Question

why alkenes are more reactive than the alkane

Answer 1

here is the answer ✨✨✌️✨
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Yes, alkenes are more reactive than alkanes.

Alkenes have one pi-bond between two (or more) carbon atoms, along with a sp2-sp2 hybridised orbital bonding (sigma bond). The pi-bond can be easily broken to free the valence shell electrons for combining with other atoms.

Alkanes have no pi-bonds between carbon atoms. They only have a sp3-sp3 hybridised orbital bonding (sigma bond). Sigma bond requires more energy to break.

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Answer 2

Yes, alkenes are more reactive. This is due to the properties of the carbon-carbon bond. In alkanes there is a single bond, denoted as σ. In alkenes the bond is double - there is a σ and a π component. At first thought, it seems that double must be stronger than single but in fact, due to the nature of the π bond, it is more reactive than a σ-bond. This principle is based on the structure of molecular orbitals. I won't go into details, just have a look at this image.

If you are just starting with chemistry, you might not have been told about nodes of orbitals but I think it will make more sense if I introduced this concept. Have a look at the blue region between the two carbon atoms (ignore the blue that is not between them) - this is a σ-bond and it is coloured uniformly. Now check out the π-bond. It is not without reason that one part is darker and the other is lighter. Orbitals, or wave functions, can have a positive or a negative value. At the point when its value becomes zero, the sign changes, or, as it is usually said, the phase changes. This is an analogy with plane waves.  

Now, recall the concept of frequency of a wave. The shorter the distance between two peaks, the higher the frequency and from Planck's law, the higher the energy. E=hν. So, higher frequency means changing the phase more often.  

Now, it should be obvious that because there is a phase change in the π-bond, it is higher in energy than the σ-bond. Higher in energy means more reactive.

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