Chem Test

Quantum

The minimum amount of energy that can be lost or gained by an atom

Electromagnetic Radiation

A form of energy that exhibits wavelike behavior as it travels through space

Atomic Orbital

A three dimensional region around the nucleus of an atom that describes an electron's probable location

Wavelength

The shortest distance between equivalent points on a continuous wave

Ground State

The lowest allowable energy state in an atom

Photon

A particle of electromagnetic radiation with no mass that carries a quantum of energy

Photoelectric effect

The emission of electrons from a metal's surface when light of a certain frequency shines on it

Principle Quantum Number

A figure indicating the relative sizes and energies of atomic orbitals

E = hν

Energy relationship developed by Plank

c

speed of light, 3 x 10^8 m/s

λ

wavelength(nm)

ν

frequency(Hz)

h

planks constant(6.626 × 10^-34)

E = hν

energy formula

c = λν

speed of light formula

λ = h/(mν)

de Brogile’s equation

ΔE = E(higher energy orbit) - E(lower energy orbit)

energy change of an electron undergoing an orbit transition

ΔE

change in energy in J

Atomic Emission Spectrum

The set of frequencies of the electromagnetic waves emitted by the atoms of an element

Aufbau Principle

in the ground state of an atom or ion, electrons fill atomic orbitals from lowest energy to highest energy

Hund’s rule

electrons fill separate atomic orbitals of equal energy singly with parallel spins before they start pairing up

Pauli exclusion principle

no two identical arrows can point the same direction in an orbital

Heisenberg's uncertainty principle

you cannot simultaneously know both the exact position and the exact momentum (or velocity) of a quantum particle

Aufabau Principle exceptions

Cr, Mo, Cu, Ag, Au

MHz

10^6

kHz

10³