Quantum Numbers and Electron Configuration Review

Practice flashcards covering quantum numbers, orbital shapes, electron configuration principles, and magnetic properties based on Chapters 7 and 8.

Principal Quantum Number (n)

Describes the energy level with allowed values of $1, 2, 3, 4 \text{ ...}$

Angular Momentum Quantum Number (l)

Describes the orbital shape with allowed values from $0 \text{ to } n-1$.

Magnetic Quantum Number ($m_l$)

Describes the orbital orientation with allowed values from $-l \text{ to } +l$.

Spin Quantum Number ($m_s$)

Describes the electron spin with allowed values of $+1/2 \text{ or } -1/2$.

s Orbital

Corresponding to $l = 0$, it has a sphere shape and contains $1$ orbital (max $2$ electrons).

p Orbital

Corresponding to $l = 1$, it has a peanut (dumbbell) shape and contains $3$ orbitals (max $6$ electrons).

d Orbital

Corresponding to $l = 2$, it has a daisy (cloverleaf) shape and contains $5$ orbitals (max $10$ electrons).

f Orbital

Corresponding to $l = 3$, it has a fancy/complicated shape and contains $7$ orbitals (max $14$ electrons).

Sublevel Orbital Formula

The number of orbitals in a sublevel is calculated using $2l + 1$.

Total Orbitals Formula

The total number of orbitals in an energy level is calculated using $n^2$.

Pauli Exclusion Principle

No two electrons in the same atom can have the same four quantum numbers; each orbital holds $2$ electrons maximum with opposite spins.

Aufbau Principle

The 'build up' principle stating that electrons fill lowest-energy orbitals first in the order: $1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s$.

Hund's Rule

Electrons fill empty orbitals before pairing (fill singly first).

Valence Electrons

Electrons located in the highest $n$ level of an atom.

Cations (+)

Ions formed by removing electrons from the highest $n$ level first.

Anions (-)

Ions formed by adding electrons to the atom.

Transition Metal Ion Rule

When forming ions, remove electrons from the highest $n$ first, which means removing $4s$ before $3d$.

Paramagnetic

A state where an atom or ion has at least one unpaired electron and is attracted to a magnetic field.

Diamagnetic

A state where all electrons in an atom or ion are paired and it is not attracted to a magnetic field.

Condensed Electron Configuration

A notation that uses the nearest noble gas to represent the inner-shell electron configuration.