What Are Some Common Uses of Nitrogen Family

Group fifteen elements of the periodic tabular array with valency 5

Pnictogens
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 Silvery Cadmium Indium Tin can 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 (chemical 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 carbon group ← → chalcogens
IUPAC group number xv Proper name by element nitrogen group Petty name pnictogens, pentels CAS group number (United states of america, pattern A-B-A) VA sometime IUPAC number (Europe, design A-B) VB
↓Menstruation
ii	Nitrogen (N) 7 Other nonmetal
iii	Phosphorus (P) 15 Other nonmetal
4	Arsenic (As) 33 Metalloid
5	Antimony (Sb) 51 Metalloid
half dozen	Bismuth (Bi) 83 Other metal
vii	Moscovium (Mc) 115 other metallic
Fable primordial element synthetic element Diminutive number color: ruby-red=gas,blackness=solid
5 t due east

A pnictogen ^[1] ( or ; from Aboriginal Greek: πνῑ́γω "to asphyxiate" and -gen, "generator") is any of the chemical elements in group 15 of the periodic tabular array. This group is too known equally the nitrogen family unit. Information technology consists of the elements nitrogen (N), phosphorus (P), arsenic (Equally), antimony (Sb), bismuth (Bi), and perhaps the chemically uncharacterized synthetic element moscovium (Mc).

In modern IUPAC note, information technology is called Group 15. In CAS and the quondam IUPAC systems information technology was called Group VA and Group VB respectively (pronounced "grouping five A" and "grouping five B", "V" for the Roman numeral five).^[ii] In the field of semiconductor physics, it is still normally called Group V.^[3] The "five" ("V") in the historical names comes from the "pentavalency" of nitrogen, reflected past the stoichiometry of compounds such equally N₂O₅. They have as well been called the pentels.

Characteristics [edit]

Chemical [edit]

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

Z	Element	Electrons per beat out
7	nitrogen	ii, 5
15	phosphorus	ii, viii, 5
33	arsenic	2, 8, 18, 5
51	antimony	two, 8, eighteen, eighteen, v
83	bismuth	2, eight, eighteen, 32, 18, 5
115	moscovium	2, 8, 18, 32, 32, xviii, 5 (predicted)

This grouping has the defining characteristic that all the component elements have 5 electrons in their outermost shell, that is 2 electrons in the southward 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 land. The Russell–Saunders term symbol of the basis state in all elements in the grouping is ⁴S _3⁄two .

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

Compounds [edit]

Binary compounds of the grouping can be referred to collectively as pnictides. Pnictide compounds tend to exist exotic. Various properties that some pnictides have include beingness diamagnetic and paramagnetic at room temperature, being transparent, and generating electricity when heated. Other pnictides include the ternary rare-earth main-group multifariousness of pnictides. These are in the form of RE_aM_bPn_c, where Thousand is a carbon group or boron group element and Pn is any pnictogen except nitrogen. These compounds are betwixt ionic and covalent compounds and thus have unusual bonding backdrop.^[four]

These elements are besides noted for their stability in compounds due to their tendency for forming double and triple covalent bonds. This is the holding of these elements which leads to their potential toxicity, virtually evident in phosphorus, arsenic and antimony. When these substances react with various chemicals of the torso, they create strong free radicals not easily processed by the liver, where they accrue. Paradoxically, it is this strong bonding which causes nitrogen and bismuth's reduced toxicity (when in molecules), as these form strong bonds with other atoms which are difficult to separate, creating very unreactive molecules. For instance, N₂, the diatomic form of nitrogen, is used as an inert gas in situations where using argon or another noble gas would exist 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 (similar in NH + four ). When a pnictogen forms only three single bonds, effects of the lone pair typically upshot in trigonal pyramidal molecular geometry.

Oxidation states [edit]

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

−iii oxidation land [edit]

Pnictogens can react with hydrogen to grade 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 than toxic, and has a smaller hydrogen-hydrogen angle (from 107.eight° in ammonia^[half-dozen] to 90.48° in bismuthane).^[seven] (Also, technically, only ammonia and phosphane have the pnictogen in the −3 oxidation state considering, 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 2d-most widely-used semiconductor after silicon.

+3 oxidation state [edit]

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 simply stable nitrogen trihalide, with nitrogen trichloride, nitrogen tribromide and nitrogen triiodide being explosive—nitrogen triiodide being so shock-sensitive that the bear on of a plumage detonates it (the concluding three actually characteristic nitrogen in the -3 oxidation state). Phosphorus forms a +Iii oxide which is stable at room temperature, phosphorous acrid, and several trihalides, although the triiodide is unstable. Arsenic forms +III compounds with oxygen as arsenites, arsenous acid, and arsenic(III) oxide, and information technology forms all four trihalides. Antimony forms antimony(Three) oxide and antimonite but not oxyacids. Its trihalides, antimony trifluoride, antimony trichloride, antimony tribromide, and antimony triiodide, like all pnictogen trihalides, each take trigonal pyramidal molecular geometry.

The +3 oxidation country is bismuth'south most common oxidation state considering its ability to course the +5 oxidation state is hindered by relativistic backdrop on heavier elements, effects that are even more pronounced concerning moscovium. Bismuth(Three) forms an oxide, an oxychloride, an oxynitrate, and a sulfide. Moscovium(3) is predicted to conduct similarly to bismuth(3). Moscovium is predicted to form all iv trihalides, of which all simply the trifluoride are predicted to be soluble in water. It is also predicted to class an oxychloride and oxybromide in the +III oxidation state.

+5 oxidation land [edit]

For nitrogen, the +5 state is typically serves every bit only a formal caption of molecules like Northward_iiO_v, every bit the high electronegativity of nitrogen causes the electrons to be shared nigh 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 substantially non-relativistic typical pnictogens phosphorus, arsenic, and antimony, as shown in their oxides, phosphorus(V) oxide, arsenic(Five) oxide, and antimony(V) oxide, and their fluorides, phosphorus(5) fluoride, arsenic(V) fluoride, antimony(V) fluoride. At least two also form related fluoride-anions, hexafluorophosphate and hexafluoroantimonate, that role as non-coordinating anions. Phosphorus even forms mixed oxide-halides, known as oxyhalides, like phosphorus oxychloride, and mixed pentahalides, like phosphorus trifluorodichloride. Pentamethylpnictogen(5) compounds exist for arsenic, antimony, and bismuth. Withal, for bismuth, the +5 oxidation state becomes rare due to the relativistic stabilization of the 6s orbitals known as the inert pair effect, and then that the 6s electrons are reluctant to bail chemically. This causes bismuth(5) oxide to be unstable^[viii] and bismuth(V) fluoride to exist more reactive than the other pnictogen pentafluorides, making information technology an extremely powerful fluorinating agent.^[nine] This consequence is even more pronounced for moscovium, prohibiting it from attaining a +5 oxidation state.

Other oxidation states [edit]

• Nitrogen forms a variety of compounds with oxygen in which the nitrogen can take on a diverseness of oxidation states, including +Ii, +IV, and even some mixed-valence compounds and very unstable +Vi oxidation land.
• In hydrazine, diphosphane, and organic derivatives of the two, the nitrogen/phosphorus atoms have the −2 oxidation land. Likewise, diimide, which has ii 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(C_{half dozen}H₅)_iv, where the antimony'southward oxidation country is +II.
• Phosphorus has the +ane oxidation state in hypophosphorous acid and the +4 oxidation land in hypophosphoric acid.
• Antimony tetroxide is a mixed-valence compound, where half of the antimony atoms are in the +three oxidation land, and the other half are in the +5 oxidation state.
• It is expected that moscovium will accept an inert pair issue for both the 7s and the 7p_1/2 electrons, as the bounden energy of the solitary 7p_3/2 electron is noticeably lower than that of the 7p_1/2 electrons. This is predicted to crusade +I to exist a common oxidation state for moscovium, although it likewise occurs to a lesser extent for bismuth and nitrogen.^[ten]

Physical [edit]

The pnictogens consist of 2 non-metals (one gas, one solid), two metalloids, one metal, and 1 element with unknown chemic backdrop. All the elements in the grouping 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 1000/cm^three at STP.^[11] Phosphorus's density is 1.82 g/cm³ at STP, arsenic's is five.72 yard/cm³, antimony'due south is 6.68 thou/cm³, and bismuth's is nine.79 k/cm³.^[12]

Nitrogen's melting point is −210 °C and its boiling point is −196 °C. Phosphorus has a melting bespeak of 44 °C and a boiling point of 280 °C. Arsenic is one of simply ii elements to sublimate at standard pressure level; it does this at 603 °C. Antimony'due south melting point is 631 °C and its humid signal is 1587 °C. Bismuth's melting bespeak is 271 °C and its boiling point is 1564 °C.^[12]

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

History [edit]

The nitrogen chemical 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, just neither realized the presence of an undiscovered element. It was non until several years later on, in 1772, that Daniel Rutherford realized that the gas was indeed nitrogen.^[thirteen]

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

Arsenic compounds accept been known for at least 5000 years, and the aboriginal Greek Theophrastus recognized the arsenic minerals chosen 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-onetime vase made of about 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 busy caskets. The Incas were also using bismuth in knives past 1500. Bismuth was originally thought to exist the same as lead, but in 1753, Claude François Geoffroy proved that bismuth was unlike from atomic number 82.^[13]

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

Names and etymology [edit]

The term "pnictogen" (or "pnigogen") is derived from the Ancient Greek give-and-take πνίγειν ( pnígein ) significant "to choke", referring to the choking or stifling holding of nitrogen gas.^[14] Information technology can also be used as a mnemonic for the two most mutual members, P and Northward. The term "pnictogen" was suggested by the Dutch chemist Anton Eduard van Arkel in the early 1950s. It is as well spelled "pnicogen" or "pnigogen". The term "pnicogen" is rarer than the term "pnictogen", and the ratio of bookish research papers using "pnictogen" to those using "pnicogen" is two.v to ane.^[4] It comes from the Greek root πνιγ- (choke, strangle), and thus the word "pnictogen" is besides a reference to the Dutch and German names for nitrogen ( stikstof and Stickstoff , respectively, "suffocating substance": i.east., 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) as well at one time stood for this group.^[15]

Occurrence [edit]

A drove 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 globe is in the form of nitrogen gas, simply some nitrate minerals practice exist. Nitrogen makes up 2.5% of a typical human by weight.^[xiii]

Phosphorus makes upward 0.1% of the world's chaff, making information technology the 11th almost arable element there. Phosphorus makes up 0.65 parts per million of soil, and xv to 60 parts per billion of seawater. There are 200 Mt of attainable phosphates on earth. Phosphorus makes upwards 1.i% of a typical human by weight.^[13] Phosphorus occurs in minerals of the apatite family unit which are the principal components of the phosphate rocks.

Arsenic makes upwards 1.5 parts per 1000000 of the earth's crust, making it the 53rd nearly abundant element there. The soils contain 1 to x parts per meg of arsenic, and seawater contains 1.6 parts per billion of arsenic. Arsenic makes upward 100 parts per billion of a typical human by weight. Some arsenic exists in elemental form, just most arsenic is found in the arsenic minerals orpiment, realgar, arsenopyrite, and enargite.^[13]

Antimony makes up 0.two parts per 1000000 of the globe's crust, making it the 63rd most abundant element in that location. The soils contain 1 part per meg 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 upward 48 parts per billion of the globe'south 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 near commonly occurs as the mineral bismuthinite, but bismuth also occurs in elemental grade or in sulfide ores.^[13]

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

Production [edit]

Nitrogen [edit]

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

Phosphorus [edit]

The master method for producing phosphorus is to reduce phosphates with carbon in an electrical arc furnace.^[17]

Arsenic [edit]

Most arsenic is prepared by heating the mineral arsenopyrite in the presence of air. This forms As_ivO_{half dozen}, from which arsenic can be extracted via carbon reduction. Nonetheless, information technology is also possible to make metallic arsenic past heating arsenopyrite at 650 to 700 °C without oxygen.^[18]

Antimony [edit]

With sulfide ores, the method past which antimony is produced depends on the amount of antimony in the raw ore. If the ore contains 25% to 45% antimony past weight, then rough 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, too 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 past weight, the ore is reduced in a blast furnace. If the ore contains closer to 50% antimony past weight, the ore is instead reduced in a reverberatory furnace.

Antimony ores with mixed sulfides and oxides are smelted in a smash furnace.^[nineteen]

Bismuth [edit]

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

Moscovium [edit]

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 [edit]

• Liquid nitrogen is a commonly used cryogenic liquid.^[11]
• Nitrogen in the class of ammonia is a food critical to most plants' survival.^[11] Synthesis of ammonia accounts for about 1–two% of the world's energy consumption and the bulk of reduced nitrogen in food.
• Phosphorus is used in matches and incendiary bombs.^[11]
• Phosphate fertilizer helps feed much of the globe.^[xi]
• Arsenic was historically used every bit a Paris green pigment, but is not used this fashion anymore due to its extreme toxicity.^[11]
• Arsenic in the class of organoarsenic compounds is sometimes used in craven feed.^[11]
• Antimony is alloyed with pb to produce some bullets.^[xi]
• Antimony currency was briefly used in the 1930s in parts of Prc, but this utilize was discontinued every bit antimony is both soft and toxic.^[22]
• Bismuth subsalicylate is the active ingredient in Pepto-Bismol.^[eleven]

Biological part [edit]

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 nowadays in the nodes of the plant. This is seen in leguminous plants such as peas^{[ description needed ]} or spinach and lettuce.^{[ commendation needed ]} A typical 70 kg human contains ane.eight 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 chiliad of phosphorus per day.^[23] Phosphorus is found in foods such every bit fish, liver, turkey, chicken, and eggs. Phosphate deficiency is a problem known every bit hypophosphatemia. A typical 70 kg human contains 480 thou of phosphorus.^[thirteen]

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

Antimony is non known to have a biological role. Plants have upwardly only trace amounts of antimony. There are approximately 2 mg of antimony in a typical 70 kg homo.^[thirteen]

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

Toxicity [edit]

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

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

Elemental arsenic is toxic, as are many of its inorganic compounds; however some of its organic compounds tin promote growth in chickens.^[11] The lethal dose of arsenic for a typical developed is 200 mg and can cause diarrhea, vomiting, colic, aridity, and blackout. Death from arsenic poisoning typically occurs inside a twenty-four hours.^[13]

Antimony is mildly toxic.^[22] Additionally, wine steeped in antimony containers tin can induce vomiting.^[xi] When taken in large doses, antimony causes airsickness 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 not-toxic, although consuming besides much of it can damage the liver. Only one person has ever been reported to accept died from bismuth poisoning.^[13] However, consumption of soluble bismuth salts can turn a person's gums blackness.^[11]

Moscovium is also unstable to conduct any toxicity chemistry.

See likewise [edit]

• Oxypnictide, including superconductors discovered in 2008.
• Ferropnictide, including oxypnictide superconductors.

References [edit]

1. ^ Connelly, NG; Damhus, T, eds. (2005). "section IR-iii.5: Elements in the periodic table" (PDF). Nomenclature of Inorganic Chemical science: IUPAC Recommendations 2005. Cambridge, U.k.: RSC Publishing. p. 51. ISBN978-0-85404-438-2.
2. ^ Fluck, E (1988). "New notations in the periodic table" (PDF). Pure and Applied Chemistry. 60 (iii): 431–half-dozen. doi:x.1351/pac198860030431. S2CID 96704008.
3. ^ Adachi, S., ed. (2005). Properties of Group-Iv, Three-V and 2-Six Semiconductors. Wiley Series in Materials for Electronic & Optoelectronic Applications. Vol. 15. Hoboken, New Bailiwick of jersey: John Wiley & Sons. Bibcode:2005pgii.book.....A. ISBN978-0470090329.
4. ^ ^{a b} "Pnicogen – Molecule of the Month". University of Bristol
5. ^ Boudreaux, Kevin A. "Group 5A — The Pnictogens". Section of Chemistry, Angelo Country University, Texas
6. ^ Greenwood, N.N.; Earnshaw, A. (1997). Chemistry of the Elements (2d ed.). Oxford: Butterworth-Heinemann. p. 423. ISBN0-7506-3365-4.
7. ^ Jerzembeck W, Bürger H, Constantin L, Margulès 50, 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:xiv<2550::Help-ANIE2550>three.0.CO;2-B.
8. ^ Scott, Thomas; Eagleson, Mary (1994). Concise encyclopedia chemistry . Walter de Gruyter. p. 136. ISBN978-3-eleven-011451-five.
9. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 561–563. ISBN978-0-08-037941-8.
10. ^ Keller, O. L., Jr.; C. W. Nestor, Jr. (1974). "Predicted properties of the superheavy elements. III. Element 115, Eka-bismuth" (PDF). Periodical of Concrete Chemistry. 78 (nineteen): 1945. doi:10.1021/j100612a015.
11. ^ ^{a b c d e f chiliad h i j chiliad l m due north} Gray, Theodore (2010). The Elements.
12. ^ ^{a b c} Jackson, Mark (2001), Periodic Table Advanced, BarCharts Publishing, Incorporated, ISBN1572225424
13. ^ ^{a b c d due east f m h i j k l thou n o p q r south t u v} Emsley, John (2011), Nature'southward Edifice Blocks, ISBN978-0-nineteen-960563-7
14. ^ ^{a b} Girolami, Gregory S. (2009). "Origin of the Terms Pnictogen and Pnictide". Journal of Chemical Pedagogy. American Chemical Society. 86 (10): 1200. Bibcode:2009JChEd..86.1200G. doi:x.1021/ed086p1200.
15. ^ Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.), Inorganic Chemical science, translated by Eagleson, Mary; Brewer, William, San Diego/Berlin: Bookish Press/De Gruyter, p. 586, ISBN0-12-352651-5
16. ^ Sanderson, R. Thomas (Feb 1, 2019). "Nitrogen: chemical element". Encyclopædia Britannica.
17. ^ "Phosphorus: chemical element". Encyclopædia Britannica. eleven Oct 2019.
18. ^ "arsenic (Equally) | chemical element". Encyclopædia Britannica.
19. ^ Butterman, C.; Carlin, Jr., J.F. (2003). Mineral Commodity Profiles: Antimony. United states of america Geological Survey.
20. ^ Bell, Terence. "Metallic Contour: Bismuth". About.com. Archived from the original on five July 2012.
21. ^ Oganessian, Yu Ts; Utyonkov, 5 K (ix March 2015). "Superheavy Element Research". Reports on Progress in Physics. 78 (3): 3. doi:ten.1088/0034-4885/78/3/036301. PMID 25746203.
22. ^ ^{a b c} Kean, Sam (2011), The Disappearing Spoon, Transworld, ISBN9781446437650
23. ^ "Phosphorus in diet". MedlinePlus. National Institutes of Health. ix Apr 2020.

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Source: https://en.wikipedia.org/wiki/Pnictogen

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