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Halogen
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This article is about the chemical series. For other uses, see Halogen (disambiguation).
Halogens
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
chalcogens ← → noble gases
IUPAC group number
17
Name by element fluorine group
Trivial name halogens
CAS group number
(US, pattern A-B-A)
VIIA
old IUPAC number
(Europe, pattern A-B)
VIIB
↓ Period
2
Fluorine (F)
9 Halogen
3
Chlorine (Cl)
17 Halogen
4
Bromine (Br)
35 Halogen
5
Iodine (I)
53 Halogen
6
Astatine (At)
85 Halogen
Legend
primordial element
element from decay
Atomic number color:
black=solid, green=liquid, red=gas
v
t
e
The halogens (/ˈhælədʒən, ˈheɪ-, -loʊ-, -ˌdʒɛn/[1][2][3]) are a group in the periodic table consisting of five chemically related elements: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). The artificially created element 117 (tennessine, Ts) may also be a halogen. In the modern IUPAC nomenclature, this group is known as group 17. The symbol X is often used generically to refer to any halogen.
The name "halogen" means "salt-producing". When halogens react with metals they produce a wide range of salts, including calcium fluoride, sodium chloride (common table salt), silver bromide and potassium iodide.
The group of halogens is the only periodic table group that contains elements in all three main states of matter at standard temperature and pressure. All of the halogens form acids when bonded to hydrogen. Most halogens are typically produced from minerals or salts. The middle halogens, that is chlorine, bromine and iodine, are often used as disinfectants. Organobromides are the most important class of flame retardants. Elemental halogens are dangerous and can potentially be lethally toxic.
Contents
[hide]
1 History
1.1 Etymology
2 Characteristics
2.1 Chemical
2.1.1 Molecules
2.1.1.1 Diatomic halogen molecules
2.1.2 Compounds
2.1.2.1 Hydrogen halides
2.1.2.2 Metal halides
2.1.2.3 Interhalogen compounds
2.1.2.4 Organohalogen compounds
2.1.2.5 Polyhalogenated compounds
2.1.3 Reactions
2.1.3.1 Reactions with water
2.2 Physical and atomic
2.2.1 Isotopes
3 Production
4 Applications
5 Biological role
6 Toxicity
7 Superhalogen
8 See also
9 Notes
10 References
11 Further reading
History[edit]
The fluorine mineral fluorospar was known as early as 1529. Early chemists realized that fluorine compounds contain an undiscovered element, but were unable to isolate it. In 1869, George Gore, an English chemist, ran a current of electricity through hydrofluoric acid and probably produced fluorine, but he was unable to prove his results at the time. In 1886, Henri Moissan, a chemist in Paris, performed electrolysis on potassium bifluoride dissolved in anhydrous hydrogen fluoride, and successfully isolated fluorine.[4]
Hydrochloric acid was known to alchemists and early chemists. However, elemental chlorine was not produced until 1774, when Carl Wilhelm Scheele heated hydrochloric acid with manganese dioxide. Scheele called the element "dephlogisticated muriatic acid", which is how chlorine was known for 33 years. In 1807, Humphry Davy investigated chlorine and discovered that it is an actual element. Chlorine was used as a poison gas during World War I.[4]
Bromine was discovered in the 1820s by Antoine-Jérôme Balard. Balard discovered bromine by passing chlorine gas through a sample of brine. He originally proposed the name muride for the new element, but the French Academy changed the element's name to bromine.[4]
Iodine was discovered by Bernard Courtois, who was using seaweed ash as part of a process for saltpeter manufacture. Courtois typically boiled the seaweed ash with water to generate potassium chloride. However, in 1811, Courtois added sulfuric acid to his process, and found that his process produced purple fumes that condensed into black crystals. Suspecting that these crystals were a new element, Courtois sent samples to other chemists for investigation. Iodine was proven to be a new element by Joseph Gay-Lussac.[4]
In 1931, Fred Allison claimed to have discovered element 85 with a magneto-optical machine, and named the element Alabamine, but was mistaken. In 1937, Jajendralal De claimed to have discovered element 85 in minerals, and called the element dakine, but he was also mistaken. An attempt at discovering element 85 in 1939 by Horia Hulubei and Yvette Cauchois via spectroscopy was also unsuccessful, as was an attempt in the same year by Walter Minder, who discovered an iodine-like element resulting from beta decay of radium. Element 85, now named astatine, was produced successfully in 1940 by Dale R. Corson, K.R. Mackenzie, and Emilio G. Segrè, who bombarded bismuth with alpha particles.[4]
Etymology[edit]
In 1842, the Swedish chemist Baron Jöns Jakob Berzelius proposed the term "halogen" – ἅλς (háls), "salt" or "sea", and γεν- (gen-), "to produce" – for the four elements (fluorine, chlorine, bromine, and iodine) that produce a sea-salt-like substance when they form a compound with a metal.[5] The word "halogen" had actually first been proposed in 1811 by Johann Salomo Christoph Schweigger as a name for the newly discovered element chlorine, but Davy's proposed term for this element eventually won out, and Schweigger's term was kept at Berzelius' suggestion as the term for the element group that contains chlorine.[6]
Fluorine's name comes from the Latin word fluere, meaning "to flow". Chlorine's name comes from the Greek word chloros, meaning "greenish-yellow". Bromine's name comes from the Greek word bromos, meaning "stench". Iodine's name comes from the Greek word iodes, meaning "violet". Astatine's name comes from the Greek word astatos, meaning "unstable".[4] Tennessine is named after the US state of Tennessee.
Characteristics[edit]
Chemical[edit]
The halogens show trends in chemical bond energy moving from top to bottom of the periodic table column with fluorine deviating slightly. (It follows trend in having the highest bond energy in compounds with other atoms, but it has very weak bonds within the diatomic F2 molecule.) This means, as you go down the periodic table, the reactivity of the element will decrease because of the increasing size of the atoms.[7]
Halogen bond energies (kJ/mol)[8]
X
X2
HX
BX3
AlX3
CX4
F
159 574 645 582 456
Cl
243 428 444 427 327
Br
193 363 368 360 272
I
151 294 272 285 239
Halogens are highly reactive, and as such can be harmful or lethal to biological organisms in sufficient quantities. This high reactivity is due to the high electronegativity of the atoms due to their high effective nuclear charge. Because the halogens have seven valence electrons in their outermost energy level, they can gain an electron by reacting with atoms of other elements to satisfy the octet rule. Fluorine is one of the most reactive elements, attacking otherwise-inert materials such as glass, and forming compounds with the usually inert noble gases. It is a corrosive and highly toxic gas. The reactivity of fluorine is such that, if used or stored in laboratory glassware, it can react with glass in the presence of small amounts of water to form silicon tetrafluoride (SiF4). Thus, fluorine must be handled with substances such as Teflon (which is itself an organofluorine compound), extremely dry glass, or metals such as copper or steel, which form a protective layer of fluoride on their surface.
The high reactivity of fluorine allows paradoxically some of the strongest bonds possible, especially to carbon. For example, Teflon is fluorine bonded with carbon and is extremely resistant to thermal and chemical attack and has a high melting point.
Molecules[edit]
Diatomic halogen molecules[edit]
The halogens form homonuclear diatomic molecules (not proven for astatine). Due to relatively weak intermolecular forces, chlorine and fluorine form part of the group known as "elemental gases".
halogen
molecule
structure
model
d(X−X) / pm
(gas phase)
d(X−X) / pm
(solid phase)
fluorine F2 143 149
chlorine Cl2 199 198
bromine Br2 228 227
iodine I2 266 272
The elements become less reactive and have higher melting points as the atomic number increases. The higher melting points are caused by stronger London dispersion forces resulting from more electrons.
Compounds[edit]
Hydrogen halides[edit]
All of the halogens have been observed to react with hydrogen to form hydrogen halides. For fluorine, chlorine, and bromine, this reaction is in the form of:
H2 + X2 → 2HX
However, hydrogen iodide and hydrogen astatide can split back into their constituent elements.[9]
The hydrogen-halogen reactions get gradually less reactive toward the heavier halogens. A fluorine-hydrogen reaction is explosive even when it is dark and cold. A chlorine-hydrogen reaction is also explosive, but only in the presence of light and heat. A bromine-hydrogen reaction is even less explosive; it is explosive only when exposed to flames. Iodine and astatine only partially react with hydrogen, forming equilibria.[9]
All halogens form binary compounds with hydrogen known as the hydrogen halides: hydrogen fluoride (HF), hydrogen chloride (HCl), hydrogen bromide (HBr), hydrogen iodide (HI), and hydrogen astatide (HAt). All of these compounds form acids when mixed with water. Hydrogen fluoride is the only hydrogen halide that forms hydrogen bonds. Hydrochloric acid, hydrobromic acid, hydroiodic acid, and hydroastatic acid are all strong acids, but hydrofluoric acid is a weak acid.[10]
All of the hydrogen halides are irritants. Hydrogen fluoride and hydrogen chloride are highly acidic. Hydrogen fluoride is used as an industrial chemical, and is highly toxic, causing pulmonary edema and damaging cells.[11] Hydrogen chloride is also a dangerous chemical. Breathing in gas with more than fifty parts per million of hydrogen chloride can cause death in humans.[12] Hydrogen bromide is even more toxic and irritating than hydrogen chloride. Breathing in gas with more than thirty parts per million of hydrogen bromide can be lethal to humans.[13] Hydrogen iodide, like other hydrogen halides, is toxic.[14]
Metal halides[edit]
Main article: Metal halides
All the halogens are known to react with sodium to form sodium fluoride, sodium chloride, sodium bromide, sodium iodide, and sodium astatide. Heated sodium's reaction with halogens produces bright-orange flames. Sodium's reaction with chlorine is in the form of:
2Na + Cl2 → 2NaCl[9]
Iron reacts with fluorine, chlorine, and bromine to form Iron(III) halides. These reactions are in the form of:
2Fe + 3X2 → 2FeX3[9]
However, when iron reacts with iodine, it forms only iron(II) iodide.
Iron wool can react rapidly with fluorine to form the white compound iron(III) fluoride even in cold temperatures. When chlorine comes into contact with heated iron, they react to form the black iron (III) chloride. However, if the reaction conditions are moist, this reaction will instead result in a reddish-brown product. Iron can also react with bromine to form iron(III) bromide. This compound is reddish-brown in dry conditions. Iron's reaction with bromine is less reactive than its reaction with fluorine or chlorine. Hot iron can also react with iodine, but it forms iron(II) iodide. This compound may be gray, but the reaction is always contaminated with excess iodine, so it is not known for sure. Iron's reaction with iodine is less vigorous than its reaction with the lighter halogens.[9]
Interhalogen compounds[edit]
Main article: Interhalogen
Interhalogen compounds are in the form of XYn where X and Y are halogens and n is one, three, five, or seven. Interhalogen compounds contain at most two different halogens. Large interhalogens, such as ClF3 can be produced by a reaction of a pure halogen with a smaller interhalogen such as ClF. All interhalogens except IF7 can be produced by directly combining pure halogens in various conditions.[15]
Interhalogens are typically more reactive than all diatomic halogen molecules except F2 because interhalogen bonds are weaker. However, the chemical properties of interhalogens are still roughly the same as those of diatomic halogens. Many interhalogens consist of one or more atoms of fluorine bonding to a heavier halogen. Chlorine can bond with up to 3 fluorine atoms, bromine can bond with up to five fluorine atoms, and iodine can bond with up to seven fluorine atoms. Most interhalogen compounds are covalent gases. However, there are some interhalogens that are liquids, such as BrF3, and many iodine-containing interhalogens are solids.[15]
Organohalogen compounds[edit]
Many synthetic organic compounds such as plastic polymers, and a few natural ones, contain halogen atoms; these are known as halogenated compounds or organic halides. Chlorine is by far the most abundant of the halogens in seawater, and the only one needed in relatively large amounts (as chloride ions) by humans. For example, chloride ions play a key role in brain function by mediating the action of the inhibitory transmitter GABA and are also used by the body to produce stomach acid. Iodine is needed in trace amounts for the production of thyroid hormones such as thyroxine. Organohalogens are also synthesized through the nucleophilic abstraction reaction.
Polyhalogenated compounds[edit]
Polyhalogenated compounds are industrially created compounds substituted with multiple halogens. Many of them are very toxic and bioaccumulate in humans, and have a very wide application range. They include PCBs, PBDEs, and perfluorinated compounds (PFCs), as well as numerous other compounds.
Reactions[edit]
Reactions with water[edit]
Fluorine reacts vigorously with water to produce oxygen (O2) and hydrogen fluoride (HF):[16]
2 F2(g) + 2 H2O(l) → O2(g) + 4 HF(aq)
Chlorine has maximum solubility of ca. 7.1 g Cl2 per kg of water at ambient temperature (21 °C).[17] Dissolved chlorine reacts to form hydrochloric acid (HCl) and hypochlorous acid, a solution that can be used as a disinfectant or bleach:
Cl2(g) + H2O(l) → HCl(aq) + HClO(aq)
Bromine has a solubility of 3.41 g per 100 g of water,[18] but it slowly reacts to form hydrogen bromide (HBr) and hypobromous acid (HBrO):
Br2(g) + H2O(l) → HBr(aq) + HBrO(aq)
Iodine, however, is minimally soluble in water (0.03 g/100 g water at 20 °C) and does not react with it.[19] However, iodine will form an aqueous solution in the presence of iodide ion, such as by addition of potassium iodide (KI), because the triiodide ion is formed.
Physical and atomic[edit]
The table below is a summary of the key physical and atomic properties of the halogens. Data marked with question marks are either uncertain or are estimations partially based on periodic trends rather than observations.
Halogen
Standard atomic weight
(u)[n 1][21]
Melting point
(K)
Melting point
(°C)
Boiling point
(K)[22]
Boiling point
(°C)[22]
Density
(g/cm3at 25 °C)
Electronegativity
(Pauling)
First ionization energy
(kJ·mol−1)
Covalent radius
(pm)[23]
Fluorine 18.9984032(5) 53.53 −219.62 85.03 −188.12 0.0017 3.98 1681.0 71
Chlorine [35.446; 35.457][n 2] 171.6 −101.5 239.11 −34.04 0.0032 3.16 1251.2 99
Bromine 79.904(1) 265.8 −7.3 332.0 58.8 3.1028 2.96 1139.9 114
Iodine 126.90447(3) 386.85 113.7 457.4 184.3 4.933 2.66 1008.4 133
Astatine [210][n 3] 575 302 ? 610 ? 337 ? 6.2–6.5[24] 2.2 ? 887.7 ?
Isotopes[edit]
Fluorine has one stable and naturally occurring isotope, fluorine-19. However, there are trace amounts in nature of the radioactive isotope fluorine-23, which occurs via cluster decay of protactinium-231. A total of eighteen isotopes of fluorine have been discovered, with atomic masses ranging from 14 to 31. Chlorine has two stable and naturally occurring isotopes, chlorine-35 and chlorine-37. However, there are trace amounts in nature of the isotope chlorine-36, which occurs via spallation of argon-36. A total of 24 isotopes of chlorine have been discovered, with atomic masses ranging from 28 to 51.[4]
There are two stable and naturally occurring isotopes of bromine, bromine-79 and bromine-81. A total of 32 isotopes of bromine have been discovered, with atomic masses ranging 67 to 98. There is one stable and naturally occurring isotope of iodine, iodine-127. However, there are trace amounts in nature of the radioactive isotope iodine-129, which occurs via spallation and from the radioactive decay of uranium in ores. Several other radioactive isotopes of iodine have also been created naturally via the decay of uranium. A total of 38 isotopes of iodine have been discovered, with atomic masses ranging from 108 to 145.[4]
There are no stable isotopes of astatine. However, there are three naturally occurring radioactive isotopes of astatine produced via radioactive decay of uranium, neptunium, and plutonium. These isotopes are astatine-215, astatine-217, and astatine-219. A total of 31 isotopes of astatine have been discovered, with atomic masses ranging from 193 to 223.[4]
Production[edit]
Approximately six million metric tons of the fluorine mineral fluorite are produced each year. Four hundred-thousand metric tons of hydrofluoric acid are made each year. Fluorine gas is made from hydrofluoric acid produced as a by-product in phosphoric acid manufacture. Approximately 15,000 metric tons of fluorine gas are made per year.[4]
The mineral halite is the mineral that is most commonly mined for chlorine, but the minerals carnallite and sylvite are also mined for chlorine. Forty million metric tons of chlorine are produced each year by the electrolysis of brine.[4]
Approximately 450,000 metric tons of bromine are produced each year. Fifty percent of all bromine produced is produced in the United States, 35% in Israel, and most of the remainder in China. Historically, bromine was produced by adding sulfuric acid and bleaching powder to natural brine. However, in modern times, bromine is produced by electrolysis, a method invented by Herbert Dow. It is also possible to produce bromine by passing chlorine through seawater and then passing air through the seawater.[4]
In 2003, 22,000 metric tons of iodine were produced. Chile produces 40% of all iodine produced, Japan produces 30%, and smaller amounts are produced in Russia and the United States. Until the 1950s, iodine was extracted from kelp. However, in modern times, iodine is produced in other ways. One way that iodine is produced is by mixing sulfur dioxide with nitrate ores, which contain some iodates. Iodine is also extracted from natural gas fields.[4]
Even though astatine is naturally occurring, it is usually produced by bombarding bismuth with alpha particles.[4]
From left to right: chlorine, bromine, and iodine at room temperature. Chlorine is a gas, bromine is a liquid, and iodine is a solid. Fluorine could not be included in the image due to its high reactivity, and astatine due to its radioactivity.
Applications[edit]
Both chlorine and bromine are used as disinfectants for drinking water, swimming pools, fresh wounds, spas, dishes, and surfaces. They kill bacteria and other potentially harmful microorganisms through a process known as sterilization. Their reactivity is also put to use in bleaching. Sodium hypochlorite, which is produced from chlorine, is the active ingredient of most fabric bleaches, and chlorine-derived bleaches are used in the production of some paper products. Chlorine also reacts with sodium to create sodium chloride, which is table salt.
Halogen lamps are a type of incandescent lamp using a tungsten filament in bulbs that have a small amounts of a halogen, such as iodine or bromine added. This enables the production of lamps that are much smaller than non-halogen incandescent lightbulbs at the same wattage. The gas reduces the thinning of the filament and blackening of the inside of the bulb resulting in a bulb that has a much greater life. Halogen lamps glow at a higher temperature (2800 to 3400 kelvins) with a whiter color than other incandescent bulbs. However, this requires bulbs to be manufactured from fused quartz rather than silica glass to reduce breakage.[25]
In drug discovery, the incorporation of halogen atoms into a lead drug candidate results in analogues that are usually more lipophilic and less water-soluble.[26] As a consequence, halogen atoms are used to improve penetration through lipid membranes and tissues. It follows that there is a tendency for some halogenated drugs to accumulate in adipose tissue.
The chemical reactivity of halogen atoms depends on both their point of attachment to the lead and the nature of the halogen. Aromatic halogen groups are far less reactive than aliphatic halogen groups, which can exhibit considerable chemical reactivity. For aliphatic carbon-halogen bonds, the C-F bond is the strongest and usually less chemically reactive than aliphatic C-H bonds. The other aliphatic-halogen bonds are weaker, their reactivity increasing down the periodic table. They are usually more chemically reactive than aliphatic C-H bonds. As a consequence, the most common halogen substitutions are the less reactive aromatic fluorine and chlorine groups.
Biological role[edit]
Fluoride anions are found in ivory, bones, teeth, blood, eggs, urine, and hair of organisms. Fluoride anions in very small amounts may be essential for humans.[27] There are 0.5 milligrams of fluorine per liter of human blood. Human bones contain 0.2 to 1.2% fluorine. Human tissue contains approximately 50 parts per billion of fluorine. A typical 70-kilogram human contains 3 to 6 grams of fluorine.[4]
Chloride anions are essential to a large number of species, humans included. The concentration of chlorine in the dry weight of cereals is 10 to 20 parts per million, while in potatoes the concentration of chloride is 0.5%. Plant growth is adversely affected by chloride levels in the soil falling below 2 parts per million. Human blood contains an average of 0.3% chlorine. Human bone typically contains 900 parts per million of chlorine. Human tissue contains approximately 0.2 to 0.5% chlorine. There is a total of 95 grams of chlorine in a typical 70-kilogram human.[4]
Some bromine in the form of the bromide anion is present in all organisms. A biological role for bromine in humans has not been proven, but some organisms contain organobromine compounds. Humans typically consume 1 to 20 milligrams of bromine per day. There are typically 5 parts per million of bromine in human blood, 7 parts per million of bromine in human bones, and 7 parts per million of bromine in human tissue. A typical 70-kilogram human contains 260 milligrams of bromine.[4]
Humans typically consume less than 100 micrograms of iodine per day. Iodine deficiency can cause intellectual disability. Organoiodine compounds occur in humans in some of the glands, especially the thyroid gland, as well as the stomach, epidermis, and immune system. Foods containing iodine include cod, oysters, shrimp, herring, lobsters, sunflower seeds, seaweed, and mushrooms. However, iodine is not known to have a biological role in plants. There are typically 0.06 milligrams per liter of iodine in human blood, 300 parts per billion of iodine in human bones, and 50 to 700 parts per billion of iodine in human tissue. There are 10 to 20 milligrams of iodine in a typical 70-kilogram human.[4]
Astatine has no biological role.[4]
Toxicity[edit]
The halogens tend to decrease in toxicity towards the heavier halogens.[28]
Fluorine gas is extremely toxic; breathing fluorine gas at a concentration of 0.1% for several minutes is lethal. Hydrofluoric acid is also toxic, being able to penetrate skin and cause highly painful burns. In addition, fluoride anions are toxic, but not as toxic as pure fluorine. Fluoride can be lethal in amounts of 5 to 10 grams. Prolonged consumption of fluoride above concentrations of 1.5 mg/L is associated with a risk of dental fluorosis, an aesthetic condition of the teeth.[29] At concentrations above 4 mg/L, there is an increased risk of developing skeletal fluorosis, a condition in which bone fractures become more common due to the hardening of bones. Current recommended levels in water fluoridation, a way to prevent dental caries, range from 0.7 to 1.2 mg/L to avoid the detrimental effects of fluoride while at the same time reaping the benefits.[30] People with levels between normal levels and those required for skeletal fluorosis tend to have symptoms similar to arthritis.[4]
Chlorine gas is highly toxic. Breathing in chlorine at a concentration of 3 parts per million can rapidly cause a toxic reaction. Breathing in chlorine at a concentration of 50 parts per million is highly dangerous. Breathing in chlorine at a concentration of 500 parts per million for a few minutes is lethal. Breathing in chlorine gas is highly painful.[28] Hydrochloric acid is a dangerous chemical.[4]
Pure bromine is somewhat toxic, but less toxic than fluorine and chlorine. One hundred milligrams of bromine is lethal.[4] Bromide anions are also toxic, but less so than bromine. Bromide has a lethal dose of 30 grams.[4]
Iodine is somewhat toxic, being able to irritate the lungs and eyes, with a safety limit of 1 milligram per cubic meter. When taken orally, 3 grams of iodine can be lethal. Iodide anions are mostly nontoxic, but these can also be deadly if ingested in large amounts.[4]
Astatine is very radioactive and thus highly dangerous, but it has not been produced in macroscopic quantities and hence it is most unlikely that its toxicity will be of much relevance to the average individual.[4]
Superhalogen[edit]
Main article: Superatom
Certain aluminium clusters have superatom properties. These aluminium clusters are generated as anions (Al−
n with n = 1, 2, 3, ... ) in helium gas and reacted with a gas containing iodine. When analyzed by mass spectrometry one main reaction product turns out to be Al
13I−
.[31] These clusters of 13 aluminium atoms with an extra electron added do not appear to react with oxygen when it is introduced in the same gas stream. Assuming each atom liberates its 3 valence electrons, this means 40 electrons are present, which is one of the magic numbers for sodium and implies that these numbers are a reflection of the noble gases.
Calculations show that the additional electron is located in the aluminium cluster at the location directly opposite from the iodine atom. The cluster must therefore have a higher electron affinity for the electron than iodine and therefore the aluminium cluster is called a superhalogen (i.e., the vertical electron detachment energies of the moieties that make up the negative ions are larger than those of any halogen atom).[32] The cluster component in the Al
13I−
ion is similar to an iodide ion or a bromide ion. The related Al
13I−
2 cluster is expected to behave chemically like the triiodide ion.[33][34]
See also[edit]
Look up halogen in Wiktionary, the free dictionary.
Pseudohalogen
Halogen bond
Halogen lamp
Interhalogen
Notes[edit]
Jump up ^ The number given in parentheses refers to the measurement uncertainty. This uncertainty applies to the least significant figure(s) of the number prior to the parenthesized value (i.e., counting from rightmost digit to left). For instance, 7000100794000000000♠1.00794(7) stands for 7000100794000000000♠1.00794±0.00007, while 7000100794000000000♠1.00794(72) stands for 7000100794000000000♠1.00794±0.00072.[20]
Jump up ^ The average atomic weight of this element changes depending on the source of the chlorine, and the values in brackets are the upper and lower bounds.[21]
Jump up ^ The element does not have any stable nuclides, and the value in brackets indicates the mass number of the longest-lived isotope of the element.[21]
References[edit]
Jump up ^ Jones, Daniel (2003) [1917], Peter Roach, James Hartmann and Jane Setter, eds., English Pronouncing Dictionary, Cambridge: Cambridge University Press, ISBN 3-12-539683-2 CS1 maint: Uses editors parameter (link)
Jump up ^ "Halogen". Merriam-Webster Dictionary.
Jump up ^ "Halogen". Dictionary.com Unabridged. Random House.
^ Jump up to: a b c d e f g h i j k l m n o p q r s t u v w x y Emsley, John (2011). Nature's Building Blocks. ISBN 0199605637.
Jump up ^ Online Etymology Dictionary halogen.
Jump up ^ Snelders, H. A. M. (1971). "J. S. C. Schweigger: His Romanticism and His Crystal Electrical Theory of Matter". Isis. 62 (3): 328. JSTOR 229946. doi:10.1086/350763.
Jump up ^ Page 43, Edexcel International GCSE chemistry revision guide, Curtis 2011
Jump up ^ Greenwood & Earnshaw 1998, p. 804.
^ Jump up to: a b c d e Jim Clark (2011). "Assorted reactions of the halogens". Retrieved February 27, 2013
Jump up ^ Jim Clark (2002). "THE ACIDITY OF THE HYDROGEN HALIDES". Retrieved February 24, 2013
Jump up ^ "Facts about hydrogen fluoride". 2005. Archived from the original on 2013-02-01. Retrieved February 2013 Check date values in: |access-date= (help)
Jump up ^ "Hydrogen chloride". Retrieved February 24, 2013
Jump up ^ "Hydrogen bromide". Retrieved February 24, 2013
Jump up ^ "Poison Facts:Low Chemicals: Hydrogen Iodid". Retrieved 2015-04-12.
^ Jump up to: a b Saxena, P. B (2007). Chemistry Of Interhalogen Compounds. ISBN 9788183562430. Retrieved February 27, 2013.
Jump up ^ "The Oxidising Ability of the Group 7 Elements". Chemguide.co.uk. Retrieved 2011-12-29.
Jump up ^ "Solubility of chlorine in water". Resistoflex.com. Retrieved 2011-12-29.
Jump up ^ "Properties of bromine". bromaid.org. Archived from the original on December 8, 2007.
Jump up ^ "Iodine MSDS". Hazard.com. 1998-04-21. Retrieved 2011-12-29.
Jump up ^ "Standard Uncertainty and Relative Standard Uncertainty". CODATA reference. National Institute of Standards and Technology. Retrieved 26 September 2011.
^ Jump up to: a b c Wieser, Michael E.; Coplen, Tyler B. (2011). "Atomic weights of the elements 2009 (IUPAC Technical Report)" (PDF). Pure Appl. Chem. IUPAC. 83 (2): 359–396. doi:10.1351/PAC-REP-10-09-14. Retrieved 5 December 2012.
^ Jump up to: a b Lide, D. R., ed. (2003). CRC Handbook of Chemistry and Physics (84th ed.). Boca Raton, FL: CRC Press.
Jump up ^ Slater, J. C. (1964). "Atomic Radii in Crystals". Journal of Chemical Physics. 41 (10): 3199–3205. Bibcode:1964JChPh..41.3199S. doi:10.1063/1.1725697.
Jump up ^ Bonchev, Danail; Kamenska, Verginia (1981). "Predicting the properties of the 113–120 transactinide elements". The Journal of Physical Chemistry. ACS Publications. 85 (9): 1177–86. doi:10.1021/j150609a021.
Jump up ^ "The Halogen Lamp". Edison Tech Center. Edison Steinmetz Center, Schenectady, New York. Retrieved 2014-09-05.
Jump up ^ Thomas, G. (2000). Medicinal Chemistry an Introduction. John Wiley & Sons, West Sussex, UK. ISBN 978-0-470-02597-0.
Jump up ^ Fawell, J. "Fluoride in Drinking-water" (PDF). World Heath Organisation. Retrieved 10 March 2016.
^ Jump up to: a b Gray, Theodore (2010). The Elements. ISBN 9781579128951.
Jump up ^ Fawell, J.; Bailey, K.; Chilton, J.; Dahi, E.; Fewtrell, L.; Magara, Y. (2006). "Guidelines and standards". Fluoride in Drinking-water (PDF). World Health Organization. pp. 37–9. ISBN 92-4-156319-2.
Jump up ^ "CDC Statement on the 2006 National Research Council (NRC) Report on Fluoride in Drinking Water". Centers for Disease Control and Prevention. July 10, 2013. Retrieved August 1, 2013.
Jump up ^ Bergeron, D. E.; Castleman, A. Welford; Morisato, Tsuguo; Khanna, Shiv N. (2004). "Formation of Al13I−: Evidence for the Superhalogen Character of Al13". Science. 304 (5667): 84. Bibcode:2004Sci...304...84B. PMID 15066775. doi:10.1126/science.1093902.
Jump up ^ Giri, Santanab; Behera, Swayamprabha; Jena, Puru (2014). "Superhalogens as Building Blocks of Halogen-Free Electrolytes in Lithium-Ion Batteries†". Angewandte Chemie. 126 (50): 14136. doi:10.1002/ange.201408648.
Jump up ^ Ball, Philip (16 April 2005). "A New Kind of Alchemy". New Scientist.
Jump up ^ Bergeron, D. E.; Roach, P. J.; Castleman, A. W.; Jones, N. O.; Khanna, S. N. (2005). "Al Cluster Superatoms as Halogens in Polyhalides and as Alkaline Earths in Iodide Salts". Science. 307 (5707): 231. Bibcode:2005Sci...307..231B. PMID 15653497. doi:10.1126/science.1105820.
Further reading[edit]
Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
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Halogens
Fluorine
F
Atomic Number: 9
Atomic Weight: 18.9984032
Melting Point: 53.63 K
Boiling Point: 85.03 K
Specific mass: 0.001696 g/cm3
Electronegativity: 3.98
Chlorine
Cl
Atomic Number: 17
Atomic Weight: 35.453
Melting Point: 172.31 K
Boiling Point: 239.11 K
Specific mass: 0.003214 g/cm3
Electronegativity: 3.16
Bromine
Br
Atomic Number: 35
Atomic Weight: 79.904
Melting Point: 266.05 K
Boiling Point: 332.0 K
Specific mass: 3.122 g/cm3
Electronegativity: 2.96
Iodine
I
Atomic Number: 53
Atomic Weight: 126.90447
Melting Point: 386.65 K
Boiling Point: 475.4 K
Specific mass: 4.93 g/cm3
Electronegativity: 2.66
Astatine
At
Atomic Number: 85
Atomic Weight: [210]
Melting Point: 575.15 K
Boiling Point: 610 K
Specific mass: 7 g/cm3
Electronegativity: 2.2
Tennessine
Ts
Atomic Number: 117
Atomic Weight: [294]
Melting Point: ? 573–773 K
Boiling Point: ? 823 K
Specific mass: ? g/cm3
Electronegativity: ?
Authority control
GND: 4158874-5
NDL: 00562982
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The Most Wonderful Time of the Year (film)
From Wikipedia, the free encyclopedia
Jump to: navigation, search
The Most Wonderful Time of the Year
DVD cover
Written by
Bruce Graham
Directed by
Michael Scott
Starring
Brooke Burns
Henry Winkler
Warren Christie
Theme music composer
Philip Giffin
Country of origin
United States
Original language(s)
English
No. of episodes
1
Production
Producer(s)
Harvey Kahn
Cinematography
Adam Sliwinski
Editor(s)
Jason Pielak
Running time
90 minutes
Distributor
Hallmark Channel
Release
Original network
Hallmark Channel
Original release
December 13, 2008 (2008-12-13)
External links
Website
www.hallmarkchannel.com/the-most-wonderful-time-of-the-year
The Most Wonderful Time of the Year is a 2008 Christmas television film directed by Michael Scott.
Contents
[hide]
1 Plot
2 Cast
3 Home media
4 References
5 External links
Plot[edit]
Ralph is a retired police officer who has worked as a New York cop for over 38 years. He plans on visiting his niece Jennifer in Chicago for the holidays. Jennifer is a successful businesswoman and the single mother of her young son Brian. She grew up all her life mostly at Ralph's, as her mother was constantly traveling and her father died when she was very young. Since then, she has lost her Christmas spirit. At the airport, Ralph has no idea where he has to be and he is helped by co-traveler Morgan Derby, a 30-year-old chef who has trouble accepting his age. When it turns out his second flight to Denver is canceled, Ralph offers Morgan to a place to stay at Jennifer's house.
Although Jennifer is initially reluctant to take in Morgan, Ralph convinces her to allow him to stay since he is a top chef and she needs someone to make her son a turkey. They soon come to the conclusion that they are two completely different people. Jennifer is irritated by his careless and adventurous behavior and Morgan feels that she is a cynical control freak, which is mostly the result of dating the successful but materialistic businessman Richard Windom. Ralph, however, feels that they are perfect for each other and tries to prevent Jennifer from sending Morgan away.
When Jennifer is about to set him off at the airport, it turns out Ralph has stolen his passport. Jennifer and Morgan end up spending the entire day together and bond. With a lot of trouble and some illegal activities, Morgan is able to get Brian the one Christmas gift he wished for: rocketwheel, a very rare bicycle. Later that night, on Christmas Eve, Morgan makes Brian believe in Santa Claus again, by climbing on the roof and pretending to be one of Santa's helpers. Meanwhile, Jenmifer and Richard attend a formal party and get engaged.
Upon hearing the news, Morgan feels disappointed and leaves. Jennifer is mad when she finds out, but softens up when Ralph tells her that Morgan nearly killed himself on the roof, trying to make Brian believe in Christmas again. Finally convinced by Ralph and Morgan's opinion on Richard and realizing she is in love with Morgan, she breaks off the engagement. She rushes to the airport, trying to stop Morgan from leaving. In the end, although there is no proposal or wedding scene, it is assumed they become a couple.
Cast[edit]
Brooke Burns as Jennifer 'Jen' Cullen
Henry Winkler as Uncle Ralph
Warren Christie as Morgan Derby
Connor Levins as Brian Cullen
Woody Jeffreys as Richard Windom
Serge Houde as Stephen Windom
Rebecca Toolan as Winnie Windom
Michael Roberds as Chet Wojorski
Rukiya Bernard as Denise
Home media[edit]
The film was released on DVD on October 13, 2009.[1]
References[edit]
Jump up ^ "Spin-ematical: New on DVD for 10/13". Cinematical. October 13, 2009. Retrieved 2009-12-25.
External links[edit]
Official website
The Most Wonderful Time of the Year on IMDb
The Most Wonderful Time of the Year at AllMovie
The Most Wonderful Time of the Year at the TCM Movie Database
Retrieved from "https://en.wikipedia.org/w/index.php?title=The_Most_Wonderful_Time_of_the_Year_(film)&oldid=810060086"
Categories:
2008 television films
American television films
American Christmas films
Christmas television films
Hallmark Channel original films
American films
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Josef Strauss
From Wikipedia, the free encyclopedia
Jump to: navigation, search
For other people with the same name, see Joseph Strauss (disambiguation).
Josef Strauss
Josef Strauss (20 August 1827 – 22 July 1870) was an Austrian composer.
He was born in Mariahilf (now Vienna), the son of Johann Strauss I and Maria Anna Streim, and brother of Johann Strauss II and Eduard Strauss. His father wanted him to choose a career in the Austrian Habsburg military. He studied music with Franz Dolleschal and learned to play the violin with Franz Anton Ries.
He received training as an engineer, and worked for the city of Vienna as an engineer and designer. He designed a horse-drawn revolving brush street-sweeping vehicle and published two textbooks on mathematical subjects.[1] Strauss had talents as an artist, painter, poet, dramatist, singer, composer and inventor.[2]
Contents
[hide]
1 Family orchestra
2 Family life
3 Music
4 Death
5 Works of Josef Strauss
6 See also
7 References
8 External links
Family orchestra[edit]
He joined the family orchestra, along with his brothers, Johann Strauss II and Eduard Strauss[3] in the 1850s. His first published work was called "Die Ersten und Letzten" (The First and the Last). When Johann became seriously ill in 1853 Josef led the orchestra for a while. The waltz-loving Viennese were appreciative of his early compositions so he decided to continue in the family tradition of composing dance music. He was known as 'Pepi' by his family and close friends, and Johann once said of him: "Pepi is the more gifted of us two; I am merely the more popular..."[1]
Family life[edit]
Josef Strauss married Caroline Pruckmayer at the church of St. Johann Nepomuk in Vienna on 8 June 1857, and had one daughter, Karolina Anna, who was born on March 27, 1858.
Music[edit]
Josef Strauss wrote 283 opus numbers. He wrote many waltzes, including: Sphären-Klänge (Music of the Spheres), Delirien (Deliriums), Transaktionen (Transactions), Mein Lebenslauf ist Lieb' und Lust (My Character is Love and Joy), and Dorfschwalben aus Österreich (Village Swallows from Austria), polkas, most famously the Pizzicato Polka (It) with his brother Johann, quadrilles, and other dance music. The waltz The Mysterious Powers of Magnetism (Dynamiden) with the use of minor keys showed a quality that distinguished his waltzes from those of his more popular elder brother.[4] The polka-mazurka shows influence by Strauss, where he wrote many examples like Die Emancipierte and Die Libelle.
Death[edit]
Josef Strauss was sickly most of his life. He suffered fainting spells and intense headaches.[5] During a tour in 1870, he fell unconscious from the conductor's podium in Warsaw, while conducting his 'Musical Potpourri', and hit his head. His wife brought him back home to Vienna, to the Hirschenhaus, where he died on 22 July 1870. A final diagnosis only reported a decomposition of blood. There were rumors that he was beaten by drunken Russian soldiers after he allegedly refused to perform music for them one night. His cause of death was not determined, as his widow forbade an autopsy.[citation needed] Originally buried in the St. Marx Cemetery, Strauss was later exhumed and reburied in the Vienna Central Cemetery, alongside his mother Anna.[citation needed]
His dance pieces might have surpassed those of his older brother, had he survived, as Johann was by then concentrating on writing music for operettas and other stage works.[citation needed]
Works of Josef Strauss[edit]
The works of Josef Strauss include:[6]
Die Ersten und Letzten ('The First and the Last') waltz op. 1 (1853)
Die Ersten nach den Letzten ('The First after the Last') waltz op. 12 (1854)
Die Guten, Alten Zeiten ('The Good Old Times') waltz op. 26 (1856)
Mai-Rosen ('May-Rose') waltz op. 34 (1857)
Perlen der Liebe ('Pearls of Love') concert-waltz op. 39 (1857)
Moulinet-Polka ('Little Mill Pond') polka francaise op. 57 (1858)
Sympathie ('Sympathy') polka-mazurka op. 73 (1859)
Lustschwärmer ('Joy Seeker') waltz op. 91 (1860)
Schabernack ('Shenanigans'), fast polka op. 98
Wiener Bonmots ('Viennese Bon-mots') waltz op. 108 (1861)
Winterlust ('Winter Joy') polka op. 121 (1862)
Brennende Liebe polka-mazurka op. 129 (1862)
Auf Ferienreisen! ('On a Holiday!') polka op. 133 (1863)
Die Schwätzerin ('The Gossip') polka-mazurka op. 144 (1863)
Wiener Couplets ('Viennese Couplets') waltz op. 150 (1863)
Dorfschwalben aus Österreich ('Village Swallows from Austria') waltz op. 164 (1864)
Frauenherz ('A Woman's Heart') polka-mazurka op. 166 (1864)
Sport-Polka op. 170 (1864)
Dynamiden (Geheimne Anziehungskräfte) ('Mysterious Powers of Magnetism') waltz op. 173 (1865)
Stiefmütterchen ('Pansies') polka-mazurka op. 183 (1865)
Transaktionen ('Transactions') waltz op. 184 (1865)
Carrière, fast polka, op. 200
Die Marketenderin ('The Camp Follower') polka op. 202 (1866)
Die Libelle ('The Dragonfly') polka-mazurka op. 204 (1866)
Delirien (ja) ('Deliriums') waltz op. 212 (1867)
Herbstrosen ('Autumn Rose') waltz op. 232 (1867)
Sphärenklänge (ja) ('Music of the Spheres') waltz op. 235 (1868)
Eingesendet ('Letters to the Editor') polka op. 240 (1868)
Plappermäulchen ('Chatterboxes') polka op. 245 (1868)
Aquarellen (waltz) (ja) ('Watercolours') waltz op. 258 (1869)
Eislauf ('Ice-Skating') polka op. 261 (1869)
Neckerei ('Teasing') polka mazur op. 262
Mein Lebenslauf Ist Lieb` Und Lust! (ja) ('My Character is Love and Joy') waltz op. 263 (1869)
Die Tanzende Muse ('The Dancing Muse') polka-mazurka op. 266 (1869)
Feuerfest! ('Fireproof!') polka francaise op. 269 (1869).
Aus der Ferne Polka Mazur op. 270 (1869)
Ohne Sorgen! ('Without a Care!') polka op. 271 (1869)
Nilfluthen ('Nile's Waters') waltz op. 275 (1870)
Frauenwürde waltz op. 277 (1870)
Jokey-Polka ('Jockey') op. 278 (1870)
Hesperusbahnen ('Hesperus’ Path') waltz op. 279 (1870)
Die Emancipierte ('The Emancipated Woman') polka-mazurka op. 282 (1870)
See also[edit]
The Strauss Family – TV Drama
Strauss Museum Vienna
References[edit]
^ Jump up to: a b "Johann Strauss Society: Josef Strauss". Johann Strauss Society of Great Britain. Retrieved 2008-10-01.
Jump up ^ Talents -Retrieved 2011-02-19
Jump up ^ Josef Strauss
Jump up ^ Program Notes
Jump up ^ Strauss
Jump up ^ Josef Strauss works Archived 2011-07-08 at the Wayback Machine.
External links[edit]
Media related to Josef Strauss at Wikimedia Commons
Josef Strauss on the Johann Strauss Society of Great Britain
Complete list of Josef Strauss's compositions
Free scores by Josef Strauss at the International Music Score Library Project (IMSLP)
Josef Strauss at Find a Grave
[hide]
v
t
e
Johann Strauss II
Operettas
Indigo und die vierzig Räuber (1871)
Der Karneval in Rom (1873)
Die Fledermaus (1874)
Cagliostro in Wien (1875)
Prinz Methusalem (1877)
Blindekuh (1878)
Das Spitzentuch der Königin (1880)
Der lustige Krieg (1881)
Eine Nacht in Venedig (1883)
Der Zigeunerbaron (1885)
Simplicius (1887)
Waldmeister (1895)
Wiener Blut (arr. by Adolf Müller, 1899)
Waltzes
Sinngedichte, Op. 1 (1844)
Gunstwerber, Op. 4 (1844)
Sträußchen, Op. 15 (1846)
Klange aus der Walachei, Op. 50 (1850)
Frohsinns-Spenden, Op. 73 (1850)
Lava-Ströme, Op. 74 (1850)
Rhadamantus-Klänge, Op. 94 (1851)
Idyllen, Op. 95 (1851)
Mephistos Höllenrufe, Op. 101 (1851)
Liebeslieder, Op. 114 (1852)
Phönix-Schwingen, Op. 125 (1853)
Novellen, Op. 146 (1854)
Nachtfalter, Op. 157 (1855)
Glossen, Op. 163 (1855)
Man lebt nur einmal!, Op. 167 (1855)
Abschieds-Rufe, Op. 179 (1856)
Phänomene, Op. 193 (1857)
Abschied von St. Petersburg, Op. 210 (1858)
Hell und voll, Op. 216 (1859)
Promotionen, Op. 221 (1859)
Accelerationen, Op. 234 (1860)
Immer heiterer, Op. 235 (1860)
Grillenbanner, Op. 247 (1861)
Klangfiguren, Op. 251, (1861)
Dividenden, Op. 252
Karnevalsbotschafter, Op. 270 (1862)
Leitartikel, Op. 273 (1863)
Morgenblätter, Op. 279 (1863)
Studentenlust, Op. 285 (1864)
Aus den Bergen, Op. 292 (1864)
Bürgersinn, Op. 295 (1865)
Flugschriften, Op. 300 (1865)
Wiener Bonbons, Op. 307 (1866)
An der schönen blauen Donau, Op. 314 (1867)
Künstlerleben, Op. 316 (1867)
Die Publicisten, Op. 321 (1868)
G'schichten aus dem Wienerwald, Op. 325 (1868)
Illustrationen, Op. 331 (1869)
Wein, Weib und Gesang, Op. 333 (1869)
Freuet Euch des Lebens, Op. 340 (1870)
Neu Wien, Op. 342 (1870)
Tausend und eine Nacht, Op. 346 (1871)
Wiener Blut (waltz), Op. 354 (1873)
Carnevalsbilder, Op. 357 (1873)
Bei uns Z'haus, Op. 361 (1873)
Wo die Zitronen blühen, Op. 364 (1874)
Du und du, Op. 367 (1874)
Cagliostro-Walzer, Op. 370 (1875)
O schöner Mai!, Op. 375 (1877)
Rosen aus dem Süden, Op. 388 (1880)
Nordseebilder, Op. 390 (1880)
Kuss-Walzer, Op. 400 (1881)
Frühlingsstimmen, Op. 410 (1883)
Lagunen-Walzer, Op. 411 (1883)
Schatz-Walzer, Op. 418 (1885)
Wiener Frauen, Op. 423 (1886)
Donauweibchen, Op. 427 (1887)
Kaiser-Jubiläum-Jubelwalzer, Op. 434 (1888)
Kaiser-Walzer, Op. 437 (1888)
Rathausball-Tänze, Op. 438 (1890)
Gross-Wien, Op. 440 (1891)
Seid umschlungen, Millionen!, Op. 443 (1892)
Trau, schau, wem!, Op. 463 (1895)
Farewell to America
Polkas
Herzenslust, Op. 3
Explosions-Polka, Op. 43
Tritsch-Tratsch-Polka, Op. 214 (1858)
Demolirer, Op. 269 (1862)
Vergnügungszug, Op. 281 (1864)
'S gibt nur a Kaiserstadt, 's gibt nur a Wien!, Op. 291
Lob der Frauen, Op. 315
Postillon d'amour, Op. 317 (1867)
Leichtes Blut, Op. 319 (1867)
Figaro-Polka, Op. 320 (1867)
Ein Herz, ein Sinn!, Op. 323
Freikugeln, Op. 326 (1868)
Éljen a Magyar!, Op. 332
Im Krapfenwald'l, Op. 336 (1869)
Die Bajadere, Op. 351
Vom Donaustrande, Op. 358
Bitte schön!, Op. 372 (1875)
Auf der Jagd, Op. 373 (1875)
Banditen-Galopp, Op. 378 (1877)
Waldine, Op. 385 (1879)
Neue Pizzicato Polka, Op. 449
Marches
Persischer Marsch, Op. 289 (1864)
Indigo-Marsch, Op. 349
Quadrille
Debut-Quadrille, Op. 2 (1844)
Le beau Monde, Op. 199 (1857)
Other
Ritter Pázmán (Opera 1892)
Aschenbrödel (Ballet 1899)
Compositions
Operettas
Family
Henrietta Treffz (wife)
Johann Strauss I (father)
Eduard Strauss (brother)
Josef Strauss (brother)
Johann Strauss III (nephew)
Eduard Strauss II (grandnephew)
In media
Waltzes from Vienna (1933)
The Great Waltz (1938)
The Strauss Family (1972)
The Great Waltz (1972)
Authority control
WorldCat Identities
VIAF: 100251784
LCCN: n79077314
ISNI: 0000 0001 2031 4611
GND: 118809555
SELIBR: 206354
SUDOC: 067019277
BNF: cb139001232 (data)
MusicBrainz: 9942ef92-91a2-46f7-aff4-32389df33c9e
NDL: 00457910
BNE: XX840806
CiNii: DA05432818
Retrieved from "https://en.wikipedia.org/w/index.php?title=Josef_Strauss&oldid=806091404"
Categories:
Strauss family
1827 births
1870 deaths
19th-century Austrian people
19th-century classical composers
Austrian classical composers
Austrian male classical composers
Austrian people of Jewish descent
Austrian Romantic composers
Burials at the Vienna Central Cemetery
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Viennese composers
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