Chapter 2: Electrons and the Periodic Table

These flashcards cover key concepts and vocabulary from Chapter 2 on Electrons and the Periodic Table.

Wavelength (λ)

The distance between identical points on successive waves.

Frequency (ν)

The number of waves that pass through a particular point in one second.

Emission Spectrum

Spectrum showing the wavelengths of light emitted by an element.

Bohr Atom

A model of the atom proposed by Niels Bohr that includes quantized energy levels.

Ground State

The lowest energy state of an electron in an atom.

Excited State

A state where an electron has absorbed energy and moved to a higher energy level.

Photon

A discrete packet of light energy.

Quantum Mechanical Model

A model that describes electrons as existing in probability-based regions called orbitals.

Orbital

A region of space where an electron is likely to be found.

Principal Quantum Number (n)

An integer that identifies the energy level of an electron in an atom.

Electron Configuration

The arrangement of electrons in an atom's orbitals.

Valence Electrons

The outermost electrons in an atom that determine its chemical behavior.

Ionization Energy

The energy required to remove an electron from an atom.

Cation

An ion that has lost one or more electrons and is positively charged.

Anion

An ion that has gained one or more electrons and is negatively charged.

Isoelectronic

When atoms or ions have the same electron configuration as a noble gas.

Lewis Dot Symbols

A representation of valence electrons as dots around an element's chemical symbol.

Atomic Radius

The size of an atom, which increases down a group and decreases across a period.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons.

Electron Affinity

The ability of an atom to gain an electron.