Lecture 13 Flashcards
stability
all simple ions are stable, once they have formed, they keep on existing
reactivity
if an electron is added, it can also be removed
any anion will react with a cation to form a lattice
electron transfer
for both cations and anions, a more electronegative element can replace the more electropositive metal
electropositive can reduce the electronegative one
complex ions
molecules are bigger than atoms
positive well
defined by the overlapping potential well of all of the nuclei
electrostatic attraction
energy levels are quantised, not all energy levels exist
these are molecular orbitals
electron transfer
high energy occupied orbitals lose electrons
low energy occupied electrons, lose electrons
dot and cross diagram
check notes
dative bonding
forms when both of the shared electrons come from one atom, rather than both sharing one each
quantum mechanics
energy is quantised, only some solutions to the Schrodinger’s equations are valid, depending on the symmetry of the potential well
born-oppenheimer approximation
nuclei are ‘big and heavy’, electrons are small and light
shake an atom, the electron will move but the nuclei won’t
quantum confinement
the more you confine something, the energy increases
allowing things to spread out, decreases energy
quantum confinement 2
atoms are formed by positive nuclei attracting negative electrons
by bringing these atoms together, electrons can delocalise around multiple nuclei, lowering their energy
delocalised = lower in energy
wave functions
as energy increases, the number of nodes increases
probability distributions are different for different energy levels
potential wells
to share electrons, the potential wells must overlap
