Which of the follow will have the longest bond length?

Question

BlackTom AI · Accepted Answer

Let's evaluate the bond types and their typical lengths to compare them meaningfully.
Option a: C=C represents a carbon–carbon double bond. Double bonds are shorter than single bonds due to greater electron sharing, so the C=C bond length is generally around 1.34 Å.
Option b: C-O refers to a carbon–oxygen bond, which in many common valence contexts is a single bond (C–O) with a bond length around 1.43 Å; this is longer than most C=O double bonds but shorter than a typical C–C single bond in some cases, depending on substrate and resonance.
Option c: C-C indicates a carbon–carbon single bond. Single bonds are typically the longest among the common C–C/C–O combinations considered here, with lengths near 1.54 Å for a plain alkane C–C single bond.
Option d: C=O denotes a carbonyl double bond in many carbonyl-containing structures (like aldehydes, ketones), which is quite short due to strong pi bonding, usually around 1.20 Å, shorter than C=C and much shorter than C–C single bonds.

Comparing these tendencies, the longest bond length among the listed options is typically the carbon–carbon single bond (C–C), because single bonds lack the additional pi-bonding that pulls atoms closer together in double bonds or bonds to highly electronegative atoms in C–O or C=O. The other options involve multiple bonding or bonds to oxygen, which generally shorten the average bond length relative to a plain C–C single bond.

In summary, based on standard bond length conventions for these bond types, option c (C-C) corresponds to the longest bond length among the choices.

Which of the follow will have the longest bond length?

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