electrons in atoms extra credit

Orbital

A region in an atom where there is a high probability of finding electrons. Orbitals have specific shapes and energy levels, which are fundamental to the arrangement of electrons in an atom.

electron density

is a measure of the probability of an electron being present in a specific region within an orbital.

quantum number

A set of numerical values that describe the unique quantum state of an electron in an atom, including its energy level, angular momentum, and orientation. Quantum numbers are essential for understanding electron configurations.

Pauli Exclusion Principle

No two electrons in an atom can have the same set of four quantum numbers, meaning each electron must have a unique state.

Principal energy level

is a designation of the major energy levels of electrons in an atom, represented by a principal quantum number (n) and indicating the distance of the electron from the nucleus.

electron density

A probability distribution that describes the likelihood of finding an electron in a particular region of space around the nucleus.

excited state

An energy state of an atom where one or more electrons have absorbed energy and transitioned to a higher energy level.

Thomson model

A historical atomic model proposed by J.J. Thomson, suggesting that atoms are composed of a positively charged 'soup' with negatively charged electrons embedded within, resembling a plum pudding.

Rutherford model

An atomic model proposed by Ernest Rutherford, demonstrating that atoms consist of a dense, positively charged nucleus surrounded by orbiting electrons, based on the results of his gold foil experiment.

Bohr model

An atomic model proposed by Niels Bohr, which describes electrons as occupying fixed orbits around the nucleus, with specific energy levels and the ability to jump between orbits by absorbing or emitting energy.

Quantum Mechanical model

A modern atomic model that describes electrons as being found in probability clouds or orbitals around the nucleus, rather than fixed orbits, and incorporates wave-particle duality.

Hunds rule

Hund's rule states that electrons will fill degenerate orbitals singly before pairing up, minimizing electron-electron repulsion and resulting in a more stable electron configuration.

Exceptional Electron configurations

Refer to electron arrangements in which atoms may have an unexpected number of electrons in their outer shells, often involving half-filled or fully-filled subshells to achieve greater stability.

Lithium

A chemical element with the symbol Li and atomic number 3, known for its soft, silvery-white metal appearance and high reactivity, especially with water.

fluorine

A highly reactive nonmetal with the symbol F and atomic number 9, known for its pale yellow color and strong electronegativity.

rubidium

A chemical element with the symbol Rb and atomic number 37, known for its softness, silvery-white metallic appearance, and high reactivity, particularly with water and air.

Electromagentic radiation

consists of waves of electric and magnetic fields that propagate through space. It includes a range of phenomena such as visible light, radio waves, and X-rays.

amplitude

the maximum extent of a wave's oscillation from its rest position.

wavelength

is the distance between consecutive peaks of a wave, typically measured in meters. It is inversely related to frequency and directly affects the wave's energy.

frequency

is the number of oscillations or cycles of a wave that occur in a given time period, usually measured in hertz (Hz). It is inversely related to wavelength.