53, Iod (I)

Iodine, gr. ioeides = veilchenfarben

Thermodynamik:
         
  Se Br Kr  
  Te I Xe  
  Po At Rn  
         
  kJ/mol
Schmelzenthalpie: 7.76
Verdampfungsenthalpie: 20.9
Sublimationsenthalpie: 28.66
   
Atomisierungsenthalpie: 106.84
Kovalente Bindungs-Enthalpien ΔH:

Bindung: Energie
(kJ/mol)		 Länge
(pm)		   Bindung: Energie
(kJ/mol)		 Länge
(pm)
H−I[1] 298   170   H−I[2] 298.3   170
Li−I[2] 345.2 ±1.2% 267   Be−I[2] 261   235
B−I[2] 361   223   C−I[1] 218   215
C−I[2] 253.1 ±14.1% 215   N−I[2] 159 ±10.7% 210
Na−I[2] 304.2 ±0.7% 305   Mg−I[2] 229   280
Al−I[1] 370   260   Al−I[2] 369.9 ±0.6% 260
Si−I[1] 234   250   Si−I[2] 243.1 ±3.5% 250
P−I[1] 184   246   Ar−I[2][3] 5.3 ±0.9% 245
K−I[2] 322.5 ±0.7% 342   Ca−I[2] 284.7 ±3% 315
Ti−I[2] 306   299   Cr−I[2] 287 ±8.5% 278
Mn−I[2] 282.2 ±3.4% 278   Fe−I[2] 123   271
Co−I[2] 280 ±7.5% 265   Ni−I[2] 293 ±7.2% 263
Cu−I[2] 289 ±21.8% 271   Zn−I[2] 153.1 ±4.1% 261
Ga−I[2] 334 ±3.9% 261   Ge−I[1] 217   259
Ge−I[2] 268 ±9.3% 259   As−I[1] 200   258
As−I[2] 296.6 ±8.1% 258   Kr−I[2] 5.67   255
Rb−I[2] 318.8 ±0.7% 359   Sr−I[2] 301   334
Y−I[2] 422.6 ±3% 329   Zr−I[2] 127   314
Mo−I[2] 266.9   293   Ag−I[2] 234 ±12.4% 284
Cd−I[2] 97.2 ±2.2% 283   In−I[2] 306.9   281
Sn−I[2] 235 ±1.3% 278   Sb−I[1] 195   278
Te−I[1] 121   277   Te−I[2] 192 ±21.9% 277
I−N[1] 201   210   I−O[1] 201   205
I−O[2] 233.4 ±0.6% 205   I−F[1] 280   196
I−Cl[1] 211   241   I−Cl[2] 211.3 ±0.2% 241
I−Br[1] 179.1 ±0.2% 259   I−I[1] 152.3 ±0.4% 278
Xe−I[2] 6.9 ±0.7% 279   Cs−I[2] 338.5 ±0.6% 383
Ba−I[2] 322.6 ±2% 354   La−I[2] 411.7   346
Ce−I[2] 333.8   343   Pr−I[2] 306.2   342
Nd−I[2] 301.5   340   Sm−I[2] 293.1   337
Eu−I[2] 288.3   337   Gd−I[2] 333.8   335
Tb−I[2] 336.2   333   Dy−I[2] 269 ±3.1% 331
Ho−I[2] 275.1   331   Er−I[2] 315.8   328
Tm−I[2] 260.8   329   Yb−I[2] 257.3   326
Lu−I[2] 263.2   326   Au−I[2] 276   275
Hg−I[2] 34.7 ±2.9% 271   Tl−I[2] 285 ±7.4% 284
Pb−I[2] 194 ±19.6% 285   Bi−I[2] 186.1 ±3.1% 287
Th−I[2] 361 ±6.9% 345   U−I[2] 299 ±9% 335

[1] Kovalente Bindung innerhalb eines Moleküles, Durchschnittswert.
[2] Bindung innerhalb eines diatomaren Moleküles in der Gasphase.
[3] Original-Angabe: ~5.3.

Thermodynamische Daten der Iod-Modifikationen:

Phasenbezogene thermodynamische Daten:
  ΔFHo
in kJ/mol		 ΔFGo
in kJ/mol		 So
in J/mol•K		 cp
in J/mol•K
Fest: -- -- 116.1 54.4
Flüssig: 13.52 -- 150.36 80.67
Gas: 62.4 19.3 260.7 36.9

Thermodynamische Daten der Phasenübergänge:
  Enthalpie ΔH Entropie ΔS  
Schmelzen: 15.52 kJ/mol 40.12 J/(mol•K)  
Verdampfen: 41.798 kJ/mol 91.37 J/(mol•K)  


Hydratisierungsenthalpien der Ionen:

Ladung: Vorgang Hydratisierungs-
enthalpie ΔHhydr. in kJ/mol		    
-1 I-(g) + H2O → I-(aq) -307    
Legende: (g) = gaseous, gasförmig  (aq) = aqueous, in Wasser gelöst.
Quelle: Holleman-Wiberg, Lehrbuch der anorg. Chemie, 102. Auflage.