Ch 1 Atomic Structure Flashcards
(20 cards)
equation for light
c = (lambda)v
particle nature equation
E(photon) = h*v
Bohr model for hydrogen atom
E(n) = (-Rh)/(n)^2
Rh = rydberg constant
n = principal quantum number
emission of light
delta E = hv –> -Rh(1/n^2f - 1/n^2i)
principle quantum number (n)
designates size of atomic orbital
angular momentum (l)
shape of atomic orbital
magnetic quantum number (ml)
orientation of atomic orbital
electron spin quantum number (ms)
orientation of electron
Rules of principle quantum number
- larger n = larger size and high energy
- collection of orbitals with same n = shell
rules of angular momentum
- depends on n and range from 0 to n-1
- larger l = higher energy orbitals
- collection of orbitals with same value of l = subshell (s, p, d, f)
rules of magnetic quantum number
- depends on l and range from -l to +l
- each value of ml stands for an atomic orbital
- orbitals with same n and l value = same energy, no matter of different ml values
Pauli exclusion principle
no more than 2 e- in a single orbital; if there’s 2, there spins must be paired in opposite directions
nodes
regions where wave functions pass thru zero
radical nodes
n-l
angular nodes
of angular nodes / nodal planes is equal to the l value of that orbital
shielding
in multiple electronegative atoms, the e- repel and reduce the actual charge of the nucleus, Z, to a lower Zeff (effective nuclear charge)
penetration
e- can penetrate into inner shell of other e- and reduce shielding effects
s > p > d > f
effective nuclear charge
Zeff = Z - delta
delta = shielding constant estimated by Sater’s rule
Aufbau’s principle
e- are added to the lowest energy orbitals first before moving to higher energy orbitals
- energy of orbitals depend on both n and l
Hund’s rule
when several orbitals of equal energy (same n and l, but different ml) are available, e- enter singly with parallel spins
