Soviet Census (1989)
The 1989 Soviet census, conducted between 12-19 January of that year, was the last one that took place in the former USSR. The census found the total population to be 286,730,819 inhabitants. In 1989, the Soviet Union ranked as the third most populous in the world, above the United States, although it was well behind China and India. In 1989, about half of the Soviet Union's total population lived in the Russian SFSR, one-sixth of them in Ukraine. Two-thirds of the population was urban, leaving the rural population with 34.3%. In this way, its gradual increase continued, as shown by the series represented by 47.9%, 56.3% and 62.3% of 1959, 1970 and 1979 respectively. The last two national censuses showed that the country had been experiencing an average annual increase of about 2.5 million people, although it was a slight decrease from a figure of around 3 million per year in the previous intercensal period, 1959-1970. This post-war increase had contributed to the USSR's partial demographic recovery from the significant population loss that the USSR had suffered during the Great Patriotic War, before it, during Stalin's Great Purge of 1936-1938.
The previous postwar censuses, conducted in 1959, 1970 and 1979, had enumerated 208,826,650, 241,720,134, 262,436,227 inhabitants respectively. In 1990, the Soviet Union was more populated than both the United States and Canada together, having some 40 million more inhabitants than the U. S. alone. However, after the dissolution of the Soviet Union in late 1991, the combined population of the 15 former Soviet republics stagnated at around 290 million inhabitants for the period 1995-2000; this significant slowdown may in part be due to the remarkable socio-economic changes that followed the disintegration of the USSR, that have tended to reduce more the decreasing birth rates. The next census was planned for 1999. Demographics of the Soviet Union Republics of the Soviet Union Soviet Census First All-Union Census of the Soviet Union Soviet Union Barbara A. Anderson and Brian D. Silver, "Growth and diversity of the population of the Soviet Union", The Annals of the American Academy of Political and Social Science, Vol. 510, No.
1, 155-177, 1990. Ralph S. Clem, Ed. Research Guide to Russian and Soviet Censuses, Ithaca: Cornell University Press, 1986. John C. Dewdney, "Population change in the Soviet Union, 1979-1989," Geography, Vol. 75, Pt. 3, No. 328, July 1990, 273-277. Subjects of Russia, on the www.statoids.com website
Iron is a chemical element with symbol Fe and atomic number 26. It is a metal, that belongs to group 8 of the periodic table, it is by mass the most common element on Earth, forming much of Earth's inner core. It is the fourth most common element in the Earth's crust. Pure iron is rare on the Earth's crust being limited to meteorites. Iron ores are quite abundant, but extracting usable metal from them requires kilns or furnaces capable of reaching 1500 °C or higher, about 500 °C higher than what is enough to smelt copper. Humans started to dominate that process in Eurasia only about 2000 BCE, iron began to displace copper alloys for tools and weapons, in some regions, only around 1200 BCE; that event is considered the transition from the Bronze Age to the Iron Age. Iron alloys, such as steel and special steels are now by far the most common industrial metals, because of their mechanical properties and their low cost. Pristine and smooth pure iron surfaces are mirror-like silvery-gray. However, iron reacts with oxygen and water to give brown to black hydrated iron oxides known as rust.
Unlike the oxides of some other metals, that form passivating layers, rust occupies more volume than the metal and thus flakes off, exposing fresh surfaces for corrosion. The body of an adult human contains about 3 to 5 grams of elemental iron in hemoglobin and myoglobin; these two proteins play essential roles in vertebrate metabolism oxygen transport by blood and oxygen storage in muscles. To maintain the necessary levels, human iron metabolism requires a minimum of iron in the diet. Iron is the metal at the active site of many important redox enzymes dealing with cellular respiration and oxidation and reduction in plants and animals. Chemically, the most common oxidation states of iron are +2 and +3. Iron shares many properties of other transition metals, including the other group 8 elements and osmium. Iron forms compounds in a wide range of oxidation states, −2 to +7. Iron forms many coordination compounds. At least four allotropes of iron are known, conventionally denoted α, γ, δ, ε; the first three forms are observed at ordinary pressures.
As molten iron cools past its freezing point of 1538 °C, it crystallizes into its δ allotrope, which has a body-centered cubic crystal structure. As it cools further to 1394 °C, it changes to its γ-iron allotrope, a face-centered cubic crystal structure, or austenite. At 912 °C and below, the crystal structure again becomes the bcc α-iron allotrope; the physical properties of iron at high pressures and temperatures have been studied extensively, because of their relevance to theories about the cores of the Earth and other planets. Above 10 GPa and temperatures of a few hundred kelvin or less, α-iron changes into another hexagonal close-packed structure, known as ε-iron; the higher-temperature γ-phase changes into ε-iron, but does so at higher pressure. Some controversial experimental evidence exists for a stable β phase at pressures above 50 GPa and temperatures of at least 1500 K, it is supposed to have a double hcp structure. The inner core of the Earth is presumed to consist of an iron-nickel alloy with ε structure.
The melting and boiling points of iron, along with its enthalpy of atomization, are lower than those of the earlier 3d elements from scandium to chromium, showing the lessened contribution of the 3d electrons to metallic bonding as they are attracted more and more into the inert core by the nucleus. This same trend appears for ruthenium but not osmium; the melting point of iron is experimentally well defined for pressures less than 50 GPa. For greater pressures, published data still varies by tens of gigapascals and over a thousand kelvin. Below its Curie point of 770 °C, α-iron changes from paramagnetic to ferromagnetic: the spins of the two unpaired electrons in each atom align with the spins of its neighbors, creating an overall magnetic field; this happens because the orbitals of those two electrons do not point toward neighboring atoms in the lattice, therefore are not involved in metallic bonding. In the absence of an external source of magnetic field, the atoms get spontaneously partitioned into magnetic domains, about 10 micrometres across, such that the atoms in each domain have parallel spins, but different domains have other orientations.
Thus a macroscopic piece of iron will have a nearly zero overall magnetic field. Application of an external magnetic field causes the domains that are magnetized in the same general direction to grow at the expense of adjacent ones that point in other directions, reinforcing the external field; this effect is exploited in devices that needs to channel magnetic fields, such as electrical transformers, magnetic recording heads, electric motors. Impurities, lattice defects, or grain and particle boundaries can "pin" the domains in the new positions, so that the effect persists after the external field is removed -- thus turning the iron object into a magnet. Similar behavior is exhibited by some iron compounds, such as the fer
Russian Federal State Statistics Service
Russian Federal State Statistics Service is the governmental statistics agency in Russia. Since 2017, it is again part of the Ministry of Economic Development, having switched several times in the previous decades between that ministry and being directly controlled by the federal government. Goskomstat was the centralised agency dealing with statistics in the Soviet Union. Goskomstat was created in 1987 to replace the Central Statistical Administration, while maintaining the same basic functions in the collection, analysis and distribution of state statistics, including economic and population statistics; this renaming amounted to a formal demotion of the status of the agency. In addition to overseeing the collection and evaluation of state statistics, Goskomstat was responsible for planning and carrying out the population and housing censuses, it carried out seven such censuses, in 1926, 1937, 1939, 1959, 1970, 1980, 1989. House No. 39, on Ulitsa Myasnitskaya, Tsentrosoyuz building, home to Goskomstat, was designed by the Swiss-born architect, Le Corbusier.
Interstate Statistical Committee of the Commonwealth of Independent States Federal State Statistics Service of the Russian Federation
The Neiva or Nevya is a 294-kilometre long river in the Sverdlovsk Oblast of Russia, which flows out of Lake Tavatui along the slopes of the Ural Mountains through the urban-type settlement Verkh-Neyvinsky and the towns of Nevyansk and Alapaevsk. The basin formed by the river has a total catchment area of 5,600 square kilometres; the upper reaches are punctuated by a series of lakes and reservoirs that cover 72.4 square kilometres. After joining the Nitsa River, the Neyva enters the Tura River, a tributary of the Tobol
A posad was a settlement in the Russian Empire surrounded by ramparts and a moat, adjoining a town or a kremlin, but outside of it, or adjoining a monastery in the 10th to 15th centuries. The posad was inhabited by craftsmen and merchants and was its own distinct community, separate from the city it adjoined; some posads developed into towns, such as Sergiev Posad. During the 1920s administrative territorial reform in the Soviet Union, posads were converted into urban-type settlements; the posad was the center of trade in Ancient Rus. Merchants and craftsmen resided there and sold goods such as pottery, armor and copperware, clothing. Most large cities were adjoined by a posad situated below the main citadel and by a river. Posads were sometimes fortified with earthen walls; as posads developed, they became like villages. Membership in the community became hereditary, posad residents were expected to pay taxes and perform other duties to the state. Leaving the posad required the permission of an elected official.
Until the 18th century, the posad had its own elected assembly, the "posadskiy skhod," though the wealthiest members of the posad tended to dominate the governance of the community in "a tight self-perpetuating oligarchy."A number of posads evolved into towns. Those by a kremlin gave rise to local toponyms, such as Nagorny Posad, Kazanski Posad for the historical center of Kazan; those by a monastery gave rise to cities named after the monastery, e.g. Sergiev Posad is named after the nearby Troitse-Sergiyeva Lavra. Lischke Shtetl Mariinsky Posad Gavrilov Posad
Peter the Great
Peter the Great, Peter I or Peter Alexeyevich ruled the Tsardom of Russia and the Russian Empire from 7 May 1682 until his death in 1725, jointly ruling before 1696 with his elder half-brother, Ivan V. Through a number of successful wars, he expanded the Tsardom into a much larger empire that became a major European power and laid the groundwork for the Russian navy after capturing ports at Azov and the Baltic Sea, he led a cultural revolution that replaced some of the traditionalist and medieval social and political systems with ones that were modern, scientific and based on the Enlightenment. Peter's reforms made a lasting impact on Russia, many institutions of Russian government trace their origins to his reign, he is known for founding and developing the city of Saint Petersburg, which remained the capital of Russia until 1917. The imperial title of Peter the Great was the following: By the grace of God, the most excellent and great sovereign prince Pyotr Alekseevich the ruler of all the Russias: of Moscow, of Kiev, of Vladimir, of Novgorod, Tsar of Kazan, Tsar of Astrakhan and Tsar of Siberia, sovereign of Pskov, great prince of Smolensk, Yugorsk, Vyatsky and others, sovereign and great prince of Novgorod Nizovsky lands, Chernigovsky, of Ryazan, of Rostov, Belozersky, Udorsky and the sovereign of all the northern lands, the sovereign of the Iverian lands, of the Kartlian and Georgian Kings, of the Kabardin lands, of the Circassian and Mountain princes and many other states and lands western and eastern here and there and the successor and sovereign and ruler.
Named after the apostle, described as a newborn as "with good health, his mother's black, vaguely Tatar eyes, a tuft of auburn hair", from an early age Peter's education was put in the hands of several tutors, most notably Nikita Zotov, Patrick Gordon, Paul Menesius. On 29 January 1676, Tsar Alexis died, leaving the sovereignty to Peter's elder half-brother, the weak and sickly Feodor III of Russia. Throughout this period, the government was run by Artamon Matveev, an enlightened friend of Alexis, the political head of the Naryshkin family and one of Peter's greatest childhood benefactors; this position changed when Feodor died in 1682. As Feodor did not leave any children, a dispute arose between the Miloslavsky family and Naryshkin family over who should inherit the throne. Peter's other half-brother, Ivan V of Russia, was next in line for the throne, but he was chronically ill and of infirm mind; the Boyar Duma chose the 10-year-old Peter to become Tsar with his mother as regent. This arrangement was brought before the people of Moscow, as ancient tradition demanded, was ratified.
Sophia Alekseyevna, one of Alexis' daughters from his first marriage, led a rebellion of the Streltsy in April–May 1682. In the subsequent conflict some of Peter's relatives and friends were murdered, including Matveev, Peter witnessed some of these acts of political violence; the Streltsy made it possible for Sophia, the Miloslavskys and their allies to insist that Peter and Ivan be proclaimed joint Tsars, with Ivan being acclaimed as the senior. Sophia exercised all power. For seven years, she ruled as an autocrat. A large hole was cut in the back of the dual-seated throne used by Peter. Sophia would sit behind the throne and listen as Peter conversed with nobles, while feeding him information and giving him responses to questions and problems; this throne can be seen in the Kremlin Armoury in Moscow. Peter was not concerned that others ruled in his name, he engaged in such pastimes as sailing, as well as mock battles with his toy army. Peter's mother sought to force him to adopt a more conventional approach and arranged his marriage to Eudoxia Lopukhina in 1689.
The marriage was a failure, ten years Peter forced his wife to become a nun and thus freed himself from the union. By the summer of 1689, Peter age 17, planned to take power from his half-sister Sophia, whose position had been weakened by two unsuccessful Crimean campaigns against the Crimean Khanate in an attempt to stop devastating Crimean Tatar raids into Russia's southern lands; when she learned of his designs, Sophia conspired with the leaders of the Streltsy, who continually aroused disorder and dissent. Peter, warned by the Streltsy, escaped in the middle of the night to the impenetrable monastery of Troitse-Sergiyeva Lavra. Sophia was overthrown, with Peter I and Ivan V continuing to act as co-tsars. Foy de la Neuville records that Sophia requested influential members of Peter's family, notably her aunts Tatyana and Anna, to mediate with him. Peter forced Sophia to enter a convent, where she gave up her name and her position as a member of the royal family. Still, Peter could not acquire actual control over Russian affairs.
Power was instead exercised by Natalya Naryshkina. It was only. Formally, Ivan V remained a co-ruler with Peter. Peter became the sole ruler when Ivan died in 1696. Peter was 24 years old. Peter grew to be tall as an a
Gold is a chemical element with symbol Au and atomic number 79, making it one of the higher atomic number elements that occur naturally. In its purest form, it is a bright reddish yellow, soft and ductile metal. Chemically, gold is a group 11 element, it is solid under standard conditions. Gold occurs in free elemental form, as nuggets or grains, in rocks, in veins, in alluvial deposits, it occurs in a solid solution series with the native element silver and naturally alloyed with copper and palladium. Less it occurs in minerals as gold compounds with tellurium. Gold is resistant to most acids, though it does dissolve in aqua regia, a mixture of nitric acid and hydrochloric acid, which forms a soluble tetrachloroaurate anion. Gold is insoluble in nitric acid, which dissolves silver and base metals, a property that has long been used to refine gold and to confirm the presence of gold in metallic objects, giving rise to the term acid test. Gold dissolves in alkaline solutions of cyanide, which are used in mining and electroplating.
Gold dissolves in mercury, forming amalgam alloys. A rare element, gold is a precious metal, used for coinage and other arts throughout recorded history. In the past, a gold standard was implemented as a monetary policy, but gold coins ceased to be minted as a circulating currency in the 1930s, the world gold standard was abandoned for a fiat currency system after 1971. A total of 186,700 tonnes of gold exists above ground, as of 2015; the world consumption of new gold produced is about 50% in jewelry, 40% in investments, 10% in industry. Gold's high malleability, resistance to corrosion and most other chemical reactions, conductivity of electricity have led to its continued use in corrosion resistant electrical connectors in all types of computerized devices. Gold is used in infrared shielding, colored-glass production, gold leafing, tooth restoration. Certain gold salts are still used as anti-inflammatories in medicine; as of 2017, the world's largest gold producer by far was China with 440 tonnes per year.
Gold is the most malleable of all metals. It can be drawn into a monoatomic wire, stretched about twice before it breaks; such nanowires distort via formation and migration of dislocations and crystal twins without noticeable hardening. A single gram of gold can be beaten into a sheet of 1 square meter, an avoirdupois ounce into 300 square feet. Gold leaf can be beaten thin enough to become semi-transparent; the transmitted light appears greenish blue, because gold reflects yellow and red. Such semi-transparent sheets strongly reflect infrared light, making them useful as infrared shields in visors of heat-resistant suits, in sun-visors for spacesuits. Gold is a good conductor of electricity. Gold has a density of 19.3 g/cm3 identical to that of tungsten at 19.25 g/cm3. By comparison, the density of lead is 11.34 g/cm3, that of the densest element, osmium, is 22.588±0.015 g/cm3. Whereas most metals are gray or silvery white, gold is reddish-yellow; this color is determined by the frequency of plasma oscillations among the metal's valence electrons, in the ultraviolet range for most metals but in the visible range for gold due to relativistic effects affecting the orbitals around gold atoms.
Similar effects impart a golden hue to metallic caesium. Common colored gold alloys include the distinctive eighteen-karat rose gold created by the addition of copper. Alloys containing palladium or nickel are important in commercial jewelry as these produce white gold alloys. Fourteen-karat gold-copper alloy is nearly identical in color to certain bronze alloys, both may be used to produce police and other badges. White gold alloys can be made with nickel. Fourteen- and eighteen-karat gold alloys with silver alone appear greenish-yellow and are referred to as green gold. Blue gold can be made by alloying with iron, purple gold can be made by alloying with aluminium. Less addition of manganese, aluminium and other elements can produce more unusual colors of gold for various applications. Colloidal gold, used by electron-microscopists, is red. Gold has only one stable isotope, 197Au, its only occurring isotope, so gold is both a mononuclidic and monoisotopic element. Thirty-six radioisotopes have been synthesized, ranging in atomic mass from 169 to 205.
The most stable of these is 195Au with a half-life of 186.1 days. The least stable is 171Au. Most of gold's radioisotopes with atomic masses below 197 decay by some combination of proton emission, α decay, β+ decay; the exceptions are 195Au, which decays by electron capture, 196Au, which decays most by electron capture with a minor β− decay path. All of gold's radioisotopes with atomic masses above 197 decay by β− decay. At least 32 nuclear isomers have been characterized, ranging in atomic mass from 170 to 200. Within that range, only 178Au, 180Au, 181Au, 182Au, 188Au do not have isomers. Gold's most stable isomer is 198m2Au with a half-life of 2.27 days. Gold's least stable isomer is 177m2Au with a half-life of only 7 ns. 184m1Au has three decay paths: β+ decay, isomeric