ଉଇକିପିଡ଼ିଆ ରୁ
(ଉଦଜାନ ରୁ ଲେଉଟି ଆସିଛି)
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Hydrogen,  1H
Hydrogen discharge tube.jpg
Purple glow in its plasma state
Hydrogen Spectra.jpg
Spectral lines of hydrogen
ସାଧାରଣ ଗୁଣ
ନାମ, ପ୍ରତୀକhydrogen, H
Appearancecolorless gas
ଉଚ୍ଚାରଣ /ˈhdrəən/ HY-drə-jən[୧]
Hydrogen in the periodic table
Hydrogen (other non-metal)
Helium (noble gas)
Lithium (alkali metal)
Beryllium (alkaline earth metal)
Boron (metalloid)
Carbon (other non-metal)
Nitrogen (other non-metal)
Oxygen (other non-metal)
Fluorine (halogen)
Neon (noble gas)
Sodium (alkali metal)
Magnesium (alkaline earth metal)
Aluminium (post-transition metal)
Silicon (metalloid)
Phosphorus (other non-metal)
Sulfur (other non-metal)
Chlorine (halogen)
Argon (noble gas)
Potassium (alkali metal)
Calcium (alkaline earth metal)
Scandium (transition metal)
Titanium (transition metal)
Vanadium (transition metal)
Chromium (transition metal)
Manganese (transition metal)
Iron (transition metal)
Cobalt (transition metal)
Nickel (transition metal)
Copper (transition metal)
Zinc (transition metal)
Gallium (post-transition metal)
Germanium (metalloid)
Arsenic (metalloid)
Selenium (other non-metal)
Bromine (halogen)
Krypton (noble gas)
Rubidium (alkali metal)
Strontium (alkaline earth metal)
Yttrium (transition metal)
Zirconium (transition metal)
Niobium (transition metal)
Molybdenum (transition metal)
Technetium (transition metal)
Ruthenium (transition metal)
Rhodium (transition metal)
Palladium (transition metal)
Silver (transition metal)
Cadmium (transition metal)
Indium (post-transition metal)
Tin (post-transition metal)
Antimony (metalloid)
Tellurium (metalloid)
Iodine (halogen)
Xenon (noble gas)
Caesium (alkali metal)
Barium (alkaline earth metal)
Lanthanum (lanthanoid)
Cerium (lanthanoid)
Praseodymium (lanthanoid)
Neodymium (lanthanoid)
Promethium (lanthanoid)
Samarium (lanthanoid)
Europium (lanthanoid)
Gadolinium (lanthanoid)
Terbium (lanthanoid)
Dysprosium (lanthanoid)
Holmium (lanthanoid)
Erbium (lanthanoid)
Thulium (lanthanoid)
Ytterbium (lanthanoid)
Lutetium (lanthanoid)
Hafnium (transition metal)
Tantalum (transition metal)
Tungsten (transition metal)
Rhenium (transition metal)
Osmium (transition metal)
Iridium (transition metal)
Platinum (transition metal)
Gold (transition metal)
Mercury (transition metal)
Thallium (post-transition metal)
Lead (post-transition metal)
Bismuth (post-transition metal)
Polonium (post-transition metal)
Astatine (halogen)
Radon (noble gas)
Francium (alkali metal)
Radium (alkaline earth metal)
Actinium (actinoid)
Thorium (actinoid)
Protactinium (actinoid)
Uranium (actinoid)
Neptunium (actinoid)
Plutonium (actinoid)
Americium (actinoid)
Curium (actinoid)
Berkelium (actinoid)
Californium (actinoid)
Einsteinium (actinoid)
Fermium (actinoid)
Mendelevium (actinoid)
Nobelium (actinoid)
Lawrencium (actinoid)
Rutherfordium (transition metal)
Dubnium (transition metal)
Seaborgium (transition metal)
Bohrium (transition metal)
Hassium (transition metal)
Meitnerium (unknown chemical properties)
Darmstadtium (unknown chemical properties)
Roentgenium (unknown chemical properties)
Copernicium (transition metal)
Ununtrium (unknown chemical properties)
Flerovium (unknown chemical properties)
Ununpentium (unknown chemical properties)
Livermorium (unknown chemical properties)
Ununseptium (unknown chemical properties)
Ununoctium (unknown chemical properties)


- ← hydrogenhelium
ପରମାଣୁ କ୍ରମାଙ୍କ (Z)1
ଶ୍ରେଣୀ, ବ୍ଳକgroup 1, s-block
ପର୍ଯ୍ୟାୟperiod 1
ମୌଳିକ ପ୍ରକାର  nonmetal
ମାନକ ପରମାଣବିକ ଓଜନ (±) (Ar)1.008(1)
ଇଲେକ୍‌ଟ୍ରୋନ୍ ବିନ୍ୟାସ1s1
per shell
ଭୌତିକ ଗୁଣ
ଗଳନାଙ୍କ14.01 K ​(-259.14 °C, ​-434.45 °F)
ସ୍ଫୁଟନାଙ୍କ20.28 K ​(-252.87 °C, ​-423.17 °F)
ଘନତା at stp (0 °C and 101.325 kPa)0.08988 g/L
when liquid, at m.p.0.07 (0.0763 solid)[୨] g/cm3
when liquid, at b.p.0.07099 g/cm3
Triple point13.8033 K, ​7.042 kPa
Critical point32.97 K, 1.293 MPa
Heat of fusion(H2) 0.117 kJ/mol
Heat of (H2) 0.904 kJ/mol
Molar heat capacity(H2) 28.836 J/(mol·K)
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 15 20
Atomic properties
Oxidation states1, -1 ​amphoteric oxide
ElectronegativityPauling scale: 2.20
Covalent radius31±5 pm
Van der Waals radius120 pm
Crystal structurehexagonal
Hexagonal crystal structure for hydrogen
Speed of sound(gas, 27 °C) 1310 m/s
Thermal conductivity0.1805 W/(m·K)
Magnetic orderingdiamagnetic[୩]
CAS Number1333-74-0
ଆବିଷ୍କାରHenry Cavendish[୪][୫] (1766)
Named byAntoine Lavoisier[୬] (1783)
Most stable isotopes of hydrogen
iso NA half-life DM DE (MeV) DP
1H 99.985% 1H is stable with 0 neutrons
2H 0.015% 2H is stable with 1 neutron
3H trace 12.32 y β 0.01861 3He
| references

ଉଦଜାନ (ଇଂରାଜୀ: Hydrogen; ହାଇଡ୍ରୋଜେନ୍) ଏକ ରାସାୟନିକ ମୌଳିକ ଓ ଏହାର ପ୍ରତୀକ H, ପରମାଣୁ କ୍ରମାଙ୍କ ୧, ପରମାଣବିକ ବସ୍ତୁତ୍ୱ ୧.୦୦୭ ୯୪ amu । ଉଦଜାନ ସବୁଠାରୁ ହାଲୁକା ମୌଳିକ ଓ ଏହାର ଏକ-ପରମାଣବିକ ଅବସ୍ଥା ବିଶ୍ୱର ସବୁଠାରୁ ପ୍ରଚୁର ପରିମାଣରେ ମିଳୁଥିବା ମୌଳିକ ଅଟେ (ପାଖାପାଖି ୭୫% ପ୍ରତିଶତ) ।[୭][ଟୀକା ୧]


  1. Simpson, J.A.; Weiner, E.S.C. (1989). "Hydrogen". Oxford English Dictionary. 7 (2nd ed.). Clarendon Press. ISBN 0-19-861219-2.
  2. Wiberg, Egon; Wiberg, Nils; Holleman, Arnold Frederick (2001). Inorganic chemistry. Academic Press. p. 240. ISBN 0123526515.CS1 maint: multiple names: authors list (link)
  3. "Magnetic susceptibility of the elements and inorganic compounds". [[CRC Handbook of Chemistry and Physics]] (PDF) (81st ed.). CRC Press. URL–wikilink conflict (help)
  4. "Hydrogen". Van Nostrand's Encyclopedia of Chemistry. Wylie-Interscience. 2005. pp. 797–799. ISBN 0-471-61525-0.
  5. Emsley, John (2001). Nature's Building Blocks. Oxford: Oxford University Press. pp. 183–191. ISBN 0-19-850341-5.
  6. Stwertka, Albert (1996). A Guide to the Elements. Oxford University Press. pp. 16–21. ISBN 0-19-508083-1.
  7. Palmer, D. (13 September 1997). "Hydrogen in the Universe". NASA. Retrieved 2008-02-05.

freshney.org periodic table

Sources Found chiefly combined with oxygen in the form of water, also found in mines and oil and gas wells. Stars contain a virtually unlimited supply of hydrogen and in the universe, hydrogen is the most abundant element (hydrogen makes up 75% of the mass of the visible universe and over 90% by number of atoms.). Annual world production of hydrogen is around 350 billion cubic metres.


Universe: 7.5 x 105 ppm (by weight)  
Sun: 7.5 x 105 ppm (by weight)  
Carbonaceous meteorite: 24000 ppm 
Earth's Crust: 1500 ppm 
Seawater: 107800 ppm 
  1 x 108 ppb by weight  
  6.2 x 108 ppb by atoms  

Uses Hydrogen's uses include: being used in the production of ammonia (NH3), ethanol (C2H5OH), hydrogen chloride (HCl) and hydrogen bromide (HBr); the hydrogenation of vegetable oils; hydrocracking, hydroforming and hydrofining of petroleum; atomic-hydrogen welding; instrument-carrying balloons; fuel in rockets; and cryogenic research. Its two heavier isotopes, deuterium (D) and tritium (T), are used respectively for nuclear fission and fusion. Hydrogen fuel cells are being investigated as mobile power sources with lower emissions than hydrogen-burning internal combustion engines. The low emissions of hydrogen in internal combustion engines and fuel cells are currently offset by the pollution created by hydrogen production. This may change if the substantial amounts of electricity required for water electrolysis can be generated primarily from low pollution sources such as solar energy or wind. Research is being conducted on H2 as a replacement for fossil fuels.

History Hydrogen gas, H2, was first artificially produced and formally described by T. Von Hohenheim (also known as Paracelsus, 1493 - 1541) via the mixing of metals with strong acids. He was unaware that the flammable gas produced by this chemical reaction was a new chemical element. In 1671, Robert Boyle rediscovered and described the reaction between iron filings and dilute acids, which results in the production of hydrogen gas. In 1766, Henry Cavendish was the first to recognize hydrogen gas as a discrete substance, by identifying the gas from a metal-acid reaction as "inflammable air" and further finding that the gas produces water when burned. Cavendish had stumbled on hydrogen when experimenting with acids and mercury. Although he wrongly assumed that hydrogen was a liberated component of the mercury rather than the acid, he was still able to accurately describe several key properties of hydrogen. He is usually given credit for its discovery as an element. In 1783, Antoine Lavoisier gave the element the name of hydrogen when he (with Laplace) reproduced Cavendish's finding that water is produced when hydrogen is burned. Lavoisier's name for the gas won out. One of the first uses of H2 was for balloons, and later airships. The H2 was obtained by reacting sulphuric acid and metallic iron. Infamously, H2 was used in the Hindenburg airship that was destroyed in a midair fire. The highly flammable hydrogen (H2) was later replaced for airships and most balloons by the unreactive helium (He).

Notes At standard temperature and pressure, hydrogen exists as the diatomic gas, H2, with a boiling point of 20.27 K, and a melting point of 14.02 K. Under extreme pressures, such as those at the center of gas giants, the molecules lose their identity and the hydrogen becomes a metal (metallic hydrogen). Under the extremely low pressure in space - virtually a vacuum - the element tends to exist as individual atoms, simply because it is statistically unlikely for them to combine. A unique property of hydrogen is that its flame is nearly invisible in air.

Hazards Hydrogen is a tasteless, colourless, odourless and extremely flammable gas, it is also the lightest chemical element.


ଆହୁରି ପଢନ୍ତୁ[ସମ୍ପାଦନା]

  • Chart of the Nuclides (17th ed.). Knolls Atomic Power Laboratory. 2010. ISBN 978-0-9843653-0-2.
  • Ferreira-Aparicio, P (2005). "New Trends in Reforming Technologies: from Hydrogen Industrial Plants to Multifuel Microreformers". Catalysis Reviews. 47 (4): 491–588. doi:10.1080/01614940500364958. Unknown parameter |coauthors= ignored (|author= suggested) (help)
  • Newton, David E. (1994). The Chemical Elements. New York: Franklin Watts. ISBN 0-531-12501-7.
  • Rigden, John S. (2002). Hydrogen: The Essential Element. Cambridge, Massachusetts: Harvard University Press. ISBN 0-531-12501-7.
  • Romm, Joseph, J. (2004). The Hype about Hydrogen, Fact and Fiction in the Race to Save the Climate. Island Press. ISBN 1-55963-703-X.CS1 maint: multiple names: authors list (link) Author interview at Global Public Media.
  • Scerri, Eric (2007). The Periodic System, Its Story and Its Significance,. New York: Oxford University Press. ISBN 0-19-530573-6.

ବାହାର ଲିଙ୍କ[ସମ୍ପାଦନା]

ଆଧାର ଭୁଲ: <ref> ଟ୍ୟାଗସବୁ କେବଳ "ଟୀକା" ନାମକ ଦଳ ପାଇଁ ରହିଥିଲେ ହେଁ କୌଣସି ସମ୍ବନ୍ଧିତ <references group="ଟୀକା"/> ଟ୍ୟାଗ ମିଳିଲା ନାହିଁ କିମ୍ବା </ref> ବନ୍ଦ କରିବା ଟ୍ୟାଗଟି ନାହିଁ ।