Atomic Structure and Mass Spectrometry

A set of vocabulary flashcards covering key concepts from atomic structure and mass spectrometry.

Plum Pudding Model

An early atomic model that described atoms as a sphere of positive charge with small negative charges evenly distributed within it.

Electron Shell Model

The current model of atomic structure that describes the atom as having a small, dense nucleus surrounded by orbiting electrons in shells.

Mass Number (A)

The sum of protons and neutrons in an atom.

Atomic Number (Z)

The number of protons in an atom, which determines the element.

Isotopes

Atoms of the same element with the same atomic number but different numbers of neutrons and mass numbers.

Relative Atomic Mass (Ar)

The mean mass of an atom of an element compared to one twelfth of the mean mass of an atom of carbon-12.

Ions

Atoms that have lost or gained electrons, resulting in a net charge.

Mass Spectrometry

An analytical technique used to identify different isotopes and find the relative atomic mass of an element.

Ionisation

The process of removing electrons from atoms, typically resulting in positively charged ions.

Ion Drift

The movement of ions through a magnetic field, where their path curvature depends on their mass and charge.

Electron Configuration

The distribution of electrons among the orbitals of an atom.

Orbital

An electron cloud where electrons are likely to be found, characterized by different shapes and energy levels.

Spin

A property of electrons that must be paired with opposite spin within an orbital.

Ionisation Energy

The minimum energy required to remove one mole of electrons from one mole of gaseous atoms.

Successive Ionisation Energies

The energies required to remove additional electrons after the first one, generally increasing due to attraction to the nucleus.

Period Trend in Ionisation Energy

Ionisation energy increases across a period due to decreasing atomic radius and stronger electrostatic attraction.

Group Trend in Ionisation Energy

Ionisation energy decreases down a group due to increasing atomic radius and electron shielding.