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 - 

FREE Expert Solution
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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]


94% (458 ratings)
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 - 

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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 .

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