Quantum Numbers

Question 1

What shape is principle (n)?

Answer 1

shell

Question 2

What values is principle (n)?

Answer 2

zero, positive integers

Question 3

What is the position of a lower n?

Answer 3

closer to nucleus

Question 4

What are the characteristics of a higher n?

Answer 4

larger atom and more energy

Question 5

n=1 distance to nucleus

Answer 5

closer

Question 6

n=5 distance to nucleus

Answer 6

farther

Question 7

n=1 relative size of orbital

Answer 7

smaller

Question 8

n=5 relative size of orbital

Answer 8

larger

Question 9

n=1 relative energy

Answer 9

smaller

Question 10

n=5 relative energy

Answer 10

larger

Question 11

What is angular momentum (𝓵)

Answer 11

subshell
shape of the orbital

Question 12

What are the values of angular momentum (𝓵)?

Answer 12

0…n-1
if n=1, 𝓵=0
if n=3, 𝓵=0, 1, 2
values correspond to certain shapes

Question 13

What is magnetic (m𝓵)

Answer 13

number of orbitals in a subshell

Question 14

What are the values of magnetic (m𝓵)?

Answer 14

integers from -𝓵 to 𝓵
if 𝓵=1, m𝓵=-1, 0, 1 (3 total)
all equal energy

Question 15

What are the 𝓵, m𝓵, # of orbitals, and orbital name for n=1?

Answer 15

0) 0) 1 orbital) 1s

Question 16

What are the 𝓵, m𝓵, # of orbitals, and orbital name for n=2?

Answer 16

0) 0) 1 orbital) 2s
1) -1, 0, 1) 3 orbitals) 2p

Question 17

What are the 𝓵, m𝓵, # of orbitals, and orbital name for n=3?

Answer 17

0) 0) 1 orbital) 3s
1) -1, 0, 1) 3 orbitals) 3p
2) -2, -1, 0, 1, 2) 5 orbitals) 3d

Question 18

What are the 𝓵, m𝓵, # of orbitals, and orbital name for n=4?

Answer 18

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

Question 19

How do we apply quantum numbers?

Answer 19

identify size, shape, and relative energy of orbital where electron is likely to be

Question 20

What are the characteristics of 𝓵=1?

Answer 20

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

Question 20

What are the characteristics of 𝓵=0?

Answer 20

spherical
one orientation (m𝓵=0)
all principle numbers (shells) have an s-orbital

Question 21

What are nodes?

Answer 21

area of no electron density

Question 22

What is phasing?

Answer 22

product of constructive/destructive interference

Question 23

What are the characteristics of 𝓵=2?

Answer 23

4 leaf clover (mostly)
5 orientations (m𝓵=-2, -1, 0, 1, 2)
degenerate
2 nodes
Phasing
principal energies above n=2 have d-orbitals

Question 24

More nodes=

Answer 24

higher energies

Question 25

What are the characteristics of 𝓵=3?

Answer 25

irregular shapes
7 orientations (m𝓵=-3, -2, -1, 0, 1, 2, 3)
degenerate
shells above n=3 have f-orbitals

Question 26

What is spin (ms)?

Answer 26

rotation of electron

Question 27

How does spin act?

Answer 27

like a tiny magnet––create current

Question 28

How many orientations does spin have?

Answer 28

2
spin up (ms=1/2)
spin down (ms=-1/2)

Question 29

What is the Pauli Exclusion Principle?

Answer 29

no 2 electrons have same quantum numbers (n, 𝓵, m𝓵, ms)
add 2 electrons to orbital tree

Question 30

What is Pauli?

Answer 30

each orbital can have max 2 electrons (spin paired)

Question 31

What is the Aufbau Principle?

Answer 31

fill electrons from lowest to highest energy orbitals

Question 32

What is Hund’s Rule?

Answer 32

single occupy degenerate orbitals, then pair

Question 33

What does degenerate mean?

Answer 33

a situation where two or more quantum states (like orbitals) have the exact same energy level