{"id":1139,"date":"2019-07-23T21:13:15","date_gmt":"2019-07-24T01:13:15","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/chapter\/occurrence-preparation-and-properties-of-phosphorus\/"},"modified":"2020-04-29T12:19:01","modified_gmt":"2020-04-29T16:19:01","slug":"occurrence-preparation-and-properties-of-phosphorus","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/chapter\/occurrence-preparation-and-properties-of-phosphorus\/","title":{"raw":"Occurrence, Preparation, and Properties of Phosphorus","rendered":"Occurrence, Preparation, and Properties of Phosphorus"},"content":{"raw":"[latexpage]<div class=\"textbox textbox--learning-objectives\"><h3>Learning Objectives<\/h3>By the end of this section, you will be able to: <ul><li>Describe the properties, preparation, and uses of phosphorus<\/li><\/ul><\/div><p id=\"fs-idp52194704\">The industrial preparation of phosphorus is by heating calcium phosphate, obtained from phosphate rock, with sand and coke:<\/p><div data-type=\"equation\" id=\"fs-idp51821104\">\\({\\text{2Ca}}_{3}{\\left({\\text{PO}}_{4}\\right)}_{2}\\left(s\\right)+{\\text{6SiO}}_{2}\\left(s\\right)+\\text{10C}\\left(s\\right)\\phantom{\\rule{0.2em}{0ex}}\\stackrel{\\phantom{\\rule{0.4em}{0ex}}\\text{\u0394}\\phantom{\\rule{0.4em}{0ex}}}{\\to }\\phantom{\\rule{0.2em}{0ex}}{\\text{6CaSiO}}_{3}\\left(l\\right)+\\text{10CO}\\left(g\\right)+{\\text{P}}_{4}\\left(g\\right)\\)<\/div><p id=\"fs-idp5816832\">The phosphorus distills out of the furnace and is condensed into a solid or burned to form P<sub>4<\/sub>O<sub>10<\/sub>. The preparation of many other phosphorus compounds begins with P<sub>4<\/sub>O<sub>10<\/sub>. The acids and phosphates are useful as fertilizers and in the chemical industry. Other uses are in the manufacture of special alloys such as ferrophosphorus and phosphor bronze. Phosphorus is important in making pesticides, matches, and some plastics. Phosphorus is an active nonmetal. In compounds, phosphorus usually occurs in oxidation states of 3\u2212, 3+, and 5+. Phosphorus exhibits oxidation numbers that are unusual for a group 15 element in compounds that contain phosphorus-phosphorus bonds; examples include diphosphorus tetrahydride, H<sub>2<\/sub>P-PH<sub>2<\/sub>, and tetraphosphorus trisulfide, P<sub>4<\/sub>S<sub>3<\/sub>, illustrated in <a href=\"#CNX_Chem_18_08_P4S3\" class=\"autogenerated-content\">(Figure)<\/a>.<\/p><div class=\"scaled-down\" id=\"CNX_Chem_18_08_P4S3\"><div class=\"bc-figcaption figcaption\">P<sub>4<\/sub>S<sub>3<\/sub> is a component of the heads of strike-anywhere matches.<\/div><span data-type=\"media\" id=\"fs-idm5144976\" data-alt=\"A ball-and-stick model is shown. Three orange atoms labeled \u201cP\u201d are single bonded together in a triangle shape. Each \u201cP\u201d is single bonded to yellow atoms labeled \u201cS,\u201d which are each single bonded to one other orange atom labeled \u201cP.\u201d\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2019\/07\/CNX_Chem_18_08_P4S3.jpg\" data-media-type=\"image\/jpeg\" alt=\"A ball-and-stick model is shown. Three orange atoms labeled \u201cP\u201d are single bonded together in a triangle shape. Each \u201cP\u201d is single bonded to yellow atoms labeled \u201cS,\u201d which are each single bonded to one other orange atom labeled \u201cP.\u201d\"><\/span><\/div><div class=\"bc-section section\" data-depth=\"1\" id=\"fs-idm31898272\"><h3 data-type=\"title\">Phosphorus Oxygen Compounds<\/h3><p id=\"fs-idp85748768\">Phosphorus forms two common oxides, phosphorus(III) oxide (or tetraphosphorus hexaoxide), P<sub>4<\/sub>O<sub>6<\/sub>, and phosphorus(V) oxide (or tetraphosphorus decaoxide), P<sub>4<\/sub>O<sub>10<\/sub>, both shown in <a href=\"#CNX_Chem_18_08_P4O6P4O10\" class=\"autogenerated-content\">(Figure)<\/a>. Phosphorus(III) oxide is a white crystalline solid with a garlic-like odor. Its vapor is very poisonous. It oxidizes slowly in air and inflames when heated to 70 \u00b0C, forming P<sub>4<\/sub>O<sub>10<\/sub>. Phosphorus(III) oxide dissolves slowly in cold water to form phosphorous acid, H<sub>3<\/sub>PO<sub>3<\/sub>.<\/p><div class=\"scaled-down\" id=\"CNX_Chem_18_08_P4O6P4O10\"><div class=\"bc-figcaption figcaption\">This image shows the molecular structures of P<sub>4<\/sub>O<sub>6<\/sub> (left) and P<sub>4<\/sub>O<sub>10<\/sub> (right).<\/div><span data-type=\"media\" id=\"fs-idp57250912\" data-alt=\"Two ball-and-stick models are shown. In the left model, three orange atoms labeled, \u201cP,\u201d are single bonded to red atoms labeled, \u201cO,\u201d in an alternating, six-sided ring structure. Each of the orange atoms are also single bonded to another red atom, which are in turn single bonded to a single orange atom. The right model shows three orange atoms labeled, \u201cP,\u201d single bonded to red atoms labeled, \u201cO,\u201d in an alternating, six-sided ring structure. Each of the orange atoms are also single bonded to two more red atoms, one in an upward position and one facing the outside of the molecule. The upward red atoms are single bonded to a single orange atom which is single bonded to a final red atom.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_P4O6P4O10.jpg\" data-media-type=\"image\/jpeg\" alt=\"Two ball-and-stick models are shown. In the left model, three orange atoms labeled, \u201cP,\u201d are single bonded to red atoms labeled, \u201cO,\u201d in an alternating, six-sided ring structure. Each of the orange atoms are also single bonded to another red atom, which are in turn single bonded to a single orange atom. The right model shows three orange atoms labeled, \u201cP,\u201d single bonded to red atoms labeled, \u201cO,\u201d in an alternating, six-sided ring structure. Each of the orange atoms are also single bonded to two more red atoms, one in an upward position and one facing the outside of the molecule. The upward red atoms are single bonded to a single orange atom which is single bonded to a final red atom.\"><\/span><\/div><p id=\"fs-idm7162480\">Phosphorus(V) oxide, P<sub>4<\/sub>O<sub>10<\/sub>, is a white powder that is prepared by burning phosphorus in excess oxygen. Its enthalpy of formation is very high (\u22122984 kJ), and it is quite stable and a very poor oxidizing agent. Dropping P<sub>4<\/sub>O<sub>10<\/sub> into water produces a hissing sound, heat, and orthophosphoric acid:<\/p><div data-type=\"equation\" id=\"fs-idp704592\">\\({\\text{P}}_{4}{\\text{O}}_{10}\\left(s\\right)+{\\text{6H}}_{2}\\text{O}\\left(l\\right)\\phantom{\\rule{0.2em}{0ex}}\u27f6\\phantom{\\rule{0.2em}{0ex}}{\\text{4H}}_{3}{\\text{PO}}_{4}\\left(aq\\right)\\)<\/div><p id=\"fs-idm64278832\">Because of its great affinity for water, phosphorus(V) oxide is an excellent drying agent for gases and solvents, and for removing water from many compounds.<\/p><\/div><div class=\"bc-section section\" data-depth=\"1\" id=\"fs-idm11573280\"><h3 data-type=\"title\">Phosphorus Halogen Compounds<\/h3><p id=\"fs-idp70568512\">Phosphorus will react directly with the halogens, forming trihalides, PX<sub>3<\/sub>, and pentahalides, PX<sub>5<\/sub>. The trihalides are much more stable than the corresponding nitrogen trihalides; nitrogen pentahalides do not form because of nitrogen\u2019s inability to form more than four bonds.<\/p><p id=\"fs-idp182518880\">The chlorides PCl<sub>3<\/sub> and PCl<sub>5<\/sub>, both shown in <a href=\"#CNX_Chem_18_08_PCl3PCl5\" class=\"autogenerated-content\">(Figure)<\/a>, are the most important halides of phosphorus. Phosphorus trichloride is a colorless liquid that is prepared by passing chlorine over molten phosphorus. Phosphorus pentachloride is an off-white solid that is prepared by oxidizing the trichloride with excess chlorine. The pentachloride sublimes when warmed and forms an equilibrium with the trichloride and chlorine when heated.<\/p><div class=\"scaled-down\" id=\"CNX_Chem_18_08_PCl3PCl5\"><div class=\"bc-figcaption figcaption\">This image shows the molecular structure of PCl<sub>3<\/sub> (left) and PCl<sub>5<\/sub> (right) in the gas phase.<\/div><span data-type=\"media\" id=\"fs-idp189314192\" data-alt=\"Two ball-and-stick models are shown. In the left model, an orange atom labeled, \u201cP,\u201d is single bonded to three green atoms labeled, \u201cC l.\u201d The right model shows an orange atom labeled, \u201cP,\u201d single bonded to five green atoms labeled, \u201cC l.\u201d\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_PCl3PCl5.jpg\" data-media-type=\"image\/jpeg\" alt=\"Two ball-and-stick models are shown. In the left model, an orange atom labeled, \u201cP,\u201d is single bonded to three green atoms labeled, \u201cC l.\u201d The right model shows an orange atom labeled, \u201cP,\u201d single bonded to five green atoms labeled, \u201cC l.\u201d\"><\/span><\/div><p id=\"fs-idp21181152\">Like most other nonmetal halides, both phosphorus chlorides react with an excess of water and yield hydrogen chloride and an oxyacid: PCl<sub>3<\/sub> yields phosphorous acid H<sub>3<\/sub>PO<sub>3<\/sub> and PCl<sub>5<\/sub> yields phosphoric acid, H<sub>3<\/sub>PO<sub>4<\/sub>.<\/p><p id=\"fs-idm44217280\">The pentahalides of phosphorus are Lewis acids because of the empty valence <em data-effect=\"italics\">d<\/em> orbitals of phosphorus. These compounds readily react with halide ions (Lewis bases) to give the anion \\({\\text{PX}}_{6}{}^{\\text{\u2212}}.\\) Whereas phosphorus pentafluoride is a molecular compound in all states, X-ray studies show that solid phosphorus pentachloride is an ionic compound, \\({\\left[\\text{PCl}}_{4}{}^{\\text{+}}\\right]\\left[{\\text{PCl}}_{6}{}^{\\text{\u2212}}\\right],\\) as are phosphorus pentabromide, \\({\\left[\\text{PBr}}_{4}{}^{\\text{+}}\\right]\\)[Br<sup>\u2212<\/sup>], and phosphorus pentaiodide, \\({\\left[\\text{PI}}_{4}{}^{\\text{+}}\\right]\\)[I<sup>\u2212<\/sup>].<\/p><\/div><div class=\"summary\" data-depth=\"1\" id=\"fs-idp183301136\"><h3 data-type=\"title\">Key Concepts and Summary<\/h3><p id=\"fs-idp219295376\">Phosphorus (group 15) commonly exhibits oxidation states of 3\u2212 with active metals and of 3+ and 5+ with more electronegative nonmetals. The halogens and oxygen will oxidize phosphorus. The oxides are phosphorus(V) oxide, P<sub>4<\/sub>O<sub>10<\/sub>, and phosphorus(III) oxide, P<sub>4<\/sub>O<sub>6<\/sub>. The two common methods for preparing orthophosphoric acid, H<sub>3<\/sub>PO<sub>4<\/sub>, are either the reaction of a phosphate with sulfuric acid or the reaction of water with phosphorus(V) oxide. Orthophosphoric acid is a triprotic acid that forms three types of salts.<\/p><\/div><div class=\"exercises\" data-depth=\"1\" id=\"fs-idp185176672\"><h3 data-type=\"title\">Chemistry End of Chapter Exercises<\/h3><div data-type=\"exercise\" id=\"fs-idp52847792\"><div data-type=\"problem\" id=\"fs-idp188554560\"><p id=\"fs-idm63439584\">Write the Lewis structure for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry.<\/p><p id=\"fs-idp210380672\">(a) PH<sub>3<\/sub><\/p><p id=\"fs-idp153159872\">(b) \\({\\text{PH}}_{4}{}^{+}\\)<\/p><p id=\"fs-idm27147360\">(c) P<sub>2<\/sub>H<sub>4<\/sub><\/p><p id=\"fs-idm44280352\">(d) \\({\\text{PO}}_{4}{}^{3-}\\)<\/p><p id=\"fs-idp332959120\">(e) PF<sub>5<\/sub><\/p><\/div><div data-type=\"solution\" id=\"fs-idm55639488\"><p id=\"fs-idm28792464\">(a)<span data-type=\"newline\"><br><\/span><\/p><span data-type=\"media\" id=\"fs-idm55213168\" data-alt=\"This Lewis structure shows a phosphorus atom with a lone pair of electrons single bonded to three hydrogen atoms.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise1a_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom with a lone pair of electrons single bonded to three hydrogen atoms.\"><\/span><p><span data-type=\"newline\"><br><\/span> (b)<span data-type=\"newline\"><br><\/span><\/p><span data-type=\"media\" id=\"fs-idm1170240\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to four hydrogen atoms. The structure is surrounded by brackets and has a superscript positive sign outside the brackets.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise1b_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to four hydrogen atoms. The structure is surrounded by brackets and has a superscript positive sign outside the brackets.\"><\/span><p><span data-type=\"newline\"><br><\/span> (c)<span data-type=\"newline\"><br><\/span><\/p><span data-type=\"media\" id=\"fs-idp56334352\" data-alt=\"This Lewis structure shows two phosphorus atoms, each with a lone pair of electrons, single bonded to one another. Each phosphorus atom is also single bonded to two hydrogen atoms.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise1c_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows two phosphorus atoms, each with a lone pair of electrons, single bonded to one another. Each phosphorus atom is also single bonded to two hydrogen atoms.\"><\/span><p><span data-type=\"newline\"><br><\/span> (d)<span data-type=\"newline\"><br><\/span><\/p><span data-type=\"media\" id=\"fs-idm66638800\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to four oxygen atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript 3 negative sign outside the brackets.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise1d_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to four oxygen atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript 3 negative sign outside the brackets.\"><\/span><p><span data-type=\"newline\"><br><\/span> (e)<span data-type=\"newline\"><br><\/span><\/p><span data-type=\"media\" id=\"fs-idm5269184\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to five fluorine atoms, each with three lone pairs of electrons.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise1e_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to five fluorine atoms, each with three lone pairs of electrons.\"><\/span><\/div><\/div><div data-type=\"exercise\" id=\"fs-idp101864208\"><div data-type=\"problem\" id=\"fs-idp20141648\"><p id=\"fs-idp227455632\">Describe the molecular structure of each of the following molecules or ions listed. You may wish to review the chapter on chemical bonding and molecular geometry.<\/p><p id=\"fs-idp157002384\">(a) PH<sub>3<\/sub><\/p><p id=\"fs-idp149580544\">(b) \\({\\text{PH}}_{4}{}^{+}\\)<\/p><p id=\"fs-idp222519424\">(c) P<sub>2<\/sub>H<sub>4<\/sub><\/p><p id=\"fs-idp28824176\">(d) \\({\\text{PO}}_{4}{}^{3-}\\)<\/p><\/div><\/div><div data-type=\"exercise\" id=\"fs-idm2951584\"><div data-type=\"problem\" id=\"fs-idp167269664\"><p id=\"fs-idp93162752\">Complete and balance each of the following chemical equations. (In some cases, there may be more than one correct answer.)<\/p><p id=\"fs-idp111486400\">(a) \\({\\text{P}}_{4}+\\text{Al}\\phantom{\\rule{0.2em}{0ex}}\u27f6\\)<\/p><p id=\"fs-idp104794544\">(b) \\({\\text{P}}_{4}+\\text{Na}\\phantom{\\rule{0.2em}{0ex}}\u27f6\\)<\/p><p id=\"fs-idp54180608\">(c) \\({\\text{P}}_{4}+{\\text{F}}_{2}\\phantom{\\rule{0.2em}{0ex}}\u27f6\\)<\/p><p id=\"fs-idp167891792\">(d) \\({\\text{P}}_{4}+{\\text{Cl}}_{2}\\phantom{\\rule{0.2em}{0ex}}\u27f6\\)<\/p><p id=\"fs-idp187537152\">(e) \\({\\text{P}}_{4}+{\\text{O}}_{2}\\phantom{\\rule{0.2em}{0ex}}\u27f6\\)<\/p><p id=\"fs-idp9601440\">(f) \\({\\text{P}}_{4}{\\text{O}}_{6}+{\\text{O}}_{2}\\phantom{\\rule{0.2em}{0ex}}\u27f6\\)<\/p><\/div><div data-type=\"solution\" id=\"fs-idp70485376\"><p id=\"fs-idp112136256\">(a) \\({\\text{P}}_{4}\\left(s\\right)+\\text{4Al}\\left(s\\right)\\phantom{\\rule{0.2em}{0ex}}\u27f6\\phantom{\\rule{0.2em}{0ex}}\\text{4AlP}\\left(s\\right);\\) (b) \\({\\text{P}}_{4}\\left(s\\right)+\\text{12Na}\\left(s\\right)\\phantom{\\rule{0.2em}{0ex}}\u27f6\\phantom{\\rule{0.2em}{0ex}}{\\text{4Na}}_{3}\\text{P}\\left(s\\right);\\) (c) \\({\\text{P}}_{4}\\left(s\\right)+{\\text{10F}}_{2}\\left(g\\right)\\phantom{\\rule{0.2em}{0ex}}\u27f6\\phantom{\\rule{0.2em}{0ex}}{\\text{4PF}}_{5}\\left(l\\right);\\) (d) \\({\\text{P}}_{4}\\left(s\\right)+{\\text{6Cl}}_{2}\\left(g\\right)\\phantom{\\rule{0.2em}{0ex}}\u27f6\\phantom{\\rule{0.2em}{0ex}}{\\text{4PCl}}_{3}\\left(l\\right)\\) or \\({\\text{P}}_{4}\\left(s\\right)+{\\text{10Cl}}_{2}\\left(g\\right)\\phantom{\\rule{0.2em}{0ex}}\u27f6\\phantom{\\rule{0.2em}{0ex}}{\\text{4PCl}}_{5}\\left(l\\right);\\) (e) \\({\\text{P}}_{4}\\left(s\\right)+{\\text{3O}}_{2}\\left(g\\right)\\phantom{\\rule{0.2em}{0ex}}\u27f6\\phantom{\\rule{0.2em}{0ex}}{\\text{P}}_{4}{\\text{O}}_{6}\\left(s\\right)\\) or \\({\\text{P}}_{4}\\left(s\\right)+{\\text{5O}}_{2}\\left(g\\right)\\phantom{\\rule{0.2em}{0ex}}\u27f6\\phantom{\\rule{0.2em}{0ex}}{\\text{P}}_{4}{\\text{O}}_{10}\\left(s\\right);\\) (f) \\({\\text{P}}_{4}{\\text{O}}_{6}\\left(s\\right)+{\\text{2O}}_{2}\\left(g\\right)\\phantom{\\rule{0.2em}{0ex}}\u27f6\\phantom{\\rule{0.2em}{0ex}}{\\text{P}}_{4}{\\text{O}}_{10}\\left(s\\right)\\)<\/p><\/div><\/div><div data-type=\"exercise\" id=\"fs-idm43491296\"><div data-type=\"problem\" id=\"fs-idm23325584\"><p id=\"fs-idm66070064\">Describe the hybridization of phosphorus in each of the following compounds: P<sub>4<\/sub>O<sub>10<\/sub>, P<sub>4<\/sub>O<sub>6<\/sub>, PH<sub>4<\/sub>I (an ionic compound), PBr<sub>3<\/sub>, H<sub>3<\/sub>PO<sub>4<\/sub>, H<sub>3<\/sub>PO<sub>3<\/sub>, PH<sub>3<\/sub>, and P<sub>2<\/sub>H<sub>4<\/sub>. You may wish to review the chapter on advanced theories of covalent bonding.<\/p><\/div><\/div><div data-type=\"exercise\" id=\"fs-idp54197664\"><div data-type=\"problem\" id=\"fs-idp153098096\"><p id=\"fs-idp219284192\">What volume of 0.200 <em data-effect=\"italics\">M<\/em> NaOH is necessary to neutralize the solution produced by dissolving 2.00 g of PCl<sub>3<\/sub> is an excess of water? Note that when H<sub>3<\/sub>PO<sub>3<\/sub> is titrated under these conditions, only one proton of the acid molecule reacts.<\/p><\/div><div data-type=\"solution\" id=\"fs-idp154481504\"><p id=\"fs-idp25603936\">291 mL<\/p><\/div><\/div><div data-type=\"exercise\" id=\"fs-idm123772752\"><div data-type=\"problem\" id=\"fs-idp61842448\"><p id=\"fs-idp57482752\">How much POCl<sub>3<\/sub> can form from 25.0 g of PCl<sub>5<\/sub> and the appropriate amount of H<sub>2<\/sub>O?<\/p><\/div><\/div><div data-type=\"exercise\" id=\"fs-idp32430320\"><div data-type=\"problem\" id=\"fs-idp99491104\"><p id=\"fs-idp2366736\">How many tons of Ca<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub> are necessary to prepare 5.0 tons of phosphorus if the yield is 90%?<\/p><\/div><div data-type=\"solution\" id=\"fs-idp181983232\"><p id=\"fs-idm45323824\">28 tons<\/p><\/div><\/div><div data-type=\"exercise\" id=\"fs-idp208490096\"><div data-type=\"problem\" id=\"fs-idm44808352\"><p id=\"fs-idp59081184\">Write equations showing the stepwise ionization of phosphorous acid.<\/p><\/div><\/div><div data-type=\"exercise\" id=\"fs-idm54656592\"><div data-type=\"problem\" id=\"fs-idp210409264\"><p id=\"fs-idp69434528\">Draw the Lewis structures and describe the geometry for the following:<\/p><p id=\"fs-idp201777712\">(a) \\({\\text{PF}}_{4}{}^{+}\\)<\/p><p id=\"fs-idm8400224\">(b) PF<sub>5<\/sub><\/p><p id=\"fs-idp11683376\">(c) \\({\\text{PF}}_{6}{}^{-}\\)<\/p><p id=\"fs-idm63931648\">(d) POF<sub>3<\/sub><\/p><\/div><div data-type=\"solution\" id=\"fs-idp5842752\"><p id=\"fs-idp12097488\">(a)<span data-type=\"newline\"><br><\/span><\/p><span data-type=\"media\" id=\"fs-idp215036560\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to four fluorine atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript positive sign outside the brackets. The label, \u201cTetrahedral,\u201d is written under the structure.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise8a_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to four fluorine atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript positive sign outside the brackets. The label, \u201cTetrahedral,\u201d is written under the structure.\"><\/span><p><span data-type=\"newline\"><br><\/span> (b)<span data-type=\"newline\"><br><\/span><\/p><span data-type=\"media\" id=\"fs-idp42036672\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to five fluorine atoms, each with three lone pairs of electrons. The label, \u201cTrigonal bipyramidal,\u201d is written under the structure.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise8b_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to five fluorine atoms, each with three lone pairs of electrons. The label, \u201cTrigonal bipyramidal,\u201d is written under the structure.\"><\/span><p><span data-type=\"newline\"><br><\/span> (c)<span data-type=\"newline\"><br><\/span><\/p><span data-type=\"media\" id=\"fs-idp41412448\" data-alt=\"A Lewis structure shows a phosphorus atom single bonded to six fluorine atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript negative sign outside the brackets. The label, \u201cOctahedral,\u201d is written under the structure.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise8c_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"A Lewis structure shows a phosphorus atom single bonded to six fluorine atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript negative sign outside the brackets. The label, \u201cOctahedral,\u201d is written under the structure.\"><\/span><p><span data-type=\"newline\"><br><\/span> (d)<span data-type=\"newline\"><br><\/span><\/p><span data-type=\"media\" id=\"fs-idm23148096\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to three fluorine atoms, each with three lone pairs of electrons. The phosphorus atom is also double bonded to an oxygen atom with two lone pairs of electrons. The label, \u201cTetrahedral,\u201d is written under the structure.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise8d_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to three fluorine atoms, each with three lone pairs of electrons. The phosphorus atom is also double bonded to an oxygen atom with two lone pairs of electrons. The label, \u201cTetrahedral,\u201d is written under the structure.\"><\/span><\/div><\/div><div data-type=\"exercise\" id=\"fs-idm55936272\"><div data-type=\"problem\" id=\"fs-idp51272480\"><p id=\"fs-idp27849968\">Why does phosphorous acid form only two series of salts, even though the molecule contains three hydrogen atoms?<\/p><\/div><\/div><div data-type=\"exercise\" id=\"fs-idp5265904\"><div data-type=\"problem\" id=\"fs-idm14862528\"><p id=\"fs-idp219241728\">Assign an oxidation state to phosphorus in each of the following:<\/p><p id=\"fs-idp97854512\">(a) NaH<sub>2<\/sub>PO<sub>3<\/sub><\/p><p id=\"fs-idm63479760\">(b) PF<sub>5<\/sub><\/p><p id=\"fs-idm869408\">(c) P<sub>4<\/sub>O<sub>6<\/sub><\/p><p id=\"fs-idp20195696\">(d) K<sub>3<\/sub>PO<sub>4<\/sub><\/p><p id=\"fs-idp24284416\">(e) Na<sub>3<\/sub>P<\/p><p id=\"fs-idp208579360\">(f) Na<sub>4<\/sub>P<sub>2<\/sub>O<sub>7<\/sub><\/p><\/div><div data-type=\"solution\" id=\"fs-idm62423664\"><p id=\"fs-idp9609632\">(a) P = 3+; (b) P = 5+; (c) P = 3+; (d) P = 5+; (e) P = 3\u2212; (f) P = 5+<\/p><\/div><\/div><div data-type=\"exercise\" id=\"fs-idp126473504\"><div data-type=\"problem\" id=\"fs-idp53092352\"><p id=\"fs-idp46924640\">Phosphoric acid, one of the acids used in some cola drinks, is produced by the reaction of phosphorus(V) oxide, an acidic oxide, with water. Phosphorus(V) oxide is prepared by the combustion of phosphorus.<\/p><p id=\"fs-idm28349936\">(a) Write the empirical formula of phosphorus(V) oxide.<\/p><p id=\"fs-idm64288464\">(b) What is the molecular formula of phosphorus(V) oxide if the molar mass is about 280.<\/p><p id=\"fs-idp40764960\">(c) Write balanced equations for the production of phosphorus(V) oxide and phosphoric acid.<\/p><p id=\"fs-idp1024\">(d) Determine the mass of phosphorus required to make 1.00 \\(\u00d7\\) 10<sup>4<\/sup> kg of phosphoric acid, assuming a yield of 98.85%.<\/p><\/div><\/div><\/div>","rendered":"<div class=\"textbox textbox--learning-objectives\">\n<h3>Learning Objectives<\/h3>\n<p>By the end of this section, you will be able to: <\/p>\n<ul>\n<li>Describe the properties, preparation, and uses of phosphorus<\/li>\n<\/ul>\n<\/div>\n<p id=\"fs-idp52194704\">The industrial preparation of phosphorus is by heating calcium phosphate, obtained from phosphate rock, with sand and coke:<\/p>\n<div data-type=\"equation\" id=\"fs-idp51821104\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-a37d71c8c0acf88a7d63e3859a384ad2_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#50;&#67;&#97;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#108;&#101;&#102;&#116;&#40;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#79;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#125;&#95;&#123;&#50;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#54;&#83;&#105;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#48;&#67;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#115;&#116;&#97;&#99;&#107;&#114;&#101;&#108;&#123;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#52;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&Delta;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#52;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#125;&#123;&#92;&#116;&#111;&#32;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#54;&#67;&#97;&#83;&#105;&#79;&#125;&#125;&#95;&#123;&#51;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#108;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#48;&#67;&#79;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#103;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#103;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"19\" width=\"572\" style=\"vertical-align: -5px;\" \/><\/div>\n<p id=\"fs-idp5816832\">The phosphorus distills out of the furnace and is condensed into a solid or burned to form P<sub>4<\/sub>O<sub>10<\/sub>. The preparation of many other phosphorus compounds begins with P<sub>4<\/sub>O<sub>10<\/sub>. The acids and phosphates are useful as fertilizers and in the chemical industry. Other uses are in the manufacture of special alloys such as ferrophosphorus and phosphor bronze. Phosphorus is important in making pesticides, matches, and some plastics. Phosphorus is an active nonmetal. In compounds, phosphorus usually occurs in oxidation states of 3\u2212, 3+, and 5+. Phosphorus exhibits oxidation numbers that are unusual for a group 15 element in compounds that contain phosphorus-phosphorus bonds; examples include diphosphorus tetrahydride, H<sub>2<\/sub>P-PH<sub>2<\/sub>, and tetraphosphorus trisulfide, P<sub>4<\/sub>S<sub>3<\/sub>, illustrated in <a href=\"#CNX_Chem_18_08_P4S3\" class=\"autogenerated-content\">(Figure)<\/a>.<\/p>\n<div class=\"scaled-down\" id=\"CNX_Chem_18_08_P4S3\">\n<div class=\"bc-figcaption figcaption\">P<sub>4<\/sub>S<sub>3<\/sub> is a component of the heads of strike-anywhere matches.<\/div>\n<p><span data-type=\"media\" id=\"fs-idm5144976\" data-alt=\"A ball-and-stick model is shown. Three orange atoms labeled \u201cP\u201d are single bonded together in a triangle shape. Each \u201cP\u201d is single bonded to yellow atoms labeled \u201cS,\u201d which are each single bonded to one other orange atom labeled \u201cP.\u201d\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2019\/07\/CNX_Chem_18_08_P4S3.jpg\" data-media-type=\"image\/jpeg\" alt=\"A ball-and-stick model is shown. Three orange atoms labeled \u201cP\u201d are single bonded together in a triangle shape. Each \u201cP\u201d is single bonded to yellow atoms labeled \u201cS,\u201d which are each single bonded to one other orange atom labeled \u201cP.\u201d\" \/><\/span><\/div>\n<div class=\"bc-section section\" data-depth=\"1\" id=\"fs-idm31898272\">\n<h3 data-type=\"title\">Phosphorus Oxygen Compounds<\/h3>\n<p id=\"fs-idp85748768\">Phosphorus forms two common oxides, phosphorus(III) oxide (or tetraphosphorus hexaoxide), P<sub>4<\/sub>O<sub>6<\/sub>, and phosphorus(V) oxide (or tetraphosphorus decaoxide), P<sub>4<\/sub>O<sub>10<\/sub>, both shown in <a href=\"#CNX_Chem_18_08_P4O6P4O10\" class=\"autogenerated-content\">(Figure)<\/a>. Phosphorus(III) oxide is a white crystalline solid with a garlic-like odor. Its vapor is very poisonous. It oxidizes slowly in air and inflames when heated to 70 \u00b0C, forming P<sub>4<\/sub>O<sub>10<\/sub>. Phosphorus(III) oxide dissolves slowly in cold water to form phosphorous acid, H<sub>3<\/sub>PO<sub>3<\/sub>.<\/p>\n<div class=\"scaled-down\" id=\"CNX_Chem_18_08_P4O6P4O10\">\n<div class=\"bc-figcaption figcaption\">This image shows the molecular structures of P<sub>4<\/sub>O<sub>6<\/sub> (left) and P<sub>4<\/sub>O<sub>10<\/sub> (right).<\/div>\n<p><span data-type=\"media\" id=\"fs-idp57250912\" data-alt=\"Two ball-and-stick models are shown. In the left model, three orange atoms labeled, \u201cP,\u201d are single bonded to red atoms labeled, \u201cO,\u201d in an alternating, six-sided ring structure. Each of the orange atoms are also single bonded to another red atom, which are in turn single bonded to a single orange atom. The right model shows three orange atoms labeled, \u201cP,\u201d single bonded to red atoms labeled, \u201cO,\u201d in an alternating, six-sided ring structure. Each of the orange atoms are also single bonded to two more red atoms, one in an upward position and one facing the outside of the molecule. The upward red atoms are single bonded to a single orange atom which is single bonded to a final red atom.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_P4O6P4O10.jpg\" data-media-type=\"image\/jpeg\" alt=\"Two ball-and-stick models are shown. In the left model, three orange atoms labeled, \u201cP,\u201d are single bonded to red atoms labeled, \u201cO,\u201d in an alternating, six-sided ring structure. Each of the orange atoms are also single bonded to another red atom, which are in turn single bonded to a single orange atom. The right model shows three orange atoms labeled, \u201cP,\u201d single bonded to red atoms labeled, \u201cO,\u201d in an alternating, six-sided ring structure. Each of the orange atoms are also single bonded to two more red atoms, one in an upward position and one facing the outside of the molecule. The upward red atoms are single bonded to a single orange atom which is single bonded to a final red atom.\" \/><\/span><\/div>\n<p id=\"fs-idm7162480\">Phosphorus(V) oxide, P<sub>4<\/sub>O<sub>10<\/sub>, is a white powder that is prepared by burning phosphorus in excess oxygen. Its enthalpy of formation is very high (\u22122984 kJ), and it is quite stable and a very poor oxidizing agent. Dropping P<sub>4<\/sub>O<sub>10<\/sub> into water produces a hissing sound, heat, and orthophosphoric acid:<\/p>\n<div data-type=\"equation\" id=\"fs-idp704592\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-4b526b8f98b2de4df9cb53679fe150f9_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#95;&#123;&#49;&#48;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#54;&#72;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#108;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#52;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#79;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"268\" style=\"vertical-align: -4px;\" \/><\/div>\n<p id=\"fs-idm64278832\">Because of its great affinity for water, phosphorus(V) oxide is an excellent drying agent for gases and solvents, and for removing water from many compounds.<\/p>\n<\/div>\n<div class=\"bc-section section\" data-depth=\"1\" id=\"fs-idm11573280\">\n<h3 data-type=\"title\">Phosphorus Halogen Compounds<\/h3>\n<p id=\"fs-idp70568512\">Phosphorus will react directly with the halogens, forming trihalides, PX<sub>3<\/sub>, and pentahalides, PX<sub>5<\/sub>. The trihalides are much more stable than the corresponding nitrogen trihalides; nitrogen pentahalides do not form because of nitrogen\u2019s inability to form more than four bonds.<\/p>\n<p id=\"fs-idp182518880\">The chlorides PCl<sub>3<\/sub> and PCl<sub>5<\/sub>, both shown in <a href=\"#CNX_Chem_18_08_PCl3PCl5\" class=\"autogenerated-content\">(Figure)<\/a>, are the most important halides of phosphorus. Phosphorus trichloride is a colorless liquid that is prepared by passing chlorine over molten phosphorus. Phosphorus pentachloride is an off-white solid that is prepared by oxidizing the trichloride with excess chlorine. The pentachloride sublimes when warmed and forms an equilibrium with the trichloride and chlorine when heated.<\/p>\n<div class=\"scaled-down\" id=\"CNX_Chem_18_08_PCl3PCl5\">\n<div class=\"bc-figcaption figcaption\">This image shows the molecular structure of PCl<sub>3<\/sub> (left) and PCl<sub>5<\/sub> (right) in the gas phase.<\/div>\n<p><span data-type=\"media\" id=\"fs-idp189314192\" data-alt=\"Two ball-and-stick models are shown. In the left model, an orange atom labeled, \u201cP,\u201d is single bonded to three green atoms labeled, \u201cC l.\u201d The right model shows an orange atom labeled, \u201cP,\u201d single bonded to five green atoms labeled, \u201cC l.\u201d\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_PCl3PCl5.jpg\" data-media-type=\"image\/jpeg\" alt=\"Two ball-and-stick models are shown. In the left model, an orange atom labeled, \u201cP,\u201d is single bonded to three green atoms labeled, \u201cC l.\u201d The right model shows an orange atom labeled, \u201cP,\u201d single bonded to five green atoms labeled, \u201cC l.\u201d\" \/><\/span><\/div>\n<p id=\"fs-idp21181152\">Like most other nonmetal halides, both phosphorus chlorides react with an excess of water and yield hydrogen chloride and an oxyacid: PCl<sub>3<\/sub> yields phosphorous acid H<sub>3<\/sub>PO<sub>3<\/sub> and PCl<sub>5<\/sub> yields phosphoric acid, H<sub>3<\/sub>PO<sub>4<\/sub>.<\/p>\n<p id=\"fs-idm44217280\">The pentahalides of phosphorus are Lewis acids because of the empty valence <em data-effect=\"italics\">d<\/em> orbitals of phosphorus. These compounds readily react with halide ions (Lewis bases) to give the anion <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-1cd87317855c44a486569801632dc694_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#88;&#125;&#125;&#95;&#123;&#54;&#125;&#123;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#8722;&#125;&#125;&#46;\" title=\"Rendered by QuickLaTeX.com\" height=\"16\" width=\"38\" style=\"vertical-align: -3px;\" \/> Whereas phosphorus pentafluoride is a molecular compound in all states, X-ray studies show that solid phosphorus pentachloride is an ionic compound, <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-f5a813863c9a57e13f54fba761344375_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#108;&#101;&#102;&#116;&#91;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#67;&#108;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#93;&#92;&#108;&#101;&#102;&#116;&#91;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#67;&#108;&#125;&#125;&#95;&#123;&#54;&#125;&#123;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#8722;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#93;&#44;\" title=\"Rendered by QuickLaTeX.com\" height=\"20\" width=\"115\" style=\"vertical-align: -5px;\" \/> as are phosphorus pentabromide, <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-28a86c56faf93aeaf51f859272729274_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#108;&#101;&#102;&#116;&#91;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#66;&#114;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#93;\" title=\"Rendered by QuickLaTeX.com\" height=\"20\" width=\"57\" style=\"vertical-align: -5px;\" \/>[Br<sup>\u2212<\/sup>], and phosphorus pentaiodide, <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-1905622bd6488e20a6e21475e7b03f36_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#108;&#101;&#102;&#116;&#91;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#73;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#93;\" title=\"Rendered by QuickLaTeX.com\" height=\"20\" width=\"44\" style=\"vertical-align: -5px;\" \/>[I<sup>\u2212<\/sup>].<\/p>\n<\/div>\n<div class=\"summary\" data-depth=\"1\" id=\"fs-idp183301136\">\n<h3 data-type=\"title\">Key Concepts and Summary<\/h3>\n<p id=\"fs-idp219295376\">Phosphorus (group 15) commonly exhibits oxidation states of 3\u2212 with active metals and of 3+ and 5+ with more electronegative nonmetals. The halogens and oxygen will oxidize phosphorus. The oxides are phosphorus(V) oxide, P<sub>4<\/sub>O<sub>10<\/sub>, and phosphorus(III) oxide, P<sub>4<\/sub>O<sub>6<\/sub>. The two common methods for preparing orthophosphoric acid, H<sub>3<\/sub>PO<sub>4<\/sub>, are either the reaction of a phosphate with sulfuric acid or the reaction of water with phosphorus(V) oxide. Orthophosphoric acid is a triprotic acid that forms three types of salts.<\/p>\n<\/div>\n<div class=\"exercises\" data-depth=\"1\" id=\"fs-idp185176672\">\n<h3 data-type=\"title\">Chemistry End of Chapter Exercises<\/h3>\n<div data-type=\"exercise\" id=\"fs-idp52847792\">\n<div data-type=\"problem\" id=\"fs-idp188554560\">\n<p id=\"fs-idm63439584\">Write the Lewis structure for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry.<\/p>\n<p id=\"fs-idp210380672\">(a) PH<sub>3<\/sub><\/p>\n<p id=\"fs-idp153159872\">(b) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-aa7808b0902c5cbfadf907a69918d5a6_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#72;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#125;&#94;&#123;&#43;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"43\" style=\"vertical-align: -3px;\" \/><\/p>\n<p id=\"fs-idm27147360\">(c) P<sub>2<\/sub>H<sub>4<\/sub><\/p>\n<p id=\"fs-idm44280352\">(d) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-06bd1e68e4dd8bc1d66de678152b6fd9_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#79;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#125;&#94;&#123;&#51;&#45;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"51\" style=\"vertical-align: -3px;\" \/><\/p>\n<p id=\"fs-idp332959120\">(e) PF<sub>5<\/sub><\/p>\n<\/div>\n<div data-type=\"solution\" id=\"fs-idm55639488\">\n<p id=\"fs-idm28792464\">(a)<span data-type=\"newline\"><br \/><\/span><\/p>\n<p><span data-type=\"media\" id=\"fs-idm55213168\" data-alt=\"This Lewis structure shows a phosphorus atom with a lone pair of electrons single bonded to three hydrogen atoms.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise1a_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom with a lone pair of electrons single bonded to three hydrogen atoms.\" \/><\/span><\/p>\n<p><span data-type=\"newline\"><br \/><\/span> (b)<span data-type=\"newline\"><br \/><\/span><\/p>\n<p><span data-type=\"media\" id=\"fs-idm1170240\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to four hydrogen atoms. The structure is surrounded by brackets and has a superscript positive sign outside the brackets.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise1b_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to four hydrogen atoms. The structure is surrounded by brackets and has a superscript positive sign outside the brackets.\" \/><\/span><\/p>\n<p><span data-type=\"newline\"><br \/><\/span> (c)<span data-type=\"newline\"><br \/><\/span><\/p>\n<p><span data-type=\"media\" id=\"fs-idp56334352\" data-alt=\"This Lewis structure shows two phosphorus atoms, each with a lone pair of electrons, single bonded to one another. Each phosphorus atom is also single bonded to two hydrogen atoms.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise1c_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows two phosphorus atoms, each with a lone pair of electrons, single bonded to one another. Each phosphorus atom is also single bonded to two hydrogen atoms.\" \/><\/span><\/p>\n<p><span data-type=\"newline\"><br \/><\/span> (d)<span data-type=\"newline\"><br \/><\/span><\/p>\n<p><span data-type=\"media\" id=\"fs-idm66638800\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to four oxygen atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript 3 negative sign outside the brackets.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise1d_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to four oxygen atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript 3 negative sign outside the brackets.\" \/><\/span><\/p>\n<p><span data-type=\"newline\"><br \/><\/span> (e)<span data-type=\"newline\"><br \/><\/span><\/p>\n<p><span data-type=\"media\" id=\"fs-idm5269184\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to five fluorine atoms, each with three lone pairs of electrons.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise1e_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to five fluorine atoms, each with three lone pairs of electrons.\" \/><\/span><\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idp101864208\">\n<div data-type=\"problem\" id=\"fs-idp20141648\">\n<p id=\"fs-idp227455632\">Describe the molecular structure of each of the following molecules or ions listed. You may wish to review the chapter on chemical bonding and molecular geometry.<\/p>\n<p id=\"fs-idp157002384\">(a) PH<sub>3<\/sub><\/p>\n<p id=\"fs-idp149580544\">(b) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-aa7808b0902c5cbfadf907a69918d5a6_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#72;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#125;&#94;&#123;&#43;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"43\" style=\"vertical-align: -3px;\" \/><\/p>\n<p id=\"fs-idp222519424\">(c) P<sub>2<\/sub>H<sub>4<\/sub><\/p>\n<p id=\"fs-idp28824176\">(d) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-06bd1e68e4dd8bc1d66de678152b6fd9_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#79;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#125;&#94;&#123;&#51;&#45;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"51\" style=\"vertical-align: -3px;\" \/><\/p>\n<\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idm2951584\">\n<div data-type=\"problem\" id=\"fs-idp167269664\">\n<p id=\"fs-idp93162752\">Complete and balance each of the following chemical equations. (In some cases, there may be more than one correct answer.)<\/p>\n<p id=\"fs-idp111486400\">(a) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-c8084d634d888349ffde406a5f1bbee7_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#65;&#108;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;\" title=\"Rendered by QuickLaTeX.com\" height=\"16\" width=\"59\" style=\"vertical-align: -3px;\" \/><\/p>\n<p id=\"fs-idp104794544\">(b) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-7eb713424bd9a32228465d891abc3110_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#78;&#97;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;\" title=\"Rendered by QuickLaTeX.com\" height=\"15\" width=\"63\" style=\"vertical-align: -3px;\" \/><\/p>\n<p id=\"fs-idp54180608\">(c) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-549ed13520c20838fc1e7a814ca47735_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#70;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;\" title=\"Rendered by QuickLaTeX.com\" height=\"15\" width=\"60\" style=\"vertical-align: -3px;\" \/><\/p>\n<p id=\"fs-idp167891792\">(d) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-6453dee6de614a074308411ece77e850_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#108;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;\" title=\"Rendered by QuickLaTeX.com\" height=\"16\" width=\"66\" style=\"vertical-align: -3px;\" \/><\/p>\n<p id=\"fs-idp187537152\">(e) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-832114265652d9b77764937b1619c7ec_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;\" title=\"Rendered by QuickLaTeX.com\" height=\"15\" width=\"62\" style=\"vertical-align: -3px;\" \/><\/p>\n<p id=\"fs-idp9601440\">(f) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-d9f94b804725d2bb5fe018083f8e2685_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#95;&#123;&#54;&#125;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;\" title=\"Rendered by QuickLaTeX.com\" height=\"15\" width=\"84\" style=\"vertical-align: -3px;\" \/><\/p>\n<\/div>\n<div data-type=\"solution\" id=\"fs-idp70485376\">\n<p id=\"fs-idp112136256\">(a) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-76b58f7017e05a6c9439bd2f2e40ef4e_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#52;&#65;&#108;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#52;&#65;&#108;&#80;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#59;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"200\" style=\"vertical-align: -4px;\" \/> (b) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-919ab695fa4388cea04c7ae7a6a5ec51_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#50;&#78;&#97;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#52;&#78;&#97;&#125;&#125;&#95;&#123;&#51;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#59;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"224\" style=\"vertical-align: -4px;\" \/> (c) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-43cbdea9a2609380654be18c29830f24_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#48;&#70;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#103;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#52;&#80;&#70;&#125;&#125;&#95;&#123;&#53;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#108;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#59;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"209\" style=\"vertical-align: -4px;\" \/> (d) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-a00898e5830584d3804298cf5f8bfc3d_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#54;&#67;&#108;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#103;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#52;&#80;&#67;&#108;&#125;&#125;&#95;&#123;&#51;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#108;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"204\" style=\"vertical-align: -4px;\" \/> or <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-86135c9737a5164b3726c4e868ff6ead_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#48;&#67;&#108;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#103;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#52;&#80;&#67;&#108;&#125;&#125;&#95;&#123;&#53;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#108;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#59;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"221\" style=\"vertical-align: -4px;\" \/> (e) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-829733ed03349ee752a27b2f6089f560_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#51;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#103;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#95;&#123;&#54;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"198\" style=\"vertical-align: -4px;\" \/> or <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-5612baa627806511546dd92733ebbe1f_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#53;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#103;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#95;&#123;&#49;&#48;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#59;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"213\" style=\"vertical-align: -4px;\" \/> (f) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-c39db6859f4aac3f2edac5883e69e8f8_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#95;&#123;&#54;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#50;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#103;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#10230;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#95;&#123;&#49;&#48;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#115;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"226\" style=\"vertical-align: -4px;\" \/><\/p>\n<\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idm43491296\">\n<div data-type=\"problem\" id=\"fs-idm23325584\">\n<p id=\"fs-idm66070064\">Describe the hybridization of phosphorus in each of the following compounds: P<sub>4<\/sub>O<sub>10<\/sub>, P<sub>4<\/sub>O<sub>6<\/sub>, PH<sub>4<\/sub>I (an ionic compound), PBr<sub>3<\/sub>, H<sub>3<\/sub>PO<sub>4<\/sub>, H<sub>3<\/sub>PO<sub>3<\/sub>, PH<sub>3<\/sub>, and P<sub>2<\/sub>H<sub>4<\/sub>. You may wish to review the chapter on advanced theories of covalent bonding.<\/p>\n<\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idp54197664\">\n<div data-type=\"problem\" id=\"fs-idp153098096\">\n<p id=\"fs-idp219284192\">What volume of 0.200 <em data-effect=\"italics\">M<\/em> NaOH is necessary to neutralize the solution produced by dissolving 2.00 g of PCl<sub>3<\/sub> is an excess of water? Note that when H<sub>3<\/sub>PO<sub>3<\/sub> is titrated under these conditions, only one proton of the acid molecule reacts.<\/p>\n<\/div>\n<div data-type=\"solution\" id=\"fs-idp154481504\">\n<p id=\"fs-idp25603936\">291 mL<\/p>\n<\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idm123772752\">\n<div data-type=\"problem\" id=\"fs-idp61842448\">\n<p id=\"fs-idp57482752\">How much POCl<sub>3<\/sub> can form from 25.0 g of PCl<sub>5<\/sub> and the appropriate amount of H<sub>2<\/sub>O?<\/p>\n<\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idp32430320\">\n<div data-type=\"problem\" id=\"fs-idp99491104\">\n<p id=\"fs-idp2366736\">How many tons of Ca<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub> are necessary to prepare 5.0 tons of phosphorus if the yield is 90%?<\/p>\n<\/div>\n<div data-type=\"solution\" id=\"fs-idp181983232\">\n<p id=\"fs-idm45323824\">28 tons<\/p>\n<\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idp208490096\">\n<div data-type=\"problem\" id=\"fs-idm44808352\">\n<p id=\"fs-idp59081184\">Write equations showing the stepwise ionization of phosphorous acid.<\/p>\n<\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idm54656592\">\n<div data-type=\"problem\" id=\"fs-idp210409264\">\n<p id=\"fs-idp69434528\">Draw the Lewis structures and describe the geometry for the following:<\/p>\n<p id=\"fs-idp201777712\">(a) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-e0fd6518b6c2f9989332a4a292273d5a_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#70;&#125;&#125;&#95;&#123;&#52;&#125;&#123;&#125;&#94;&#123;&#43;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"41\" style=\"vertical-align: -3px;\" \/><\/p>\n<p id=\"fs-idm8400224\">(b) PF<sub>5<\/sub><\/p>\n<p id=\"fs-idp11683376\">(c) <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-c7fa9adc197a28b855e13c5ded027039_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#80;&#70;&#125;&#125;&#95;&#123;&#54;&#125;&#123;&#125;&#94;&#123;&#45;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"15\" width=\"41\" style=\"vertical-align: -3px;\" \/><\/p>\n<p id=\"fs-idm63931648\">(d) POF<sub>3<\/sub><\/p>\n<\/div>\n<div data-type=\"solution\" id=\"fs-idp5842752\">\n<p id=\"fs-idp12097488\">(a)<span data-type=\"newline\"><br \/><\/span><\/p>\n<p><span data-type=\"media\" id=\"fs-idp215036560\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to four fluorine atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript positive sign outside the brackets. The label, \u201cTetrahedral,\u201d is written under the structure.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise8a_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to four fluorine atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript positive sign outside the brackets. The label, \u201cTetrahedral,\u201d is written under the structure.\" \/><\/span><\/p>\n<p><span data-type=\"newline\"><br \/><\/span> (b)<span data-type=\"newline\"><br \/><\/span><\/p>\n<p><span data-type=\"media\" id=\"fs-idp42036672\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to five fluorine atoms, each with three lone pairs of electrons. The label, \u201cTrigonal bipyramidal,\u201d is written under the structure.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise8b_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to five fluorine atoms, each with three lone pairs of electrons. The label, \u201cTrigonal bipyramidal,\u201d is written under the structure.\" \/><\/span><\/p>\n<p><span data-type=\"newline\"><br \/><\/span> (c)<span data-type=\"newline\"><br \/><\/span><\/p>\n<p><span data-type=\"media\" id=\"fs-idp41412448\" data-alt=\"A Lewis structure shows a phosphorus atom single bonded to six fluorine atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript negative sign outside the brackets. The label, \u201cOctahedral,\u201d is written under the structure.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise8c_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"A Lewis structure shows a phosphorus atom single bonded to six fluorine atoms, each with three lone pairs of electrons. The structure is surrounded by brackets and has a superscript negative sign outside the brackets. The label, \u201cOctahedral,\u201d is written under the structure.\" \/><\/span><\/p>\n<p><span data-type=\"newline\"><br \/><\/span> (d)<span data-type=\"newline\"><br \/><\/span><\/p>\n<p><span data-type=\"media\" id=\"fs-idm23148096\" data-alt=\"This Lewis structure shows a phosphorus atom single bonded to three fluorine atoms, each with three lone pairs of electrons. The phosphorus atom is also double bonded to an oxygen atom with two lone pairs of electrons. The label, \u201cTetrahedral,\u201d is written under the structure.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/unromantest\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_18_08_Exercise8d_img.jpg\" data-media-type=\"image\/jpeg\" alt=\"This Lewis structure shows a phosphorus atom single bonded to three fluorine atoms, each with three lone pairs of electrons. The phosphorus atom is also double bonded to an oxygen atom with two lone pairs of electrons. The label, \u201cTetrahedral,\u201d is written under the structure.\" \/><\/span><\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idm55936272\">\n<div data-type=\"problem\" id=\"fs-idp51272480\">\n<p id=\"fs-idp27849968\">Why does phosphorous acid form only two series of salts, even though the molecule contains three hydrogen atoms?<\/p>\n<\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idp5265904\">\n<div data-type=\"problem\" id=\"fs-idm14862528\">\n<p id=\"fs-idp219241728\">Assign an oxidation state to phosphorus in each of the following:<\/p>\n<p id=\"fs-idp97854512\">(a) NaH<sub>2<\/sub>PO<sub>3<\/sub><\/p>\n<p id=\"fs-idm63479760\">(b) PF<sub>5<\/sub><\/p>\n<p id=\"fs-idm869408\">(c) P<sub>4<\/sub>O<sub>6<\/sub><\/p>\n<p id=\"fs-idp20195696\">(d) K<sub>3<\/sub>PO<sub>4<\/sub><\/p>\n<p id=\"fs-idp24284416\">(e) Na<sub>3<\/sub>P<\/p>\n<p id=\"fs-idp208579360\">(f) Na<sub>4<\/sub>P<sub>2<\/sub>O<sub>7<\/sub><\/p>\n<\/div>\n<div data-type=\"solution\" id=\"fs-idm62423664\">\n<p id=\"fs-idp9609632\">(a) P = 3+; (b) P = 5+; (c) P = 3+; (d) P = 5+; (e) P = 3\u2212; (f) P = 5+<\/p>\n<\/div>\n<\/div>\n<div data-type=\"exercise\" id=\"fs-idp126473504\">\n<div data-type=\"problem\" id=\"fs-idp53092352\">\n<p id=\"fs-idp46924640\">Phosphoric acid, one of the acids used in some cola drinks, is produced by the reaction of phosphorus(V) oxide, an acidic oxide, with water. Phosphorus(V) oxide is prepared by the combustion of phosphorus.<\/p>\n<p id=\"fs-idm28349936\">(a) Write the empirical formula of phosphorus(V) oxide.<\/p>\n<p id=\"fs-idm64288464\">(b) What is the molecular formula of phosphorus(V) oxide if the molar mass is about 280.<\/p>\n<p id=\"fs-idp40764960\">(c) Write balanced equations for the production of phosphorus(V) oxide and phosphoric acid.<\/p>\n<p id=\"fs-idp1024\">(d) Determine the mass of phosphorus required to make 1.00 <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-c9448d0c3ab42155fc705b58fe04b3b0_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&times;\" title=\"Rendered by QuickLaTeX.com\" height=\"1\" width=\"1\" style=\"vertical-align: 0px;\" \/> 10<sup>4<\/sup> kg of phosphoric acid, assuming a yield of 98.85%.<\/p>\n<\/div>\n<\/div>\n<\/div>\n","protected":false},"author":801,"menu_order":9,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-1139","chapter","type-chapter","status-publish","hentry"],"part":1053,"_links":{"self":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1139","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/users\/801"}],"version-history":[{"count":1,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1139\/revisions"}],"predecessor-version":[{"id":1140,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1139\/revisions\/1140"}],"part":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/parts\/1053"}],"metadata":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1139\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/media?parent=1139"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapter-type?post=1139"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/contributor?post=1139"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/license?post=1139"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}