quantum numbers Flashcards
principle QN
n - size of orbital
angular momentum QN
l - shape (n=1, l= 1, 0, n=2, l=2,1,0) s-0 p-1d-2f-3)
same vale of n= shell
same value of n & l= subshell
magnetic QN
m (l) orientation of orbital in space (2l+1) -l….0…l (number of orbitals in a subshell with a particular l value)
of orbitals in a shell
n squared
of subshells in a shell
n
electron spin QN
m (s) describes electron occupying orbital, tiny magnets spinning on axis (+1/2 or -1/2),
2 electrons with opposite s[pins in same orbital
paired
s subshells contains 1 orbital
s orbital
as principle QN increases
sphere/radius increase
radial probability distribution
where electron spends most of its time
probability drops to zero (node)
in between maxima
p orbitals
n ≥ 2, l can be 1 and m (l) can be -1,0,1 (each p subshell contains 3 orbitals p(x) p(y) p (z)- letters indicate axis oriented on, same in size shape and E)
d orbitals n ≥3
l=2, m(l)=-2,-1,0,1,2 3d (x squared- y squared)
E of single electronincreases
n increases
shells have same E regardless of subshells
1s
pauli exclusion principle
no 2 electrons can have exact same 4 QN (so M(s) must be different)- max of 2 electrons occupies orbital (electron configurations)
aufbau principle
build periodic table 1s,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s,5f,6d,7p
degenerate
when orbitals are of equal E (i.e. 2p)
hund’s rule
in orbitals of = E # of electrons w/ same spin is maximized ( pair last)
paired electrons
dimagnetic (repelled by magnetic field)
unpaired electrons(1 or more)
paramagnetic- have greater mass w/ magnet on in scale1
1/2 filled f and d orbitals exhibit more
stability.
