Chemistry Practice Problems Bond Order Practice Problems Solution: Use molecular orbital theory to predict whether or...

Solution: 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 - 

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 - 

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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