Answer:
All of the C-C bonds are actually identical,
The structure of the molecule is closed like a ring structure,
Explanation:
1) all benzene hydrocarbons are ChHp-2 ⇔ this is <u>false</u> the formula for benzene is C6H6 ( CnHn).
2)All C-C bonds share 2 pairs of electrons ⇔ <u>False </u>
There are not enough electrons to form double bonds on all the carbon atoms
3) Three C-C bonds share 2 pairs of electrons ⇔ False
Since there are not enough electrons to form double bonds on all the carbon atoms, although the electrons do strengthen all of the bonds on the ring equally.
4) All of the C-C bonds are actually identical ⇔ <u>correct </u>
⇒The actual structure of benzene is a resonance hybrid, with six delocalised π-electrons. (4n + 2 = π)
⇒Due to this structure with delocalised π-electrons, the structure of benzene is very stable and it's reactivity quite low.
⇒ All the C-C bonds of bezene have sp2-sp2 overlap on both sides, what makes them to form 3 π-bonds
5) The structure of the molecule is closed like a ring structure ⇔ <u>correct</u>
Since there are not enough electrons to form double bonds on all the carbon atoms, although the electrons do strengthen all of the bonds on the ring equally. This results in symmetric molecular orbital. The delocalisation of the electrons is also known as aromaticity or ring structure, what gives benzene a great stability.
