3.6 Flashcards
what is the orbital approximation and what is it for
it is an assumption that lets hydrogen be the starting point for other many electron atoms
the wavefunction for an n electron atom is the product of n single electron wavefunctions
what are the two types of electron spin
up and down spin + and - 1/2
the order electrons are put into shells according to the aufbau principle
two into 1s
two into 2s
1 in each 2p orbital then fill each one up with a second
what is the name of the principle that fills one of each pair in a shell first
hunds rule
what rule means no two electrons in an atom can have the same quantum numbers
the pauli exclusion principle
what are an anomalies in electronic configuration
the 4s being filled before the 3d because there is less electron electron repulsion even though it is higher energy
chromium has only 1 in the 4s because having the five parallel electrons in 3d and 4s have high exchange energies
why in hydrogen are the orbitals degenerate and in other atoms they are not
the other electrons cause repulsion
what is the effective nuclear charge
the actual charge felt by an electron from the nucleus taking into account the shielding
why is 2s more penetrating than 2p
because it has a node close to the nucleus meaning a area of electron density closer to 1s
do 2s and 2p orbitals get more or less stable across the period
more stable
what is slaters rules used to estimate
the effective nuclear charge
equation for slaters rule
Zeff = Z - S
where Z is atomic number and S is the shielding constant
where to find slaters rules for estimating the effective nuclear charge
page 157
drawbacks of slaters rules
they don’t tale into account stability from parallel electrons
they don’t distinguish between s and p electrons
