hydrogenic atoms
A hydrogenic atom contains this number of electrons
one electron
This quantum number determines orbital shape
l
s orbitals have this general shape
spherical
This principle states that no two electrons can share the same four quantum numbers.
This type of orbital overlap leads to the strongest covalent bond formation.
head on over lap
This equation is solved exactly for hydrogenic atoms.
schrodinger equaion
This quantum number determines orbital orientation in space.
m_l
p orbitals contain this number of lobes.
2
This rule states electrons occupy degenerate orbitals singly first.
Hunds rule
This concept explains why the 2s orbital is lower in energy than the 2p orbital in many-electron atoms.
reduced shielding
The energy of hydrogenic atoms depends primarily on this quantum number.
principle quantum number n
This quantum number has allowed values of +1/2 and –1/2.
m_s
This quantity represents regions where probability density is zero.
nodes
Inner electrons reduce the effective nuclear charge felt by outer electrons through this effect.
shielding
This property explains why electrons are removed first from outer orbitals during ionization.
higher energy
These two mathematical parts make up hydrogenic wavefunctions after separation of variables.
radial and angular functions
The number of orbitals in a subshell can be determined from this relationship.
2l+1
Orbitals with more radial nodes generally possess this.
higher energy
This describes how closely an orbital approaches the nucleus.
penetration
This explains why atoms with unpaired electrons interact strongly with magnetic fields.
electron spin/paramagnetism
As nuclear charge increases in hydrogenic species, orbital energies become this.
more negaive/lower
For n=4n = 4n=4, the maximum possible value of lll is this.
3
The angular part of the wavefunction is described mathematically using these functions.
spherical harmonics
Because s orbitals penetrate better, they are generally this relative to p orbitals of the same shell.
lower in energy
The orbital approximation is useful because it allows chemists to describe atoms using these simpler one-electron functions.
orbitals