Using the periodic table only, arrange the members of each...

Using the periodic table only, arrange the members of each of the following sets in order of increasing bond length: (a) $\mathrm{H}-\mathrm{F}, \mathrm{H}-\mathrm{I}, \mathrm{H}-\mathrm{Cl}$ (b) $\mathrm{C}-\mathrm{S}, \mathrm{C}=\mathrm{O}, \mathrm{C}-\mathrm{O}$ (c) $\mathrm{N}-\mathrm{H}, \mathrm{N}-\mathrm{S}, \mathrm{N}-\mathrm{O}$

Using the periodic table only, arrange the members of each of the following sets in order of increasing bond length:
(a) $\mathrm{H}-\mathrm{F}, \mathrm{H}-\mathrm{I}, \mathrm{H}-\mathrm{Cl}$
(b) $\mathrm{C}-\mathrm{S}, \mathrm{C}=\mathrm{O}, \mathrm{C}-\mathrm{O}$
(c) $\mathrm{N}-\mathrm{H}, \mathrm{N}-\mathrm{S}, \mathrm{N}-\mathrm{O}$

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Key Concepts

Periodic Trends

Periodic trends involve patterns in element properties such as atomic size and electronegativity across the periodic table. As you move down a group, the atomic radius increases, which generally leads to longer bond lengths. Similarly, elements in the same period can show differences in atomic sizes that influence bond distances between atoms.

Atomic Radius and Bond Length

The bond length between two atoms is largely determined by their atomic radii. Larger atoms have electrons that occupy orbitals further from the nucleus, which means that bonds involving larger atoms will typically have longer bond lengths. This concept explains why bonds involving heavier halogens or larger atoms tend to be longer than those with smaller atoms.

Bond Order

Bond order, which measures the number of shared electron pairs between two atoms, has a direct effect on bond length. Higher bond orders, as seen in double or triple bonds, result in a stronger attraction between the nuclei and a corresponding decrease in bond length. In contrast, single bonds, having a lower bond order, are typically longer.

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