Question

Of single, double, and triple covalent bonds, which is the longest? Which is the strongest?

Answer 1

What do you think...?

Explanation:

The modern chemical bond is conceived to be a region of high electron density between two positively charged atomic nuclei which NEGATES electrostatic repulsion between the positive charges, and a net attractive force operates that binds the nuclei together.

In a single bond, electron density is situated BETWEEN the nuclei...in a double bond the electron density lies in PLANES above and below the atom-atom vector...and for a triple bond the electron density lies normal to the plane of the double bond... (and yes there are quadruple bonds, but I am not going to consider it here)…

This is best addressed pictorially...

And typical carbon-carbon lengths...`C-C`, `1.54xx10^-10*m`; `C=C`, `1.40xx10^-10*m`; `C-=C`, `1.21xx10^-10*m`...

And the greater the bond order, the greater the bond strength, and the SHORTER the bond....

I will leave you to find the values associated with `N-N`, `N=N`, and `N-=N` bonds...and with `C-O-C`, `C=O`, and `""^(-):C-=O^+` bonds...do it...