P Orbitals Flashcards

1
Q

What is meant by directional and what orbitals are directional?

A

These are orbitals that prefer a specific orientation in space where the lobes representing electron density lie along an axis

P orbitals are directional

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2
Q

What does the directionality of the p orbitals mean?

A

This means they all interact differently

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3
Q

Describe the different orientations of the p orbitals

A

The pz orbitals are directed towards each other whereas px and py orbitals on each atom are orientated 90 degrees to each other to the direction of the other atom

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4
Q

Describe the inphase combination of pz orbitals

A

Constructive interference
End on overlap forms sigma bonding orbitals

( see diagrams)

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5
Q

Describe the out of phase combination of pz orbitals

A

Destructive interference forms sigma antibonding orbitals
There is a node in the middle of this orbital
The more nodes= higher energy

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6
Q

Describe the in phase combination of px orbitals

A

Constructive interference
Side on overlap forms pi bonding orbitals
The pi bonds have a nodal plane along the internuclear axis
Electrons are delocalised in pi clouds (increased region of electron density above and below the plane
(See diagram)

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7
Q

Describe the out of phase overlap of px orbitals

A

Destructive interference forms pi antibonding orbitals
(Side on overlap)
Node along plane and in between the orbital

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8
Q

What is the internuclear axis?

A

This is the z axis that horizontally goes through the nucleus

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9
Q

What is a HOMO?

A

Highest occupied molecular orbital

This is where electrons are donated from

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10
Q

What is a LUMO?

A

Lowest unoccupied molecular orbitals

This is where electrons are donated to

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11
Q

Describe sigma and pi orbitals around the internuclear axis

A

Sigma bonds are cyndrically symmetrical along the internuclear axis
Pi bonds have nodal plane along the internuclear axis

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12
Q

Why are antibonding orbitals higher in energy than bonding orbitals?

A

Antibonding orbitals have more nodes than sigma

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13
Q

Why are pi orbitals stabilised and destabilised to a lesser degree than sigma orbitals

A

The interaction between px, px and py, py is less effective than the interaction between pz and px and py don’t point towards each other
This means overlap is not as good

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14
Q

Why does BDE decrease faster for pi bonds as internuclear separation increases?

A

Pi overlap is more distance sensitive

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15
Q

Why is there no net interaction between a pz orbital and a px/y orbital?

A

This is because there is both a bonding and antibonding interaction (where in phase and out of phase px interacts with one phase lobe of pz orbital)
The antibonding and bonding interaction cancels out
(See diagram)

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16
Q

Why do sigma bonding stabilise more and sigma antibonding destabilise more than pi bonding?

A

This is because sigma overlap is greater than pi overlap