chemistry unit 2

Isotopes

Atoms of the same element with different mass numbers, differing in the number of neutrons.

Atomic Absorption Spectrum

A spectrum that shows the specific wavelengths of EM radiation absorbed by atoms as they move from lower to higher energy levels.

Atomic Emission Spectrum

A spectrum produced when an atom releases energy as electrons move from higher to lower energy levels.

Bohr Model

Niels Bohr's theory that describes electron transitions in atoms, where energy absorption causes electrons to move to higher orbits.

Quantum

A packet of energy released when an electron transitions between energy levels.

Ionization Energy

The energy required to remove an electron from the ground state of an atom.

Heisenberg's Uncertainty Principle

The principle stating that one cannot simultaneously know the exact position and momentum of an electron.

Schrodinger Model

A model that uses wave equations to describe the behavior of electrons in atoms, leading to the concept of atomic orbitals.

Atomic Orbitals

Regions around an atomic nucleus where there is a high probability of finding an electron.

Pauli Exclusion Principle

A principle stating that no more than two electrons can occupy the same orbital, and they must have opposite spins.

Aufbau Principle

The principle that electrons occupy the lowest energy orbitals first.

Hund's Third Rule

A rule stating that electrons will occupy separate orbitals in the same sublevel before pairing up, to minimize repulsion.