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Alkenes have pi bond which have less Bond Dissociation Energy compared to the sigma bond in the Alkanes which have higher Bond Dissociation Energy.
Quoting the data booklet,
C-C => 350 kJ/mol
C=C => 610 kJ/mol
The alkene has a significantly higher bond energy (which translates into a significantly higher bond dissociation energy), which also explains why N2 is unreactive.
Just read my comment again. Before SHOUTING IN A PUBLIC FORUM.
Geesh! You got it right, we all got it wrong. Does that make your "annoying face" -_- happy now?
I'm a debater. I tend to use capitals to emphasize on key words, not to shout. Communication via keyboard really has its limitations.
Regardless, it's not about me being right or someone else being wrong. This isn't a competition. I'm just saying, a Carbonyl isn't possible there. Secondly, about reading again, I did mention up there that I replied when you had originally posted, but it was visible to everyone publicly when I next came online. So, yeah.
And about the annoying face. That's just habit. Hate it or love it, the -_- show up quite often in my posts -___-