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Hydrogen (/ˈhaɪdrɵdʒən/ HY-drə-jən)[7] is a chemical element with symbol H and atomic number 1. With an average atomic weight of 1.00794 u (1.007825 u for hydrogen-1), hydrogen is the lightest element and its monatomic form (H1) is the most abundant chemical substance. At standard temperature and pressure, hydrogen is a colourless, odorless, tasteless, non-toxic, nonmetallic, highly combustible diatomic gas with the molecular formula H2. Naturally occurring atomic hydrogen is rare on Earth because hydrogen readily forms covalent compounds with most elements and is present in the water molecule and in most organic compounds. Hydrogen plays a particularly important role in acid-base chemistry with many reactions exchanging protons between soluble molecules. In ionic compounds, it can take a negative charge (an anion known as a hydride and written as H−), or as a positively charged species H+. The latter cation is written as though composed of a bare proton, but in reality, hydrogen cations in ionic compounds always occur as more complex species. The most common isotope of hydrogen is protium (name rarely used, symbol 1H) with a single proton and no neutrons. As the simplest atom known, the hydrogen atom has been of theoretical use. For example, as the only neutral atom with an analytic solution to the Schrödinger equation, the study of the energetics and bonding of the hydrogen atom played a key role in the development of quantum mechanics. Deuterium (symbol D or 2H, also known as heavy hydrogen) is one of two stable isotopes of hydrogen. It has a natural abundance in Earth's oceans of about one atom in 6,420 of hydrogen (~156.25 ppm on an atom basis). Deuterium accounts for approximately 0.0156 percent (or on a mass basis: 0.0312 percent) of all the naturally occurring hydrogen in the oceans, while the most common isotope (hydrogen-1 or protium) accounts for more than 99.98 percent. The abundance of deuterium changes slightly from one kind of natural water to another. The nucleus of deuterium, called a deuteron, contains one proton and one neutron, whereas the far more common hydrogen isotope, protium, has no neutron in the nucleus. The deuterium isotope's name is formed from the Greek deuteros meaning "second", to denote the two particles composing the nucleus. Deuterium was discovered and named in 1931 by Harold Urey, earning him a Nobel Prize in 1934. This followed the discovery of the neutron in 1932, which made the nuclear structure of deuterium obvious. Soon after deuterium's discovery, Urey and others produced samples of "heavy water" in which the deuterium has been highly concentrated with respect to the protium. Tritium (/ˈtrɪtiəm/ or /ˈtrɪʃiəm/; symbol T or 3H, also known as hydrogen-3) is a radioactive isotope of hydrogen. The nucleus of tritium (sometimes called a triton) contains one proton and two neutrons, whereas the nucleus of protium (by far the most abundant hydrogen isotope) contains one proton and no neutrons. Naturally occurring tritium is extremely rare on Earth, where trace amounts are formed by the interaction of the atmosphere with cosmic rays. The name of this isotope is formed from the Greek word "tritos" meaning "third". Standard form of the periodic table. The colors represent different series of elements explained below. A periodic table is a tabular display of the chemical elements, organized on the basis of their atomic numbers, electron configurations, and recurring chemical properties. Elements are presented in increasing atomic number. The main body of the standard form of table is an 18 × 7 grid, and elements with the same number of valence electrons are kept together in groups, such as the halogens and the noble gases. There are four distinct rectangular areas or blocks. The f-block is usually not included in the main table, but rather is floated below, as an inline f-block would often make the table impractically wide. Using periodic trends, the periodic table can help predict the properties of various elements and the relations between properties. As a result it provides a useful framework for analyzing chemical behavior, and is widely used in chemistry and other sciences. t e Periodic table (standard form) Group → 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 ↓ Period 1 1 2 He H 3 2 4 LB ie 5 B 3 1 112 M Ng a 13 14 15 16 17 18 Al Si P S Cl Ar 6 C 7 8 N O 9 10 F Ne 4 5 6 7 1 920 25 21 22 23 24 26 27 28 29 30 31 32 33 34 35 36 C M Sc Ti V Cr Fe Co Ni Cu Zn Ga Ge As Se Br Kr Ka n 3 7 42 38 39 40 41 43 44 45 46 47 48 49 50 51 52 53 54 M RSr Y Zr Nb Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe o b 5 5 56 * 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 B C Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn a s 8 7 11 11 11 88 10 10 10 10 10 10 11 11 11 11 11 ** 3 5 7 R 4 5 6 7 8 9 0 1 2 4 6 F Uu Uu Uu a Rf Db Sg Bh Hs Mt Ds Rg Cn Fl Lv r t p s * Lanthanides ** Actinides 69 57 58 59 60 61 62 63 64 65 66 67 68 70 T La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Yb m 10 95 96 10 10 89 90 91 92 93 94 97 98 99 1 A C 0 2 Ac Th Pa U Np Pu Bk Cf Es M m m Fm No d 11 8 Uu o 71 Lu 10 3 Lr This is an 18-column periodic table layout, which has come to be referred to as the common or standard form, on account of its popularity. It is also sometimes referred to as the long form, in comparison to the short form or Mendeleev-style, which omits groups 3–12. The wide periodic table incorporates the lanthanides and the actinides, rather than separating them from the main body of the table. The extended periodic table adds the 8th and 9th periods, including the superactinides. Some element categories in the periodic table Metals Nonmetals Unkno wn Alkali Inner transition Alka Post- Metallo Nob chemic ne metals Transit Other li transiti ids Halog le al earth ion nonmet meta on ens gase propert metal Lanthani Actini metals als ls metals s des des ies s Color of the atomic number shows state of matter Border shows (at standard conditions: 0 °C and 1 atm): black=S green=Li red= grey=Unkn olid quid Gas own natural occurrence : Primordial From decay Synthetic