Electron Configurations and Quantum Numbers

These flashcards cover key concepts related to electron configurations and quantum numbers, aiding in the understanding of atomic structure.

Principal Quantum Number (n)

A positive integer that indicates the shell and relative size of orbital(s).

Orbital Quantum Number (l)

An integer from 0 to n-1 that defines the shape of the orbital and sub-shell.

0 (s) 1 (p) 2 (d) 3 (f) 4 (g)

Magnetic Quantum Number (ml)

An integer with a value from -l to +l that defines the orientation of an orbital in space.

Spin Quantum Number (ms)

Accounts for the two possible spin states with values +1/2 and -1/2.

Quantum Numbers

P orbitals

three 2p orbitals

D orbitals

five 3d orbitals

Pauli Exclusion Principle

Orbitals can contain a maximum of two electrons which must be of opposite spin.

Aufbau Principle

Electrons enter and fill lower energy orbitals before higher energy orbitals.

Hund's Rule

Electrons will enter the orbitals one-at-a-time to maximize degeneracy.

Madelung's Rule

Orbitals fill with electrons as n + l

Degenerate Orbitals

Orbitals that have the same energy level.

Valence Electrons

Electrons in the outermost shell that influence an atom's chemical behavior.

Core Electrons

Electrons in the filled, inner shells that are not involved in chemical reactions.

Radial Distribution Plot

A graphical representation of the probability of finding an electron in a thin spherical layer near the nucleus.

Electromagnetic Character

Refers to the behavior of atoms with unpaired electrons when exposed to a magnetic field.

Anomalous Electron Configurations

Configurations that deviate from expected patterns to achieve lower energy states.

Isoelectronic

Atoms or ions that have identical numbers and configurations of electrons.

Electron Configuration

The arrangement of electrons in an atom's orbitals.

Compactness of d Orbitals

3d orbitals are more compact than 4s orbitals, leading to greater electron-electron repulsion.