Após os dados terem sido todos baixados, teremos um diretório local com 118 arquivos com o formato json, com os dados relativos a cada um dos elementos da tabela periódica.
O conteúdo dos arquivos é semelhante, sendo apresentado a seguir
{
"Record": {
"RecordType": "AtomicNumber",
"RecordNumber": 1,
"RecordTitle": "Hydrogen",
"Section": [
{
"TOCHeading": "Identifiers",
"Description": "Element names and identifiers, inluding atomic symbol, InChI string and InChI key.",
"Section": [
{
"TOCHeading": "Element Name",
"Description": "Element name refers to a formal name for a given elemnt originating from factors such as common usage and the person or place involved in its discovery. Element, also called chemical element, refers to a species of atoms; all atoms with the same number of protons in the atomic nucleus.",
"URL": "https://goldbook.iupac.org/html/C/C01022.html",
"Information": [
{
"ReferenceNumber": 1,
"Name": "Element Name",
"Value": {
"StringWithMarkup": [
{
"String": "Hydrogen"
}
]
}
},
{
"ReferenceNumber": 3,
"Name": "Element Name",
"Value": {
"StringWithMarkup": [
{
"String": "Hydrogen"
}
]
}
}
]
},
{
"TOCHeading": "Element Symbol",
"Description": "Element symbol, Also called atomic symbol, typically consists of one or two letters from the Latin alphabet derived from the element name in one of several languages.",
"URL": "https://goldbook.iupac.org/html/A/A00503.html",
"Information": [
{
"ReferenceNumber": 1,
"Name": "Element Symbol",
"Value": {
"StringWithMarkup": [
{
"String": "H"
}
]
}
},
{
"ReferenceNumber": 3,
"Name": "Element Symbol",
"Value": {
"StringWithMarkup": [
{
"String": "H"
}
]
}
}
]
},
{
"TOCHeading": "InChI",
"Description": "International Chemical Identifier (InChI) computed from chemical structure using the International Union of Pure and Applied Chemistry (IUPAC) standard.",
"URL": "http://www.iupac.org/home/publications/e-resources/inchi.html",
"Information": [
{
"ReferenceNumber": 1,
"Name": "InChI",
"Value": {
"StringWithMarkup": [
{
"String": "InChI=1S/H"
}
]
}
}
]
},
{
"TOCHeading": "InChI Key",
"Description": "International Chemical Identifier hash (InChIKey) computed from chemical structure using the International Union of Pure and Applied Chemistry (IUPAC) standard.",
"URL": "http://www.iupac.org/home/publications/e-resources/inchi.html",
"Information": [
{
"ReferenceNumber": 1,
"Name": "InChI Key",
"Value": {
"StringWithMarkup": [
{
"String": "YZCKVEUIGOORGS-UHFFFAOYSA-N"
}
]
}
}
]
}
]
},
{
"TOCHeading": "Properties",
"Description": "Element property refers to a set of data elements common to a set of particular properties, including atomic number, atomic mass, density, melting point, boiling point etc.",
"URL": "https://goldbook.iupac.org/html/P/P04883.html",
"Section": [
{
"TOCHeading": "Atomic Weight",
"Description": "Also called relative atomic mass, is the ratio of the average mass of the atom to the unified atomic mass unit. The Standard atomic weights refer to recommended values of relative atomic masses of the elements revised biennially by the IUPAC Commission on Atomic Weights and Isotopic Abundances and applicable to elements in any normal sample with a high level of confidence. The number in the parenthesis refers to an uncertainty when exist. The unit of atomic weight is [u] or [da], means unified atomic mass unit or dalton.",
"URL": "https://goldbook.iupac.org/html/R/R05258.html",
"Information": [
{
"ReferenceNumber": 3,
"Name": "Atomic Weight",
"Value": {
"StringWithMarkup": [
{
"String": "[1.007 84, 1.008 11]"
}
]
}
},
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "1.00794"
}
]
}
},
{
"ReferenceNumber": 5,
"Value": {
"StringWithMarkup": [
{
"String": "1.008"
}
]
}
},
{
"ReferenceNumber": 6,
"Name": "Atomic Weight",
"Value": {
"StringWithMarkup": [
{
"String": "[1.00784,1.00811]"
}
]
}
}
]
},
{
"TOCHeading": "Electron Configuration",
"Description": "The electron configuration refers a distribution of the electrons of an atom or a molecular entity over a set of one-electron wavefunctions called orbitals, according to the Pauli principle. From one configuration several states with different multiplicities may result.",
"URL": "https://goldbook.iupac.org/html/C/C01248.html",
"Information": [
{
"ReferenceNumber": 5,
"Value": {
"StringWithMarkup": [
{
"String": "1s1",
"Markup": [
{
"Start": 2,
"Length": 1,
"Type": "Superscript"
}
]
}
]
}
},
{
"ReferenceNumber": 6,
"Name": "Electron Configuration",
"Value": {
"StringWithMarkup": [
{
"String": "1s"
}
]
}
}
]
},
{
"TOCHeading": "Atomic Radius",
"Description": "Atomic radius is the distance from the centre of the nucleus to the outermost shell containing electrons.",
"URL": "https://en.wikipedia.org/wiki/Atomic_radius",
"Information": [
{
"ReferenceNumber": 5,
"Name": "Van der Waals Atomic Radius",
"Value": {
"StringWithMarkup": [
{
"String": "120 pm (Van der Waals)"
}
]
}
},
{
"ReferenceNumber": 8,
"Name": "Empirical Atomic Radius",
"Reference": [
"J.C. Slater, J Chem Phys, 1964, 41(10), 3199-3205. DOI:10.1063/1.1725697"
],
"Value": {
"Number": [
25
],
"Unit": "pm (Empirical)"
}
},
{
"ReferenceNumber": 8,
"Name": "Covalent Atomic Radius",
"Reference": [
"B. Cordero, V. Gómez, A.E. Platero-Prats, M. Revés, J. Echeverría, E. Cremades, F. Barragán, S. Alvarez, Dalton Trans. 2008, 21, 2832-2838. DOI:10.1039/b801115j PMID:18478144."
],
"Value": {
"StringWithMarkup": [
{
"String": "31(5) pm (Covalent)"
}
]
}
}
]
},
{
"TOCHeading": "Oxidation States",
"Description": "Oxidation state gives the degree of oxidation of an atom in terms of counting electrons.",
"URL": "https://goldbook.iupac.org/html/O/O04365.html",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "+1, -1"
}
]
}
},
{
"ReferenceNumber": 5,
"Value": {
"StringWithMarkup": [
{
"String": "−1, +1 (an amphoteric oxide)"
}
]
}
}
]
},
{
"TOCHeading": "Ground Level",
"Description": "Also called ground-state level. The ground state electron configuration is the arrangement of electrons around the nucleus of an atom with lower energy levels.",
"URL": "https://physics.nist.gov/PhysRefData/ASD/Html/iehelp.html#IEGROUNDLEV",
"Information": [
{
"ReferenceNumber": 6,
"Name": "Ground Level",
"Value": {
"StringWithMarkup": [
{
"String": "2S1/2",
"Markup": [
{
"Start": 0,
"Length": 1,
"Type": "Superscript"
},
{
"Start": 2,
"Length": 3,
"Type": "Subscript"
}
]
}
]
}
}
]
},
{
"TOCHeading": "Ionization Energy",
"Description": "Ionization energy is the minimum energy required to eject an electron out of a neutral atom or molecule in its ground state.",
"URL": "https://goldbook.iupac.org/html/I/I03199.html",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "13.598 eV"
}
]
}
},
{
"ReferenceNumber": 6,
"Name": "Ionization Energy",
"Value": {
"StringWithMarkup": [
{
"String": "13.598434599702 eV (Theoretical value.)"
}
]
}
}
]
},
{
"TOCHeading": "Electronegativity",
"Description": "The concept electronegativity was introduced by L. Pauling as the power of an atom to attract electrons to itself.",
"URL": "http://dev.goldbook.iupac.org/terms/view/E01990",
"Information": [
{
"ReferenceNumber": 8,
"Name": "Pauling Scale Electronegativity",
"Reference": [
"A.L. Allred, J. Inorg. Nucl. Chem., 1961, 17(3-4), 215-221. DOI:10.1016/0022-1902(61)80142-5"
],
"Value": {
"Number": [
2.2
],
"Unit": "(Pauling Scale)"
}
},
{
"ReferenceNumber": 8,
"Name": "Allen Scale Electronegativity",
"Reference": [
"L.C. Allen, J. Am. Chem. Soc., 1989, 111, 9003. DOI:10.1021/ja00207a003; J.B. Mann, T.L. Meek and L.C. Allen, J. Am. Chem. Soc., 2000, 122, 2780. DOI:10.1021/ja992866e; J.B. Mann, T.L. Meek, E.T. Knight, J.F. Capitani and L.C Allen, J. Am. Chem. Soc., 2000, 122, 5132. DOI:10.1021/ja9928677"
],
"Value": {
"Number": [
2.3
],
"Unit": "(Allen Scale)"
}
}
]
},
{
"TOCHeading": "Electron Affinity",
"Description": "Electron affinity refers to energy required to detach an electron from the singly charged negative ion.",
"URL": "http://dev.goldbook.iupac.org/terms/view/E01977",
"Information": [
{
"ReferenceNumber": 8,
"Name": "Electron Affinity",
"Reference": [
"R.T Myers, J. Chem. Edu., 1990, 67(4), 307. DOI:10.1021/ed067p307"
],
"Value": {
"Number": [
0.754
],
"Unit": "eV"
}
},
{
"ReferenceNumber": 8,
"Name": "Electron Affinity",
"Reference": [
"R.J. Zollweg, J. Chem. Phys., 1969, 50, 4251. DOI:10.1063/1.1670890"
],
"Value": {
"Number": [
0.77
],
"Unit": "eV"
}
}
]
},
{
"TOCHeading": "Atomic Spectra",
"Description": "Atomic and ionic spectral lines originate from specified electronic transitions between energy levels of atoms and ions, respectively.",
"URL": "https://goldbook.iupac.org/html/A/A00502.html",
"Information": [
{
"ReferenceNumber": 6,
"Name": "Atomic Spectra",
"URL": "https://physics.nist.gov/cgi-bin/ASD/lines_hold.pl?el=H",
"Value": {
"StringWithMarkup": [
{
"String": "Lines Holdings"
}
]
}
},
{
"ReferenceNumber": 6,
"Name": "Atomic Spectra",
"URL": "https://physics.nist.gov/cgi-bin/ASD/levels_hold.pl?el=H",
"Value": {
"StringWithMarkup": [
{
"String": "Levels Holdings"
}
]
}
}
]
},
{
"TOCHeading": "Physical Description",
"Description": "Physical description, also know as physical characteristics, refers to physical appearance of element substances.",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "Gas"
}
]
}
}
]
},
{
"TOCHeading": "Element Classification",
"Description": "Elements can be classified few groups according to each element's chemical properties.",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "Non-metal"
}
]
}
}
]
},
{
"TOCHeading": "Element Period Number",
"Description": "The element period number refers to a horizontal row of the periodic table. The periodic table has 7 periods.",
"URL": "https://www.britannica.com/science/periodic-table-of-the-elements/The-periodic-table#ref80835",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "1"
}
]
}
}
]
},
{
"TOCHeading": "Element Group Number",
"Description": "Element group refers to a set of chemical elements in the same vertical column of the periodic table",
"URL": "https://www.britannica.com/science/group-periodic-table",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "1"
}
]
}
}
]
},
{
"TOCHeading": "Density",
"Description": "Density is a degree of consistency measured by the quantity of mass per unit volume",
"URL": "https://goldbook.iupac.org/html/D/D01590.html",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "0.00008988 grams per cubic centimeter"
}
]
}
}
]
},
{
"TOCHeading": "Melting Point",
"Description": "The melting point is the temperature at which a substance changes state from solid to liquid at atmospheric pressure",
"URL": "https://www.britannica.com/science/melting-point",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "13.81 K (-259.34°C or -434.81°F)"
}
]
}
},
{
"ReferenceNumber": 5,
"Value": {
"StringWithMarkup": [
{
"String": "-259.16°C"
}
]
}
}
]
},
{
"TOCHeading": "Boiling Point",
"Description": "Boiling Point is the temperature at which a substance changes state from liquid to gas at atmospheric pressure",
"URL": "https://en.wikipedia.org/wiki/Boiling_point",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "20.28 K (-252.87°C or -423.17°F)"
}
]
}
}
]
},
{
"TOCHeading": "Estimated Crustal Abundance",
"Description": "The estimated element abundance in earth crust",
"URL": "https://en.wikipedia.org/wiki/Abundance_of_elements_in_Earth%27s_crust",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "1.40×103 milligrams per kilogram",
"Markup": [
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"Start": 7,
"Length": 1,
"Type": "Superscript"
}
]
}
]
}
}
]
},
{
"TOCHeading": "Estimated Oceanic Abundance",
"Description": "The estimated element abundance in ocean",
"Information": [
{
"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
{
"String": "1.08×105 milligrams per liter",
"Markup": [
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"Start": 7,
"Length": 1,
"Type": "Superscript"
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}
]
}
}
]
}
]
},
{
"TOCHeading": "History",
"Description": "Element discovery and related information in history",
"Information": [
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"ReferenceNumber": 3,
"Name": "History",
"Value": {
"StringWithMarkup": [
{
"String": "The name derives from the Greek hydro for \"water\" and genes for \"forming\" because it burned in air to form water. Hydrogen was discovered by the English physicist Henry Cavendish in 1766.",
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"String": "Scientists had been producing hydrogen for years before it was recognized as an element. Written records indicate that Robert Boyle produced hydrogen gas as early as 1671 while experimenting with iron and acids. Hydrogen was first recognized as a distinct element by Henry Cavendish in 1766. Composed of a single proton and a single electron, hydrogen is the simplest and most abundant element in the universe. It is estimated that 90% of the visible universe is composed of hydrogen."
},
{
"String": "Hydrogen is the raw fuel that most stars 'burn' to produce energy. The same process, known as fusion, is being studied as a possible power source for use on earth. The sun's supply of hydrogen is expected to last another 5 billion years."
}
]
}
},
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"String": "From the Greek word hydro (water), and genes (forming). Hydrogen was recognized as a distinct substance by Henry Cavendish in 1776. Diagram of a simple hydrogen atom.",
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"String": "Hydrogen is the most abundant of all elements in the universe. The heavier elements were originally made from hydrogen atoms or from other elements that were originally made from hydrogen atoms."
}
]
}
}
]
},
{
"TOCHeading": "Uses",
"Description": "Uses information in industry and other fields",
"Information": [
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"ReferenceNumber": 4,
"Value": {
"StringWithMarkup": [
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"String": "Hydrogen is a commercially important element. Large amounts of hydrogen are combined with nitrogen from the air to produce ammonia (NH3) through a process called the Haber process. Hydrogen is also added to fats and oils, such as peanut oil, through a process called hydrogenation. Liquid hydrogen is used in the study of superconductors and, when combined with liquid oxygen, makes an excellent rocket fuel.",
"Markup": [
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]
},
{
"String": "Hydrogen combines with other elements to form numerous compounds. Some of the common ones are: water (H2O), ammonia (NH3), methane (CH4), table sugar (C12H22O11), hydrogen peroxide (H2O2) and hydrochloric acid (HCl).",
"Markup": [
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"Length": 1,
"Type": "Subscript"
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"Start": 119,
"Length": 1,
"Type": "Subscript"
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"Start": 134,
"Length": 1,
"Type": "Subscript"
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"Start": 152,
"Length": 2,
"Type": "Subscript"
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"Start": 155,
"Length": 2,
"Type": "Subscript"
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"Start": 158,
"Length": 2,
"Type": "Subscript"
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"Start": 183,
"Length": 1,
"Type": "Subscript"
},
{
"Start": 185,
"Length": 1,
"Type": "Subscript"
}
]
},
{
"String": "Hydrogen has three common isotopes. The simplest isotope, called protium, is just ordinary hydrogen. The second, a stable isotope called deuterium, was discovered in 1932. The third isotope, tritium, was discovered in 1934."
}
]
}
},
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"Value": {
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"String": "Great quantities of hydrogen are required commercially for nitrogen fixation using the Haber ammonia process, and for the hydrogenation of fats and oils. It is also used in large quantities in methanol production, in hydrodealkylation, hydrocracking, and hydrodesulfurization. Other uses include rocket fuel, welding, producing hydrochloric acid, reducing metallic ores, and filling balloons."
},
{
"String": "The lifting power of 1 cubic foot of hydrogen gas is about 0.07 lb at °C, 760 mm pressure."
},
{
"String": "The hydrogen fuel cell is a developing technology that will allow great amounts of electrical power to be obtained using a source of hydrogen gas."
},
{
"String": "Consideration is being given to an entire economy based on solar- and nuclear-generated hydrogen. Public acceptance, high capital investment, and the high cost of hydrogen with respect to today's fuels are but a few of the problems facing such an economy. Located in remote regions, power plants would electrolyze seawater; the hydrogen produced would travel to distant cities by pipelines. Pollution-free hydrogen could replace natural gas, gasoline, etc., and could serve as a reducing agent in metallurgy, chemical processing, refining, etc. It could also be used to convert trash into methane and ethylene."
}
]
}
}
]
},
{
"TOCHeading": "Sources",
"Description": "Sources (where the element come from) information for the given element",
"Information": [
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"ReferenceNumber": 5,
"Value": {
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"String": "Hydrogen is estimated to make up more than 90% of all the atoms three quarters of the mass of the universe! This element is found in the stars, and plays an important part in powering the universe through both the proton-proton reaction and carbon-nitrogen cycle. Stellar hydrogen fusion processes release massive amounts of energy by combining hydrogens to form helium."
},
{
"String": "Production of hydrogen in the U.S. alone amounts to about 3 billion cubic feet per year. Hydrogen is prepared by"
},
{
"String": "▸ steam on heated carbon,"
},
{
"String": "▸ decomposition of certain hydrocarbons with heat,"
},
{
"String": "▸ reaction of sodium or potassium hydroxide on aluminum"
},
{
"String": "▸ electrolysis of water, or"
},
{
"String": "▸ displacement from acids by certain metals."
},
{
"String": "Liquid hydrogen is important in cryogenics and in the study of superconductivity, as its melting point is only 20 degrees above absolute zero."
},
{
"String": "Tritium is readily produced in nuclear reactors and is used in the production of the hydrogen bomb."
},
{
"String": "Hydrogen is the primary component of Jupiter and the other gas giant planets. At some depth in the planet's interior the pressure is so great that solid molecular hydrogen is converted to solid metallic hydrogen."
},
{
"String": "In 1973, a group of Russian experimenters may have produced metallic hydrogen at a pressure of 2.8 Mbar. At the transition the density changed from 1.08 to 1.3 g/cm3. Earlier, in 1972, at Livermore, California, a group also reported on a similar experiment in which they observed a pressure-volume point centered at 2 Mbar. Predictions say that metallic hydrogen may be metastable; others have predicted it would be a superconductor at room temperature.",
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},
{
"TOCHeading": "Compounds",
"Description": "Related compounds information to this element",
"Information": [
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"String": "Although pure hydrogen is a gas, we find very little of it in our atmosphere. Hydrogen gas is so light that, uncombined, hydrogen will gain enough velocity from collisions with other gases that they will quickly be ejected from the atmosphere. On earth, hydrogen occurs chiefly in combination with oxygen in water, but it is also present in organic matter such as living plants, petroleum, coal, etc. It is present as the free element in the atmosphere, but only less than 1 ppm by volume. The lightest of all gases, hydrogen combines with other elements sometimes explosively to form compounds."
}
]
}
},
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"Name": "Molecular Forms",
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"String": "Quite apart from isotopes, it has been shown that under ordinary conditions hydrogen gas is a mixture of two kinds of molecules, known as ortho- and para-hydrogen, which differ from one another by the spins of their electrons and nuclei."
},
{
"String": "Normal hydrogen at room temperature contains 25% of the para form and 75% of the ortho form. The ortho form cannot be prepared in the pure state. Since the two forms differ in energy, the physical properties also differ. The melting and boiling points of parahydrogen are about 0.1°C lower than those of normal hydrogen."
}
]
}
},
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"ReferenceNumber": 7,
"Name": "Compounds",
"URL": "https://pubchem.ncbi.nlm.nih.gov/compound/Hydrogen",
"Value": {
"StringWithMarkup": [
{
"String": "See more information at the Hydrogen compound page."
}
]
}
}
],
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"TOCHeading": "Element Forms",
"Description": "Other element forms, ions, isotopes, etc.",
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