Quantum Test Flashcards
for emission the change in energy =
initial energy - final energy
large change in energy = _____ frequency and _______ wavelength
high frequency
short wavelength
small change in energy = ______ frequency and ______ wavelength
low frequency
high wavelength
in the balmer series n final =
2
balmer series color emitted when n initial=6
purple
balmer series color emitted when n initial =5
blue
balmer series color emitted when n initial =4
green
balmer series color emitted when n initial =3
red
principle quantum #
n
n determines
binding energy/shell
n =
1,2,3,…
angular momentum
l
l describes the
subshell/shape of the orbital
l =
0,1,2,3, … n-1
magnetic quantum #
mℓ
mℓ determines
behavior in the magnetic field, the specific orbital and orientation
mℓ =
-l, …. 0 … +l
what orbital when l = 0
s orbital
what orbital when l = 1
p orbital
what orbital when l = 2
d orbital
what orbital when l = 3
f orbital
when mℓ = -1 or 1 it is
x or y
when mℓ =0 it is
z
physical interpretation of a wave function
the probabbility of a finding an electron in a defined region is proportional to the square of the wave function
probability density =
[Ψnlm (r,θ,Φ)]^2
▪probability/volume
▪likelihood of locating an electron in a given region of space
bohrs radius
a sub 0
52.9 pm for 1s
RPD
radial probability distribution
r sub mp
distance from the nucleus (r) you will most likely find an electron at
Ψnlm(r,θ,Φ)=
radial wave function x angular wave function
E subn
binding energy
radial node
▪where the radial wave function =0
▪means there is 0 possibility of measuring the particle at that value of r
nodal plane
arise from angular nodes in the wave function
of angular nodes =
l
angular node
where the angukar wave function changes signs
number of radial nodes
n-l-1
total # of nodes =
n-1
l=2 mℓ=0
dz^2
radial wave function (R)
probability of finding an electron at some distance from the nucleus and its energy
angular wave function (Y)
sets an orientation of the orbital in 3d space
energy of the electron increases as the distance from the nucleus ______
increases
shading depicts what?
different signs of the wave function
magnetic spin
ms
ms =
+ 1/2 (up) or -1/2 (down)
ms describes
electron, not orbital
Ψ(nl)mℓ(ms) describes
electron
how many p orbitals
e
how many d orbitals
5
how many s orbitals
1
how many quantum numbers define an electron
4
pauli exclusion principle
▪no 2 electrons can be in the same orbital and have the same spin
▪no 2 electrons in the same atom can have the samr 4 quantum numbers
as n increases the probability of finding an electron moves
farther away from the nucleus
energy of an electron in the hydrogen atom is determined by
n
energy of an electron in a mulrielectron system depends on
n and l
max # of electrons that can occupy an energy level descrubed by n is
2n^2
of f orbitals
7
wavelength associated with a moving particle
debroglie wavelength
degenerate orbitals
have the sams amount if energy
electron configuration
the arrangement of electeons in the orbitals of an atom
