Quantum Numbers and Atomic Models

These flashcards cover key concepts related to atomic models and quantum numbers discussed in lecture notes.

Bohr Model

A model of the atom that suggests electrons move in circular orbits around the nucleus.

Heisenberg Uncertainty Principle

States it is impossible to simultaneously determine the position and velocity of an electron.

Quantum Numbers

Numeric values that specify properties of atomic orbitals and electrons within those orbitals.

Principal Quantum Number (n)

Indicates the main energy level occupied by an electron; higher values mean higher energy and distance from the nucleus.

Angular Momentum Quantum Number (l)

Indicates the shape of the orbital; values depend on the principal quantum number (n).

Magnetic Quantum Number (ml)

Indicates the orientation of an orbital in space, with values derived from the angular momentum quantum number.

Spin Quantum Number (ms)

Indicates the spin direction of an electron, can be +1/2 (spin up) or -1/2 (spin down).

Orbital

Regions around a nucleus where electrons are likely to be found; sometimes referred to as electron clouds.

Sublevels

Different energy levels within the principal quantum levels that allow the division of energy corresponding to the shape of orbitals.

Bohr Model

A model of the atom that suggests electrons move in circular orbits around the nucleus.

Heisenberg Uncertainty Principle

States it is impossible to simultaneously determine the position and velocity of an electron.

Quantum Numbers

Numeric values that specify properties of atomic orbitals and electrons within those orbitals.

Principal Quantum Number (n)

Indicates the main energy level occupied by an electron; higher values mean higher energy and distance from the nucleus.

Angular Momentum Quantum Number (l)

Indicates the shape of the orbital; values depend on the principal quantum number (n).

Magnetic Quantum Number (ml)

Indicates the orientation of an orbital in space, with values derived from the angular momentum quantum number.

Spin Quantum Number (ms)

Indicates the spin direction of an electron, can be +1/2 (spin up) or -1/2 (spin down).

Orbital

Regions around a nucleus where electrons are likely to be found; sometimes referred to as electron clouds.

Sublevels

Different energy levels within the principal quantum levels that allow the division of energy corresponding to the shape of orbitals.

Pauli Exclusion Principle

States that no two electrons in an atom can have the same set of four quantum numbers.

Aufbau Principle

Electrons fill atomic orbitals in an atom from the lowest energy level to the highest.

Hund's Rule

Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Electron Configuration

The distribution of electrons of an atom or molecule in atomic or molecular orbitals.

s-orbital

An orbital with an angular momentum quantum number (l=0), which has a spherical shape.

p-orbital

An orbital with an angular momentum quantum number (l=1), which has a dumbbell shape and three possible orientations.