in a fume hood to prevent exposure
by inhalation, and splash goggles and impermeable gloves should be worn at all times to
prevent eye and skin contact. Cylinders of chlorine should be stored in locations appropriate
for compressed gas storage and separated from incompatible compounds such as hydrogen,
acetylene, ammonia, and flammable materials. | [Purification Methods]
Pass the gas in succession through aqueous KMnO4, dilute H2SO4, conc H2SO4, and a drying tower containing Mg(ClO4)2. Or bubble it through water, dry it over P2O5 and distil it from bulb to bulb in a vacuum line. One volume of water dissolves 4.6 volumes of Cl2 at 0o, 2.15 volumes at 20o, 1.22 volumes at 50o and 0.39 volumes at 90o. [Schmeisser in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I p 272 1963.] HIGHLY TOXIC. | [GRADES AVAILABLE]
Chlorine for commercial and industrial use has
much the same quality from all producers. High
purity grades (99.9 percent) are available from
specialty gas suppliers. |
| Safety Data | Back Directory | [Hazard Codes ]
T,N | [Risk Statements ]
R23:Toxic by inhalation.
R36/37/38:Irritating to eyes, respiratory system and skin .
R50:Very Toxic to aquatic organisms. | [Safety Statements ]
S9:Keep container in a well-ventilated place .
S45:In case of accident or if you feel unwell, seek medical advice immediately (show label where possible) .
S61:Avoid release to the environment. Refer to special instructions safety data sheet . | [RIDADR ]
UN 1017 2.3
| [WGK Germany ]
2
| [RTECS ]
FO2100000
| [DOT Classification]
2.3, Hazard Zone B (Gas poisonous by inhalation) | [HazardClass ]
2.3 | [Safety Profile]
Moderately toxic to
humans by inhalation. Very irritating by
inhalation. Human mutation data reported.
Human respiratory system effects by
inhalation: changes in the trachea or
bronchi, emphysema, chronic pulmonary
edema or congestion, A strong irritant to
eyes and mucous membranes. Questionable
carcinogen.
Chlorine is extremely irritating to the
mucous membranes of the eyes and the
respiratory tract at 3 ppm. Combines with
moisture to form HCl. Both these
substances, if present in quantity, cause
inflammation of the tissues with which they
come in contact. A concentration of 3.5
ppm produces a detectable odor; 15 ppm
causes immediate irritation of the throat.
Concentrations of 50 pprn are dangerous for
even short exposures; 1000 pprn may be
fatal, even when exposure is brief. Because
of its intensely irritating properties, severe
industrial exposure seldom occurs, as the
worker is forced to leave the exposure area
before he can be seriously affected. In cases
where this is impossible, the initial irritation
of the eyes and mucous membranes of the
nose and throat is followed by coughing, a
feeling of suffocation, and, later, pain and a
feeling of constriction in the chest. If
exposure has been severe, pulmonary edemamay follow, with rales being heard over the
chest. It is a common air contaminant.
or UV light, air + ethylene, molten
aluminum, ammonia, amidosulfuric acid,
antimony trichloride + tetramethyl silane (at
loo'), benzene + light, biuret, bromine
pentafluoride + heat, tert-butanol, butyl
rubber + naphtha, carbon disulfide + iron
catalyst, chlorinated pyridine + iron powder,
3-chloropropyne, cobalt(Ⅱ) chloride +
methanol, dborane, dbutyl phthalate (at
1 18'), dchloro(methy1)arsine (in a sealed
container), diethyl ether, dimethyl
phosphoramidiate, dioxygen difluoride,
dsilyl oxide, 4,4'-dithiodimorpholine, ethane
over activated carbon (at 350'), fluorine +
sparks, gasoline, glycerol (above 70' in a
sealed container), hexachlorodisilane (above
300'), hydrocarbon oils or waxes, iron(IⅡ)
chloride + monomers (e.g., styrene),
methane over mercury oxide, methanol,
methanol + tetrapyridme cobalt(Ⅱ) chloride,
naphtha + sodium hydroxide, nitrogen
triiodide, oxygen difluoride, whte
phosphorus (in liquid Cl2), phosphorus
compounds, polypropylene + zinc oxide,
propane (at 300°), shcones when heated in a
sealed container [e.g., polydimethyl siloxane
(above 88'), polymethyl trifluoropropylsiloxane (above 68')], stibine, synthetic
rubber (in liquid Cl2), tetraselenium
tetranitride, trimethyl thionophosphate.
Explosive products are formed on reaction
with alkylthiouronium salts, amidosulfuric
acid, acidc ammonium chloride solutions,
aziridine, bis(2,4-dinitrophenyl)disulfide,
cyanuric acid, phenyl magnesium bromide.
Mixtures with ethylene are explosives
initiated by light, heat, or by the presence of
mercury, mercury oxide, silver oxide, lead
oxide (at 100°). Mxtures with hydrogen are
explosives initiated by sparks, light, heating
to over 280°, or the presence of yellow
mercuric oxide or nitrogen trichloride.
Murtures with hydrogen and other gases
(e.g., air, hydrogen chloride, oxygen) are also
explosive. Iption or explosive reaction with metals
(e.g., aluminum, antimony powder, bismuth
powder, brass, calcium powder, copper,
germanium, iron, manganese, potassium, tin,
vanadium powder). Reaction with some
metals requires moist Cl2 or heat. Ignites
with diethyl zinc (on contact),
polyisobutylene (at 130'), metal acetylides,
metal carbides, metal hydrides (e.g.,
potassium hydride, sodium hydride, copper
hydride), metal phosphtdes (e.g., copper(Ⅱ)
phosphide), methane + oxygen, hydrazine,
hydroxylamine, calcium nitride, nonmetals
(e.g., boron, active carbon, silicon,
phosphorus), nonmetal hydrides (e.g., arsine,
phosphine, silane), steel (above 200' or as
low as 50℃ when impurities are present),
sulfides (e.g., arsenic disulfide, boron
trisulfide, mercuric sulfide), trialkyl boranes.
Violent reaction with alcohols, N-aryl
sulfinamides, dimethyl formamide,
polychlorobiphenyl, sodium hydroxide,
hydrochloric acid + dinitroanilines.
Incandescent reaction when warmed with
cesium oxide (above 1 50°), tellurium,
arsenic, tungsten dioxide. Potentially
dangerous reaction with hydrocarbons +
Lewis acids releases toxic and reactive HCl
gas.
Can react to cause fires or explosions
upon contact with turpentine, illuminating
gas, polypropylene, rubber, sulfamic acid,
As2(CH3)4, UC2, acetaldehyde, alcohols,
alkylisothiourea salts, alkyl phosphtnes, Al,
Sb, As, AsS2, AsH3, Ba3P2, C6H6, Bi, B,
BPI2, B2S3, brass, BrF5, Ca, (CaC2 + KOH),
Ca(ClO2)2, Ca3N2, Ca3P, C, CS2, Cs, CsHC2,
CO20, Cs3N, (C + Cr(OCl)2), CuH2, CuC2,
dialklyl phosphines, diborane, dibutyl
phthalate, Zn(C2H5)2, C2H6, C2H4, ethylene
imine, C2H5PH2, F2, Ge, glycerol, (NH2)2,
(H20 + KOH), I2, hydroxylamine, Fe, FeC2,
Li, Li2C2, Li6c2, Mg, Mg2P3, Mn, Mn3P2,
HgO, HgS, Hg, Hg3P2, CH4,Nb,NI3, OF2,
H2SiO, (OF2 + Cu), PH3, P, P(SNC)3, P203,
PCB's, K, KHC2, KH, Ru, RuHC2, Si, SiH2,
Ag2O, Na, NaHC2, Na2C2, SnF2, SbH3, Sr3P,
Te, Th, Sn, WO2, U, V, Zn, ZrC2. | [Hazardous Substances Data]
7782-50-5(Hazardous Substances Data) | [Toxicity]
LC50 (1 hr) in rats, mice (ppm): 293, 137 (K. C. Back et al., Reclassification of Materials Listed as Transportation Health Hazards (TSA-20-72-3; PB 214-270, 1972) pp A-182-183) | [IDLA]
10 ppm |
| Raw materials And Preparation Products | Back Directory | [Raw materials]
Sodium chloride-->Ammonia-->CARBON MONOXIDE-->Barium chloride dihydrate-->Bifenthrin-->Calcium chloride hexahydrate-->Cistern car | [Preparation Products]
Diethylcarbamyl chloride-->3-Chlorobenzotrifluoride-->Chlorinated rubber-->SULFURYL FLUORIDE-->4,4'-Thiobis(6-tert-butyl-m-cresol)-->2-Chlorobenzothiazole-->2-Amino-5-chloro-3-picoline-->Vat Orange 9-->diammonium tetrachloromercurate-->Aminomercuric chloride-->(1S)-(+)-3-Carene-->POLYETHYLENE, CHLORINATED-->2-AMINO-3,5-DICHLORO-4-METHYLPYRIDINE-->4,4'-Azobis(4-cyanovaleric acid)-->Tricresyl Phosphate-->4'-Hydroxy-3'-methylacetophenone-->2,6-Dichlorobenzoxazole-->DICHLOROISOCYANURIC ACID-->Reactive Yellow 3-->VINYLIDENE CHLORIDE-->OCTACHLOROCYCLOPENTENE-->NITROFEN-->3-Chloropivaloyl chloride-->Acetoin-->Isobutenyl sulfide-->Pentachloropyridine-->Diphosphoryl chloride-->Perchloromethylmercaptan-->BIS(A,2-DICHLORO-BENZAL)HYDRAZINE-->o-methoxycarbonyl benzyl sulfonyl chloride-->4-(AMINOMETHYL)BENZENESULFONAMIDE-->N,N'-DINITROSOPENTAMETHYLENETETRAMINE-->2-Acetyl-3-methylpyrazine-->1,2,2,3-TETRACHLOROPROPANE-->Isothiazolinones-->Chlorthal-->1,1-BIS(4-CHLOROPHENYL)-1,2,2,2-TETRACHLOROETHANE-->4-Fluorobenzoyl chloride-->Dimethyl chloromalonate-->Clopyralid |
| Questions And Answer | Back Directory | [Occurrence and Uses]
Chlorine does not occur in the elemental state because of its high reactivity. In nature the element occurs mainly as sodium chloride in seawater. Its abundance in seawater is 1.9% by weight. It also exists as chloride in many rocks and minerals such as carnallite (KMgCl3•6H2O) and sylvite (KCl).
Chlorine was discovered by Scheele in 1774 and named by Davy in 1810.Chlorine is extensively used in the production of paper products, dyestuffs, textiles, petroleum products, medicines, antiseptics, insecticides, food, solvents, paints, plastics, and many other consumer products. Chlorine is mainly used as a bleach in the manufacture of paper and cloth and to make a wide variety of products. Most of the chlorine produced is used in the manufacture of chlorinated compounds for sanitation, pulp bleaching, disinfectants, and textile processing. Further use is in the manufacture of chlorates, chloroform, and carbon tetrachloride and in the extraction of bromine. Organic chemistry demands much from chlorine, both as an oxidising agent and in substitution. In fact, chlorine was used as a war gas in 1915 as a choking (pulmonary) agent. Chlorine itself is not flammable, but it can react explosively or form explosive compounds with other chemicals such as turpentine and ammonia.
Chlorine gas is used to synthesise other chemicals and to make bleaches and disinfectants. Chlorine is a powerful disinfectant and in small quantities ensures clean drinking water. It is used in swimming pool water to kill harmful bacteria. Chlorine has a huge variety of uses, for instance, as a disinfectant and purifier, in plastics and polymers, solvents, agrochemicals, and pharmaceuticals, as well as an intermediate in manufacturing other substances where it is not contained in the final product. Also, a very large percentage of pharmaceuticals contain and are manufactured using chlorine. Thus, chlorine is essential in the manufacture of medicines to treat illnesses such as allergies, arthritis, and diabetes.
| [Physical Properties]
Greenish-yellow gas; suffocating odor (odor threshold 3 ppm); gas density in the air 2.46 (air = 1); becomes a pale yellow liquid at –34.04°C; the color decreases with lowering temperature; becomes a pale yellow crystal at –101.5°C; critical temperature 143.8°C; critical pressure 76.89 atm; critical volume 123 cm3/mol; moderately soluble in water; solubility in water 0.061 mol Cl2/L at 20°C; bulk solubility in water (including all species formed) 0.091 mol/L.
| [Production]
Chlorine is produced industrially by electrolysis of brine using either mercury cathode cells or, preferably, various commercially available membrane cells. Chlorine gas is liberated at the anode while sodium hydroxide and hydrogen are liberated at the cathode:
Na+ + Cl– + H2O → Na+ + OH– + ½Cl2 + ½H2
Also, Cl is made by electrolysis of fused sodium chloride, magnesium chloride salt, or hydrochloric acid. The electrolytic process has practically superseded the Weldon and Deacon processes employed earlier to produce chlorine. The Weldon process involves the action of HCl on manganese dioxide ores to produce chlorine and manganese chloride. The MnCl2 liquor obtained is first converted into calcium manganite (CaO•2MnO2) or “Weldon mud,” from which MnO2 is generated back for reuse. Deacon’s process involves catalytic oxidation of hydrogen chloride, catalyzed by copper:
2HCl + ½O2→Cl2 + H2O
The efficiency of Deacon’s process is improved by passing the HCl over CuO at 200°C. The product CuCl2 is oxidized at 300°C by treatment with oxygen:
2HCl + CuO→ CuCl2 + H2O
2CuCl2 + O2→2Cl2 + 2CuO
In the laboratory, chlorine may be prepared by oxidation of HCl with manganese dioxide:
4HCl + MnO2 → MnCl2 + Cl2 + 2H2O
| [Hazard]
Chlorine is a pungent suffocating gas, exposure to which can cause irritation of the eyes, nose and throat; burning of mouth; coughing; choking; nausea, vomiting; dizziness and respiratory distress. Exposure to 15–20 ppm of chlorine in air can cause irritation and coughing. A 30 minute exposure to 500–800 ppm can be fatal to humans (Patnaik, P. 1999. A Comprehensive Guide to the Hazardous Properties of Chemical Substances, 2nd ed. New York: John Wiley & Sons).
Chlorine-hydrogen mixture can explode in the presence of sunlight, heat or a spark. Also, it can explode when mixed with acetylene or diborane at ordinary temperatures, and with ethylene, fluorine, and many hydrocarbons in the presence of heat, spark or catalysts.
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