The C-C bond length of the following molecules are in the order (a) C2 H6>C2 H4>C6 H6>C2 H2 (b)

step 1 In this problem, the correct order of bond length of the given molecules. I am writing about the

The C-C bond length of the following molecules are in the...

The $\mathrm{C}-\mathrm{C}$ bond length of the following molecules are in the order (a) $\mathrm{C}_{2} \mathrm{H}_{6}>\mathrm{C}_{2} \mathrm{H}_{4}>\mathrm{C}_{6} \mathrm{H}_{6}>\mathrm{C}_{2} \mathrm{H}_{2}$ (b) $\mathrm{C}_{2} \mathrm{H}_{2}<\mathrm{C}_{2} \mathrm{H}_{4}<\mathrm{C}_{6}{ }^{0} \mathrm{H}_{6}<\mathrm{C}_{2} \mathrm{H}_{6}^{2}$ (c) $\mathrm{C}_{2} \mathrm{H}_{6}>\mathrm{C}_{2} \mathrm{H}_{2}>\mathrm{C}_{6} \mathrm{H}_{6}>\mathrm{C}_{2} \mathrm{H}_{4}$ (d) $\mathrm{C}_{2} \mathrm{H}_{4}>\mathrm{C}_{2} \mathrm{H}_{6}>\mathrm{C}_{2}^{\circ} \mathrm{H}_{2}>\mathrm{C}_{6}^{2} \mathrm{H}_{6}$

The $\mathrm{C}-\mathrm{C}$ bond length of the following molecules are in the order
(a) $\mathrm{C}_{2} \mathrm{H}_{6}>\mathrm{C}_{2} \mathrm{H}_{4}>\mathrm{C}_{6} \mathrm{H}_{6}>\mathrm{C}_{2} \mathrm{H}_{2}$
(b) $\mathrm{C}_{2} \mathrm{H}_{2}<\mathrm{C}_{2} \mathrm{H}_{4}<\mathrm{C}_{6}{ }^{0} \mathrm{H}_{6}<\mathrm{C}_{2} \mathrm{H}_{6}^{2}$
(c) $\mathrm{C}_{2} \mathrm{H}_{6}>\mathrm{C}_{2} \mathrm{H}_{2}>\mathrm{C}_{6} \mathrm{H}_{6}>\mathrm{C}_{2} \mathrm{H}_{4}$
(d) $\mathrm{C}_{2} \mathrm{H}_{4}>\mathrm{C}_{2} \mathrm{H}_{6}>\mathrm{C}_{2}^{\circ} \mathrm{H}_{2}>\mathrm{C}_{6}^{2} \mathrm{H}_{6}$

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Key Concepts

Bond Order

Bond order refers to the number of chemical bonds between a pair of atoms. In general, a higher bond order, which indicates more shared electron pairs, results in a shorter and stronger bond. Understanding bond order is essential when comparing bonds because it directly influences bond length; more bonding interactions pull the atoms closer together.

Hybridization

Hybridization describes the mixing of atomic orbitals to form new hybrid orbitals that dictate the geometry and bonding characteristics of a molecule. For instance, atoms with sp, sp2, and sp3 hybridizations exhibit different bond lengths because the extent of s-character in the hybrid orbitals affects how tightly electrons are held around the nucleus. Greater s-character typically leads to shorter bonds due to the electrons being closer to the atomic nuclei.

Resonance Stabilization

Resonance stabilization occurs when electrons are delocalized over multiple atoms, rather than being confined to a single bond. This delocalization creates bonds with characteristics intermediate between typical single and double bonds. By averaging the bond characteristics, resonance can lead to bond lengths that do not correspond exactly to a standard single or double bond, and this concept is especially important in understanding aromatic compounds.

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