In a Bond Energy problem, does the diatomic oxygen have a single bond or double?

I read in my chem book that diatomic oxygen is an exception to the octet rule and that it exists with two valence electrons and a single O-O bond. However... after doing some research i learned that both O-O and O=O are inaccurate models of dioxygen and O÷O is a more accurate depiction. That said, the exam question was:
For: (2)C3H6 + (9)O2 -> (6)CO2 + (6)H2O
a) balance the equation
b) what is the dot structure of the molecules? (i only need to know O2)
c) what is the net bond energy?

I already took the exam using this dot structure ∙O-O∙ and got 1566 or close to that for the energy.

your help would be greatly appreciated...

Answer:
::O=O::

Double bond for those bond-energy problems.

The bond order in O2 is a double bond. MO theory confirms this but the distinction between the Lewis and MO treatments comes in the prediction of paramagnetism for O2.

Diatomic oxygen , has two Oxygen atoms double bonded, it means they share two pairs of electrons, two from each atom. The representation is:
x .
x x O xx . . O ..
x .

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In a Bond Energy problem, does the diatomic oxygen have a single bond or double?

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