This chapter relates back to chapter 2 (lewis structures) and Chapter 7 (electronic configuration). We study how some molecules are able to have double bonds and why some can’t create double bonds.
-
this
↳ But is also another way of drawing [N5] where it is linear
Molecular orbital
Theory
·
orbitals of molecules
↳) wave function superpositions
↳) superpositions change location of electron density
Example: Hd (hydrogen gas) Is Hydrogen
H atOm #atom
& ⑧
M
It.? # ↑
is (
A
-
super position
graph
bond formed
->
graph
~ epresen + ation
M * *
Bonding
↳ molecular orbitals
↳> increases electron density in
region between nuclei
& estructive interference
forms antibonding no
-
an
-
decrease in amplitude
-
When wave function is negative
A
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