Term
| What does the red area within an electrostatic potential map indicate? |
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Definition
The area that is red is most likely to attract atoms or molecules that are positively charged since this area is negatively charged. |
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Term
| What does the blue area on an electrostatic potential map indicate? |
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Definition
The blue area indicates where negatively charged molecules or atoms are most likely to be attracted to since this area is positively charged |
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Term
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Definition
Atomic orbitals are fuctions that describe the motion of electrons either around the nucleus of the atom to which they currently belong or the nuclei to which they are currently in a bond with |
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Term
| What occurs when an atomic orbital equals 0? |
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Definition
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Term
| How do you determine electron density? |
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Definition
You square the orbital function |
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Term
| Describe the way(s) in which a 2p orbital can be represented |
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Definition
A 2p orbital can be represented 3 ways: 2px, 2py, and 2pz. In each version the node lies along the plane specified and the orbitals are typically drawn as mushroomhead-like structure flat along the plane of reference (see slide #7 from the first lecture for a real diagram and probably an easier explanation to this) |
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Term
| Describe how bonding is represented in Valence Bond Theory (VB/VBT) |
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Definition
Bonding is represented by the positive addition of 2 or more atomic orbitals on neighboring atoms |
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Term
| What is represented by the lowest point of a potential energy chart on an atomic level? |
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Definition
| Bond length (see slide #9 from lec 1) |
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Term
| What is represented by the total area under the curve of a potential energy graph on an atomic level? Is there anything else that is important to note about this? |
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Definition
The area under the graph is the bond dissociation energy. Its units are kcal/mol. |
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Term
| Why can't some molecules be represented normally using normal bond labeling procedures and how is this corrected? |
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Definition
Some valence electrons that are involved are delocalized. They therefore form resonance structures which depict constantly shifting and alternating bonds to the atoms involved |
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Term
| What do HOMO and LUMO stand for and why are they important terms? |
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Definition
HOMO: Highest Occupied Molecular Orbital. LUMO: Lowest Unoccupied MO. They denote the readiness and unreadiness (respectively) of a set of electrons to bind together to form a bond. |
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Term
| How can a sigma bond be formed? |
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Definition
It can be formed by the overlap of 2 p orbitals (see slide 13 lec 1 for diagram) |
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Term
| How can a pi bond be formed? |
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Definition
A pi bond can be formed by the sideways overlap of 2 parallel p orbitals (see slide 14, lec 1) |
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Term
| Describe what exactly happens when a compound like methane is formed in regards to what electrons do. |
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Definition
| Electrons go through a process called hybridization. Since there is only 1 s and 3 p orbitals from the original atoms they must be combined to form 4 idential bonds. They combine to form sp3 orbitals. |
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Term
| What is the degree at which hydrogens are at in a tetrahedral setup? |
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Definition
They're at 109.5 degrees. |
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