Quantum Numbers Flashcards

1
Q

What shape is principle (n)?

A

shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What values is principle (n)?

A

zero, positive integers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is the position of a lower n?

A

closer to nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are the characteristics of a higher n?

A

larger atom and more energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

n=1 distance to nucleus

A

closer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

n=5 distance to nucleus

A

farther

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

n=1 relative size of orbital

A

smaller

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

n=5 relative size of orbital

A

larger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

n=1 relative energy

A

smaller

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

n=5 relative energy

A

larger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is angular momentum (𝓡)

A

subshell
shape of the orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are the values of angular momentum (𝓡)?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is magnetic (m𝓡)

A

number of orbitals in a subshell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are the values of magnetic (m𝓡)?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are the 𝓡, m𝓡, # of orbitals, and orbital name for n=1?

A

0) 0) 1 orbital) 1s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What are the 𝓡, m𝓡, # of orbitals, and orbital name for n=2?

A

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

17
Q

What are the 𝓡, m𝓡, # of orbitals, and orbital name for n=3?

A

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

18
Q

What are the 𝓡, m𝓡, # of orbitals, and orbital name for n=4?

A

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

19
Q

How do we apply quantum numbers?

A

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

20
Q

What are the characteristics of 𝓡=1?

A

peanut shape
3 orientations (m𝓡=-1, 0, 1)
degenerate––equal energy
differ only based on axis(plane)
contains one node
Phasing
principle energies above n=1 have p-orbitals

20
Q

What are the characteristics of 𝓡=0?

A

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

21
Q

What are nodes?

A

area of no electron density

22
Q

What is phasing?

A

product of constructive/destructive interference

23
Q

What are the characteristics of 𝓡=2?

A

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

24
More nodes=
higher energies
25
What are the characteristics of 𝓡=3?
irregular shapes 7 orientations (m𝓡=-3, -2, -1, 0, 1, 2, 3) degenerate shells above n=3 have f-orbitals
26
What is spin (ms)?
rotation of electron
27
How does spin act?
like a tiny magnet––create current
28
How many orientations does spin have?
2 spin up (ms=1/2) spin down (ms=-1/2)
29
What is the Pauli Exclusion Principle?
no 2 electrons have same quantum numbers (n, 𝓡, m𝓡, ms) add 2 electrons to orbital tree
30
What is Pauli?
each orbital can have max 2 electrons (spin paired)
31
What is the Aufbau Principle?
fill electrons from lowest to highest energy orbitals
32
What is Hund's Rule?
single occupy degenerate orbitals, then pair
33
What does degenerate mean?
a situation where two or more quantum states (like orbitals) have the exact same energy level