1. Chapter 10 Chemical Bonding II: Sections 10.5-10.7
By: Raphiel O’Connor

2. 10.5 - Molecular Shape and Polarity
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One Dimension Vectors
A B = R
A B = R N
Common Cases in Determining Polarity with Dipole Moments
Linear, nonpolar, 180°
Trigonal Planar, nonpolar, 120°
Tetrahedral, nonpolar, 190.5°
Bent, polar, less than 180°
Trigonal Pyramidal, polar, 190.5° H H H H C
Two Dimension Vectors
A R B H H H
Three or More Dimensions of Vectors
R R
A R’ B
C C + + + -

3. 10.6 - Valence Bond Theory: Orbital Overlap as a Chemical Bond
Electrons exist in a quantum state.
The simplest theory is the Valence Bond Theory that support the idea of quantum mechanics.
The graph showing the change in energy between bonding H atoms shows the determination of shape based on bond type and also how energy changes during bonding.
The energy increases as the nuclei approach one another.
Interacting Energy of Two Hydrogen Atoms E
H-H distance

4. 10.7 - Valence Bond Theory: Hybridization of Atomic Orbitals
The orbitals of molecules will not necessarily act the same as those of an atom.
In short, hybridization is a mathematical process that standard orbitals undergo to create new orbitals called hybrids that more accurately represent the distribution of electrons.
The total number of electrons stays the same between the standard and hybrid orbital formations.
The types of standard bonds used to make the hybrid determines its shape and properties.
The hybridization that yields the least amount of energy overall will occur instead of the other options.

5. sp³ Hybridization y y x x z z + y y x x z z
*Not proportionally accurate*

6. sp² Hybridization y x z + y y x x z z
Two kinds of orbital creates two different types of bonds, the pi bond:π, for standard orbitals. And the sigma bond:σ, for hybridized orbitals. π= σ= y x z + y y x x z z
*Not proportionally accurate*

7. sp Hybridization y
2xπ= σ= y x + x z z
*Not proportionally accurate*