Why bond energy of acetone is more though it is more polar than formaldehyde? I was going through the general properties of carbonyl compounds and then found this (in the pic) data, where it says that dipole moment of acetone (if we assume $\ce{R = -CH3}$) is more than acetaldehyde which in turn is greater than that of formaldehyde.
But I think, as $\ce{-CH3}$ is a $+I$ effecting group, so it will satiate the residing positive pole on carbon slightly and hence will make the $\ce{C=O}$ bond less polar and hence the sequence should be reversed!

Please anyone make me correct where am I mistaking with the concept?

Picture source

EDIT :- I got my answer of the above confusion. Thanks to Physicsapproval.
But with that I came to face another confusion. In the next part of the text (see the paragraph just below the pic in the Picture source) I found that "the larger the dipole moment the greater the polar character of the carbonyl group". So that means, $\ce{C=O}$ bond in acetone is more polar and least in the case of formaldehyde! Now in the next part it is mentioned that the bond energies of $\ce{C=O}$ bond in the mentioned compounds are: $$ \ce{H2C=O} \, ; 170~\mathrm{kcal/mol}$$ $$\ce{RHC=O} ~ ; 175~\mathrm{kcal/mol}$$ $$\ce{R2C=O}~; 180~\mathrm{kcal/mol}$$
Now I know that the more polar the bond is, the less is its bond energy. So, in this case why the trend is reversed, i.e., $\ce{C=O}$ bond of acetone being more polar has the highest bond energy compared to other two?
the more polar the bond is, the less is its bond energy


I'm not sure where you are getting this from. 

Take Acid halides as an example series. As the bond get more polar ( HI (0.4 D) &lt; HBr (0.7 D) &lt; HCl (0.9 D) &lt; HF (1.9 D) ) the bond energies follow accordingly ( HI (295 kJ/mol) &lt; HBr (362 kJ/mol) &lt; HCl (428 kJ/mol) &lt; HF (565 kJ/mol) )

As the charge separation gets larger (and therfore more polar) there is a stronger will to not have that large charge separation, as nature wants to naturally come to an equilibrium - and thus the bonds are more energetic. 

Does this clear up your confusion?