|Standard atomic weight Ar, std(H)||[1.00784, 1.00811] conventional: 1.008Template:Infobox element/symbol-to-saw/CIAAW-saw-element-page|
|Hydrogen in the periodic table|
|Atomic number (Z)||1|
|Group||group 1: hydrogen and alkali metals|
|Electrons per shell||1|
|Phase at STP||gas|
|Melting point||13.99 K (−259.16 °C, −434.49 °F)|
|Boiling point||20.271 K (−252.879 °C, −423.182 °F)|
|Density (at STP)||0.08988 g/L|
|when liquid (at m.p.)||0.07 g/cm3 (solid: 0.0763 g/cm3)|
|when liquid (at b.p.)||0.07099 g/cm3|
|Triple point||13.8033 K, 7.041 kPa|
|Critical point||32.938 K, 1.2858 MPa|
|Heat of fusion||(H2) 0.117 kJ/mol|
|Heat of vaporization||(H2) 0.904 kJ/mol|
|Molar heat capacity||(H2) 28.836 J/(mol·K)|
|Oxidation states||−1, +1 (an amphoteric oxide)|
|Electronegativity||Pauling scale: 2.20|
|Covalent radius||31±5 pm|
|Van der Waals radius||120 pm|
|Spectral lines of hydrogen|
|Speed of sound||1310 m/s (gas, 27 °C)|
|Thermal conductivity||0.1805 W/(m⋅K)|
|Molar magnetic susceptibility||−3.98·10−6 cm3/mol (298 K)|
|CAS Number||12385-13-6 |
|Discovery||Henry Cavendish (1766)|
|Named by||Antoine Lavoisier (1783)|
|Main isotopes of hydrogen|
Hydrogen is the most common chemical element in the Universe, making up 75% of all normal (baryonic) matter (by mass). Most stars are mostly hydrogen. Hydrogen's most common isotope has one proton with one electron orbiting around it.
Properties[change | change source]
Hydrogen is classed as a reactive nonmetal, unlike the other elements appearing in the first column of the periodic table, which are classed alkali metals. The solid form of hydrogen is expected to behave like a metal, however.
When alone, hydrogen usually binds with itself to make dihydrogen (H2) which is very stable, due to its high bond dissociation energy of 435.7 kJ/mol. At standard temperature and pressure, this hydrogen gas (H2) has no colour, smell or taste. It is not toxic. It is a nonmetal and burns very easily.
Combustion[change | change source]
Molecular hydrogen is flammable and reacts with oxygen:
2 H2(g) + O2(g) → 2 H2O(l) + 572 kJ (286 kJ/mol)
At temperatures above 500 degrees Celsius, hydrogen spontaneously ignites in air.
Compounds[change | change source]
While hydrogen gas in its pure form is not reactive, it does form compounds with many elements, particularly halogens, which are very electronegative. Hydrogen also forms vast arrays with carbon atoms, forming hydrocarbons. The study of the properties of hydrocarbons are known as organic chemistry.
The H- anion (negatively charged atom) is called a hydride, although the term is not widely used. An example of a hydride is lithium hydride (LiH), which is used as a "spark plug" in nuclear weapons.
Acids[change | change source]
Acids dissolved in water typically contain high levels of hydrogen ions, in other words, free protons. The level of them is usually used to determine its pH, which basically means the content of hydrogen ions in a particular volume. For example, hydrochloric acid, found in people's stomachs, can dissociate into a chloride anion and a free proton, and the property of the free proton is how it can digest food by corroding it.
Although rare on Earth, the H3+ cation is one of the most common ions in the universe.
Isotopes[change | change source]
- Main article: isotopes of hydrogen
Hydrogen has 7 known isotopes, two of which are stable (1H and 2H), which are commonly referred to protium and deuterium. The isotope 3H is known as tritium and has a half life of 12.33 years, and is produced in small amounts by cosmic rays. The remaining 4 isotopes have half lives on the scale of yoctoseconds.
Hydrogen in nature[change | change source]
In its pure form on Earth, hydrogen is usually a gas. Hydrogen is also one of the parts that make up a water molecule. Hydrogen is important because it is the fuel that powers the Sun and other stars. Hydrogen makes up about 74% of the entire universe. Hydrogen's symbol on the Periodic Table of Elements is H.
Pure hydrogen is normally made of two hydrogen atoms connected together. Scientists call these diatomic molecules. Hydrogen will have a chemical reaction when mixed with most other elements. It has no color or smell.
Pure hydrogen is very uncommon in the Earth's atmosphere, because nearly all primordial hydrogen would have escaped into space due to its weight. In nature, it is usually in water. Hydrogen is also in all living things, as a part of the organic compounds that living things are made of. In addition, hydrogen atoms can combine with carbon atoms to form hydrocarbons. Petroleum and other fossil fuels are made of these hydrocarbons and commonly used to create energy for human use.
Some other facts about hydrogen:
- It is a gas at room temperature
- It acts like a metal when it is solid.
- It is the lightest element in the Universe.
- It is the most common element in the Universe.
- It burns or explodes above 1000°F / 528°C, such as in fire.
- glows purple when it is in plasma state.
History of Hydrogen[change | change source]
Uses of Hydrogen[change | change source]
The main uses are in the petroleum industry and in making ammonia by the Haber process. Some is used elsewhere in the chemical industry. A little of it is used as fuel, for example in rockets for spacecraft. Most of the hydrogen that people use comes from a chemical reaction between natural gas and steam.
Nuclear fusion[change | change source]
Nuclear fusion is a very powerful source of energy. It relies on forcing atoms together to make helium and energy, exactly as happens in a star like the Sun, or in a hydrogen bomb. This needs a large amount of energy to get started, and is not easy to do yet. A big advantage over nuclear fission, which is used in today's nuclear power stations, is that it makes less nuclear waste and does not use a toxic and rare fuel like uranium. More than 600 million tons of hydrogen undergo fusion every second on the Sun.
Using hydrogen[change | change source]
Hydrogen is mostly used in the petroleum industry, to change heavy petroleum fractions into lighter, more useful ones. It is also used to make ammonia. Smaller amounts are burned as fuel. Most hydrogen is made by a reaction between natural gas and steam.
The electrolysis of water breaks water into hydrogen and oxygen, using electricity. Burning hydrogen combines with oxygen molecules to make steam (pure water vapor). A fuel cell combines hydrogen with an oxygen molecule, releasing an electron as electricity. For these reasons, many people believe hydrogen power will eventually replace other synthetic fuels.
Hydrogen can also be burned to make heat for steam turbines or internal combustion engines. Like other synthetic fuels, hydrogen can be created from natural fuels such as coal or natural gas, or from electricity, and therefore represents a valuable addition to the power grid; in the same role as natural gas. Such a grid and infrastructure with fuel cell vehicles is now planned by a number of countries including Japan, Korea and many European countries. This allows these countries to buy less petroleum, which is an economic advantage. The other advantage is that used in a fuel cell or burned in a combustion engine as in a hydrogen car, the motor does not make pollution. Only water, and a small amount of nitrogen oxides, forms.
References[change | change source]
- Wiberg, Egon; Wiberg, Nils; Holleman, Arnold Frederick (2001). Inorganic chemistry. Academic Press. p. 240. ISBN 978-0123526519.
- Lide, D. R., ed. (2005). "Magnetic susceptibility of the elements and inorganic compounds". CRC Handbook of Chemistry and Physics (PDF) (86th ed.). Boca Raton (FL): CRC Press. ISBN 978-0-8493-0486-6.
- Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 978-0-8493-0464-4.
- "Hydrogen". Van Nostrand's Encyclopedia of Chemistry. Wylie-Interscience. 2005. pp. 797–799. ISBN 978-0-471-61525-5.
- Emsley, John (2001). Nature's Building Blocks. Oxford: Oxford University Press. pp. 183–191. ISBN 978-0-19-850341-5.
- Stwertka, Albert (1996). A Guide to the Elements. Oxford University Press. pp. 16–21. ISBN 978-0-19-508083-4.
- Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- Cain, Fraser, Universe Today (November 7, 2016). "When was the first light in the universe?". Phys.org. Retrieved 29 November 2016.
- EIA.doe.gov - What is Hydrogen?
- "The magic of syngas". chemrec.se. 2012. Retrieved 7 March 2012.
- "What is Fusion?". iter.org. ITER Organization. 2012. Retrieved 7 March 2012.
- "NASA's Cosmicopia". NASA. Archived from the original on 6 November 2011. Retrieved 28 February 2013.
Other websites[change | change source]
- Hydrogen -Citizendium