Hydrogen: Chemical element with symbol H and atomic number 1; lightest and most abundant substance in the universe

It has the symbol H and atomic number 1. It also has a standard atomic weight of 1.008, which makes it the lightest element in the periodic table.

Hydrogen, ₁H

Purple glow in its plasma state
Hydrogen
Appearance	Colorless gas
Standard atomic weight Ar°(H)
	[1.00784, 1.00811]
Hydrogen in the periodic table
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson – ↑ H ↓ Li Neutronium ← hydrogen → helium
Atomic number (Z)	1
Group	group 1: hydrogen and alkali metals
Period	period 1
Block	s-block
Electron configuration	1s1
Electrons per shell	1
Physical properties
Phase at STP	gas
Melting point	(H 2) 13.99 K ​(−259.16 °C, ​−434.49 °F)
Boiling point	(H 2) 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	(H 2) 0.117 kJ/mol
Heat of vaporization	(H 2) 0.904 kJ/mol
Molar heat capacity	(H 2) 28.836 J/(mol·K)
Vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 15 20
Atomic properties
Oxidation states	−1, 0, +1 (an amphoteric oxide)
Electronegativity	Pauling scale: 2.20
Ionization energies	1st: 1312.0 kJ/mol
Covalent radius	31±5 pm
Van der Waals radius	120 pm
Spectral lines of hydrogen
Other properties
Natural occurrence	primordial
Crystal structure	​hexagonal
Speed of sound	1310 m/s (gas, 27 °C)
Thermal conductivity	0.1805 W/(m⋅K)
Magnetic ordering	diamagnetic
Molar magnetic susceptibility	−3.98×10−6 cm3/mol (298 K)
CAS Number	12385-13-6 1333-74-0 (H 2)
History
Discovery	Henry Cavendish (1766)
Named by	Antoine Lavoisier (1783)
Isotopes of hydrogen v e
Main isotopes Decay abun­dance half-life (t1/2) mode pro­duct 1H 99.9855% stable 2H 0.0145% stable 3H trace 12.32 y β− 3He
Category: Hydrogen view talk edit | references

Hydrogen is the most common chemical element in the Universe, making up 75% of all normal (baryonic) matter (by mass). Most stars are made of mostly hydrogen. Hydrogen's most common isotope has one proton with one electron orbiting around it.

Hydrogen is grouped as a reactive nonmetal, unlike the other elements found in the first column of the periodic table, which are grouped as alkali metals. The solid form of hydrogen should behave like a metal, though.

When by itself, hydrogen normally binds with itself to make dihydrogen (H₂) which is very stable, because of its high bond-dissociation energy of 435.7 kJ/mol. At normal temperature and pressure, this hydrogen gas (H₂) has no color, smell, or taste and is not poisonous as it is a nonmetal and burns very easily.

Combustion

Molecular hydrogen is flammable and reacts with oxygen:

2 H₂(g) + O₂(g) → 2 H₂O(l) + 572 kJ (286 kJ/mol)

At temperatures higher than 500 °C, hydrogen suddenly burns in air.^[source?]

Compounds

While hydrogen gas in its natural form is not reactive, it does form compounds with many elements, especially halogens, which are very electronegative, meaning they want an electron very badly. Hydrogen also forms massive arrays with carbon atoms, forming hydrocarbons. The study of the properties of hydrocarbons is known as organic chemistry.

The H^- anion (negatively charged atom) is named a hydride, though the word is not commonly used. An example of a hydride is lithium hydride (LiH), which is used as a "spark plug" in nuclear weapons.

Acids

Acids dissolved in water normally contain high levels of hydrogen ions, in other words, free protons. Their level is generally used to determine its pH, that is, the content of hydrogen ions in a 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.

Though uncommon on Earth, the H₃⁺ cation is one of the most common ions in the universe.

Isotopes

Hydrogen has 7 known isotopes, two of which are stable (¹H and ²H), which are commonly named protium and deuterium. The isotope ³H is known as tritium, has a half-life of 12.33 years, and is produced in small amounts by cosmic rays. The 4 isotopes left have half-lives on the scale of yoctoseconds.

In its natural form on Earth, hydrogen is generally 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 complete universe.

Natural hydrogen is normally made of two hydrogen atoms connected together. Scientists name these diatomic molecules. Hydrogen will have a chemical reaction when mixed with most other elements, though it has no color or smell.

Natural hydrogen is very uncommon in the Earth's atmosphere, because nearly all primordial hydrogen would have escaped into space because of its weight. In nature, it is generally 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 join with carbon atoms to form hydrocarbons. Petroleum and other fossil fuels are made of these hydrocarbons and commonly used to make energy.

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 at temperatures higher than 1000°F / 528°C, such as in fire.
• It glows purple when it is in plasma state.

Hydrogen was first separated in 1671 by Robert Boyle. In 1776, Henry Cavendish identified it as its own element and named it "inflammable air". He saw in 1781 that burning it made water.

Antoine Lavoisier gave Hydrogen its name, from the Greek word for water, 'υδορ (read /HEEW-dor/) and gennen meaning to "produce" as it forms water in a chemical reaction with oxygen.

The most common uses are in the petroleum industry and in making ammonia by the Haber process. Some is used in other places 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

Nuclear fusion is a very powerful source of energy. It depends on forcing atoms together to make helium and energy, as 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 currently. 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 poisonous and uncommon fuel like uranium. More than 600 million tons of hydrogen undergo fusion every second on the Sun.

Using hydrogen

Hydrogen is mostly used in the petroleum industry, to change heavy petroleum parts 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 joins with oxygen molecules to make steam (natural water vapor). A fuel cell joins hydrogen with an oxygen molecule, releasing an electron as electricity. For these reasons, many people believe hydrogen power will replace other synthetic fuels in the future.

Hydrogen can also be burned to make heat for steam turbines or internal combustion engines. Like other synthetic fuels, hydrogen can be made 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, such as Japan, Korea and many European countries. This lets these countries 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 engine does not make pollution. Only water, and a small amount of nitrogen oxides, forms.