Chapter 4 - Atomic Energy Levels Flashcards
Formula for energy of a photon
E(photon)=hv
h- plancks constant ( 6.626x10^-34 J s)
v- frequency
E- energy of photon
Wave properties
c=v(lambda)
c= speed of light
v= frequency
Lambda=wavelength
de Broglie equation
p=h/wavelength
Wavelength =h/ mu
p- momentum
h- plancks constant
m- mass
u- velocity
Heisenberg uncertainty principle
We cannot simultaneously know both the position and momentum of any particle particularly electrons
Principle quantum number
(n)
have only positive integer values
Indexes both the energy of the electron and the orbital size
Azimuthal quantum number
(l)
Indexes the angular momentum of the atomic orbital and shape of orbital
Can be 0 or any positive integer smaller than n
(n-1)
Magnetic quantum number
(m subscript l)
Indexes orientation of orbital
Can have positive or negative integer from 0 to l
Azimuthal quantum number and orbital name
Atomic orbitals are labelled according to their azimuthal quantum number (l)
l=0 s orbital
l= 1 p orbital
l= 2 d orbital
Spin quantum number
(m subscript s)
Possible values of +/- 1/2
Denotes two possible spin states of an electron
Pauli exclusion principle
Each electron has a unique set of quantum numbers
Aufbau principle
Orbitals are filled in order of increasing energy
Hunds rule
Electrons occupy sets of degenerate orbitals so as to give the maximum number of unpaired spins
Diamagnetic
Atom or ion with all electrons paired and therefore not attracted to magnetic field
Paramagnetic
Atom or ion has unpaired electrons and will be attracted to a magnetic field
Atomic radius
Decreases across a period and larger down a group
