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Advanced Higher Chemistry > Molecular Orbitals > Flashcards

Molecular Orbitals Flashcards

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1
Q

What can orbitals be used to explain?

A

The bonding between atoms

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2
Q

What are atomic orbitals?

A

The volume of space that the electron of an atom is likely to be found

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3
Q

What happens when atomic orbitals overlap?

A

They combine to form molecular orbitals

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4
Q

What are sigma bonds?

A

The end on overlapping of orbitals

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5
Q

What governs the type of intermolecular bonding?

A

The shape of the molecular orbital

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6
Q

How are non-polar bonds formed?

A

When two atoms of the same element bond

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7
Q

What can be said about the molecular orbitals formed in non-polar elements?

A

The molecular orbital formed from overlapping atomic orbitals is symmetrical around a mid-point where the bonding electrons are most likely to be found

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8
Q

What is a polar covalent bond?

A

When there is a large difference between the electronegativities of the two elements involved in the bond

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9
Q

What can be said about the molecular orbits in polar covalent bonds?

A

The bonding molecular orbitals will be asymmetrical

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10
Q

What happens when ionic bonds form?

A

There is extreme asymmetry

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11
Q

What does hybrid theory assume?

A

That the 2s and 2p orbitals of carbon atoms combine to form four degenerate orbitals

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12
Q

What are the hybrid orbitals formed from 1 s orbital and 3p orbitals called?

A

They are called sp³ orbitals

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13
Q

What happens in alkanes?

A

All four hybrid orbitals are used to form sigma bonds

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14
Q

What can be said about sigma bonds?

A

They allow free rotation around orbitals

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15
Q

How are C-C bonds in alkanes formed?

A

From the overlapping of sp³ orbitals forming sigma bonds

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16
Q

How many sigma bonds are in ethane?

A

7

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17
Q

What does an electron being promoted to higher energy levels result in?

A

The formation of 3 hybrid orbitals, with one remaining unhybridised 2p orbital

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18
Q

What is bonding in alkanes due to?

A

hybridisation

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19
Q

What are the hybrid orbitals from one s orbital and two p orbitals called?

A

sp² orbitals

20
Q

What is the angle between sp² orbitals?

A

120 degrees

21
Q

What is a pi bond?

A

The sideways overlap of two parallel atomic orbitals

22
Q

What is the comparison between sigma and pi bonds?

A

Pi bonds are weaker than sigma bonds

23
Q

What bonding orbitals are present in C-C bonds?

A

1 sigma bond

24
Q

What bonding orbitals are present in C=C bonds?

A

1 sigma and 1 pi

25
Q

What bonding orbitals are present in C≡C bonds?

A

1 sigma and 2 pi

26
Q

What are isomers?

A

Molecules with the same chemical formula but different structural formula

27
Q

What can be said about structural isomers?

A

They have different physical and chemical properties

28
Q

What are the two types of stereoisomerism?

A
  • geometric isomerism

* optical isomerism

29
Q

What is geometric isomerism a result of?

A

A lack of rotation around a bond

30
Q

What is a cis isomer?

A

cis means the functional group is on the same side of the C=C

31
Q

What is a trans isomer?

A

When the functional group is on opposite sides of the C=C bond

32
Q

Why do trans isomers have higher mpts?

A

As these molecules can pack more closely together thus maximising the intermolecular forces

33
Q

Why do cis molecules have higher bpts?

A

Because of their PD-PD interactions

34
Q

What are the types of geometric isomerism?

A
  • cis isomerism

* trans isomerism

35
Q

Why are cis isomers more readily dehydrated than trans isomers?

A

because of the close proximity of the OH groups

36
Q

What are optical isomers?

A

They are mirror images of each other but are not superimposable

37
Q

What does a tetrahedral molecule have the potential to be?

A

chiral

38
Q

How does chirality occur?

A

when the middle atom is attached to four different groups

39
Q

What does a polariser allow?

A

Light vibrating in only a single plane to pass through them

40
Q

What are enantiomers?

A

Another term used to describe optical isomers

41
Q

What is a racemic mixture?

A

One which contains equal amounts of each enantiomer

42
Q

What type of hybridisation is present in alkynes?

A

sp hybridisation

43
Q

What type of hybridisation is present in alkenes?

A

sp² hybridisation

44
Q

What type of hybridisation is present in alkanes?

A

sp³ hybridisation

45
Q

What does the combination of two atomic orbitals result in?

A

the formation of a bonding and an antibonding orbital

46
Q

When electrons fill bonding molecular orbitals, what do they leave behind?

A

Higher energy antibonding orbitals unfilled

47
Q

How many groups are changed in enantiomers ?

A

Only 2.

Advanced Higher Chemistry (12 decks)

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