Problem: Use molecular orbital theory to predict whether or not each of the following molecules or ions should exist in a relatively stable form.H2 2 - 

🤓 Based on our data, we think this question is relevant for Professor Prado's class at UCLA.

FREE Expert Solution

We’re being asked to predict whether or not H22- should exist in a relatively stable form


For this, we need to determine the bond order for each species. The bond order tells us the stability of a bond


The higher the bond order, the more electrons holding the atoms together, and therefore the greater the stability


We will do the following steps to solve the problem:

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:


Bond Order = 12[# of e- in bonding MO -# of e- in antibonding MO]


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Problem Details

Use molecular orbital theory to predict whether or not each of the following molecules or ions should exist in a relatively stable form.

H2 2 - 

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 Bond Order concept. If you need more Bond Order practice, you can also practice Bond Order practice problems.

What professor is this problem relevant for?

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