Problem: Use molecular orbital theory to complete this table BY FILLING FLANKS, 0,1,2,3, or 4NF = (δ1s) ___(δ1s*) ___(δ2s) ___(δ2s*) ___(π2p)___ (δ2p) ___(π2p*)   Bonding order=NF+ = (δ1s) ___(δ1s*) ___(δ2s) ___(δ2s*) ___(π2p)___ (δ2p) ___(π2p*)   Bonding order=NF- = (δ1s) ___(δ1s*) ___(δ2s) ___(δ2s*) ___(π2p)___ (δ2p) ___(π2p*)    Bonding order=

FREE Expert Solution

We’re being asked which species is the most stable. For this, we need to determine the bond order for each species. The bond order tells us the stability of a bonda higher bond order means the bond is more stable.


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 MO-# of e- in antibonding MO]


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Problem Details

Use molecular orbital theory to complete this table BY FILLING FLANKS, 0,1,2,3, or 4

NF = (δ1s) ___(δ1s*) ___(δ2s) ___(δ2s*) ___(π2p)___ (δ2p) ___(π2p*)   Bonding order=

NF+ = (δ1s) ___(δ1s*) ___(δ2s) ___(δ2s*) ___(π2p)___ (δ2p) ___(π2p*)   Bonding order=

NF- = (δ1s) ___(δ1s*) ___(δ2s) ___(δ2s*) ___(π2p)___ (δ2p) ___(π2p*)    Bonding order=

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