Which of the following molecular oxygen ions would be expected tohave the larges

Question

Which of the following molecular oxygen ions would be expected tohave the largest bond enthalpy?

a. O2 (i.e.molecular oxygen)
b. O2 + (i.e.molecular oxygen with a +1 charge)
c. O2 2+ (i.e.molecular oxygen with a +2 charge)
d. O2 2- (i.e.molecular oxygen with a -2 charge)
e. O2 - (i.e.molecular oxygen with a -1 charge)

Please explain this problem to me. I have NO idea how onearth to answer this type of problem on an exam. Where do Ibegin? What rules must I use? Please would you give mesome tools with which I can work such a problem.

Explanation / Answer

-remember that shorter bond lengths = bigger bond enthalpy -since we are only looking at ions of O2, it is notnecessary to know the specific bond length of O---O -cations make the same compound shorter than anions of that samecompound -so anions > cations in bond enthalpy - D) O22- has the largest negative charge,there fore it is the largest bond enthalpy

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