Sulfur tetra-fluoride (SF4) reacts slowly with O2 to form sulfur tetra-fluoride monoxide (OSF4) according to the following unbalanced reaction:
SF4 (g) + O2 (g) †’ OSF4 (g)
The O atom and the four F atoms in OSF4 are bonded to a central S atom.
(a) Balance the equation.
(b) Write a Lewis structure of OSF4 in which the formal charges of all atoms are zero.
(c) Use average bond enthalpies (Table 8.4) to estimate the enthalpy of the reaction. Is it endothermic or exothermic?
(d) Determine the electron-domain geometry of OSF4, and write two possible molecular geometries for the molecule based on this electron-domain geometry.
(e) Which of the molecular geometries in part (d) is more likely to be observed for the molecule? Explain.

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TABLE 8.4 .Average Bond Enthalpies (kJ/mol) Single Bonds C-H 413 348 293 358 485 328 276 240 259 391 O-H 163 201 OF 272 200 o 243 N-H N-N 463 146 190 203 234 155 C-N C-O C-F C-CI C Br CIF ClCI 253 242 N F N CI N Br O_Cİ 237 218 193 339 327 253 218 266 BrCl 436 SF 567 431 366 S 299 S Cl S Br -S I-CI H-Cl H Br H-I 208 175 151 Si H Si Si SiC Si-O SiCl Multiple Bonds 323 226 301 368 464 614 839 615 891 799 1072 418 941 607 495 523 418 C- N