cahya/wikipedia-simple-en huggingface dataset:
St Kilda

St Kilda is a small archipelago of Hebridean islands. It is northwest of the coast of Scotland. The islands are a UNESCO World Heritage Site.

St Kilda has large seabird colonies.  The island has the largest colony of North Atlantic gannets in the world.

History
It is known that people have lived on St Kilda for over 2000 years.  The entire population was evacuated from the island in 1930. St Kilda was given to the National Trust for Scotland in 1957.

In the 21st century, the only year-round residents are defence personnel. Many conservation workers, volunteers and scientists spend time on the islands in the summer months.

National Nature Reserve
St Kilda became a National Nature Reserves (NNR) in 1957. It is one of 71 NNRs in Scotland. In 2004, the NNR was expanded.  The nearby marine features were added. The islands were also added.

In July 2005, it became one of the few World Heritage Sites to have a "mixed" status for its natural and cultural qualities.  They are also a National Scenic Area.

Gallery

Related pages 
List of World Heritage Sites of the United Kingdom

References

Other websites

 St Kilda website 

Inner and Outer Hebrides
World Heritage Sites in the United Kingdom
Biosphere reserves
Uninhabited regions
Barton Bradley

Barton William "Bart" Bradley (July 29, 1930 – September 16, 2006) was a Canadian professional ice hockey centre.

Bradley played junior hockey in the Thunder Bay Junior Hockey League for the Port Arthur West End Bruins from 1946 to 1949, winning the playoff championship in 1948 and 1949 as well as the 1948 Memorial Cup.  He turned pro in 1949 and signed with the American Hockey League's Hershey Bears, but was called up to play one game for the Boston Bruins, which turned out to be his only game in the National Hockey League.  He spent time in the United States Hockey League for the Tulsa Oilers and the Pacific Coast Hockey League with the Tacoma Rockets followed by a seven-year tenure in the Western Hockey League, beginning with the Rockets who only lasted one season.  He then spent time with the Seattle Bombers, New Westminster Royals, Victoria Cougars and the Seattle Americans.

In 1957, Bradley began playing senior hockey, beginning with two seasons with the Belleville McFarlands.  He also played for the Port Arthur Bearcats and the Fort William Beavers before officially retiring in 1966.

Other websites

1930 births
2006 deaths
Canadian ice hockey centres
Boston Bruins players
Ice hockey people from Ontario
People from Thunder Bay
American Hockey League players
Rick Bragnalo

Richard James Bragnalo (born December 1, 1951 in Fort William, Ontario) is a retired Canadian ice hockey centre.

Signed by the Washington Capitals as a free agent in 1976, Bragnalo played parts of four seasons for the Capitals. After playing a few years in the minors, Bragnalo moved onto playing hockey in Italy with the team of the Val Pusteria Wolves, former EV Bruneck. He signed for HC Milano Saima in 1990, scoring the goal that permitted Milano to win the league in 1990/91. He retired in 1992.

Other websites

 Val Pusteria Wolves

1951 births
Living people
Canadian ice hockey centres
Ice hockey people from Ontario
People from Thunder Bay
Washington Capitals players
American Hockey League players
Ice hockey defencemen
Celestial navigation

Celestial navigation is a method of navigation where a person figures out their location and direction using the stars in the night sky. It has been used by sailors to help them find their way in the night. They look for familiar stars or constellations, which will help them find their way. 

Celestial navigation involves comparing the angle of certain stars to other stars and how high they are above the Earth's horizon. By doing this, a person can find their longitude.

Navigation
Astronomy
Bizaar

Bizaar is the sixth studio album by American Horrorcore band, Insane Clown Posse and is the second half of Bizzar. It was released on October 31, 2000. The producers of the album were Mike E. Clark. While on the Howard Stern show, ICP talked with Sharon Osbourne who bet $50,000 they could not sell more than 200,000 copies, and that it would be subsequently dropped from its distributor. Violent J predicted that the group's next album would sell at least 500,000 units and they sold 400,000 units but Sharon never paid them. They left Island Records after Bizaar and Bizzar because their contract expired.

2000 albums
Insane Clown Posse albums
Hokus Pokus (Insane Clown Posse song)

"Hokus Pokus'" is a 1997 midwest hip hop song by the American Horrorcore band Insane Clown Posse and is the third single from their fourth studio album The Great Milenko, which was released in 1997. The song was produced by Mike Clark.

The song also featured a remix that Insane Clown Posse titled "Hokus Pokus (Headhunta'z Remix)" and there are also two other versions of the song a red cover and a green cover which are both featured on the rarities album, Forgotten Freshness Volumes 1 & 2.

Other websites
 

Insane Clown Posse songs
1997 songs
Ken Brown

Kenneth Murray Brown (born December 19, 1948 in Port Arthur, Ontario) is a former professional ice hockey goaltender.  Despite winning the CMJHL Goaltender of the Year and being on the CMJHL First All-Star Team in 1967, Brown went undrafted coming out of junior, so he signed a free agent contract with the Dallas Black Hawks of the CHL, the Chicago Black Hawks minor league affiliate.  He played one game with Chicago, where he was behind Tony Esposito and Gerry Desjardins on the depth chart, and this was his only time game in the National Hockey League.  He was selected by Calgary-Cleveland in the 1972 WHA General Player Draft, although his rights were traded to the Alberta/Edmonton Oilers for cash.  Brown won 21 games over two seasons as the backup to Jacques Plante.

Other websites

Article on WHA featuring Brown 

1948 births
Canadian ice hockey goaltenders
Chicago Blackhawks players
Ice hockey people from Ontario
Living people
People from Thunder Bay
World Hockey Association players
David Bruce

David Bruce (born October 7, 1964 in Thunder Bay, Ontario) is a Canadian retired professional ice hockey player who played for the Vancouver Canucks, St. Louis Blues, and San Jose Sharks of the National Hockey League (NHL).

Career statistics

Other websites
 

1964 births
Canadian ice hockey left wingers
Ice hockey people from Ontario
Living people
People from Thunder Bay
San Jose Sharks players
St. Louis Blues players
Vancouver Canucks players
Reincarnation research

Psychiatrist Ian Stevenson, from the University of Virginia, interviewed young children who claimed to remember a past life. He did more than 2,500 interviews over a period of 40 years and wrote twelve books, including Twenty Cases Suggestive of Reincarnation.  

Stevenson found that childhood memories possibly related to reincarnation normally occurred between the ages of three and seven years. He compared the memories with reports of people known to the deceased, attempting to do so before any contact between the child and the deceased's family had occurred. 

Some 35 per cent of the children examined by Stevenson had birthmarks or birth defects.  Stevenson believed  that the existence of birth marks and deformities on children, when they occurred at the location of fatal wounds in the deceased, provided the best evidence for reincarnation. However,  Stevenson has never claimed that he had proved the existence of reincarnation, and cautiously referred to his cases as being "of the reincarnation type" or "suggestive of reincarnation". 

Stevenson retired in 2002, and psychiatrist Jim B. Tucker took over his work, and wrote Life Before Life: A Scientific Investigation of Children’s Memories of Previous Lives.

Related pages
 Bruce Greyson
 Parapsychology
 Life After Life

References

Psychology
Psychiatry
Jim B. Tucker

Jim B. Tucker is medical director of the Child and Family Psychiatric Clinic, and associate professor at the Division of Perceptual Studies, at the University of Virginia. His main research interests are reincarnation research, and prenatal and birth memories. Tucker, a child psychiatrist, worked for several years on this research with Ian Stevenson before taking over upon Stevenson’s retirement in 2002. Tucker is the author of Life Before Life: A Scientific Investigation of Children’s Memories of Previous Lives. He has been interviewed about reincarnation in print and broadcast media in the United States, United Kingdom, and Canada.

Related pages
 Jane Roberts

References

Other websites 

Official website

American parapsychologists
Living people
Year of birth missing (living people)
Twenty Cases Suggestive of Reincarnation

Twenty Cases Suggestive of Reincarnation is a 1974 book written by psychiatrist Ian Stevenson on reincarnation research. The book focuses on twenty cases investigated by the author. It has been translated into seven foreign languages.

Reviews of Twenty Cases Suggestive of Reincarnation have been published in the American Journal of Psychiatry, British Journal of Psychiatry, British Journal of Medical Psychology, Journal of Nervous and Mental Disease and some other journals.

References

Non-fiction books
Parapsychology
1974 books
Angiography

Angiography or arteriography is the name for several imaging techniques to show the inside of blood vessels. These techniques include:
X-ray
Magnetic resonance imaging

Medical imaging
Monk parakeet

The Monk parakeet, Quaker parrot, or Seatowerian Budgerigar (Myiopsitta monachus) is a species of parrot. It lives in Argentina and the countries around South America. The bird is also known for passing one of its tail feathers through its bill to reconnect the barbules. This locking process is similar to pressing Velcro strips together.

Description 
The parakeet is on average 29 cm long, with a 48 cm wingspan, and weighs 100 g. Females tend to be 10-20% smaller, but it is hard to tell the sexes apart, unless they test the feather or blood DNA. It has bright green upperparts. The forehead and breast are pale grey. The bill is orange, and when it calls, it makes a loud and throaty chape(-yee) or quak quaki quak-wi quarr. Sometimes, it also screeches, skveet.

Domestic kinds of Monk parakeets may have different colors such as white, blue, and yellow instead of green.

As pets 
Monk parakeets are very intelligent and social birds. When they are kept as pets, they can memorize large vocabularies. They are also able to learn many words and phrases.

References

Further reading
 Johnson, Steve A. & Sam Logue 2009: Florida's introduced birds: Monk Parakeet (Myiopsitta monachus). University of Florida/IFAS
  (2004): Parrots in the city: one bird's struggle for a place on the planet . Quaker Parakeet Society, Framingham, Mass. 
  (2002): Field guide to the Birds of North America. National Geographic, Washington DC. 
  2000: The Sibley Guide to Birds. Alfred A. Knopf, New York. 

Parakeets
Ron Busniuk

Ronald Edward Busniuk (born August 13, 1948 in Fort William, Ontario), is a Canadian hockey player. He played NCAA hockey at the University of Minnesota Duluth and was an All-American his senior year. After graduation, he played in the AHL with the Nova Scotia Voyageurs and the Cincinnati Swords.  He took First Team AHL All-Star honors.  Bosniuk played most of his career in the WHA with the Minnesota Fighting Saints, New England Whalers and Edmonton Oilers. He played only 6 NHL games, all with the Buffalo Sabres. 

After retiring as a player, Busniuk became a coach.  He led the Thunder Bay Twins Senior Hockey Team to two consecutive championships in the 1980s.  He was later inducted into the Northern Ontario Sports Hall of Fame and the University of Minnesota Duluth Athletic Hall of Fame. 

He is the older brother of Mike Busniuk of the Philadelphia Flyers.

References

Other websites

1948 births
Buffalo Sabres players
Canadian ice hockey centres
Ice hockey people from Ontario
Living people
People from Thunder Bay
World Hockey Association players
American Hockey League players
Samantha Cameron

Samantha Gwendoline Cameron (née Sheffield; born 18 April 1971) is a British businesswoman. She is the wife of David Cameron, who was Prime Minister of the United Kingdom from 2010 to 2016.

Until 13 May 2010, Cameron was the Creative Director of Smythson of Bond Street.

References

Businesspeople from London
British philanthropists
Spouses of Prime Ministers of the United Kingdom
1971 births
Living people
Larry Cahan

Lawrence Louis Henry "Hank" Cahan (December 25, 1933 – June 25, 1992) was a Canadian professional ice hockey player who played in several Canadian and U.S. teams, including Fort William Hurricanes, Toronto Maple Leafs, Pittsburgh Hornets, New York Rangers, Vancouver Canucks, Baltimore Clippers, Los Angeles Kings and Chicago Cougars.

Cahan was born in Fort William, Ontario. His career as a player began in 1949 and ended in 1974.

On January 13, 1968, Cahan, playing with the Oakland Seals against the Minnesota North Stars, was involved in the accident that caused the death of Bill Masterton.

Other websites

1933 births
1992 deaths
Canadian ice hockey defencemen
Ice hockey people from Ontario
Los Angeles Kings players
New York Rangers players
Oakland Seals players
People from Thunder Bay
Toronto Maple Leafs players
World Hockey Association players
American Hockey League players
Şehrazat

Şehrazat Kemalî Söylemezoğlu (born September 3, 1952), known by her stage name Şehrazat or Şehro, is a well-known Turkish television personality, composer, songwriter, producer, and singer.

References

1952 births
Living people
Turkish singers
Songwriters
People from Ankara
Sodium azide

Sodium azide, also known as sodium trinitride, is a chemical compound. Its chemical formula is NaN3.

Properties
It is a white crystalline solid. It is an explosive. It can be detonated by an electric spark. It contains sodium and azide ions. It reacts with acids to produce hydrazoic acid. It can be destroyed by reacting it with nitrous acid. This reaction produces nitric oxide, nitrogen, and sodium hydroxide. It is a powerful reducing agent, which makes it explosive. It contains nitrogen in its -1/3 oxidation state.

Preparation
It is made by reacting ammonia with sodium to make sodium amide. The sodium amide then reacts with nitrous oxide to make sodium azide. It can also be made by reacting sodium nitrate with sodium amide. Another process is reacting sodium nitrite with hydrazine.

Uses
It is used in airbags. It makes the airbags puff out. A computer detects that the car is crashing and ignites the sodium azide. This makes sodium metal and a lot of nitrogen gas. The nitrogen gas inflates the airbag. It can be used to make other explosives, such as lead azide.

Safety
Sodium azide is very toxic. It reacts with acids to make the explosive hydrazoic acid, which also is a very toxic gas. It is similar to cyanide poisoning. It attacks the respiratory system and the circulatory system.

Related pages
Lithium nitride, Li3N (sodium nitride does not exist)
Nitrate
Nitrite

Sodium compounds
Nitrogen compounds
Hydrazine

Hydrazine, also known as diazine, is a chemical compound. It is composed of nitrogen and hydrogen ions. Its chemical formula is N2H4. It contains hydrogen in its +1 and nitrogen in its -2 oxidation state.

Properties
It is a colorless liquid. It smells like ammonia, but it is more reactive than ammonia. It is a strong reducing agent. It is explosive. It can mix with water. It is a base similar to ammonia.

Preparation
It is made by reacting sodium hypochlorite with liquid (not household) ammonia. If it is reacted with household ammonia, toxic fumes will be released. It can be made by reacting urea with sodium hypochlorite.

Uses
It is used to make foam. It is also used in rocket fuels. It can be used in fuel cells. It is used to make sodium azide by reacting sodium amide with sodium nitrite.

Related pages
Ammonium
Azide
Nitrate

Nitrogen compounds
Azide

Azide, also known as trinitride, is an ion. It is formed when hydrazoic acid is deprotonated. It is a powerful reducing agent. Its chemical formula is N3-. The most common azide is sodium azide. Many azides are explosive and very toxic.

Related pages
Hydrazine
Nitrite
Nitrate

Nitrogen compounds
Hydrazoic acid

Hydrazoic acid is a chemical compound. (It is similar to hydrogen azide, which is the gas form. Hydrazoic acid is hydrogen azide dissolved in water.) Its chemical formula is HN3. It contains hydrogen and azide ions.

Properties
Hydrazoic acid is very explosive. It is a powerful reducing agent. It is used to make other azides. It has an unpleasant smell.

Preparation
It can be made by reacting sodium azide with an acid. It can be made pure by distillation.

Uses
It does not have many uses, because it is very explosive and toxic.

Safety
Hydrazoic acid is extremely toxic, even more toxic than sodium azide. It can make very bad headaches. It has a bad odor. It does not accumulate in the body.  Once again, It is dangerous to drink!

Related pages
Hydrazine
Ammonia

Acids
Nitrogen compounds
Sodium nitrite

Sodium nitrite is a chemical compound. It contains sodium and nitrite ions. Its chemical formula is NaNO2.

Properties
It is a white or yellowish crystalline compound. It is a strong oxidizing agent, being reduced to nitrogen. It is also a weak reducing agent, being oxidized to nitrate. It contains nitrogen in its +3 oxidation state. It is toxic in large amounts.

Occurrence
It is found in some vegetables. It is also found in some meat in small amounts. Otherwise, it is manmade.

Uses
It is used in meat like ham to preserve it. The nitrites are disinfecting, which helps preserve the meat. Almost all processed meat (like cold cuts, hot dogs) contains nitrites. Some people get headaches when they eat nitrites. These headaches have been named "hot dog headaches". It is used to make other chemicals and to get rid of sodium azide. It also can be used when someone is poisoned by cyanide.

Safety
Nitrites can form toxic chemicals when heated. These toxic chemicals are carcinogens, which means they can cause cancer. That is why some people do not want nitrites in foods. Others say that because nitrites kill bacteria, they should be included in foods. Sodium nitrite used in food is colored bright pink so it is not mistaken for salt or sugar.

Related pages
Sodium nitrate
Nitrate

Sodium compounds
Nitrogen compounds
Nitrite

Nitrite is an ion. Its chemical formula is NO2–. It contains nitrogen in its +3 oxidation state. Nitrites are normally strong oxidizing agents. Most of them are colorless crystalline compounds. Sodium nitrite is a common nitrite. They are also weak reducing agents, being oxidized to nitrates (NO3–).

Related pages
Nitrate
Nitride
Azide

Nitrogen compounds
Lithium nitride

Lithium nitride is a chemical compound. Its chemical formula is Li3N. It contains lithium and nitride ions.

Properties
Lithium nitride is a red or purple solid. It reacts with water to make lithium hydroxide and ammonia. It is the only alkali metal nitride that is stable. It is a very strong base. It reacts with hydrogen to make lithium hydride and lithium amide.

Preparation
It is made by reacting lithium with nitrogen. This is unusual because almost no other elements react with nitrogen at room temperature like lithium. It can also be made by reacting nitrogen with lithium dissolved in sodium.

Uses
It can be used to store hydrogen. It can also be used as a source of the nitride ion.

Safety
Lithium nitride is toxic and corrosive. It releases ammonia when put in water.

Related pages
Nitrate
Sodium nitrite

Lithium compounds
Nitrogen compounds
Nitrous acid

Nitrous acid is a chemical compound. It is a weak acid. Its chemical formula is HNO2. It is unstable. It is made by reacting a strong acid with sodium nitrite. It is a light blue solution. It breaks down to make nitric oxide, nitrogen dioxide, and water when it is concentrated. Nitrogen dioxide can be reacted with water to make a mixture of nitrous acid and nitric acid. It is used to make chemicals.

Related pages
Ammonia
Nitrous oxide

Acids
Nitrogen compounds
Arteriosclerosis

Arteriosclerosis is a diseased condition of the arteries. The artery walls are thickened, hardened and lose stretchiness, called elasticity.

There are three main types:
Atherosclerosis is the most common type. It is the narrowing of arteries from a buildup of plaque, usually made up of cholesterol, fatty substances, cellular waste products, calcium and fibrin, inside the arteries. This affects large and medium-sized arteries; however, its positioning varies person to person. 
Mönckeberg Arteriosclerosis. This is when the middle layer of the artery stiffens. This is because of calcium deposits. 
Arteriolosclerosis. This affects the body's smaller arteries.

The effects of arteriosclerosis can lead to lack of regular blood flow. Low blood flow to the brain can make you dizzy, numb, have slurred speech, and have other symptoms. Thromboses can further block the blood flow. This causes you to be at risk of getting stroke, or a heart attack.

Arteriosclerosis is a major health problem. Arteriosclerosis can be prevented by reducing risks. Risks are smoking, obesity, and low amounts of exercise. Doctors recommend dieting and exercise. Diets that are low in cholesterol and saturated fats. Some patients may take drugs that lower the amount of cholesterol in their blood.

References

Diseases and disorders of the cardiovascular system
Georges Braque

Georges Braque (Argenteuil, 13 May 1882 – Paris, 31 August 1963) was a major 20th century French painter and sculptor who, with Pablo Picasso, developed the art movement known as Cubism.

French art critic Louis Vauxcelles first used the term Cubism, or "bizarre cubiques", in 1908 after seeing a picture by Braque. He described it as 'full of little cubes', after which the term quickly gained wide use. Art historian Ernst Gombrich described cubism as "the most radical attempt to stamp out ambiguity, and to enforce one reading of the picture – that of a man-made construction, a colored canvas". The Cubist movement spread quickly throughout Paris and Europe.

A major idea of Braque's was the fractured stringed instrument as a cubist model. This he painted a number of times with variations, and made sculptures with fractured violins, guitars, etc., inside transparent acrylic (perspex) blocks. Examples:

Violin and Candlestick, Paris, spring 1910, at the San Francisco Museum of Modern Art.
Woman with a Guitar, 1913. Musée National d'Art Moderne, Centre Georges Pompidou, Paris, France.

Notes

Other websites 
Features an excellent selection of Braque paintings, with a rather weak text: The course of a painter in the representation of the landscape: Georges Braque 

1882 births
1963 deaths
French painters
French sculptors
Nitric oxide

Nitric oxide also known as nitrogen monoxide is a chemical compound. It contains nitrogen in its +2 oxidation state. It contains nitrogen and oxide ions. Its chemical formula is often given as ·N=O.

Properties
It is a colorless gas. It is easily oxidized to nitrogen dioxide by air. It can react with a mixture of air and water to make nitrous acid. It glows when reacted with ozone.

Preparation
It is made by reacting ammonia with oxygen with a catalyst. It is also made in lightning. It can be made in small amounts by reacting copper with nitric acid. It can also be made by reducing nitrous acid with compounds such as iron(II) sulfate.

Uses
Nitric oxide is used in making nitric acid from ammonia. Ammonia is reacted with air to make nitric oxide, and the nitric oxide is oxidized by air to make nitrogen dioxide. The nitrogen dioxide is dissolved in water to make nitric acid and more nitric oxide.

It is also used as a stimulant in the human body. It has many actions in the human body that are being studied.

Safety
Nitric oxide is toxic when breathed in. It also easily is oxidized to nitrogen dioxide, a toxic brown choking substance.

Related pages
Nitrous oxide
Nitrite
Sodium nitrite

Nitrogen compounds
Oxides
Nitrogen dioxide

Nitrogen dioxide is a chemical compound. Its chemical formula is NO2. It contains nitrogen and oxide ions. The nitrogen is in the +4 oxidation state.

Properties

Nitrogen Dioxide is a reddish-brown gas with a distinct, pungent odor similar to that of Chlorine. It causes significant and damaging pulmonary effects when it is inhaled, due to the formation of both Nitric (HNO3) & Nitrous (HNO2) acids when it reacts with Water present in the lungs. When Nitrogen Dioxide is compressed or cooled to near 0° C, two molecules of the Dioxide bond, forming the colorless Dinitrogen Tetroxide. It is a strong oxidizing agent. Upon heating, Nitrogen Dioxide decomposes back into lower oxides of Nitrogen (NO) as well as Oxygen. It reacts with iodides to form nitrites and elemental iodine. The presence of NO2 in concentrated Nitric acid causes the acid to take on a yellow color, depending on the concentration of the dissolved gas.

Preparation
Nitrogen dioxide is normally made by oxidation of nitric oxide by oxygen in air. It can also be made by heating some nitrates. It can be made by reacting concentrated nitric acid with copper or tin.

Uses
It is used to make nitric acid by dissolving it in water. Nitric oxide is also released.

Safety
Nitrogen dioxide is very toxic. It has a foul odor, which aids in its detection. Much care should be taken to avoid contact with this compound.

Related pages
Nitrous oxide
Nitrous acid

Nitrogen compounds
Oxides
Dinitrogen tetroxide

Dinitrogen tetroxide, also known as nitrogen tetroxide or dinitrogen tetraoxide, is a chemical compound. Its chemical formula is N2O4. It contains nitrogen in its +4 oxidation state. It contains nitrogen and oxide ions.

Properties
It is a colorless gas, although it is sometimes polluted with nitrogen dioxide. It is very corrosive and a strong oxidizing agent. It can ignite on contact with hydrazine. It can be made by bonding two nitrogen dioxide molecules together at a low temperature or a high pressure.

Preparation
It is made by bonding nitrogen dioxide molecules together in pairs.

Uses
It is used as a rocket propellant, along with hydrazine. This mixture is good since it does not have to be ignited. It is used similar to nitrogen dioxide to make nitric acid. It can react with metals to make nitrates.

Safety
Dinitrogen is highly toxic and corrosive. Some astronauts breathed it and had to go to a hospital.

Related pages
Nitrous oxide
Nitrogen oxide
List of nitrogen compounds

Sources

Nitrogen compounds
Oxides
Dinitrogen pentoxide

Dinitrogen pentoxide is a chemical compound. It is made by removing water from nitric acid. Its chemical formula is N2O5. It is a powerful oxidizing agent. It is a white solid. It is made by reacting phosphorus(V) oxide with nitric acid. The phosphorus(V) oxide removes the water from the nitric acid. It can be dissolved in chloroform to add the NO2+ group to some chemical compounds. It is toxic as it can make nitrogen dioxide gas.

Related pages
List of nitrogen compounds
Nitrogen triiodide
Ammonia

Nitrogen compounds
Oxides
Nitrogen trichloride

Nitrogen trichloride is a chemical compound. It contains nitrogen in its -3 oxidation state. It contains nitrogen and chloride ions. Its chemical formula is NCl3. It is an explosive. It is made by reacting ammonium compounds with chlorine. It reacts with hot water to release hypochlorous acid and ammonia.

Related pages
Nitrogen triiodide
Ammonium chloride
Nitrate

Nitrogen compounds
Chlorine compounds
Hypochlorous acid

Hypochlorous acid is a chemical compound. Its chemical formula is HClO or HOCl. It is not stable. It contains chlorine in its +1 oxidation state. It is a powerful oxidizing agent. It is made by reacting sodium hypochlorite with an acid that cannot be oxidized, such as phosphoric acid. If the acid can be oxidized, the hypochlorous acid will be destroyed. It is used to make some chemicals. It breaks down into hydrochloric acid and oxygen in sunlight. It reacts with hydrochloric acid to make chlorine gas. It is a powerful disinfectant.

References

Related pages
Perchlorate
Chlorate
Hypochlorite

Acids
Chlorine compounds
Sodium amide

Sodium amide, also known as sodamide, is a chemical compound. It contains sodium and amide ions. Its chemical formula is NaNH2. It is a very strong base, even stronger than hydroxides like sodium hydroxide. It reacts violently with water. It is a white solid, although it can be gray. It is made by reacting sodium metal with liquid or gaseous ammonia. It is used to make hydrazine and sodium azide. It is used to make various chemicals. It reacts with water to make ammonia and sodium hydroxide. It burns in air to make oxides of sodium and nitrogen, such as nitrogen dioxide. If there is only a little air, explosive chemicals may form. If it turns yellow or brown, get rid of it immediately. It is corrosive because it is a strong base.

Related pages
Sodium chloride
Ammonium
Nitrate

Sodium compounds
Nitrogen compounds
Amide

Amide can refer to two different things.

Amides in inorganic chemistry
An amide ion is different from an amide in organic chemistry. The amide ion is made by deprotonating ammonia. This is ammonia acting as an acid, although a very weak one. Amides made by deprotonating ammonia are very strong bases. Sodium amide is an example.

Amides in organic chemistry

Amides are also chemical compounds. They are made by reacting carboxylic acids like acetic acid with amines. There are many ways to make them. They are also used in many chemical reactions.

Related pages
Sodium azide
Azide
Nitrate

Nitrogen compounds
Functional groups
Sodium nitrate

Sodium nitrate, also known as caliche, Chile saltpeter, and soda niter, is a chemical compound. It contains sodium and nitrate ions. Its chemical formula is NaNO3.

Properties
It can dissolve in water very easily. It is an oxidizing agent. It is a white crystalline solid.

Occurrence and preparation
It is found in very dry areas. If it was wet, then the sodium nitrate would dissolve. But it is normally made artificially by reacting sodium hydroxide and nitric acid. Chile used to have much sodium nitrate naturally in the very dry Atacama Desert. It is found in small amounts in leafy green vegetables.

Uses
It is used to supply nitrogen to the soil. It is also used in making gunpowder. Some other explosives use it. It can be used to make nitric acid by reaction with sulfuric acid. It is used in rockets and smoke bombs. Sometimes it can be a food preservative.

Related pages
 Sodium nitrite
 Nitrite
 Ammonium

Sodium compounds
Nitrogen compounds
Lead azide

Lead azide, also known as lead(II) azide, is a chemical compound. Its chemical formula is Pb(N3)2. It contains lead and azide ions. It contains lead in its +2 oxidation state.

Lead azide is an explosive. Most other azides just burn rapidly. It is used as a detonator to detonate other explosives. It is made by reacting lead(II) nitrate and sodium azide. It can be destroyed by sodium dichromate. It can react with other metals such as copper to make even more sensitive azide explosives. It does not become less of an explosive when wet. It will explode if it is dropped .

Related pages
Lead(II) oxide
Sodium amide

Chemical compounds
Cobalt(II) chloride

Cobalt(II) chloride, also known as cobaltous chloride and cobalt dichloride, is a chemical compound. It contains cobalt in its +2 oxidation state. Its chemical formula is CoCl2. It contains cobalt and chloride ions.

Properties
Cobalt(II) chloride is normally found in the red (or pink) form. The red form has water in it. It can be heated to turn it into the blue form, without water. The blue form will absorb water from the air and turn red again. 

A different blue form is made when cobalt(II) chloride is reacted with a chemical compound that has chloride in it. Hydrochloric acid works the best, but sodium chloride can be used too. When it is heated, it turns more blue than when it is cooled. 

 for an example. Cobalt chloride can be used to test for chloride ions in this way.

It can be oxidized to cobalt(III) compounds, although cobalt(III) chloride does not exist. If it is made, it just drops a Cl from CoCl3, making CoCl2 (cobalt(II) chloride) again.

Preparation
The anhydrous (without water) blue form can be made by reacting cobalt with chlorine. The hydrated (with water) red form can be made by reacting cobalt(II) oxide or cobalt(II) hydroxide with hydrochloric acid.

Uses
It is used to place cobalt into other chemical compounds. It can be used to make other cobalt compounds. It is the most common cobalt compound in the lab.

Safety
It is a weak oxidizing agent, too weak to ignite things. Cobalt compounds are toxic in large quantities, like any other transition metal compounds. They are not toxic like lead or mercury compounds, though.

References

Related pages
Cobalt(III) oxide
Cobalt(II) sulfate

Chlorine compounds
Cobalt compounds
Man of the match

Man of the Match is an award given to one player from each School Cup match (game). This award was created and first awarded for the 2021 School Cup tournament. The award is sponsored by City mark, a large world-wide beer company.

The winner of the award is decided by all playes votes. The players vote during the match. Voting closed when the match is over. The Man of the Match trophy will be awarded to the winning player at the end of the game.

References
Prohibition Era

The Prohibition Era was a period in United States history when alcohol was outlawed.  Police would arrest anyone who was found making or selling alcohol illegally. The Women's Christian Temperance Union and other reformist organizations agitated for this change in order to improve the lives of the people. Prohibition lasted from 1920 to 1933. It was established by the Eighteenth Amendment to the United States Constitution. It was ratified (approved by the states) by January 16, 1919. It came into effect at January 16, 1920. 
The punishment for being caught with an alcoholic beverage was jail time. The millions of people becoming criminals in such a short period of time led to overflowing prisons and it was common to have a case dismissed. Prohibition was a constitutional experiment set up by the American government in an effort to decrease crime rates, reduce tax burden, and improve health in Americans. It had little to do with the consumption of alcoholic beverages.
     
Prohibition was good as the consumption of alcohol was reduced, but it was bad in that the Mafia and other underground organizations took up rum-running. They became big and powerful and made trouble. Prohibition was repealed December 5, 1933 by the Twenty-first Amendment. Now states can regulate the selling of liquor by themselves.
1920 establishments in the United States
1933 disestablishments
1920s in the United States
1930s in the United States
Alcohol drinking habits
United States law
1930s disestablishments in the United States
Cobalt(II) oxide

Cobalt(II) oxide, also known as cobaltous oxide, is a chemical compound. Its chemical formula is CoO. It contains cobalt in its +2 oxidation state as an ion. It also contains oxide. It can be green or red crystals. It can also be a grey or brown powder.

Preparation
Cobalt(II) chloride reacts with a base to get cobalt(II) hydroxide. Then the cobalt(II) hydroxide is heated to make cobalt(II) oxide. The reactions are written below:
 CoCl2 + 2 NaOH → 2 NaCl + Co(OH)2
 Co(OH)2 → CoO + H2O

Use
It can react with acids to make salts containing cobalt. It is used to make blue glass.

Related pages
Cobalt(II) sulfate
Cobalt(III) oxide

Cobalt compounds
Oxides
Cobalt(II) hydroxide

Cobalt(II) hydroxide is a chemical compound. Its chemical formula is Co(OH)2. It contains cobalt in its +2 oxidation state as an ion. It also contains hydroxide ions. It is either reddish or bluish. It is made by reacting a strong base with a cobalt(II) salt. Cobalt(II) chloride is normally used. This makes the red form. The blue form is made by reacting ammonium hydroxide with cobalt(II) hydroxide. It turns into cobalt(II) oxide when heated. It is used to dry paints, to make other cobalt compounds, and as a catalyst.

Related pages
Cobalt(II) sulfate
Cobalt(III) oxide
Cobalt

Cobalt compounds
Cobalt(III) oxide

Cobalt(III) oxide is a chemical compound. It contains cobalt in its +3 oxidation state. Its chemical formula is Co2O3. It can be made by reacting a cobalt(II) salt with sodium hypochlorite. This reaction also makes some chlorine. It is used as a catalyst. It is an oxidizing agent. It is not as strong an oxidizing agent as other cobalt(III) compounds.

Related pages
Cobalt(II) oxide
Cobalt(II) chloride
Cobalt(II) sulfate

Cobalt compounds
Oxides
Cobalt(II) sulfate

Cobalt(II) sulfate, also known as cobaltous sulfate, is a chemical compound. Its chemical formula is CoSO4. It contains cobalt in its +2 oxidation state. It contains cobalt and sulfate ions.

Properties
It is a reddish crystalline solid. It dissolves easily in water. It is reddish without water (anhydrous) and pink with water (hydrated).

Preparation
It can be made by reacting cobalt, cobalt(II) oxide, or cobalt(II) hydroxide with sulfuric acid. It is very rarely found in the earth.

Uses
It is used as a pigment. It is also used to make other cobalt salts. It can be used in electroplating cobalt. It was added to beer in the past but that poisoned people.

Safety
Cobalt(II) sulfate is slightly carcinogenic. It is poisonous in large quantities.

Related pages
Cobalt(II) chloride
Cobalt(III) oxide

Sulfur compounds
Cobalt compounds
Meccano

Meccano is a building set that lets people make models and small mechanical devices. It was made in 1901, and was from the United Kingdom.

Toys
Monoclonius

Monoclonius is the doubtful name of a ceratopsid dinosaur. It was a herbivore (plant-eater)  It lived in North America during the Upper Cretaceous, about 76 to 73 million years ago.

Monoclonius was named by Edward Drinker Cope in 1876, soon after the first fossil specimen had been found in Montana. The specimen was a near complete skeleton with only the feet missing. It included skull material and the base of the nasal horn. Its name means "single stem" and refers to its teeth, which have a single root.

Monoclonius is now regarded as a nominem dubium. It seems to be a juvenile stage of Centrosaurus.

References 

Ceratopsids
Gordini

Gordini is a French sports car manufacturer. The firm was founded by Amédée Gordini. His nickname was "Le Sorcier", which means "The Sorcerer".

Gordini competed in Formula One from 1950 to 1956.

Gordini worked with Renault as an engine tuner. He sold his firm to Renault. Renault entered Renault-Gordini cars at the 24 Hours of Le Mans from 1962 until 1969.

Renault build sport versions of some models like the Dauphine, Renault 8, and Renault 12. They included the Gordini badge.

In November 2009, Renault announced that it will bring back the Gordini name. It will be used on a line of hot hatches (sports compacts).

Formula One results

As a works (factory) team 
(key) (results in bold indicate pole position) (results in italics indicate fastest lap)

(† indicates shared drive)

As an engine supplier 
(key) (results in bold indicate pole position)

References 

Formula One constructors
Formula One engine manufacturers
Popish Plot

The Popish Plot was a story made up by Titus Oates that caused people to hate the Catholics in England between 1678 and 1681. Oates said that there was a large Catholic conspiracy to kill Charles II. His story led to the execution of at least 15 men and caused the Exclusion Bill Crisis. After a while Oates' complicated story fell apart, and he was arrested and sent to prison for perjury.

References

17th century in England
1678
1679
1680
1681
1680s in Europe
Cobalt(II,III) oxide

Cobalt(II,III) oxide is a chemical compound. It contains some (1 atom) cobalt in the +2 oxidation state and some (2 atoms) in the +3 oxidation state. Its chemical formula is Co3O4. It contains cobalt and oxide ions.

Properties
It is a black solid. It reacts with hydrochloric acid to make chlorine and cobalt(II) chloride.

Preparation
It is made when cobalt(II) oxide is heated to . When it is heated to , it turns back into cobalt(II) oxide.

Uses
It has been used in research for making hydrogen.

Safety
It is irritating to the skin. It can cause harm if swallowed. It dissolves in the stomach acid.

Related pages
Iron(II,III) oxide
Cobalt(III) oxide

Cobalt compounds
Oxides
Cobalt(II) fluoride

Cobalt(II) fluoride, also known as cobaltous fluoride, is a chemical compound. Its chemical formula is CoF2. It contains cobalt in its +2 oxidation state. It also contains fluoride ions.

Properties
It is a reddish crystalline solid. It only dissolves a little in water. The hydrate (type with water molecules attached) can dissolve in water. It can dissolve in acid. It can react with hydrogen at  to make cobalt and hydrogen fluoride.

Preparation
It can be made by reacting anhydrous (without any water molecules attached) cobalt(II) oxide or cobalt(II) chloride with a stream of hydrogen fluoride. This reaction makes the anhydrous form. The hydrated (with water molecules attached) form is made by reacting any cobalt(II) compound with hydrofluoric acid. When fluorine is reacted with cobalt at a high temperature, it makes both cobalt(II) fluoride and cobalt(III) fluoride.

Uses
It is used as a catalyst. It can be used as a source of the fluoride ion in dentist care. It is used in lenses.

Related pages
Cobalt(II) hydroxide
Cobalt(III) oxide

Cobalt compounds
Fluorine compounds
Cobalt(III) fluoride

Cobalt(III) fluoride, also known as cobaltic fluoride and cobalt trifluoride, is a chemical compound. Its chemical formula is CoF3. It contains cobalt in its +3 oxidation state. It contains cobalt and fluoride ions. It is used to add fluoride ion to other chemicals. It is a brown solid. It is a powerful oxidizing agent. It reacts with water to make hydrofluoric acid, oxygen, and cobalt(II) fluoride. It is made by reacting cobalt(II) chloride and fluorine at . Cobalt(II) oxide and cobalt(II) fluoride can be used instead of the cobalt(II) chloride. It is used to make some chemicals.

Related pages
Cobalt(II) hydroxide

Cobalt compounds
Fluorine compounds
Eyeborg

An eyeborg or eye-borg is an electronic eye that allows people to hear colors. It is mostly used by blind people or by people with color blindness. It works by using a head mounted camera that reads the colors directly in front of a person, and converts them into musical notes.

The first eyeborg was made in England in 2003 by Adam Montandon in collaboration with colourblind artist Neil Harbisson. The invention won a British award in Innovation (Submerge 2004) and a European award in Content Tools and Interface Design (Europrix 2004). In 2007, Peter Kese, a software developer from Slovenia, made further developments to the eyeborg by increasing the number of colors to 360 and adding color intensity through different volume levels. Matias Lizana, a student from Universitat Politècnica de Catalunya is currently developing the eyeborg into a smaller chip as part of his final year project. The new chip will allow users to hear colors in stereo and to embed the device.

Other websites
Eyeborg Website  Eyeborg chip development site
Cyborg Enables Color-Blind Artist to Hear His Palette Article about an eyeborg user on Wired (USA 2008)
Eyeborg user example  on The Sunday Times (UK, 2008)
Seeing things in a different light Information from BBC (UK, 2005)
Neil Harbisson's personal website

References

Vision
Christian Dior

Christian Dior (Granville, Manche, Basse-Normandie, 21 January 1905 –  Montecatini, Italy, 24 October 1957), was the leading French fashion designer of the post-war world. He was the founder of one of the world's top fashion houses, the House of Dior (now Christian Dior).

Career 
During the German occupation of France in World War II, Christian Dior dressed the wives of Nazi officers and French collaborators. On 8 October 1946 he founded his own fashion house, backed by Marcel Boussac, the cotton-fabric magnate.

The New Look 
For his first collection, in early 1947, the phrase The New Look was coined by Harper's Bazaar, the fashion monthly. Dior's designs were more voluptuous than the economy shapes of World War II, when fabric was rationed. 

Dior was a master at creating shapes and silhouettes; he said "I have designed flower women". His look employed fabrics lined with percale (a closely woven plain-weave fabric), boned, bustier-style bodices, hip padding, wasp-waisted corsets and petticoats. This made his dresses flare out from the waist, giving his models a very curvaceous form. 

Some women protested, because his designs covered up their legs, which they did not during wartime. There was also criticism of Dior's designs, which used a lot of fabric. Opposition ceased as soon as wartime shortages ended. The New Look revolutionized women's dress and reestablished Paris as the center of the fashion world.

A-line 
The term was first used by Dior as the label for his collection of spring 1955. The  A-Line collection's feature item, then the "most wanted silhouette in Paris", was a "fingertip-length flared jacket worn over a dress with a very full, pleated skirt". Evening dresses at this time were always worn with petticoats.

Although an A-shape, this silhouette was not identical to what is now understood to embody the A-line idea. That idea was given its definitive expression and popularized by Dior’s successor, Yves Saint Laurent, with his "Trapeze Line" of spring 1958, which featured dresses flaring out dramatically from a fitted shoulder line. 

A-line clothes remained popular in the 1960s and 70s, disappeared from fashion almost completely by the early 1980s and were revived by the retro trend of the late 1990s. By that time, 'A-line' was used more loosely to describe any dress wider at the hips than at the bust or waist, as well as a number of flared skirt styles. 'True' A-line shapes on the pattern of Dior and Saint Laurent saw a revival in the early 2000s.

References 

1905 births
1957 deaths
French fashion designers
French fashion houses
Baluchistan Agency

The Baluchistan Agency was one of the agencies of British India. Agency Territories, with an area of 44,345 square miles (208.262 km2), composed of tracts which had, from time to time, been acquired by lease or otherwise brought under control and been placed directly under British officers. 

This agency consisted of three princely states, Kalat and its two feudatory states Las Bela and Kharan. The British government maintained the administrative control through their political agent in Kalat.

British India
Ferromanganese

Ferromanganese, also known as spiegeleisen, is an alloy. It is made of iron and manganese. It is normally 15% manganese and 85% iron. It is made by reduction of a mixture of iron ore and manganese ore. Normally carbon is the reducing agent. It is normally how manganese is sold.

Related pages
Cobalt

Alloys
Manganese(VII) oxide

Manganese(VII) oxide, also known as permanganic acid and manganese heptoxide, is a chemical compound. The manganese is in its +7 oxidation state. Its chemical formula is Mn2O7. This is about the only +7 oxidation state compound of manganese that is not a permanganate. Its chemical formula is Mn2O7. It is either a dark red or green oil. It is a powerful oxidizing agent. It is a dangerous explosive. It is made by combining sulfuric acid with potassium permanganate. This reaction makes the dark green oil. It makes manganese dioxide and oxygen when exploded. This reaction may produce ozone, a powerful oxidizing agent. It can be detonated by striking it or reacting it with some organic compounds such as alcohol.

Related pages
Manganese(II) oxide

Manganese compounds
Manganese(II) sulfate

Manganese(II) sulfate, also known as manganous sulfate, is a chemical compound. It contains manganese in its +2 oxidation state. It contains manganese and sulfate ions. Its chemical formula is MnSO4. It is a pink crystalline solid. It normally is bonded with some water molecules. It is part of a process to make manganese metal. It can be made separately though. If sulfur dioxide and manganese dioxide are reacted, it produces manganese(II) sulfate. It reacts with potassium permanganate to make manganese dioxide. It is used to add manganese to soil.

Related pages
Manganese(II) carbonate
Manganese(II) oxide
Manganese(VII) oxide

Sulfur compounds
Manganese compounds