Honors: Atomic Structure

Magnetic (m)

the quantum number that shows the spatial orientation of the orbitals around the nucleus

Magnetic (m)

the quantum number that explains that each sublevel consists of orbitals

Magnetic (m)

the quantum number that provides the maximum number of orbitals in each sublevel

Sublevel

made up of orbitals, there are 4 different sublevels (s, p, d and f) each has its own shape and each holds a different maximum number of electrons in quantum theory

Orbital

makes up the sublevels in quantum theory

Priniciple (n)

the quantum number that indicates the main energy level

Orbital (l)

the quantum number that shows the maximum number of electrons in each sublevel

Orbital (l)

the quantum number that provides the shape of each orbital

Orbital (l)

the quantum number that indicates there are 4 sublevels

Spin (s)

the quantum number that indicates the spin value of an electron

Spin (s)

the quantum number that demonstrates that a single orbital can hold a maximum of 2 electrons, each with an opposite spin

Alpha Decay

A nuclear reaction in which an atom emits an alpha particle (helium nucleus) and transforms into a smaller atomic nucleus.

Alpha Decay

A type of decay that reduces the atomic number by 2 and the mass number by 4, changing the original element present.

Beta Decay

A nuclear reaction in which an atom emits a beta particle creating an atom where a proton becomes a neutron or a neutron becomes a proton.

Beta Decay

A type of decay in which the mass number (protons + neutrons) stays the same but the atomic number (protons) increases or decreases by 1, changing the original element present.

Gamma Decay

A nuclear reaction in which high-energy gamma-ray photons are emitted from an unstable nucleus. The number of protons and neutrons remains the same.

Hund's Rule

States that each orbital must contain one electron before pairing occurs.

Aufbau Principle

States an electron occupies the lowest energy orbital that can receive it