Quantum Mechanics

0.0(0)
linked notesView linked note
learnLearn
examPractice Test
spaced repetitionSpaced Repetition
heart puzzleMatch
flashcardsFlashcards
Card Sorting

1/26

encourage image

There's no tags or description

Looks like no tags are added yet.

Study Analytics
Name
Mastery
Learn
Test
Matching
Spaced

No study sessions yet.

27 Terms

1
New cards
What does the wavefunction (Ψ) describe?
The movement of a particle.
2
New cards
What is probability density (Ψ²)?
The probability of finding the particle in a region.
3
New cards
Where is a node located?
Where the probability of finding an electron is zero.
4
New cards
How many nodes do wavefunctions have?
Wavefunctions have (n-1) nodes.
5
New cards
What can an electron do at a node?
An electron can never be at a node, but can 'cross' nodes as they are delocalized standing waves.
6
New cards
For which energy levels do s orbitals exist?
For all energy levels n ≥ 1.
7
New cards
What is the angular momentum quantum number (l) for s orbitals?
L = 0.
8
New cards
For which quantum number do p orbitals exist?
Exists for n ≥ 2.
9
New cards
What is the angular momentum quantum number (l) for p orbitals?
L = 1.
10
New cards
For which quantum number do d orbitals exist?
Exists for n ≥ 3.
11
New cards
What do penetrating orbitals refer to?
Orbitals with radial probability closer to the nucleus.
12
New cards
What is the difference between paramagnetism and diamagnetism?
Paramagnetism has unpaired electrons and is drawn towards magnets; diamagnetism has paired electrons and is slightly repelled by magnets.
13
New cards
What does the principle quantum number (n) define?
The size and energy of the orbital.
14
New cards
What is the allowed value for the principle quantum number (n)?
Must be positive whole numbers.
15
New cards
How do you calculate the number of orbitals in a shell?
Using the formula n².
16
New cards
What does the angular momentum quantum number (l) define?
The 3D shape of the orbital.
17
New cards
What are the possible values for the angular momentum quantum number (l)?
Any integer from 0 to (n-1).
18
New cards
What does the magnetic quantum number (ml) define?
The spatial orientation of the orbital.
19
New cards
What are the allowed values for the magnetic quantum number (ml)?
From -l, …, 0,... +l.
20
New cards
How many spatial orientations are there of orbitals in a subshell?
2l + 1.
21
New cards
How many electrons can an s sublevel hold?
2 electrons.
22
New cards
How many electrons can a p sublevel hold?
6 electrons.
23
New cards
How many electrons can a d sublevel hold?
10 electrons.
24
New cards
How many electrons can an f sublevel hold?
14 electrons.
25
New cards
What does the spin quantum number (ms) define?
The spin axis of an electron.
26
New cards
What are the allowed values for the spin quantum number (ms)?
+½ or -½.
27
New cards
How many electrons are allowed per orbital?
Only two electrons are allowed per orbital.