Question 17

The bonds linking two carbon atoms in an acetylene molecule are triple bonds.

In an acetylene molecule (C2H2), the two carbon atoms are connected by a triple bond, which consists of one sigma bond and two pi bonds. This type of bond results in a strong connection between the carbon atoms, contributing to the molecule's linear structure.

A) Single bond

A single bond consists of one sigma bond and connects two atoms with a single pair of shared electrons. In the case of acetylene, the bond between carbon atoms is not a single bond, as the molecule's structure requires a stronger connection to stabilize the compound.

B) Triple bond

The correct description of the bond between the two carbon atoms in an acetylene molecule is a triple bond. This bond is formed by one sigma bond and two pi bonds, allowing for a very strong and short bond that characterizes the linear geometry of acetylene.

C) Double bond

A double bond consists of one sigma bond and one pi bond, which is not the case for acetylene. The carbon atoms in acetylene are bonded by a triple bond, making a double bond an incorrect description of their linkage.

D) Quadruple bond

Quadruple bonds are not a standard type of bond in organic chemistry and are not applicable to the bonding in acetylene. The bonding between the two carbon atoms is effectively satisfied by a triple bond, making the notion of a quadruple bond irrelevant for this molecule.

Conclusion

The bonds linking the two carbon atoms in acetylene are definitively triple bonds, as this arrangement provides the required stability and structure for the molecule. Other options, including single and double bonds, do not accurately reflect the nature of the bonding in acetylene, while the concept of a quadruple bond is not applicable in this context.