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CHMA10H3 Introductory Chemistry 1 Lecture Notes (study guide solution) University of Toronto
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CHMA10H3 Introductory Chemistry 1 Lecture Notes (study guide solution) University of Toronto
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CHMA10H3 Introductory Chemistry 1Lecture Notes (study guide solution)
University of Toronto
, CHMA10H3 Lecture Notes
Monday November 5th
The sp orbital:
- Two electron groups, linear shape, 180 degrees.
- Hybridized or unhybridized orbitals for the sigma bonds, while unhybridized p orbitals
for pi
bonds.
- Usually, a double/triple bond is a sigma accompanied by pi bonds.
- Linear structure caused by the hybridization of orbitals into either
Example: acetylene CH--- CH
Note that the 2sp hybrid orbital for Nitrogen contains a lone pair (the left one is already filled
with two electrons)
Predicting Hybridization, Bonding
Scheme One: Lewis structure
Two: VSEPR THEORY: electron group geometry around each
central atom Two b: Hybridization scheme
Three: Sketch atomic and hybrid orbitals in the molecule, overlap of appropriate
orbitals Four: Pi or sigma bonds.
Take for example: CH3CHO
C1: 4 electron groups, therefore
tetrahedral, sp3 C2: 3 electron groups, sp2
trigonal planar
Next step: Label the bonds: usually pi bonds are involved in double to triple
bonds. Limits with Valence Bond Theory
VB theory predicts many properties better than Lewis theory, such as schemes, strengths,
lengths, rigidity, etc.
However, it still isn't perfect. It can't predict all properties perfectly, such as the magnetic
behaviour of O2.
Additionally, valence bond theory assumes that the electrons are localized in orbitals on the
atoms in the molecule, delocalization is ignored.
Molecular Orbital Theory
In MO theory, we apply Schrodinger's wave equation to the molecule to find a set of molecular
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