(c) Would you expect the O—O bond in O₂ to be shorter or longer than the O—O bond in compounds that contain an O—O single bond? Explain.

Verified step by step guidance

1. Understand the types of bonds: In molecular oxygen (O2), the O—O bond is a double bond, whereas in compounds with an O—O single bond, such as hydrogen peroxide (H2O2), the bond is a single bond.
2. Recall bond length principles: Generally, double bonds are shorter than single bonds because they involve more shared electrons, which increases the attraction between the bonded atoms and pulls them closer together.
3. Consider the bond order: The bond order is the number of chemical bonds between a pair of atoms. A higher bond order typically indicates a shorter bond length. In O2, the bond order is 2 (double bond), while in a single bond, the bond order is 1.
4. Compare bond lengths: Since double bonds (like in O2) are shorter than single bonds due to the increased electron sharing and bond order, the O—O bond in O2 is expected to be shorter than the O—O bond in compounds with an O—O single bond.
5. Conclude with reasoning: Therefore, based on the bond order and the nature of double versus single bonds, the O—O bond in O2 should be shorter than the O—O bond in compounds that contain an O—O single bond.