chemistry ch 6 quantum numbers

What does Schrödinger’s equation mainly describe?

The exact path of electrons

What does the wave function (ψ) represent?

Probability of finding an electron in a specific area

What is the principal quantum number (n)?

Energy level/shell

What are the possible values of n?

1–7

What does the angular momentum quantum number (l) describe?

Orbital shape

Which value corresponds to a “p” orbital?

1

What does the magnetic quantum number (ml (lowercase)) describe?

Orbital orientation

What are possible values of the spin quantum number (ms)?

+½ and –½

What shape is an s orbital?

Sphere

Which orbital is most complex in shape?

f

Hund’s Rule

Electrons fill empty orbitals in a subshell individually before they pair up. (The "Empty Seat" Rule)

Pauli Exclusion Principle

Electrons in the same orbital must have opposite spins (one up, one down)

Paramagnetic vs. Diamagnetic

Paramagnetic = contains unpaired electrons (magnetic). Diamagnetic = all electrons are paired (not magnetic)