'link to webMO'

ch08/note05.md

@@ -4,6 +4,12 @@
 Which atomic orbitals mix to form molecular orbitals and what are their
 relative energies? The graph on the left can be used to obtain the energy order of molecular orbitals and indicates the atomic orbital limits.
 
+<iframe src="https://al2me6.github.io/evanescence/"
+        width="800"
+        height="500"
+        allowfullscreen>
+</iframe>
+
 
 ### The non-crossing rule: States with the same symmetry never cross.
 

ch08/note06.md

@@ -102,18 +102,13 @@ value $104\degree$). Thus $H_2O$ has two lone-pair electrons.
 ![](images/watMO-diag.png)
 
 
-### 5. NH$_3$ molecule. 
-
-- In this molecule, nitrogen is also $sp^3$ 
-hybridized. The N atom electron configuration is $1s^22s^22p_x^12p_y^12p_z^1$. Thus
-a total of 5 electrons should be placed on the four hybrid orbitals. One of the
-hybrid orbitals becomes doubly occupied (``lone-pair electrons'') and the three
-remaining singly occupied hybrid orbitals form three sigma bonds to H atoms.
-Because of the lone-pair electrons, the geometry of $NH_3$ is tetrahedral with
-a bond angle of 109\degree (experimental value 107\degree).
-
-
+### Other Molecules
 
+<iframe src="https://al2me6.github.io/evanescence/"
+        width="800"
+        height="500"
+        allowfullscreen>
+</iframe>
 
 ### Numerical Calculations