Kafli 18 - Svör við æfingum

Svör við æfingum

18.1 Lotubundnir eiginleikar

Alkalímálmarnir hafa allir eina s-rafeind í ystu skel sinni. Aftur á móti hafa jarðalkalímálmar fullskipað s-undirhvolf í ystu skel sinni. Almennt hvarfast alkalímálmar hraðar og eru hvarfgjarnari en samsvarandi jarðalkalímálmar í sömu lotu.

$\begin{aligned} \text{Na}+{\text{I}}_{2}\, \longrightarrow \, \text{2NaI} \\ \text{2Na}+\text{Se}\, \longrightarrow \, {\text{Na}}_{2}\text{Se} \\ \text{2Na}+{\text{O}}_{2}\, \longrightarrow \, {\text{Na}}_{2}{\text{O}}_{2} \end{aligned}$
$\begin{aligned} \text{Sr}+{\text{I}}_{2}\, \longrightarrow \, {\text{SrI}}_{2} \\ \text{Sr}+\text{Se}\, \longrightarrow \, \text{SrSe} \\ \text{2Sr}+{\text{O}}_{2}\, \longrightarrow \, \text{2SrO} \end{aligned}$
$\begin{aligned} \text{2Al}+{\text{3I}}_{2}\, \longrightarrow \, {\text{2AlI}}_{3} \\ \text{2Al}+\text{3Se}\, \longrightarrow \, {\text{Al}}_{2}{\text{Se}}_{3} \\ \text{4Al}+{\text{3O}}_{2}\, \longrightarrow \, {\text{2Al}}_{2}{\text{O}}_{3} \end{aligned}$

Mögulegar leiðir til að greina á milli efnanna tveggja eru meðal annars innrauð litrófsgreining með samanburði við þekkt efnasambönd, logapróf sem gefur einkennandi gulan lit fyrir natríum (strontíum hefur rauðan loga) eða samanburður á leysni þeirra í vatni. Við 20 °C leysist NaCl upp að ${\frac{{\text{35,7 g}}}{{\text{100 mL}}}}$ samanborið við ${\frac{{\text{53,8 g}}}{{\text{100 mL}}}}$ fyrir SrCl₂. Upphitun í 100 °C er auðveld prófun þar sem leysni NaCl er ${\frac{{\text{39,12 g}}}{{\text{100 mL}}},}$ en leysni SrCl₂ er ${\frac{{\text{100,8 g}}}{{\text{100 mL}}}.}$ . Eðlismassaákvörðun á föstu efni getur stundum verið erfið, en munurinn er nægur (2,165 g/ml fyrir NaCl og 3,052 g/ml fyrir SrCl₂) til að þessi aðferð væri raunhæf og kannski auðveldasta og ódýrasta prófið til að framkvæma.

(a) ${\text{2Sr}(s)+{\text{O}}_{2}(g)\, \longrightarrow \, \text{2SrO}(s);}$ (b) ${\text{Sr}(s)+\text{2HBr}(g)\, \longrightarrow \, {{\text{SrBr}}}_{2}(s)+{\text{H}}_{2}(g);}$ (c) ${\text{Sr}(s)+{\text{H}}_{2}(g)\, \longrightarrow \, {{\text{SrH}}}_{2}(s);}$ (d) ${\text{6Sr}(s)+{\text{P}}_{4}(s)\, \longrightarrow \, {{\text{2Sr}}}_{3}{\text{P}}_{2}(s);}$ (e) ${\text{Sr}(s)+{{\text{2H}}}_{2}\text{O}(l)\, \longrightarrow \, \text{Sr}{{(\text{OH})}}_{2}(aq)+{\text{H}}_{2}(g)}$

11 pund

Já, tin hvarfast við saltsýru og myndar vetnisgas.

Í PbCl₂ er tengið jónískt, eins og bræðslumark þess, 501 °C, gefur til kynna. Í PbCl₄ er tengið samgilt, sem sést af því að það er óstöðugur vökvi við stofuhita.

18.2 Tilvist og framleiðsla dæmigerðra málma

${\text{2CsCl}(l)+\text{Ca}(g)\, \overset{{\, \begin{aligned} {\text{countercurrent}} \\ {\text{fractionating}} \\ {\text{tower}} \end{aligned}}}{\rightarrow}\, \text{2Cs}(g)+{{\text{CaCl}}}_{2}(l)}$

Katóða (afoxun): ${{{\text{2Li}}}^{+}+{{\text{2e}}}^{-}\, \longrightarrow \, \text{2Li}(l)\text{;}}$ Anóða (oxun): ${{{\text{2Cl}}}^{-}\, \longrightarrow \, {{\text{Cl}}}_{2}(g)+{{\text{2e}}}^{\text{−}};}$ Heildarefnahvarf: ${{{\text{2Li}}}^{+}+{{\text{2Cl}}}^{-}\, \longrightarrow \, \text{2Li}(l)+{\text{Cl}}_{2}(g)}$

0,5035 g H₂

Þrátt fyrir hvarfgirni sína er hægt að nota magnesíum í mannvirkjagerð, jafnvel þótt magnesíumið komist í snertingu við loga, vegna þess að verndandi oxíðhúð myndast sem kemur í veg fyrir stórfellda oxun. Aðeins ef málmurinn er fíndreift eða í þunnri plötu mun sterkur logi valda hröðum bruna hans.

Unnið úr málmgrýti: ${\text{AlO}(\text{OH})(s)+\text{NaOH}(aq)+{\text{H}}_{2}\text{O}(l)\, \longrightarrow \, \text{Na}{[ {\text{Al}{{(\text{OH})}}_{4}} ]}(aq)}$
Endurheimt: ${\text{2Na}{[ {\text{Al}{{(\text{OH})}}_{4}} ]}(s)+{\text{H}}_{2}{{\text{SO}}}_{4}(aq)\, \longrightarrow \, \text{2Al}{{(\text{OH})}}_{3}(s)+{{\text{Na}}}_{2}{{\text{SO}}}_{4}(aq)+{{\text{2H}}}_{2}\text{O}(l)}$
Herting: ${\text{2Al}{{(\text{OH})}}_{3}(s)\, \longrightarrow \, {{\text{Al}}}_{2}{\text{O}}_{3}(s)+{{\text{3H}}}_{2}\text{O}(g)}$
Leyst upp í Na₃AlF₆(l) og rafgreint: ${{{\text{Al}}}^{{3+}}+{{\text{3e}}}^{-}\, \longrightarrow \, \text{Al}(s)}$

25,83%

39 kg

18.3 Uppbygging og almennir eiginleikar hálfmálma

(a) H₃BPH₃:

(b) ${{{\text{BF}}}_{4}^{\text{−}}:}$

(c) BBr₃:

(d) B(CH₃)₃:

(e) B(OH)₃:

This Lewis structure is composed of a boron atom single bonded to a phosphorus atom. Each of these atoms is single bonded to three hydrogen atoms.

This Lewis structure is composed of a boron atom single bonded to four fluorine atoms, each of which has three lone pairs of electrons. The structure is surrounded by brackets, and a negative sign appears as a superscript outside the brackets.

This Lewis structure is composed of a boron atom single bonded to three bromine atoms, each of which has three lone pairs of electrons.

This Lewis structure is composed of a boron atom that is single bonded to three carbon atoms, each of which is single bonded to three hydrogen atoms.

This Lewis structure is composed of a boron atom that is single bonded to three oxygen atoms, each of which has two lone pairs of electrons. Each oxygen atom is single bonded to a hydrogen atom.

1s²2s²2p⁶3s²3p²3d⁰.

(a) (CH₃)₃SiH: sp³ efnatengi umhverfis Si; byggingin er ferflötungur; (b) ${{{\text{SiO}}}_{4}^{\text{4−}}:}$ sp³ efnatengi umhverfis Si; byggingin er ferflötungur; (c) Si₂H₆: sp³ efnatengi umhverfis hvort Si; byggingin er línuleg meðfram Si-Si efnatenginu; (d) Si(OH)₄: sp³ efnatengi umhverfis Si; byggingin er ferflötungur; (e) ${{{\text{SiF}}}_{6}^{\text{2−}}:}$ sp³d² efnatengi umhverfis Si; byggingin er áttflötungur

(a) óskautaður; (b) óskautaður; (c) skautaður; (d) óskautaður; (e) skautaður

(a) tellúrdíoxíð eða tellúr(IV)oxíð; (b) antímon(III)súlfíð; (c) german(IV)flúoríð; (d) silan eða kísil(IV)hýdríð; (e) german(IV)hýdríð

Bór hefur aðeins s- og p-svigrúm tiltæk, sem geta rúmað að hámarki fjögur rafeindapör. Ólíkt kísli eru engin d-svigrúm tiltæk í bór.

(a) ΔHb0 = 87 kJ; ΔGb0 = 44 kJ; (b) ΔHb0 = −109,9 kJ; ΔGb0 = −154,7 kJ; (c) ΔHb0 = −510 kJ; ΔGb0 = −601,5 kJ

Veik lausn af flúorsýru myndi leysa upp sílikatið en ekki skemma demantinn.

18.4 Bygging og almennir eiginleikar málmleysingja

Í N₂-sameindinni hafa niturfrumeindirnar eitt σ-efnatengi og tvö π-efnatengi sem halda frumeindunum tveimur saman. Tilvist þriggja sterkra efnatengja gerir N₂ að mjög stöðugri sameind. Fosfór er frumefni í lotu þrjú og myndar því ekki π-efnatengi á skilvirkan hátt. Þess vegna verður það að uppfylla kröfur sínar um efnatengi með því að mynda þrjú σ-efnatengi.

(a) H = 1+, C = 2+ og N = 3−; (b) O = 2+ og F = 1−; (c) As = 3+ og Cl = 1−

S < Cl < O < F

18.5 Tilvist, framleiðsla og efnasambönd vetnis

Rafneikvæðni málmleysingja er meiri en vetnis. Því er neikvæða hleðslan betur staðsett á málmleysingjanum, sem hefur meiri tilhneigingu til að draga að sér rafeindir í efnatenginu.

Vetni hefur aðeins eitt svigrúm til að tengjast öðrum frumeindum. Þar af leiðandi getur aðeins eitt tveggja rafeinda efnatengi myndast.

0,43 g H₂

18.6 Tilvist, framleiðsla og eiginleikar karbónata

(a) ${\text{Ca}{{(\text{OH})}}_{2}(aq)+{{\text{CO}}}_{2}(g)\, \longrightarrow \, {{\text{CaCO}}}_{3}(s)+{\text{H}}_{2}\text{O}(l);}$ (b) ${\text{CaO}(s)+{{\text{SO}}}_{2}(g)\, \longrightarrow \, {{\text{CaSO}}}_{3}(s);}$
(c) ${{{\text{2NaHCO}}}_{3}(s)+{{\text{NaH}}}_{2}{{\text{PO}}}_{4}(aq)\, \longrightarrow \, {{\text{Na}}}_{3}{{\text{PO}}}_{4}(aq)+{{\text{2CO}}}_{2}(g)+{{\text{2H}}}_{2}\text{O}(l)}$

18.7 Tilvist, framleiðsla og eiginleikar niturs

(a) NH²⁻:

(b) N₂F₄:

(c) ${{{\text{NH}}}_{2}^{\text{−}}:}$

(d) NF₃:

(e) ${{{\text{N}}}_{3}^{\text{−}}:}$

This Lewis structure shows a nitrogen atom with three lone pairs of electrons single bonded to a hydrogen atom. The structure is surrounded by brackets. Outside and superscript to the brackets is a two negative sign.

This Lewis structure shows two nitrogen atoms, each with one lone pair of electrons, single bonded to one another and each single bonded to two fluorine atoms. Each fluorine atom has three lone pairs of electrons.

This Lewis structure shows a nitrogen atom with two lone pairs of electrons single bonded to two hydrogen atoms. The structure is surrounded by brackets. Outside and superscript to the brackets is a negative sign.

This Lewis structure shows a nitrogen atom, with one lone pair of electrons, single bonded to three fluorine atoms. Each fluorine atom has three lone pairs of electrons.

Three Lewis structures are shown and connected by double-headed arrows in between. The left structure shows a nitrogen atom with a lone pair of electrons triple bonded to a second nitrogen which is single bonded to a third nitrogen. The third nitrogen has three lone pairs of electrons. The entire structure is surrounded by brackets, and outside and superscript to the brackets is a negative sign. The middle structure shows a nitrogen atom with three lone pair of electrons single bonded to a second nitrogen which is triple bonded to a third nitrogen. The third nitrogen which has one lone pair of electrons. The entire structure is surrounded by brackets, and outside and superscript to the brackets is a negative sign. The right structure shows a nitrogen atom with two lone pairs of electrons double bonded to a second nitrogen which is double bonded to a third nitrogen. The third nitrogen atom has two lone pairs of electrons. The entire structure is surrounded by brackets, and outside and superscript to the brackets is a negative sign.

Ammoníak virkar sem Brønsted-basi vegna þess að það tekur auðveldlega við róteindum og sem Lewis-basi að því leyti að það hefur rafeindapar til að gefa.
Brønsted-basi: ${{{\text{NH}}}_{3}+{\text{H}}_{3}{\text{O}}^{+}\, \longrightarrow \, {{\text{NH}}}_{4}^{+}+{\text{H}}_{2}\text{O}}$
Lewis-basi: ${{{\text{2NH}}}_{3}+{{\text{Ag}}}^{+}\, \longrightarrow \, {{{{\text{[H}}}_{3}\text{N}-\text{Ag}-{{\text{NH}}}_{3}]}}^{+}}$

(a) NO₂:

Nitur er með sp² blendingssvigrúm. Sameindin hefur beygða lögun með ONO-tengishorn sem er um það bil 120°.
(b) ${{{\text{NO}}}_{2}^{\text{−}}:}$

Nitur er með sp² blendingssvigrúm. Sameindin hefur beygða lögun með ONO-tengishorn sem er aðeins minna en 120°.
(c) ${{{\text{NO}}}_{2}^{\text{+}}:}$

Nitur er með sp blendingssvigrúm. Sameindin hefur línulega lögun með ONO-tengishorn sem er 180°.

Two Lewis structures are shown and connected by double-headed arrows in between. The left structure shows a nitrogen atom with a single electron double bonded to an oxygen atom which has two lone pairs of electrons. The nitrogen atom is also single bonded to an oxygen atom with three lone pairs of electrons. The right structure is a mirror image of the left structure.

Two Lewis structures are shown and connected by double-headed arrows in between. Each structure is surrounded by brackets, and outside and superscript to the brackets is a negative sign. The left structure shows a nitrogen atom with a lone pair of electrons double bonded to an oxygen atom which has two lone pairs of electrons. The nitrogen atom is also single bonded to an oxygen atom with three lone pair of electrons. The right structure is a mirror image of the left structure.

This Lewis structure shows a nitrogen atom double bonded on both sides to an oxygen atom which has two lone pairs of electrons each. The structure is surrounded by brackets and outside and superscript to the brackets is a negative sign.

Nitur getur ekki myndað NF₅ sameind vegna þess að það hefur ekki d-svigrúm til að tengjast við tvær flúorfrumeindir til viðbótar.

18.8 Tilvist, framleiðsla og eiginleikar fosfórs

(a)

(b)

(c)

(d)

(e)

This Lewis structure shows a phosphorus atom with a lone pair of electrons single bonded to three hydrogen atoms.

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.

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.

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.

This Lewis structure shows a phosphorus atom single bonded to five fluorine atoms, each with three lone pairs of electrons.

(a) ${{\text{P}}_{4}(s)+\text{4Al}(s)\, \longrightarrow \, \text{4AlP}(s);}$ (b) ${{\text{P}}_{4}(s)+\text{12Na}(s)\, \longrightarrow \, {{\text{4Na}}}_{3}\text{P}(s);}$ (c) ${{\text{P}}_{4}(s)+{{\text{10F}}}_{2}(g)\, \longrightarrow \, {{\text{4PF}}}_{5}(l);}$ (d) ${{\text{P}}_{4}(s)+{{\text{6Cl}}}_{2}(g)\, \longrightarrow \, {{\text{4PCl}}}_{3}(l)}$ eða ${{\text{P}}_{4}(s)+{{\text{10Cl}}}_{2}(g)\, \longrightarrow \, {{\text{4PCl}}}_{5}(l);}$ (e) ${{\text{P}}_{4}(s)+{{\text{3O}}}_{2}(g)\, \longrightarrow \, {\text{P}}_{4}{\text{O}}_{6}(s)}$ eða ${{\text{P}}_{4}(s)+{{\text{5O}}}_{2}(g)\, \longrightarrow \, {\text{P}}_{4}{\text{O}}_{{10}}(s);}$ (f) ${{\text{P}}_{4}{\text{O}}_{6}(s)+{{\text{2O}}}_{2}(g)\, \longrightarrow \, {\text{P}}_{4}{\text{O}}_{{10}}(s)}$

291 ml

28 tonn

(a)

(b)

(c)

(d)

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, “Tetrahedral,” is written under the structure.

This Lewis structure shows a phosphorus atom single bonded to five fluorine atoms, each with three lone pairs of electrons. The label, “Trigonal bipyramidal,” is written under the structure.

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, “Octahedral,” is written under the structure.

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, “Tetrahedral,” is written under the structure.

(a) P = 3+; (b) P = 5+; (c) P = 3+; (d) P = 5+; (e) P = 3−; (f) P = 5+

18.9 Tilvist, framleiðsla og efnasambönd súrefnis

FrO₂

(a) ${\text{2Zn}(s)+{\text{O}}_{2}(g)\, \longrightarrow \, \text{2ZnO}(s);}$ (b) ${{{\text{ZnCO}}}_{3}(s)\, \longrightarrow \, \text{ZnO}(s)+{{\text{CO}}}_{2}(g);}$ (c) ${{{\text{ZnCO}}}_{3}(s)+2{{\text{CH}}}_{3}\text{COOH}(aq)\, \longrightarrow \, \text{Zn}{({\text{CH}}3\text{COO})}2(aq)+{{\text{CO}}}_{2}(g)+{\text{H}}_{2}\text{O}(l);}$ (d) ${\text{Zn}(s)+\text{2HBr}(aq)\, \longrightarrow \, {{\text{ZnBr}}}_{2}(aq)+{\text{H}}_{2}(g)}$

${\text{Al}{{(\text{OH})}}_{3}(s)+3{\text{H}}^{\text{+}}(aq)\, \longrightarrow \, {{\text{Al}}}^{{3+}}+3{\text{H}}_{2}\text{O}(l);}$ ${\text{Al}{{(\text{OH})}}_{3}(s)+{{\text{OH}}}^{-}\, \longrightarrow \, {{{[{\text{Al}{{(\text{OH})}}_{4}}]}}}^{\text{−}}(aq)}$

(a) ${{{\text{Na}}}_{2}\text{O}(s)+{\text{H}}_{2}\text{O}(l)\, \longrightarrow \, \text{2NaOH}(aq);}$ (b) ${{{\text{Cs}}}_{2}{{\text{CO}}}_{3}(s)+\text{2HF}(aq)\, \longrightarrow \, \text{2CsF}(aq)+\, {{\text{CO}}}_{2}(g)+{\text{H}}_{2}\text{O}(l);}$ (c) ${{{\text{Al}}}_{2}{\text{O}}_{3}(s)+6{{\text{HClO}}}_{4}(aq)\, \longrightarrow \, \text{2Al}{({\text{ClO}}4)}3(aq)+3{\text{H}}_{2}\text{O}(l);}$ (d) ${{{\text{Na}}}_{2}{{\text{CO}}}_{3}(aq)+\text{Ba}{({\text{NO}}3)}2(aq)\, \longrightarrow \, 2{{\text{NaNO}}}_{3}(aq)+{{\text{BaCO}}}_{3}(s);}$ (e) ${{{\text{TiCl}}}_{4}(l)+\text{4Na}(s)\, \longrightarrow \, \text{Ti}(s)+\text{4NaCl}(s)}$

HClO₄ er sterkari sýran því í röð oxósýra með svipaðar formúlur gildir að því hærri sem rafneikvæðni miðfrumeindarinnar er, því sterkara er aðdráttarafl miðfrumeindarinnar fyrir rafeindir súrefnisins/súrefnanna. Sterkara aðdráttarafl súrefnisrafeindarinnar leiðir til sterkara aðdráttarafls súrefnis fyrir rafeindirnar í O-H efnatenginu, sem gerir það að verkum að vetnið losnar auðveldar. Því veikara sem þetta efnatengi er, því sterkari er sýran.

Þar sem H₂SO₄ og H₂SeO₄ eru báðar oxósýrur og miðfrumeindir þeirra hafa báðar sömu oxunartölu, þá fer sýrustyrkurinn eftir hlutfallslegri rafneikvæðni miðfrumeindarinnar. Þar sem brennisteinn er rafneikvæðari en selen er H₂SO₄ sterkari sýran.

18.10 Tilvist, framleiðsla og eiginleikar brennisteins

SO₂, sp² 4+; SO₃, sp², 6+; H₂SO₄, sp³, 6+

SF₆: S = 6+; SO₂F₂: S = 6+; KHS: S = 2−

Brennisteinn getur aðeins myndað tvítengi við hátt hitastig (verulega innvermin skilyrði), sem á ekki við um súrefni.

Mörg svör eru möguleg, þar á meðal: ${\text{Cu}(s)+2{\text{H}}_{2}{{\text{SO}}}_{4}(l)\, \longrightarrow \, {{\text{CuSO}}}_{4}(aq)+{{\text{SO}}}_{2}(g)+2{\text{H}}_{2}\text{O}(l)}$ og ${\text{C}(s)+2{\text{H}}_{2}{{\text{SO}}}_{4}(l)\, \longrightarrow \, {{\text{CO}}}_{2}(g)+2{{\text{SO}}}_{2}(g)+2{\text{H}}_{2}\text{O}(l)}$

5,1 $\times$ 10⁴ g

18.11 Tilvist, framleiðsla og eiginleikar halógena

SnCl₄ er ekki salt vegna þess að það er samgilt tengt. Salt verður að hafa jónatengi.

Í oxósýrum með svipaðar formúlur eykst sýrustyrkurinn eftir því sem rafneikvæðni miðatómsins eykst. HClO₃ er sterkari en HBrO₃; Cl er rafneikvæðara en Br.

(a)

(b)

(c)

(d)

(e)

This Lewis structure shows an iodine atom with one lone pair of electrons single bonded to five fluorine atoms, each of which has three lone pairs of electrons. The image is labeled, “Square pyramidal.”

This Lewis structure shows an iodine atom with three lone pairs of electrons single bonded to two iodine atoms, each of which has three lone pairs of electrons. The image is surrounded by brackets. A superscript negative sign appears outside the brackets. The image is labeled, “Linear.”

This Lewis structure shows a phosphorus atom single bonded to five chlorine atoms, each of which has three lone pairs of electrons. The image is labeled, “Trigonal bipyramidal.”

This Lewis structure shows a selenium atom with one lone pair of electrons single bonded to four fluorine atoms, each of which has three lone pairs of electrons. The image is labeled “Seesaw.”

This Lewis structure shows a chlorine atom with two lone pairs of electrons single bonded to three fluorine atoms, each of which has three lone pairs of electrons. The image is labeled, “T-shaped.”

(a) brómtríflúoríð; (b) natríumbrómat; (c) fosfórpentabromíð; (d) natríumperklórat; (e) kalíumhýpóklórít

(a) I: 7+; (b) I: 7+; (c) Cl: 4+; (d) I: 3+; Cl: 1−; (e) F: 0

18.12 Tilvist, framleiðsla og eiginleikar eðalgastegunda

(a) sp³d-blendin; (b) sp³d²-blendin; (c) sp³-blendin; (d) sp³-blendin; (e) sp³d²-blendin;

(a) óskautuð; (b) óskautuð; (c) skautuð; (d) óskautuð; (e) skautuð

Reynsluformúlan er XeF₆ og stilltu efnahvörfin eru: $\begin{aligned} \text{Xe}(g)+{\text{3F}}_{2}(g)\, \overset{{\, \text{Δ}\,}}{\rightarrow}\, {\text{XeF}}_{6}(s) \\ {\text{XeF}}_{6}(s)+{\text{3H}}_{2}(g)\, \longrightarrow \, \text{6HF}(g)+\text{Xe}(g) \end{aligned}$