Differences in Bond Length

[JakeSaum_1A]

I'm a little unclear as to what accounts for differences in bond length. Why were double bonds about 120 Angstroms and Single bonds 140 Angstroms?

[Benjamin Chen 1H]

I think it has something to do with hybridization of atomic orbitals, where the character ratios of p and s tell us why single bonds are longer than double bonds. Maybe this link helps.

sp hybridization | AP Chemistry | Khan Academy:
https://www.youtube.com/watch?v=BRHfy7envyQ

[Samuel Flores 1E]

Hello! Conceptually, you can also think of the difference in bond lengths as a result of the strength of the single/double bond. Since double bonds involve more electrons, they are stronger, and they will pull the atoms closer together, resulting in a shorter bond length. On the other hand, a single bond is not as strong, so it does not pull the atoms as close together, resulting in a longer bond length.

Hope this helps!

[Peter DePaul 1E]

Double bonds pull the atoms closer together so the bond length will be shorter than that of single bonds. This is why a double bond is 120 Angstroms and single bonds are 140 Angstroms.

[aashmi_agrawal_3d]

This is because single bonds have less electrons so they are not as strong and cannot pull the atoms as close to one another. However, a double bond is stronger and can pull the atoms closer together, making the bond shorter.

[Jaclyn Dang 3B]

The bonds get shorter due to the fact that they are pulled in closer. Double bonds have more electrons and are pulled in more tightly. Using this, you would know that triple bonds are shorter than double bonds and double bonds are shorter than single bonds.

[Jason Knight - 1F]

The length of a bond typically is in relation to the type of bond associated with the molecule. Double bonds are typically shorter and stronger compared to single bonds. Conceptually, the length of a bond is approximately the sum of the covalent radii of the atoms.