Week 16 Flashcards
Gas phase electron transfer
Favourable gas phases are those where the the element that is taking the electron has a higher electronegativity = lower valence orbital energy
Born-Oppenheimer
States that electrons are small and can move quickly whilst atomic nuclei are larger and heavier so don’t move as fast
Coulomb interactions
Coulomb’s law states opposites attract and like charges repel, energy is given out if two opposite charges move towards each other. Work is needed to pull two opposite charges apart. Interactions get weaker as distance increases
Quantum confinement
The more restricted a particle is to stay in a particular volume of space, the higher it’s energy.
The more a particle is allowed to delocalise, the lower it’s energy becomes
Potential well
A potential well is the region surrounding a local minimum of potential energy. Energy captured in it cannot convert to another type of energy because it’s captured in the local minimum of a potential well.
Valence bond theory
When two orbitals on different atoms overlap, a new bigger orbital forms which allows two electrons to delocalise across the two atoms, lowering them both in energy.
Bonding
In phase combination produced an orbital which is lower in energy than the original atomic orbitals
Anti-bonding
Out of phase - produced an orbital which is higher in energy than the original orbitals
Aufbau principle
Fill the orbitals from the lowest energy up
Hunds rule of maximum multiplicity
for orbitals of the same energy, electrons first fill up with all spins parallel, then anti parallel pairings
Bond order
Bonding orbital electrons - anti bonding orbital electrons / 1/2
Valence on periodic tables
First column is +1
Second Column is + 2
Penultimate colomn is -1
Last colomn is no charge
Orbital stability based off of MO
E.g. H2+ has one electron in a bonding orbital and an empty anti bonding so will have a bond order of 0.5 for a weak but stable bond
H2- has two electrons in bonding and one electron in anti bonding and also has a bond order of 0.5 giving the same result
H2 2- is not stable because it has two electrons in a bonding orbital and 2 in the anti bonding so has a bond order of zero
HOMO
Highest occupier molecular orbital
Bottom of the MO
LUMO
lowest unoccupied molecular orbital