Quantum Mechanics and Periodic Table Flashcards

Flashcards for vocabulary related to quantum mechanics and the periodic table.

Electromagnetic Radiation

Light that travels in the form of waves; all different types together are called the Electromagnetic Spectrum (EMS).

Wavelength

The distance between two successive crests/troughs, measured in meters or nanometers.

Frequency

The number of waves that pass a certain point per second, measured in seconds or Hertz (Hz).

Photoelectric Effect

The phenomenon where certain amounts of light energy strike the surface of a metal.

Quantum

A packet of energy that light can carry.

Planck's Constant

Constant (h) that relates energy to frequency; h = 6.626 x 10^-34 J*sec

Photon

A particle of light that carries energy in units of quanta and has no mass.

Emission Spectra

The unique wavelengths of light seen as small bars of color when electrified light passed through a gas is sent through a prism; wavelength is unique for each element.

Ground State

The lowest energy state of an electron.

Excited State

A higher energy state that an electron temporarily occupies after gaining energy.

Uncertainty Principle

It is impossible to know the exact location and position of an electron simultaneously.

Orbital

A specific region within the electron cloud where there is a 90% chance of finding an electron.

Principle Quantum Number (n)

Indicates the energy level or shell of an electron and its size; possible values are positive whole numbers (1, 2, 3, etc.).

Orbital Quantum Number (l)

Indicates the energy sublevel or subshell of an electron; possible values range from 0 to n-1 and corresponds to the shape of the orbital.

Magnetic Quantum Number (ml)

Indicates a specific orbital and corresponds to the number of orbitals possible in a sublevel; possible values range from -l to +l.

Spin Quantum Number (ms)

Indicates the specific spin of an electron; possible values are +1/2 and -1/2.

Aufbau Principle

Electrons occupy the lowest energy levels first.

Pauli Exclusion Principle

No two electrons in an atom can have the same set of 4 quantum numbers; within an orbital, electrons must have opposite spin.

Hund's Rule

Electrons occupy degenerate orbitals (orbitals of the same energy) with one electron each before pairing will occur.

Valence Electrons

Electrons in the highest occupied energy level (outermost level) for an atom.

Periods/Series

Horizontal rows on the periodic table; indicate the energy level.

Groups/Families

Vertical columns on the periodic table; clues to chemical behavior.

Atomic Radius

A measure of ½ the distance across an atom.

Ionic Radius

The radius of an atom's ion; smaller for cations (formed by losing electrons), larger for anions (formed by gaining electrons).

Ionization Energy (IE)

The energy required to remove a valence electron from an atom.

Electronegativity (EN)

The ability of an atom to attract a bonded pair of electrons to itself.