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**Problem**: Explain the following.The O22+ ion has a stronger O-O bond than O2 itself.

###### FREE Expert Solution

We’re being asked why O_{2}^{2+} ion has a stronger O-O bond than O_{2} itself.

For this, we need to determine the bond order for each species.

The ** bond order** tells us the stability of a bond:

*a higher bond order means the bond is more stable and stronger*.

* Step 1:* Calculate the total number of valence electrons present.

* Step 2:* Draw the molecular orbital diagram.

**Step 3:**** **Calculate the bond order of the molecule/ion.

Recall that the formula for ** bond order** is:

$\overline{){\mathbf{Bond}}{\mathbf{}}{\mathbf{Order}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{1}}{\mathbf{2}}{\mathbf{[}}{\mathbf{\#}}{\mathbf{}}{\mathbf{of}}{\mathbf{}}{{\mathbf{e}}}^{{\mathbf{-}}}{\mathbf{}}{\mathbf{in}}{\mathbf{}}{\mathbf{bonding}}{\mathbf{}}{\mathbf{MO}}{\mathbf{}}{\mathbf{-}}{\mathbf{}}{\mathbf{\#}}{\mathbf{}}{\mathbf{of}}{\mathbf{}}{{\mathbf{e}}}^{{\mathbf{-}}}{\mathbf{}}{\mathbf{in}}{\mathbf{}}{\mathbf{antibonding}}{\mathbf{}}{\mathbf{MO}}{\mathbf{]}}}$

###### Problem Details

Explain the following.

The O_{2}^{2+} ion has a stronger O-O bond than O_{2} itself.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the MO Theory: Bond Order concept. You can view video lessons to learn MO Theory: Bond Order Or if you need more MO Theory: Bond Order practice, you can also practice MO Theory: Bond Order practice problems .

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Altomare's class at UCF.