Slightly Foxed is a British quarterly literary magazine. Its primary focus is books and book culture. It was established by former John Murray editors Hazel Wood and Gail Pirkis. Notable authors to have written for the magazine include Penelope Lively , Richard Mabey , Diana Athill , Ronald Blythe and Robert Macfarlane .
39-431: Instead of books currently marketed by big publishers, Slightly Foxed tends to examine older and more obscure titles. Its title comes from the term "slightly foxed" as a description of a book's physical quality, commonly used in the second-hand book trade to describe minor foxing , the occurrence of brown spots on older paper. As well as the magazine itself, Slightly Foxed has a books imprint. Original books published by
78-507: A Δ H of –2884.5 kJ / kg and a Δ S of 70.5 J/(mol·K): The rate of decomposition increases with rise in temperature, concentration, and pH . H 2 O 2 is unstable under alkaline conditions. Decomposition is catalysed by various redox-active ions or compounds, including most transition metals and their compounds (e.g. manganese dioxide ( MnO 2 ), silver , and platinum ). The redox properties of hydrogen peroxide depend on pH. In acidic solutions, H 2 O 2
117-510: A variant form of the English West country dialect term foust and Scots foze , to become moldy. Alternatively, it may derive from the fox -like reddish-brown color of the stains. Paper so affected is said to be "foxed". Foxing is seldom found in incunabula , or books printed before 1501. Decrease in rag fibre quality may be a culprit; as demand for paper rose in later centuries, papermakers used less water and spent less time cleansing
156-400: Is a reactive oxygen species and the simplest peroxide , a compound having an oxygen–oxygen single bond . It decomposes slowly into water and elemental oxygen when exposed to light, and rapidly in the presence of organic or reactive compounds. It is typically stored with a stabilizer in a weakly acidic solution in an opaque bottle. Hydrogen peroxide is found in biological systems including
195-399: Is a powerful oxidizer . Sulfite ( SO 2− 3 ) is oxidized to sulfate ( SO 2− 4 ). Under alkaline conditions, hydrogen peroxide is a reductant. When H 2 O 2 acts as a reducing agent, oxygen gas is also produced. For example, hydrogen peroxide will reduce sodium hypochlorite and potassium permanganate , which is a convenient method for preparing oxygen in
234-470: Is a useful "carrier" for H 2 O 2 in some reactions. Hydrogen peroxide ( H 2 O 2 ) is a nonplanar molecule with (twisted) C 2 symmetry ; this was first shown by Paul-Antoine Giguère in 1950 using infrared spectroscopy . Although the O−O bond is a single bond , the molecule has a relatively high rotational barrier of 386 cm (4.62 kJ / mol ) for rotation between enantiomers via
273-454: Is a very pale blue liquid that is slightly more viscous than water . It is used as an oxidizer , bleaching agent, and antiseptic , usually as a dilute solution (3%–6% by weight) in water for consumer use and in higher concentrations for industrial use. Concentrated hydrogen peroxide, or " high-test peroxide ", decomposes explosively when heated and has been used as both a monopropellant and an oxidizer in rocketry . Hydrogen peroxide
312-510: Is a weak acid, forming hydroperoxide or peroxide salts with many metals. It also converts metal oxides into the corresponding peroxides. For example, upon treatment with hydrogen peroxide, chromic acid ( CrO 3 and H 2 SO 4 ) forms a blue peroxide CrO(O 2 ) 2 . The aerobic oxidation of glucose in the presence of the enzyme glucose oxidase produces hydrogen peroxide. The conversion affords gluconolactone : Superoxide dismutases (SOD)s are enzymes that promote
351-456: Is also fairly high, being comparable to that of hydrazine and water, with only hydroxylamine crystallising significantly more readily, indicative of particularly strong hydrogen bonding. Diphosphane and hydrogen disulfide exhibit only weak hydrogen bonding and have little chemical similarity to hydrogen peroxide. Structurally, the analogues all adopt similar skewed structures, due to repulsion between adjacent lone pairs . Hydrogen peroxide
390-444: Is attributed to the effects of hydrogen bonding , which is absent in the gaseous state. Crystals of H 2 O 2 are tetragonal with the space group D 4 or P 4 1 2 1 2. In aqueous solutions , hydrogen peroxide forms a eutectic mixture, exhibiting freezing-point depression down as low as –56 °C; pure water has a freezing point of 0 °C and pure hydrogen peroxide of –0.43 °C. The boiling point of
429-455: Is caused by the effect on certain papers of the oxidation of iron , copper , or other substances in the pulp or rag from which the paper was made. It is possible that multiple factors are involved. High humidity may contribute to foxing. Foxed documents can be repaired, with greater or lesser success, using sodium borohydride , proprietary bleaches , dilute hydrogen peroxide or lasers . Each method risks side effects or damage to
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#1732890736448468-543: Is less than 0.014 μg/m , and in moderate photochemical smog it is 14 to 42 μg/m . The amount of hydrogen peroxide in biological systems can be assayed using a fluorometric assay . Alexander von Humboldt is sometimes said to have been the first to report the first synthetic peroxide, barium peroxide , in 1799 as a by-product of his attempts to decompose air, although this is disputed due to von Humboldt's ambiguous wording. Nineteen years later Louis Jacques Thénard recognized that this compound could be used for
507-475: Is oxidation of thioethers to form sulfoxides , such as conversion of thioanisole to methyl phenyl sulfoxide : Alkaline hydrogen peroxide is used for epoxidation of electron-deficient alkenes such as acrylic acid derivatives, and for the oxidation of alkylboranes to alcohols , the second step of hydroboration-oxidation . It is also the principal reagent in the Dakin oxidation process. Hydrogen peroxide
546-527: Is produced by various biological processes mediated by enzymes . Hydrogen peroxide has been detected in surface water, in groundwater, and in the atmosphere . It can also form when water is exposed to UV light. Sea water contains 0.5 to 14 μg/L of hydrogen peroxide, and freshwater contains 1 to 30 μg/L. Concentrations in air are about 0.4 to 4 μg/m , varying over several orders of magnitude depending in conditions such as season, altitude, daylight and water vapor content. In rural nighttime air it
585-559: Is still used, was developed during the 1930s by the German chemical manufacturer IG Farben in Ludwigshafen . The increased demand and improvements in the synthesis methods resulted in the rise of the annual production of hydrogen peroxide from 35,000 tonnes in 1950, to over 100,000 tonnes in 1960, to 300,000 tonnes by 1970; by 1998 it reached 2.7 million tonnes. Early attempts failed to produce neat hydrogen peroxide. Anhydrous hydrogen peroxide
624-414: The trans configuration, and 2460 cm (29.4 kJ/mol) via the cis configuration. These barriers are proposed to be due to repulsion between the lone pairs of the adjacent oxygen atoms and dipolar effects between the two O–H bonds. For comparison, the rotational barrier for ethane is 1040 cm (12.4 kJ/mol). The approximately 100° dihedral angle between the two O–H bonds makes
663-436: The disproportionation of superoxide into oxygen and hydrogen peroxide. Peroxisomes are organelles found in virtually all eukaryotic cells. They are involved in the catabolism of very long chain fatty acids , branched chain fatty acids , D -amino acids , polyamines , and biosynthesis of plasmalogens and ether phospholipids , which are found in mammalian brains and lungs. They produce hydrogen peroxide in
702-413: The lignin by sunlight and absorbed atmospheric pollution , typically causing the paper to become brown and crumble at the edges, and acid -related damage to cheap paper such as newsprint , which manufacturers make without neutralizing acidic contaminants . The causes of foxing are not well understood. One conjecture is that foxing is caused by a fungal growth on the paper. Another is that foxing
741-507: The 1820s, but early attempts of industrial production of peroxides failed. The first plant producing hydrogen peroxide was built in 1873 in Berlin . The discovery of the synthesis of hydrogen peroxide by electrolysis with sulfuric acid introduced the more efficient electrochemical method. It was first commercialized in 1908 in Weißenstein , Carinthia , Austria. The anthraquinone process , which
780-518: The Slightly Foxed Best First Biography Prize for the best first biography or literary memoir published each year. In 2023, the prize was won jointly by Katherine Rundell for her biography of John Donne , Super-Infinite , and Osman Yousefzada for his memoir The Go-Between. Winners from previous years include Edmund Gordon for The Invention of Angela Carter and Alan Cumming for Not My Father’s Son. In addition to
819-427: The anthraquinone. Most commercial processes achieve oxidation by bubbling compressed air through a solution of the anthrahydroquinone, with the hydrogen peroxide then extracted from the solution and the anthraquinone recycled back for successive cycles of hydrogenation and oxidation. The net reaction for the anthraquinone-catalyzed process is: The economics of the process depend heavily on effective recycling of
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#1732890736448858-443: The concentration increases above 68%) these grades are potentially far more hazardous and require special care in dedicated storage areas. Buyers must typically allow inspection by commercial manufacturers. Hydrogen peroxide has several structural analogues with H m X−XH n bonding arrangements (water also shown for comparison). It has the highest (theoretical) boiling point of this series (X = O, S, N, P). Its melting point
897-497: The extraction solvents, the hydrogenation catalyst and the expensive quinone . Hydrogen peroxide was once prepared industrially by hydrolysis of ammonium persulfate : [NH 4 ] 2 S 2 O 8 was itself obtained by the electrolysis of a solution of ammonium bisulfate ( [NH 4 ]HSO 4 ) in sulfuric acid . Small amounts are formed by electrolysis, photochemistry , electric arc , and related methods. A commercially viable route for hydrogen peroxide via
936-647: The human body. Enzymes that use or decompose hydrogen peroxide are classified as peroxidases . The boiling point of H 2 O 2 has been extrapolated as being 150.2 °C (302.4 °F), approximately 50 °C (90 °F) higher than water. In practice, hydrogen peroxide will undergo potentially explosive thermal decomposition if heated to this temperature. It may be safely distilled at lower temperatures under reduced pressure. Hydrogen peroxide forms stable adducts with urea ( hydrogen peroxide–urea ), sodium carbonate ( sodium percarbonate ) and other compounds. An acid-base adduct with triphenylphosphine oxide
975-500: The imprint include Philip Evans' Country Doctor's Common Place Book and Charles Phillipson’s Letters to Michael (selected by the Telegraph as one of the best books of 2021) . The imprint has also reissued a number of classic works and children's books, including Rosemary Sutcliff 's novels about Roman Britain and the Carey novels of Ronald Welch . Since 2014, the magazine has sponsored
1014-445: The laboratory: The oxygen produced from hydrogen peroxide and sodium hypochlorite is in the singlet state . Hydrogen peroxide also reduces silver oxide to silver : Although usually a reductant, alkaline hydrogen peroxide converts Mn(II) to the dioxide: In a related reaction, potassium permanganate is reduced to Mn by acidic H 2 O 2 : Hydrogen peroxide is frequently used as an oxidizing agent . Illustrative
1053-520: The middle of the 20th century at least half a dozen hypothetical isomeric variants of two main options seemed to be consistent with the available evidence. In 1934, the English mathematical physicist William Penney and the Scottish physicist Gordon Sutherland proposed a molecular structure for hydrogen peroxide that was very similar to the presently accepted one. In 1994, world production of H 2 O 2
1092-440: The molecule chiral . It is the smallest and simplest molecule to exhibit enantiomerism . It has been proposed that the enantiospecific interactions of one rather than the other may have led to amplification of one enantiomeric form of ribonucleic acids and therefore an origin of homochirality in an RNA world . The molecular structures of gaseous and crystalline H 2 O 2 are significantly different. This difference
1131-403: The paper or ink . Another method is to scan the image and process that image using a high-level image processing program. This can usually remove the effects of foxing while leaving text and images intact. It is generally not advisable to repair study specimens, except perhaps for mechanical damage. Type specimens should – if at all possible – not be altered in any way. If foxing affects
1170-522: The preparation of a previously unknown compound, which he described as eau oxygénée ("oxygenated water") — subsequently known as hydrogen peroxide. An improved version of Thénard's process used hydrochloric acid , followed by addition of sulfuric acid to precipitate the barium sulfate byproduct. This process was used from the end of the 19th century until the middle of the 20th century. The bleaching effect of peroxides and their salts on natural dyes had been known since Thénard's experiments in
1209-487: The quarterly magazine, Slightly Foxed produces a podcast about books, book culture and writers. Between 2009 and 2016 Slightly Foxed ran a bookshop of the same name on London's Gloucester Road . The magazine's offices are based at Hoxton Square , London, N1. Foxing Foxing is an age-related process of deterioration that causes spots and browning on old paper documents such as books , postage stamps , old paper money and certificates . The name may be
Slightly Foxed - Misplaced Pages Continue
1248-572: The rag fibres used to make paper. An early work of art to have been affected by foxing is the Portrait of a Man in Red Chalk , a drawing on paper by Leonardo da Vinci . Foxing also occurs in biological study skins or specimens , as an effect of chemical reactions or mold on melanin . Textiles, such as articles of clothing, so affected may also be said to be foxed. Aside from foxing, other types of age-related paper deterioration include destruction of
1287-447: The reaction of hydrogen with oxygen favours production of water but can be stopped at the peroxide stage. One economic obstacle has been that direct processes give a dilute solution uneconomic for transportation. None of these has yet reached a point where it can be used for industrial-scale synthesis. Hydrogen peroxide is about 1000 times stronger as an acid than water. Hydrogen peroxide disproportionates to form water and oxygen with
1326-401: The reduction of an anthraquinone (such as 2-ethylanthraquinone or the 2-amyl derivative) to the corresponding anthrahydroquinone, typically by hydrogenation on a palladium catalyst . In the presence of oxygen , the anthrahydroquinone then undergoes autoxidation : the labile hydrogen atoms of the hydroxy groups transfer to the oxygen molecule, to give hydrogen peroxide and regenerating
1365-467: The same mixtures is also depressed in relation with the mean of both boiling points (125.1 °C). It occurs at 114 °C. This boiling point is 14 °C greater than that of pure water and 36.2 °C less than that of pure hydrogen peroxide. Hydrogen peroxide is most commonly available as a solution in water. For consumers, it is usually available from pharmacies at 3 and 6 wt% concentrations. The concentrations are sometimes described in terms of
1404-415: The study value of a specimen (e.g. in bird or mammal skins or in insects , where it may affect diagnostic coloration), this might rather be remarked on the specimen label. Color standards can provide a means of documenting coloration before or in the early stages of foxing. Hydrogen peroxide Hydrogen peroxide is a chemical compound with the formula H 2 O 2 . In its pure form, it
1443-420: The volume of oxygen gas generated; one milliliter of a 20-volume solution generates twenty milliliters of oxygen gas when completely decomposed. For laboratory use, 30 wt% solutions are most common. Commercial grades from 70% to 98% are also available, but due to the potential of solutions of more than 68% hydrogen peroxide to be converted entirely to steam and oxygen (with the temperature of the steam increasing as
1482-409: Was around 1.9 million tonnes and grew to 2.2 million in 2006, most of which was at a concentration of 70% or less. In that year, bulk 30% H 2 O 2 sold for around 0.54 USD / kg , equivalent to US$ 1.50/kg (US$ 0.68/ lb ) on a "100% basis". Today, hydrogen peroxide is manufactured almost exclusively by the anthraquinone process , which was originally developed by BASF in 1939. It begins with
1521-468: Was first obtained by vacuum distillation . Determination of the molecular structure of hydrogen peroxide proved to be very difficult. In 1892, the Italian physical chemist Giacomo Carrara (1864–1925) determined its molecular mass by freezing-point depression , which confirmed that its molecular formula is H 2 O 2 . H 2 O=O seemed to be just as possible as the modern structure, and as late as in
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