Final answer:
The order of decreasing X-O bond length in compounds and ions involves evaluating electronegativity, bonding pairs, non-bonding pairs, and molecular geometry. Factors such as the presence of double bonds, resonance structures, and the effect of electronegative atoms on electron distribution must be considered for accurate arrangement.
Step-by-step explanation:
The question pertains to arranging different chemical compounds in order of decreasing X-O bond length, where 'X' represents the central atom. To tackle this question, we must consider factors such as electronegativity, the number of bonding and non-bonding pairs of electrons around the central atom, and the molecular geometry. Usually, the greater the number of double bonds or resonance structures, the shorter the X-O bond length due to increased electron sharing and greater bond strength. Conversely, single bonds are generally longer than double bonds. Moreover, the presence of electronegative atoms can pull electron density away from the central atom, affecting the X-O bond length. Based on these concepts, the CO32- ion, for instance, will have one double bond and two single bonds to oxygen due to resonance, leading to an average bond length shorter than a typical single bond but longer than a double bond.