General Chemistry 1A. Lecture 09. Breaking the Octet Rule.

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UCI Chem 1A General Chemistry (Winter 2013)
Lec 09. General Chemistry -- Breaking the Octet Rule
Instructor: Amanda Brindley, Ph.D.

License: Creative Commons BY-NC-SA

This video is part of a 23-lecture undergraduate-level course titled "General Chemistry" taught at UC Irvine by Amanda Brindley, Ph.D.

Recorded March 22, 2013.

Index of Topics:
0:00:17- Breaking the Octet Rule
0:06:44 Resonance Structures
0:14:28 Delocalized Electrons
0:16:40 Line Structures and Rules
0:24:06 What is the Formula...
0:27:55 Benzene
0:30:30 Electronegativity
0:40:06 Microwaves
0:44:29 Back to Lewis Structures

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  5. OpenCourseWare
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Комментарии
Автор

6:46 resonance structures and delocalized electrons; 20:00 line structures; 32:00 electronegativity and polarity; 38:00 O3; 40:42 microwaves

edwinchen
Автор

Terrific job here! Helpful for review.

donaldpryor
Автор

When drawing Lewis structure for carbon monoxide, we have no choice but to put -1 formal charge on C and +1 formal charge on O. But O is a lot more electronegative than C. So in real life, the partial negative end is on O or on C?

edwinchen
Автор

4:28 POCl3, for P=O to form, P is sp3 hybridized so it must use one of its 3d ortibal to form a pi bond with a 2p AO of oxygen. Can 3d orverlap sufficiently with 2p for a pi bond to form? If O's electron skip 2p and go to 3d, won't that break Hund's rule? Why is formal charge so important? This is just an electron accounting device, like oxidation state. It is not as if P really bears a positive charge.

edwinchen
Автор

0:25 "when you get to that 2nd period, you cannot have more than two." Shouldn't it be 8?

edwinchen