chem unit 3

interference

interaction between waves

constructive interference

waves are in phase and combine

destructive interference

waves are out of phase and cancel

diffraction

bending and spreading of waves as they hit an object 

photoelectric effect

observation that metals emit electrons when light is shined upon them

n

principle quantum number, determines energy level of electron

indeterminacy

present circumstances do not necessarily determine future events

l

angular momentum quantum number, determines shape of electron

ml

magnetic quantum number, determines orientation of electron

orbitals

probability distribution maps showing where electrons are likely to be found

ms

spin quantum number, determines spin of electron

phase

the sign of a waves amplitude, positive or negative

pauli exclusion principle

no two identical electrons can have the same four quantum numbers, implies there can only be two electrons per orbit

aufbau principle

electrons fill lower energy orbits before moving to higher energy levels

hunds principle

electrons will fill orbits individually before pairing up

madelung principle

explains the order in which atomic orbits are filled

radial distribution plot 

graphical representation of probability of finding electrons 

degenerate orbitals

orbitals with the same energy within the same subshell

ionization energy

energy required to remove an electron in the gaseous state

electron affinities

energy change associated from gaining an electron in the gaseous state

van der waals radius

radius between non bonded atoms

covalent radius 

radius between bonded atoms 

paramagnetic

has unpaired electrons, is attracted to a magnetic field

diamagnetic

does not have unpaired electrons, is slightly repelled by a magnetic field