[HeroWH]

a) count and list all types of bonds, then use these with their bond enthalpies to predict enthalpy reaction.
b) Calculate the enthalpy of reaction from the standard enthalpies of formation of the reactant and product molecules and compare with your answers from part a - the enthalpy of formation for fructose is -1038.2kj/mol
Can someone help me with this, how is it supposed to look?

[Arkcon]

Per forum rules you should show your attempts at solving the problem before receiving help.  Please show at least some sign that you have attempted this problem, or have at least some understanding of underlying concepts.

[HeroWH]

Ohh, i know how to do it, we were given the enthalpy of formation for fructose for the second part, but how do I estimate the bond enthalpy of fructose itself? Is there a DeltaH value for C-OH? Am i missing something, I have no clue the bonds in fructose are weird, I cant understand the lewis structure!

[HeroWH]

yea im totally lost on the fructose structure, im not getting it one bond is H2C-OH, there is no value for this

[Borek]

Bond is always just between two atoms on its ends.