Final answer:
The true statement is that triple bonds involve the sharing of three pairs of electrons between carbon atoms and are stronger than double bonds. Triple bonds contain one sigma bond and two pi bonds, making them shorter and stronger, while double bonds consist of one sigma and one pi bond.
Step-by-step explanation:
Comparing a double bond between two carbon atoms with a triple bond between two carbon atoms, the statement that is true is: B) Triple bonds involve the sharing of three pairs of electrons between carbon atoms. Triple bonds are indeed stronger than double bonds. A double bond consists of one sigma bond (σ) and one pi bond (π), summing up to two shared pairs of electrons between two atoms. A triple bond contains one sigma bond and two pi bonds, leading to three shared pairs of electrons. The presence of an additional pi bond in triple bonds makes them shorter and stronger compared to double bonds. It is important to note that triple bonds are not more reactive than double bonds due to the presence of more electrons; in fact, their increased bond strength typically makes them less reactive under most conditions. Moreover, contrary to what might be inferred from the provided reference, rotation around a triple bond is not freely possible due to the linear alignment of the p-orbitals involved in the pi bonds, limiting the rotation of connected groups.