The following diagram shows the potential energy of two atoms as a function of internuclear distance. Which bond is the strongest? Which bond is the longest?

Verified step by step guidance

1. Identify the bond strength by looking at the depth of the potential energy well. The deeper the well, the stronger the bond.
2. Compare the depth of the potential energy wells for bonds X-Y and W-Z. Determine which one is deeper.
3. Identify the bond length by looking at the internuclear distance at the minimum potential energy. The longer the distance, the longer the bond.
4. Compare the internuclear distances at the minimum potential energy for bonds X-Y and W-Z. Determine which one is longer.
5. Summarize which bond is the strongest and which bond is the longest based on the comparisons made in the previous steps.

Key Concepts

Potential Energy Curve

A potential energy curve illustrates how the potential energy of a system changes with the distance between two atoms. The curve typically shows a minimum point, indicating the most stable configuration (bond formation) and the energy required to break the bond. The depth of the well represents bond strength, while the distance at which the potential energy is minimized indicates bond length.

Bond Strength

Bond strength refers to the energy required to break a bond between two atoms. In a potential energy curve, a deeper well indicates a stronger bond, as it signifies that more energy is needed to separate the atoms. Therefore, comparing the depths of the wells for bonds X-Y and W-Z allows us to determine which bond is stronger.

Bond Length

Bond length is the distance between the nuclei of two bonded atoms at their equilibrium position. In the context of a potential energy curve, the bond length corresponds to the internuclear distance at which the potential energy reaches its minimum. By analyzing the positions of the minima for bonds X-Y and W-Z, we can identify which bond is longer based on the distance at which the potential energy is lowest.