Quantum Numbers Flashcards
What shape is principle (n)?
shell
What values is principle (n)?
zero, positive integers
What is the position of a lower n?
closer to nucleus
What are the characteristics of a higher n?
larger atom and more energy
n=1 distance to nucleus
closer
n=5 distance to nucleus
farther
n=1 relative size of orbital
smaller
n=5 relative size of orbital
larger
n=1 relative energy
smaller
n=5 relative energy
larger
What is angular momentum (𝓵)
subshell
shape of the orbital
What are the values of angular momentum (𝓵)?
0…n-1
if n=1, 𝓵=0
if n=3, 𝓵=0, 1, 2
values correspond to certain shapes
What is magnetic (m𝓵)
number of orbitals in a subshell
What are the values of magnetic (m𝓵)?
integers from -𝓵 to 𝓵
if 𝓵=1, m𝓵=-1, 0, 1 (3 total)
all equal energy
What are the 𝓵, m𝓵, # of orbitals, and orbital name for n=1?
0) 0) 1 orbital) 1s
What are the 𝓵, m𝓵, # of orbitals, and orbital name for n=2?
0) 0) 1 orbital) 2s
1) -1, 0, 1) 3 orbitals) 2p
What are the 𝓵, m𝓵, # of orbitals, and orbital name for n=3?
0) 0) 1 orbital) 3s
1) -1, 0, 1) 3 orbitals) 3p
2) -2, -1, 0, 1, 2) 5 orbitals) 3d
What are the 𝓵, m𝓵, # of orbitals, and orbital name for n=4?
0) 0) 1 orbital) 4s
1) -1, 0, 1) 3 orbitals) 4p
2) -2, -1, 0, 1, 2) 5 orbitals) 4d
3) -3, -2, -1, 0, 1, 2, 3) 7 orbitals) 4f
How do we apply quantum numbers?
identify size, shape, and relative energy of orbital where electron is likely to be
What are the characteristics of 𝓵=1?
peanut shape
3 orientations (m𝓵=-1, 0, 1)
degenerate––equal energy
differ only based on axis(plane)
contains one node
Phasing
principle energies above n=1 have p-orbitals
What are the characteristics of 𝓵=0?
spherical
one orientation (m𝓵=0)
all principle numbers (shells) have an s-orbital
What are nodes?
area of no electron density
What is phasing?
product of constructive/destructive interference
What are the characteristics of 𝓵=2?
4 leaf clover (mostly)
5 orientations (m𝓵=-2, -1, 0, 1, 2)
degenerate
2 nodes
Phasing
principal energies above n=2 have d-orbitals
More nodes=
higher energies
What are the characteristics of 𝓵=3?
irregular shapes
7 orientations (m𝓵=-3, -2, -1, 0, 1, 2, 3)
degenerate
shells above n=3 have f-orbitals
What is spin (ms)?
rotation of electron
How does spin act?
like a tiny magnet––create current
How many orientations does spin have?
2
spin up (ms=1/2)
spin down (ms=-1/2)
What is the Pauli Exclusion Principle?
no 2 electrons have same quantum numbers (n, 𝓵, m𝓵, ms)
add 2 electrons to orbital tree
What is Pauli?
each orbital can have max 2 electrons (spin paired)
What is the Aufbau Principle?
fill electrons from lowest to highest energy orbitals
What is Hund’s Rule?
single occupy degenerate orbitals, then pair
What does degenerate mean?
a situation where two or more quantum states (like orbitals) have the exact same energy level
