week 5 Flashcards
comparing hybridisation and MO theory models
see w5 vid24-25 for comparisons of the models
is metallic bonding directional or non-directional
non-directional
in metallic bonding, what are bands
how many electrons fit in a given band
- when valence orbitals interact to form molecular orbitals that are spread across the whole molecule
- a band is made from a degenerate set of orbitals with very small gaps between them
- bands extend across the whole structure
eg 2s orbital forms a band, 2p orbitals are degenerate so form a larger band
number of electrons:
- a band made of N number of orbitals can hold 2N number of electrons
what is the fermi level
the top of where the band is filled
describe using bands why metals conduct electricity in 2 ways
- there are very small energy gaps between MOs in bands so when voltage is applied, electrons can move from filled to empty MOs without much energy needed
- if the energy gap between 2 energy levels (eg 2s and 2p) is small enough, there can be overlap and electrons can conduct electricity over the bands
how do bands behave in an insulator
if a band is full and there’s a large band gap to the next band, electrons won’t be able to conduct electricity
how can bands behave in a semi-conductor
the band gap will be smaller than that of an insulator
conduction is possible if electrons are excited enough
reaction of alkene with bromine
what is step 1 in terms of orbital interaction
interaction between alkene π-orbital and bromine between:
- π-bonding MO in alkene is the HOMO
- σu* MO in Br2 is the LUMO
electrons are donated from the HOMO to the LUMO
reaction of alkene with bromine
describe the intermediate step in terms of orbitals and bonding
bromonium ion intermediate is formed
now the π-bond is broken, each C has an unhybridised pz orbital and these two have an in phase and out of phase combination
in-phase combination = adjacent lobes are same phase
- this combination interacts with the 4pz orbital of Br
out of phase combination = adjacent lobes are opposite phase
- this interacts with the 4px orbital of Br
energy gap between the two pz orbitals and the Br 4px orbital is greater because the overlap is better
6 electrons in total
- 1 from each C
- 4 from Br
reaction of alkene with bromine
what is step 2 in terms of orbital interactions
the bromide ion Br- is added to the molecule
bromide ion has a full set of valence orbitals
- donates electron density to the LUMO of the bromonium cation
- LUMO = anti-bonding MO from overlap between 4pz and carbon pz orbitals (see w5 vid27 for diagram)
- bromide attacks LUMO on the carbon side of the intermediate
- reduces bond order of bromonium ion
- C-Br bonds are formed