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Advanced Higher Chemistry Unit 3 > (a) molecular orbitals > Flashcards

(a) molecular orbitals Flashcards

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1
Q

Can VESPER explain the bonding in all compounds?

A

No

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2
Q

What, other than VESPER, can provide an explanation for complex molecules?

A

Molecular orbital theory

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3
Q

When do molecular orbitals form?

A

When atomic orbitals combine

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4
Q

What is the relationship between the number of molecular orbitals that are formed and the number of atomic orbitals which are combined?

A

They are equal

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5
Q

What does the combination of two atomic orbitals result in?

A

A bonding and an anti-bonding orbital

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6
Q

Where are the nuclei situated in molecular orbitals?

A

Both are found in the bonding molecular orbital.

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7
Q

What is the basis of the bonding between atoms?

A

The attraction between the positively charged nuclei and the negatively charged electrons.

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8
Q

What is the maximum number of electrons per molecular orbital?

A

2

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9
Q

What is the bonding molecular orbital in a non-polar covalent bond?

A

Symmetrical, about the mid-point between the 2 atoms.

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10
Q

What is the bonding molecular orbital in a polar covalent molecule?

A

Asymmetrical about the 2 midpoint between 2 atoms.

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11
Q

What atom has the greater share of the bonding electrons?

A

The atom with the greater electronegativity.

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12
Q

What is a case of extreme asymmetry?

A

Ionic compounds

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13
Q

Where are the bonding molecular orbitals in an ionic compound?

A

Almost entirely located around one atom.

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14
Q

What does extreme asymmetry result in?

A

The creation of ions.

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15
Q

What kind of atomic orbital overlap occurs in sigma bonds?

A

End-on

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16
Q

What kind of atomic overlap occurs in pi bonds?

A

Side-on

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17
Q

How can carbons bonding and shape be deciphered?

A

Hybridisation

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18
Q

What is hybridisation?

A

The process of mixing atomic orbitals within an atom to generate a set of new atomic orbitals called hybrid orbitals.

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19
Q

What is the energy said to be in hybrid orbitals?

A

Degenerate

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20
Q

In alkanes the 2s orbitals and the 2p orbitals of the carbon hybridise to form what?

A

Degenerate sp3 hybrid orbitals

21
Q

What shape is adopted by the sp3 hybrid orbitals?

A

Tetrahedral

22
Q

How do the sp3 molecules overlap with other atomic orbitals?

A

End-on

23
Q

What does the end on overlap of sp3 molecules with other atomic orbitals produce?

A

sigma bonds.

24
Q

What can the bonding of 2 alkenes be described as?

A

sp2 hybridisation

25
Q

What do the 2s orbitals and 2p orbitals hybridise to form?

A

sp2 hybrid orbitals

26
Q

What shape do sp2 hybrid orbitals adopt?

A

Trigonal planar

27
Q

How do sp2 orbitals overlap and what do they form?

A

End-on to form sigma bonds

28
Q

What happens to the remaining 2p orbital on each carbon?

A

Remains unhybridised and lies perpendicular to the axis of the pi bond.

29
Q

How do the remaining 2p orbitals overlap and what do they form?

A

Side-on to form pi bonds

30
Q

How can the bonding of benzene and other aromatic systems be described?

A

sp2 hybridisation

31
Q

What bond is between the carbon atoms in a benzene ring?

A

Sigma and pi

32
Q

What structure does a benzene ring have?

A

Cyclical

33
Q

What can the electrons in a benzene ring be described as?

A

Delocalised

34
Q

How can the bonding between alkynes be described?

A

sp hybridisation

35
Q

(sp) What do the 2s orbital and 2p orbital hybridise to form?

A

Two degenerate hybrid orbitals.

36
Q

What arrangement do the 2 degenerate hybrid orbitals adopt?

A

Linear

37
Q

How do the hybrid sp molecules overlap and what do they form?

A

End-on to form sigma bonds.

38
Q

What happens to the 2 remaining 2p orbitals (sp)?

A

The overlap side on to form 2 pi bonds.

39
Q

How else can molecular orbital theory be used?

A

To explain why organic molecules are colourless or coloured.

40
Q

What orbital do electrons fill up first?

A

Bonding molecular orbitals.

41
Q

What orbital is left unfilled?

A

Anti-bonding molecular orbitals.

42
Q

What is the highest bonding molecular orbital containing electrons called?

A

Highest Occupied Molecular Orbital (HOMO)

43
Q

What is the lowest anti bonding molecular orbital called?

A

Lowest Unoccupied Molecular Orbital (LUMO)

44
Q

An absorption of electromagnetic energy can cause what?

A

Electrons to be promoted from HOMO to LUMO.

45
Q

Why do most organic molecules appear colourless?

A

The energy difference between HOMO and LUMO is relatively large.

46
Q

What does a large difference between HOMO and LUMO result in?

A

The absorption of light from the ultraviolet region of the spectrum.

47
Q

What do some organic molecules contain?

A

Chromophores.

48
Q

What is a chromophore?

A

A group of atoms within a molecule that is responsible for absorption of light in the visible region of the spectrum.

Advanced Higher Chemistry Unit 3 (4 decks)

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