| Identification | More | [Name]
Carbon | [CAS]
7440-44-0 | [Synonyms]
ACETYLENE BLACK
ACETYLENE CARBON BLACK
ACTIVATED CARBON
ACTIVATED CARBON DARCO G-60
ACTIVATED CHARCOAL
ACTIVATED CHARCOAL NORIT
ACTIVATED CHARCOAL NORIT(R)
CALGON CPG
CARBO ACTIVATUS
CARBON
CARBON 84
CARBON, ACTIVATED
CARBON ATOMIC ABSORPTION STANDARD
CARBON BLACK
CARBON BLACK, ACETYLENE
CARBON, DECOLORIZING
CARBON, DECOLORIZING DARCO(R)
CARBON, DECOLORIZING NORIT(R) A
CARBON, DECOLORIZING NUCHAR(R) S-N
CARBON FELT | [EINECS(EC#)]
231-153-3 | [Molecular Formula]
CH4 | [MDL Number]
MFCD00133992 | [Molecular Weight]
16.04 | [MOL File]
7440-44-0.mol |
| Chemical Properties | Back Directory | [Definition]
The crystalline allotropic form of carbon. | [Appearance]
Graphite is crystallized carbon and usually
appears as soft, black scales. There are two types of graph ite, natural and artificial (activated). Natural and synthetic
graphite may be mixed with each other or contain other
additives. | [Melting point ]
3550 °C (lit.) | [Boiling point ]
500-600 °C(lit.)
| [density ]
~1.7 g/mL at 25 °C(lit.)
| [vapor pressure ]
<0.1 mm Hg ( 20 °C)
| [Fp ]
>230 °F
| [storage temp. ]
Flammables area | [solubility ]
Insoluble. | [form ]
rod
| [color ]
Black | [Specific Gravity]
1.8～2.1 (amorphous) | [Odor]
at 100.00?%. odorless | [PH]
6-9 | [Stability:]
Stable. Incompatible with strong oxidizing agents. Combustible. Highly flammable in powdered form. | [Resistivity]
1375 μΩ-cm, 20°C (graphite) | [Water Solubility ]
Insoluble in water. | [Merck ]
1807 | [BRN ]
4360473 | [History]
Carbon, an element of prehistoric discovery,
is very widely distributed in nature. It is found in abundance
in the sun, stars, comets, and atmospheres of most planets.
Carbon in the form of microscopic diamonds is found in
some meteorites. Natural diamonds are found in kimberlite
or lamporite of ancient formations called “pipes,” such as
found in South Africa, Arkansas, and elsewhere. Diamonds
are now also being recovered from the ocean floor off the
Cape of Good Hope. About 30% of all industrial diamonds
used in the U.S. are now made synthetically. The energy of
the sun and stars can be attributed at least in part to the wellknown
carbon-nitrogen cycle. Carbon is found free in nature
in three allotropic forms: amorphous, graphite, and diamond.
Graphite is one of the softest known materials while diamond
is one of the hardest. Graphite exists in two forms: alpha and
beta. These have identical physical properties, except for their
crystal structure. Naturally occurring graphites are reported
to contain as much as 30% of the rhombohedral (beta) form,
whereas synthetic materials contain only the alpha form. The
hexagonal alpha type can be converted to the beta by mechanical
treatment, and the beta form reverts to the alpha on
heating it above 1000°C. Of recent interest is the discovery
of all-carbon molecules, known as “buckyballs” or fullerenes,
which have a number of unusual properties. These interesting
molecules, consisting of 60 or 70 carbon atoms linked together,
seem capable of withstanding great pressure and trapping
foreign atoms inside their network of carbon. They are said to
be capable of magnetism and superconductivity and have potential
as a nonlinear optical material. Buckyball films are reported
to remain superconductive at temperatures as high as
45 K. In combination, carbon is found as carbon dioxide in the
atmosphere of the Earth and dissolved in all natural waters. It
is a component of great rock masses in the form of carbonates
of calcium (limestone), magnesium, and iron. Coal, petroleum,
and natural gas are chiefly hydrocarbons. Carbon is
unique among the elements in the vast number and variety of
compounds it can form. With hydrogen, oxygen, nitrogen, and
other elements, it forms a very large number of compounds,
carbon atom often being linked to carbon atom. There are
close to ten million known carbon compounds, many thousands
of which are vital to organic and life processes. Without
carbon, the basis for life would be impossible. While it has
been thought that silicon might take the place of carbon in
forming a host of similar compounds, it is now not possible
to form stable compounds with very long chains of silicon atoms.
The atmosphere of Mars contains 96.2% CO2. Some of
the most important compounds of carbon are carbon dioxide
(CO2), carbon monoxide (CO), carbon disulfide (CS2), chloroform
(CHCl3), carbon tetrachloride (CCl4), methane (CH4),
ethylene (C2H4), acetylene (C2H2), benzene (C6H6), ethyl alcohol
(C2H5OH), acetic acid (CH3COOH), and their derivatives.
Carbon has fifteen isotopes. Natural carbon consists of 98.89%
12C and 1.11% 13C. In 1961 the International Union of Pure and
Applied Chemistry adopted the isotope carbon-12 as the basis
for atomic weights. Carbon-14, an isotope with a half-life
of 5715 years, has been widely used to date such materials as
wood, archeological specimens, etc. A new brittle form of car-
4-8 The Elements
bon, known as “glassy carbon,” has been developed. It can be
obtained with high purity. It has a high resistance to corrosion,
has good thermal stability, and is structurally impermeable to
both gases and liquids. It has a randomized structure, making
it useful in ultra-high technology applications, such as crystal
growing, crucibles for high-temperature use, etc. Glassy carbon
is available at a cost of about $35/10g. Fullerene powder
is available at a cost of about $55/10mg (99%C10). Diamond
powder (99.9%) costs about $40/g. | [Uses]
Crucibles, retorts, foundry facings, molds,
lubricants, paints and coatings, boiler compounds,
powder glazing, electrotyping, monochromator in
X-ray diffraction analysis, fluorinated graphite
polymers with fluorine-to-carbon ratios of 0.1–1.25,
electrodes, bricks, chemical equipment, motor and
generator brushes, seal rings, rocket nozzles, moderator
in nuclear reactors, cathodes in electrolytic
cells, pencils, fibers, self-lubricating bearings, intercalation
compounds. | [CAS DataBase Reference]
7440-44-0(CAS DataBase Reference) | [NIST Chemistry Reference]
Carbon(7440-44-0) | [EPA Substance Registry System]
7440-44-0(EPA Substance) |
| Hazard Information | Back Directory | [Description]
All our SWNTs come packed as dry powders, which can be dispersed within the user's solvent of choice. | [General Description]
Black grains that have been treated to improve absorptive ability. May heat spontaneously if not properly cooled after manufacture. | [Reactivity Profile]
CARBON, ACTIVATED(7440-44-0) is incompatible with very strong oxidizing agents such as fluorine, ammonium perchlorate, bromine pentafluoride, bromine trifluoride, chlorine trifluoride, dichlorine oxide, chlorine trifluoride, potassium peroxide, etc. . Also incompatible with air, metals, unsaturated oils. [Lewis]. | [Air & Water Reactions]
Highly flammable. Dust is explosive when exposed to heat or flame. Freshly prepared material can heat and spontaneously ignite in air. The presence of water assists ignition, as do contaminants such as oils. Insoluble in water. | [Hazard]
(Powder, natural) Fire risk. | [Health Hazard]
Fire may produce irritating and/or toxic gases. Contact may cause burns to skin and eyes. Contact with molten substance may cause severe burns to skin and eyes. Runoff from fire control may cause pollution. | [Potential Exposure]
Natural graphite is used in foundry
facings, steel making lubricants, refractories, crucibles,
pencil “l(fā)ead,” paints, pigments, and stove polish. Artificial
graphite may be substituted for these uses with the excep tion of clay crucibles; other types of crucibles may be pro duced from artificial graphite. Additionally, it may be used
as a high temperature lubricant or for electrodes. It is uti lized in the electrical industry in electrodes, brushes, con tacts, and electronic tube rectifier elements; as a constituent
in lubricating oils and greases; to treat friction elements,
such as brake linings; to prevent molds from sticking
together; and in moderators in nuclear reactors. In addition,
concerns have been expressed about synthetic graphite in
fibrous form. Those exposed are involved in production of
graphite fibers from pitch or acrylonitrile fibers and the
manufacture and use of composites of plastics, metals, or
ceramics reinforced with graphite fibers. | [Fire Hazard]
Flammable/combustible material. May be ignited by friction, heat, sparks or flames. Some may burn rapidly with flare burning effect. Powders, dusts, shavings, borings, turnings or cuttings may explode or burn with explosive violence. Substance may be transported in a molten form at a temperature that may be above its flash point. May re-ignite after fire is extinguished. | [First aid]
If this chemical gets into the eyes, remove any
contact lenses at once and irrigate immediately for at least
15 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, includ ing 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 medi cal attention. Give large quantities of water and induce
vomiting. Do not make an unconscious person vomit. | [Shipping]
UN1362 Carbon, activated, Hazard Class: 4.2;
Labels: 4.2-Spontaneously combustible material, International. | [Incompatibilities]
Graphite is a strong reducing agent and
reacts violently with oxidizers, such as fluorine, chlorine
trifluoride, and potassium peroxide. Forms an explosive
mixture with air. May be spontaneously combustible in air. | [Chemical Properties]
Carbon, C, is a nonmetallic element, grey solid. It is found in nature as graphite (specific gravity2.25), diamond(specific gravity 3.51), and coal (specific gravity 1.88). Carbon is found in all living things, is insoluble in common solvents,and forms an almost infinite numberof organic compounds. Anaturally occurring radioactive isotope,14C, has a half-life of 5780 years and is used in archaeo logical investigations to date artifacts and ancient documents. Other uses of carbon depend on its form. For example, diamonds for jewels and abrasives,graphite for lubricants, activated carbon to absorb color and gases, and wood carbon for fuel are some common examples.
| [Chemical Properties]
Graphite is crystallized carbon and usually
appears as soft, black scales. There are two types of graph ite, natural and artificial (activated). Natural and synthetic
graphite may be mixed with each other or contain other
additives. | [Waste Disposal]
Do not incinerate. Carbon
(graphite) fibers are difficult to dispose of by incineration.
Waste fibers should be packaged and disposed of in a land fill authorized for the disposal of special wastes of this
nature, or as otherwise may be required by law. | [Physical properties]
All the elements in group 14 have four electrons in their outer valence shell. Carbon exhibitsmore nonmetallic properties than do the others in group 14 and is unique in several ways.It has four forms, called allotropes:
1. Carbon black is the amorphous allotrope (noncrystal form) of carbon. It is produced byheating coal at high temperatures (producing coke); burning natural gas (producing jetblack); or burning vegetable or animal matter (such as wood and bone), at high temperatureswith insufficient oxygen, which prevents complete combustion of the material, thusproducing charcoal.
2. Graphite is a unique crystal structure of carbon wherein layers of carbon atoms are stackedparallel to each other and can extend indefinitely in two dimensions as in the shafts ofcarbon fiber golf clubs. Graphite is also one of the softest elements, making it an excellentdry lubricant.
3. Diamonds are another allotrope whose crystal structure is similar to graphite. Naturaldiamonds were formed under higher pressure and extreme temperatures. Synthetic diamondshave been artificially produced since 1955.
4. Fullerenes are another amorphous (no crystal structure) form of carbon that have the basicformula of C60H60 and are shaped like a soccer ball. (See the “Atomic Structure” sectionof the book for more on fullerenes.)
The different allotropes of carbon were formed under varying conditions in the Earth,starting with different minerals, temperature, pressure, and periods of time. Once the distinctcrystal structures are formed, they are nearly impossible to change.
Carbon-12 is the basis for the average atomic mass units (amu) that is used to determinethe atomic weights of the elements. Carbon is one of the few elements that can form covalentbonds with itself as well as with many metals and nonmetals. | [Isotopes]
There are 15 isotopes of carbon, two of which are stable. Stable carbon-12makes up 98.89% of the element’s natural abundance in the Earth’s crust, and carbon-13 makes up just 1.11% of carbon’s abundance in the Earth’s crust. All the otherisotopes of carbon are radioactive with half-lives varying from 30 nanoseconds (C-21) to5,730 years (C-14). | [Origin of Name]
Carbon’s name is derived from the Latin word carbo, which means,
“charcoal.” | [Occurrence]
Carbon is the 14th most abundant element, making up about 0.048% of the Earth’s crust.It is the sixth most abundant element in the universe, which contains 3.5 atoms of carbonfor every atom of silicon. Carbon is a product of the cosmic nuclear process called fusion,through which helium nuclei are “burned” and fused together to form carbon atoms withthe atomic number 12. Only five elements are more abundant in the universe than carbon:hydrogen, helium, oxygen, neon, and nitrogen. | [Characteristics]
Carbon is, without a doubt, one of the most important elements on Earth. It is the majorelement found in over one million organic compounds and is the minor component in mineralssuch as carbonates of magnesium and calcium (e.g., limestone, marble, and dolomite),coral, and shells of oysters and clams.The carbon cycle, one of the most essential of all biological processes, involves the chemicalconversion of carbon dioxide to carbohydrates in green plants by photosynthesis.
Animalsconsume the carbohydrates and, through the metabolic process, reconvert the carbohydratesback into carbon dioxide, which is returned to the atmosphere to continue the cycle. | [Agricultural Uses]
Carbon (C) is found in every living being as it forms the
major constituent of living cells. As an essential element
for plants and animals, carbon is derived from
atmospheric carbon dioxide assimilated by plants and
photoautotrophic microbes during photosynthesis.
Carbon occurs in nature both in an elemental form and as
compounds. For example, coal contains elemental
carbon which, upon heating in the absence of air, loses
the volatile substances, and gives coke. Both coal and
coke are amorphous (non-crystalline) forms of carbon.
The two crystalline forms of carbon are diamond and
graphite. These are called the two allotropes of carbon.
Allotropes are two or more forms of an element that exist
in different physical forms, and differ in the bonding or
molecular structure of their fundamental units. Carbon is
found in a combined state in all living organisms, as well
as in fossil fuels such as methane and petroleum. It also
occurs in large amounts in carbonates such as limestone.
Carbon, a non-metallic element, is found at the head
of Group 14 (formerly IV) in the Periodic Table. It is unique in the variety and complexity of
compounds it forms, which is due to the ability of carbon
atoms to bond to one another in long chains, rings and
combinations of rings and chains. Carbon in combination
with H, O, N, S and other elements produces such a
variety of compounds, that a separate branch of
chemistry called organic chemistry, came into being
around carbon compounds.
Elemental carbon is a fairly inert substance. It is
insoluble in water, dilute acids and bases, and organic
solvents.
Each carbon atom has four valence electrons and
these tend to share with other atoms in the formation of
four covalent bonds. Carbon forms two oxides - carbon
monoxide (CO) and carbon dioxide (CO2)-which are
formed when carbon or carbon-containing compounds
are burned in insufficient or inexcess air, respectively.
The free element has many uses, ranging from
ornamental applications as diamond in jewelry to the
black-colored pigment of carbon black in automobile
tires and printing inks. Graphite, another form of carbon,
is used for high temperature crucibles, arc lights, dry-cell
electrodes, lead pencils and as a lubricant.
Charcoal, an amorphous form of carbon, is used as
an absorbent for gases and as a decolorizing agent in its
activated form. | [Purification Methods]
Charcoal (50g) is added to 1L of 6M HCl and boiled for 45minutes. The supernatant is discarded, and the charcoal is boiled with two more lots of HCl, then with distilled water until the supernatant no longer gives a test for chloride ion. The charcoal (now phosphate-free) is filtered onto a sintered-glass funnel and air dried at 120o for 24hours. [Lippin et al. J Am Chem Soc 76 2871 1954.] The purification can be carried out using a Soxhlet extractor (without cartridge), allowing longer extraction times. Treatment with conc H2SO4 instead of HCl has been used to remove reducing substances. |
| Safety Data | Back Directory | [Hazard Codes ]
F,Xn,Xi | [Risk Statements ]
R36/37:Irritating to eyes and respiratory system .
R36/37/38:Irritating to eyes, respiratory system and skin .
R20:Harmful by inhalation.
R10:Flammable. | [Safety Statements ]
S26:In case of contact with eyes, rinse immediately with plenty of water and seek medical advice .
S36:Wear suitable protective clothing .
S24/25:Avoid contact with skin and eyes .
S22:Do not breathe dust .
S36/37:Wear suitable protective clothing and gloves . | [RIDADR ]
UN 1325 4.1/PG 3
| [WGK Germany ]
3
| [RTECS ]
FF5250100
| [Autoignition Temperature]
842 °F | [TSCA ]
Yes | [HazardClass ]
4.2 | [PackingGroup ]
III | [HS Code ]
38021000 | [Safety Profile]
Moderately toxic by
intravenous route. Experimental
reproductive effects. It can cause a dust
irritation, particularly to the eyes and
mucous membranes. See also CARBON
BLACK, SOOT. Combustible when
exposed to heat. Dust is explosive when
exposed to heat or flame or oxides,
peroxides, oxosalts, halogens, interhalogens,
02, (NH4NO3 + heat), (NH4ClO4 @ 240°),
bromates, Ca(OCl)2, chlorates, (Cla +
Cr(OCl)2), Cl0, iodates, 105, Pb(NO3)~,
HgNO3, HNO3, (oils + air), (K + air), NaaS,
Zn(NO3)a. Incompatible with air, metals,
oxidants, unsaturated oils. | [Hazardous Substances Data]
7440-44-0(Hazardous Substances Data) | [Toxicity]
LD50 intravenous in mouse: 440mg/kg |
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