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Pnictogen

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Template:Periodic table (pnictogens) A pnictogen[1] (/ˈpnɪktədʒən/ or /ˈnɪktədʒən/; from Ancient Greek: πνῑ́γω "to choke" and -gen, "generator") is any of the chemical elements in group 15 of the periodic table. Group (V) is also known as the nitrogen group or nitrogen family. Group (V) consists of the elements nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), bismuth (Bi), and moscovium (Mc).

Since 1988, IUPAC calls it Group (V). Before that, in America it was called Group VA, owing to a text by H. C. Deming and the Sargent-Welch Scientific Company, while in Europe it was called Group VB and IUPAC recommended that in 1970.[2] (Pronounced "group five A" and "group five B"; "V" is the Roman numeral 5). In semiconductor physics, it is still usually called Group V.[3] The "five" ("V") in the historical names comes from the "pentavalency" of nitrogen, reflected by the stoichiometry of compounds such as N2O5. They have also been called the pentels.

Characteristics

Chemical

Like other groups, the members of this family show similar patterns in electron configuration, especially in the outermost shells, resulting in trends in chemical behavior.

Z Element Electrons per shell
7 nitrogen 2, 5
15 phosphorus 2, 8, 5
33 arsenic 2, 8, 18, 5
51 antimony 2, 8, 18, 18, 5
83 bismuth 2, 8, 18, 32, 18, 5
115 moscovium 2, 8, 18, 32, 32, 18, 5
(predicted)

This group has the defining characteristic that all the component elements have 5 electrons in their outermost shell, that is 2 electrons in the s subshell and 3 unpaired[relevant?] electrons in the p subshell. They are therefore 3 electrons short of filling their outermost electron shell in their non-ionized state. The Russell–Saunders term symbol of the ground state in all elements in the group is 4S3⁄2.

The most important elements of this group to life on Earth are nitrogen (N), which in its diatomic form is the principal component of air, and phosphorus (P), which, like nitrogen, is essential to all known forms of life.

Compounds

Binary compounds of the group can be referred to collectively as pnictides. Pnictide compounds tend to have exotic properties such as being diamagnetic and paramagnetic at room temperature, being transparent, or generating electricity when heated. Other pnictides include the ternary rare-earth (RE) main-group variety of pnictides. These are in the form of REaMbPnc, where M is a carbon group or boron group element and Pn is any pnictogen except nitrogen. These compounds are between ionic and covalent compounds and thus have unusual bonding properties.[4]

These elements are also noted for their stability in compounds due to their tendency to form covalent double bonds and triple bonds. This property of these elements leads to their potential toxicity, most evident in phosphorus, arsenic, and antimony. When these substances react with various chemicals of the body, they create strong free radicals that are not easily processed by the liver, where they accumulate. Paradoxically, this same strong bonding causes nitrogen's and bismuth's reduced toxicity (when in molecules), because these strong bonds with other atoms are difficult to split, creating very unreactive molecules. For example, N2, the diatomic form of nitrogen, is used as an inert gas in situations where using argon or another noble gas would be too expensive.

Formation of multiple bonds is facilitated by their five valence electrons whereas the octet rule permits a pnictogen for accepting three electrons on covalent bonding. Because 5 > 3, it leaves unused two electrons in a lone pair unless there is a positive charge around (like in NH+4). When a pnictogen forms only three single bonds, effects of the lone pair typically result in trigonal pyramidal molecular geometry.

Oxidation states

The light pnictogens (nitrogen, phosphorus, and arsenic) tend to form −3 charges when reduced, completing their octet. When oxidized or ionized, pnictogens typically take an oxidation state of +3 (by losing all three p-shell electrons in the valence shell) or +5 (by losing all three p-shell and both s-shell electrons in the valence shell). However heavier pnictogens are more likely to form the +3 oxidation state than lighter ones due to the s-shell electrons becoming more stabilized.[5]

−3 oxidation state
See also: nitride, phosphide, arsenide, antimonide, and bismuthide

Pnictogens can react with hydrogen to form pnictogen hydrides such as ammonia. Going down the group, to phosphane (phosphine), arsane (arsine), stibane (stibine), and finally bismuthane (bismuthine), each pnictogen hydride becomes progressively less stable (more unstable), more toxic, and has a smaller hydrogen-hydrogen angle (from 107.8° in ammonia[6] to 90.48° in bismuthane).[7] (Also, technically, only ammonia and phosphane have the pnictogen in the −3 oxidation state because, for the rest, the pnictogen is less electronegative than hydrogen.)

Crystal solids featuring pnictogens fully reduced include yttrium nitride, calcium phosphide, sodium arsenide, indium antimonide, and even double salts like aluminum gallium indium phosphide. These include III-V semiconductors, including gallium arsenide, the second-most widely-used semiconductor after silicon.

+3 oxidation state
See also: nitrite, phosphite, arsenite, antimonite, and bismuthite

Nitrogen forms a limited number of stable III compounds. Nitrogen(III) oxide can only be isolated at low temperatures, and nitrous acid is unstable. Nitrogen trifluoride is the only stable nitrogen trihalide, with nitrogen trichloride, nitrogen tribromide, and nitrogen triiodide being explosive—nitrogen triiodide being so shock-sensitive that the touch of a feather detonates it (the last three actually feature nitrogen in the -3 oxidation state). Phosphorus forms a +III oxide which is stable at room temperature, phosphorous acid, and several trihalides, although the triiodide is unstable. Arsenic forms +III compounds with oxygen as arsenites, arsenous acid, and arsenic(III) oxide, and it forms all four trihalides. Antimony forms antimony(III) oxide and antimonite but not oxyacids. Its trihalides, antimony trifluoride, antimony trichloride, antimony tribromide, and antimony triiodide, like all pnictogen trihalides, each have trigonal pyramidal molecular geometry.

The +3 oxidation state is bismuth's most common oxidation state because its ability to form the +5 oxidation state is hindered by relativistic properties on heavier elements, effects that are even more pronounced concerning moscovium. Bismuth(III) forms an oxide, an oxychloride, an oxynitrate, and a sulfide. Moscovium(III) is predicted to behave similarly to bismuth(III). Moscovium is predicted to form all four trihalides, of which all but the trifluoride are predicted to be soluble in water. It is also predicted to form an oxychloride and oxybromide in the +III oxidation state.

+5 oxidation state
See also: nitrate, phosphate, arsenate, antimonate, and bismuthate

For nitrogen, the +5 state is typically serves as only a formal explanation of molecules like N2O5, as the high electronegativity of nitrogen causes the electrons to be shared almost evenly.[clarification needed] Pnictogen compounds with coordination number 5 are hypervalent. Nitrogen(V) fluoride is only theoretical and has not been synthesized. The "true" +5 state is more common for the essentially non-relativistic typical pnictogens phosphorus, arsenic, and antimony, as shown in their oxides, phosphorus(V) oxide, arsenic(V) oxide, and antimony(V) oxide, and their fluorides, phosphorus(V) fluoride, arsenic(V) fluoride, antimony(V) fluoride. At least two also form related fluoride-anions, hexafluorophosphate and hexafluoroantimonate, that function as non-coordinating anions. Phosphorus even forms mixed oxide-halides, known as oxyhalides, like phosphorus oxychloride, and mixed pentahalides, like phosphorus trifluorodichloride. Pentamethylpnictogen(V) compounds exist for arsenic, antimony, and bismuth. However, for bismuth, the +5 oxidation state becomes rare due to the relativistic stabilization of the 6s orbitals known as the inert-pair effect, so that the 6s electrons are reluctant to bond chemically. This causes bismuth(V) oxide to be unstable[8] and bismuth(V) fluoride to be more reactive than the other pnictogen pentafluorides, making it an extremely powerful fluorinating agent.[9] This effect is even more pronounced for moscovium, prohibiting it from attaining a +5 oxidation state.

Other oxidation states
  • Nitrogen forms a variety of compounds with oxygen in which the nitrogen can take on a variety of oxidation states, including +II, +IV, and even some mixed-valence compounds and very unstable +VI oxidation state.
  • In hydrazine, diphosphane, and organic derivatives of the two, the nitrogen or phosphorus atoms have the −2 oxidation state. Likewise, diimide, which has two nitrogen atoms double-bonded to each other, and its organic derivatives have nitrogen in the oxidation state of −1.
    • Similarly, realgar has arsenic–arsenic bonds, so the arsenic's oxidation state is +II.
    • A corresponding compound for antimony is Sb2(C6H5)4, where the antimony's oxidation state is +II.
  • Phosphorus has the +1 oxidation state in hypophosphorous acid and the +4 oxidation state in hypophosphoric acid.
  • Antimony tetroxide is a mixed-valence compound, where half of the antimony atoms are in the +3 oxidation state, and the other half are in the +5 oxidation state.
  • It is expected that moscovium will have an inert-pair effect for both the 7s and the 7p1/2 electrons, as the binding energy of the lone 7p3/2 electron is noticeably lower than that of the 7p1/2 electrons. This is predicted to cause +I to be a common oxidation state for moscovium, although it also occurs to a lesser extent for bismuth and nitrogen.[10]

Physical

The pnictogens consist of two non-metals (one gas, one solid), two metalloids, one metal, and one element with unknown chemical properties. All the elements in the group are solids at room temperature, except for nitrogen which is gaseous at room temperature. Nitrogen and bismuth, despite both being pnictogens, are very different in their physical properties. For instance, at STP nitrogen is a transparent non-metallic gas, while bismuth is a silvery-white metal.[11]

The densities of the pnictogens increase towards the heavier pnictogens. Nitrogen's density is 0.001251 g/cm3 at STP.[11] Phosphorus's density is 1.82 g/cm3 at STP, arsenic's is 5.72 g/cm3, antimony's is 6.68 g/cm3, and bismuth's is 9.79 g/cm3.[12]

Nitrogen's melting point is −210 °C and its boiling point is −196 °C. Phosphorus has a melting point of 44 °C and a boiling point of 280 °C. Arsenic is one of only two elements to sublimate at standard pressure; it does this at 603 °C. Antimony's melting point is 631 °C and its boiling point is 1587 °C. Bismuth's melting point is 271 °C and its boiling point is 1564 °C.[12]

Nitrogen's crystal structure is hexagonal. Phosphorus's crystal structure is cubic. Arsenic, antimony, and bismuth all have rhombohedral crystal structures.[12]

History

The nitrogen compound sal ammoniac (ammonium chloride) has been known since the time of the Ancient Egyptians. In the 1760s two scientists, Henry Cavendish and Joseph Priestley, isolated nitrogen from air, but neither realized the presence of an undiscovered element. It was not until several years later, in 1772, that Daniel Rutherford realized that the gas was indeed nitrogen.[13]

The alchemist Hennig Brandt first discovered phosphorus in Hamburg in 1669. Brandt produced the element by heating evaporated urine and condensing the resulting phosphorus vapor in water. Brandt initially thought that he had discovered the Philosopher's Stone, but eventually realized that this was not the case.[13]

Arsenic compounds have been known for at least 5000 years, and the ancient Greek Theophrastus recognized the arsenic minerals called realgar and orpiment. Elemental arsenic was discovered in the 13th century by Albertus Magnus.[13]

Antimony was well known to the ancients. A 5000-year-old vase made of nearly pure antimony exists in the Louvre. Antimony compounds were used in dyes in the Babylonian times. The antimony mineral stibnite may have been a component of Greek fire.[13]

Bismuth was first discovered by an alchemist in 1400. Within 80 years of bismuth's discovery, it had applications in printing and decorated caskets. The Incas were also using bismuth in knives by 1500. Bismuth was originally thought to be the same as lead, but in 1753, Claude François Geoffroy proved that bismuth was different from lead.[13]

Moscovium was successfully produced in 2003 by bombarding americium-243 atoms with calcium-48 atoms.[13]

Names and etymology

The term "pnictogen" (or "pnigogen") is derived from the ancient Greek word πνίγειν (pnígein) meaning "to choke", referring to the choking or stifling property of nitrogen gas.[14] It can also be used as a mnemonic for the two most common members, P and N. The term "pnictogen" was suggested by the Dutch chemist Anton Eduard van Arkel in the early 1950s. It is also spelled "pnicogen" or "pnigogen". The term "pnicogen" is rarer than the term "pnictogen", and the ratio of academic research papers using "pnictogen" to those using "pnicogen" is 2.5 to 1.[4] It comes from the Greek root πνιγ- (choke, strangle), and thus the word "pnictogen" is also a reference to the Dutch and German names for nitrogen (stikstof and Stickstoff, respectively, "suffocating substance": i.e., substance in air, unsupportive of breathing). Hence, "pnictogen" could be translated as "suffocation maker". The word "pnictide" also comes from the same root.[14]

The name pentels (from Greek πέντε, pénte, five) also at one time stood for this group.[15]

Occurrence

A collection of pnictogen samples

Nitrogen makes up 25 parts per million of the Earth's crust, 5 parts per million of soil on average, 100 to 500 parts per trillion of seawater, and 78% of dry air. The majority of nitrogen on earth is in the form of nitrogen gas, but some nitrate minerals do exist. Nitrogen makes up 2.5% of a typical human by weight.[13]

Phosphorus makes up 0.1% of the earth's crust, making it the 11th most abundant element there. Phosphorus makes up 0.65 parts per million of soil, and 15 to 60 parts per billion of seawater. There are 200 Mt of accessible phosphates on earth. Phosphorus makes up 1.1% of a typical human by weight.[13] Phosphorus occurs in minerals of the apatite family which are the main components of the phosphate rocks.

Arsenic makes up 1.5 parts per million of the earth's crust, making it the 53rd most abundant element there. The soils contain 1 to 10 parts per million of arsenic, and seawater contains 1.6 parts per billion of arsenic. Arsenic makes up 100 parts per billion of a typical human by weight. Some arsenic exists in elemental form, but most arsenic is found in the arsenic minerals orpiment, realgar, arsenopyrite, and enargite.[13]

Antimony makes up 0.2 parts per million of the earth's crust, making it the 63rd most abundant element there. The soils contain 1 part per million of antimony on average, and seawater contains 300 parts per trillion of antimony on average. A typical human contains 28 parts per billion of antimony by weight. Some elemental antimony occurs in silver deposits.[13]

Bismuth makes up 48 parts per billion of the earth's crust, making it the 70th most abundant element there. The soils contain approximately 0.25 parts per million of bismuth, and seawater contains 400 parts per trillion of bismuth. Bismuth most commonly occurs as the mineral bismuthinite, but bismuth also occurs in elemental form or in sulfide ores.[13]

Moscovium is produced several atoms at a time in particle accelerators.[13]

Production

Nitrogen

Nitrogen can be produced by fractional distillation of air.[16]

Phosphorus

The principal method for producing phosphorus is to reduce phosphates with carbon in an electric arc furnace.[17]

Arsenic

Most arsenic is prepared by heating the mineral arsenopyrite in the presence of air. This forms As4O6, from which arsenic can be extracted via carbon reduction. However, it is also possible to make metallic arsenic by heating arsenopyrite at 650 to 700 °C without oxygen.[18]

Antimony

With sulfide ores, the method by which antimony is produced depends on the amount of antimony in the raw ore. If the ore contains 25% to 45% antimony by weight, then crude antimony is produced by smelting the ore in a blast furnace. If the ore contains 45% to 60% antimony by weight, antimony is obtained by heating the ore, also known as liquidation. Ores with more than 60% antimony by weight are chemically displaced with iron shavings from the molten ore, resulting in impure metal.

If an oxide ore of antimony contains less than 30% antimony by weight, the ore is reduced in a blast furnace. If the ore contains closer to 50% antimony by weight, the ore is instead reduced in a reverberatory furnace.

Antimony ores with mixed sulfides and oxides are smelted in a blast furnace.[19]

Bismuth

Bismuth minerals do occur, in particular in the form of sulfides and oxides, but it is more economic to produce bismuth as a by-product of the smelting of lead ores or, as in China, of tungsten and zinc ores.[20]

Moscovium

Moscovium is produced a few atoms at a time in particle accelerators by firing a beam of Calcium-48 ions at Americium until the nuclei fuse.[21]

Applications

Biological role

Nitrogen is a component of molecules critical to life on earth, such as DNA and amino acids. Nitrates occur in some plants, due to bacteria present in the nodes of the plant. This is seen in leguminous plants such as peas [clarification needed] or spinach and lettuce.[citation needed] A typical 70 kg human contains 1.8 kg of nitrogen.[13]

Phosphorus in the form of phosphates occur in compounds important to life, such as DNA and ATP. Humans consume approximately 1 g of phosphorus per day.[24] Phosphorus is found in foods such as fish, liver, turkey, chicken, and eggs. Phosphate deficiency is a problem known as hypophosphatemia. A typical 70 kg human contains 480 g of phosphorus.[13]

Arsenic promotes growth in chickens and rats, and may be essential for humans in small quantities. Arsenic has been shown to be helpful in metabolizing the amino acid arginine. There are 7 mg of arsenic in a typical 70 kg human.[13]

Antimony is not known to have a biological role. Plants take up only trace amounts of antimony. There are approximately 2 mg of antimony in a typical 70 kg human.[13]

Bismuth is not known to have a biological role. Humans ingest on average less than 20 μg of bismuth per day. There is less than 500 μg of bismuth in a typical 70 kg human.[13]

Toxicity

Nitrogen gas is completely non-toxic, but breathing in pure nitrogen gas is deadly, because it causes nitrogen asphyxiation.[22] The build-up of nitrogen bubbles in the blood, such as those that may occur during scuba diving, can cause a condition known as the "bends" (decompression sickness). Many nitrogen compounds such as hydrogen cyanide and nitrogen-based explosives are also highly dangerous.[13]

White phosphorus, an allotrope of phosphorus, is toxic, with 1 mg per kg bodyweight being a lethal dose.[11] White phosphorus usually kills humans within a week of ingestion by attacking the liver. Breathing in phosphorus in its gaseous form can cause an industrial disease called "phossy jaw", which eats away the jawbone. White phosphorus is also highly flammable. Some organophosphorus compounds can fatally block certain enzymes in the human body.[13]

Elemental arsenic is toxic, as are many of its inorganic compounds; however some of its organic compounds can promote growth in chickens.[11] The lethal dose of arsenic for a typical adult is 200 mg and can cause diarrhea, vomiting, colic, dehydration, and coma. Death from arsenic poisoning typically occurs within a day.[13]

Antimony is mildly toxic.[22] Additionally, wine steeped in antimony containers can induce vomiting.[11] When taken in large doses, antimony causes vomiting in a victim, who then appears to recover before dying several days later. Antimony attaches itself to certain enzymes and is difficult to dislodge. Stibine, or SbH3, is far more toxic than pure antimony.[13]

Bismuth itself is largely non-toxic, although consuming too much of it can damage the liver. Only one person has ever been reported to have died from bismuth poisoning.[13] However, consumption of soluble bismuth salts can turn a person's gums black.[11]

Moscovium is too unstable to conduct any toxicity chemistry.

See also

References

  1. ^ International Union of Pure and Applied Chemistry (2005). Nomenclature of Inorganic Chemistry (IUPAC Recommendations 2005). Cambridge (UK): RSC–IUPAC. ISBN 0-85404-438-8. p. 51. Electronic version.
  2. ^ Fluck, E (1988). "New notations in the periodic table" (PDF). Pure and Applied Chemistry. 60 (3): 431–6. doi:10.1351/pac198860030431. S2CID 96704008.
  3. ^ Adachi, S., ed. (2005). Properties of Group-IV, III-V and II-VI Semiconductors. Wiley Series in Materials for Electronic & Optoelectronic Applications. Vol. 15. Hoboken, New Jersey: John Wiley & Sons. Bibcode:2005pgii.book.....A. ISBN 978-0470090329.
  4. ^ a b "Pnicogen – Molecule of the Month". University of Bristol
  5. ^ Boudreaux, Kevin A. "Group 5A — The Pnictogens". Department of Chemistry, Angelo State University, Texas
  6. ^ Greenwood, N.N.; Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann. p. 423. ISBN 0-7506-3365-4.
  7. ^ Jerzembeck W, Bürger H, Constantin L, Margulès L, Demaison J, Breidung J, Thiel W (2002). "Bismuthine BiH3: Fact or Fiction? High-Resolution Infrared, Millimeter-Wave, and Ab Initio Studies". Angew. Chem. Int. Ed. 41 (14): 2550–2552. doi:10.1002/1521-3773(20020715)41:14<2550::AID-ANIE2550>3.0.CO;2-B. PMID 12203530.
  8. ^ Scott, Thomas; Eagleson, Mary (1994). Concise encyclopedia chemistry. Walter de Gruyter. p. 136. ISBN 978-3-11-011451-5.
  9. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 561–563. ISBN 978-0-08-037941-8.
  10. ^ Keller, O. L. Jr.; C. W. Nestor, Jr. (1974). "Predicted properties of the superheavy elements. III. Element 115, Eka-bismuth" (PDF). Journal of Physical Chemistry. 78 (19): 1945. doi:10.1021/j100612a015.
  11. ^ a b c d e f g h i j k l m n Gray, Theodore (2010). The Elements.
  12. ^ a b c Jackson, Mark (2001), Periodic Table Advanced, BarCharts Publishing, Incorporated, ISBN 1572225424
  13. ^ a b c d e f g h i j k l m n o p q r s t u v Emsley, John (2011), Nature's Building Blocks, ISBN 978-0-19-960563-7
  14. ^ a b Girolami, Gregory S. (2009). "Origin of the Terms Pnictogen and Pnictide". Journal of Chemical Education. 86 (10). American Chemical Society: 1200. Bibcode:2009JChEd..86.1200G. doi:10.1021/ed086p1200.
  15. ^ Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.), Inorganic Chemistry, translated by Eagleson, Mary; Brewer, William, San Diego/Berlin: Academic Press/De Gruyter, p. 586, ISBN 0-12-352651-5
  16. ^ Sanderson, R. Thomas (February 1, 2019). "nitrogen – Definition, Symbol, Uses, Properties, Atomic Number, and Facts". Encyclopædia Britannica.
  17. ^ "phosphorus (chemical element)". Encyclopædia Britannica. 11 October 2019.
  18. ^ "arsenic (chemical element)". Encyclopædia Britannica. 11 October 2019.
  19. ^ Butterman, C.; Carlin, Jr., J.F. (2003). Mineral Commodity Profiles: Antimony. United States Geological Survey.
  20. ^ Bell, Terence. "Metal Profile: Bismuth". About.com. Archived from the original on 5 July 2012.
  21. ^ Oganessian, Yu Ts; Utyonkov, V K (9 March 2015). "Superheavy Element Research". Reports on Progress in Physics. 78 (3): 3. Bibcode:2015RPPh...78c6301O. doi:10.1088/0034-4885/78/3/036301. PMID 25746203.
  22. ^ a b c Kean, Sam (2011), The Disappearing Spoon, Transworld, ISBN 9781446437650
  23. ^ Huang, Jia; Huang, Qiong; Liu, Min; Chen, Qiaohui; Ai, Kelong (February 2022). "Emerging Bismuth Chalcogenides Based Nanodrugs for Cancer Radiotherapy". Frontiers in Pharmacology. 13: 844037. doi:10.3389/fphar.2022.844037. PMC 8894845. PMID 35250594.
  24. ^ "Phosphorus in diet". MedlinePlus. NIH–National Library of Medicine. 9 April 2020.
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