[References]The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water:OF2(g) + H20(g)→ 0g) + 2HF(g)=-318 kJotUsing bond energies, calculate the bond dissociation energy of the O-F bond in OF7.Average Bond Energies (kJ/mol)Single BondsMultiple BondsptN-H391149C=C614432565H-H8394957451072607418941ptH--FN-N160208C=CN-F272|-Br175H-CIH-Br427363295N-CIN-BrC=0*C=D0200ptH-1243S-H347N-O201S-F327N=NN N253S-CIS-Br467413347305358C-H146218C--CC--NC-OC--FC-CIC-BrO-O891C=NC-NS-S266190203O-F6150-CI340393360452485O-I一234Si-Si339276Si-HSi-CSi-Oe F-F154253240259F-CIF-BrCl-CIC-S237239218193Cl--BrBr--Br*C==O(in CO,) - 799O-F bond dissociation energy:kJ molSubmit AnswerTry Another Version1 item attempt remainingnything%3D

Data required,∆Erxn=-318kJBond energy of O-H=467kJ/molBond energy of O=O=495kJ/molBond energy of…

The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water: OF (g) + H20(g)→02(g) + 2HF(g) AE =-318KJ Ixn Using bond energies, calculate the bond dissociation energy of the O-F bond in OF2.

The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water: OF (g) + H20(g)→02(g) + 2HF(g) AE =-318KJ Ixn Using bond energies, calculate the bond dissociation energy of the O-F bond in OF2.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.

Polarity Of Water

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Valence Bond Theory Vbt

Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Question

[References]
The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water:
OF2(g) + H20(g)→ 0g) + 2HF(g)
=-318 kJ
ot
Using bond energies, calculate the bond dissociation energy of the O-F bond in OF7.
Average Bond Energies (kJ/mol)
Single Bonds
Multiple Bonds
pt
N-H
391
149
C=C
614
432
565
H-H
839
495
745
1072
607
418
941
pt
H--F
N-N
160
208
C=C
N-F
272
|-Br
175
H-CI
H-Br
427
363
295
N-CI
N-Br
C=0*
C=D0
200
pt
H-1
243
S-H
347
N-O
201
S-F
327
N=N
N N
253
S-CI
S-Br
467
413
347
305
358
C-H
146
218
C--C
C--N
C-O
C--F
C-CI
C-Br
O-O
891
C=N
C-N
S-S
266
190
203
O-F
615
0-CI
340
393
360
452
485
O-I
一
234
Si-Si
339
276
Si-H
Si-C
Si-O
e F-F
154
253
240
259
F-CI
F-Br
Cl-CI
C-S
237
239
218
193
Cl--Br
Br--Br
*C==
O(in CO,) - 799
O-F bond dissociation energy:
kJ mol
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