| A | B |
|---|
| a form of energy that emits wave-like behavior as it travels through space | Electromagnetic Radiation |
| Examples of Electromagnetic Radiation | Visible light, microwaves, x-rays, radio waves |
| Characteristics of Electromagnetic Waves | Amplitude, Wavelength, Frequency |
| The height of a wave from the origin to the cresting point | Amplitude |
| The shortest distance between equivalent points on a continuous wave | Wavelength |
| The number of waves that pass a given point per second | Frequency |
| The spectrum placing all of the wave types in order based on wavelength and frequency(displays electromagnetic radiation) | Electromagnetic Spectrum |
| Speed of Electromagnetic Waves in a Vacuum | 3.00 X 10^8 m/s |
| Variable for the Speed of Light | c |
| Matter can gain or lose energy only in small, specific amounts called quanta | Planck's Theory of Electromagnetic Radiation |
| The minimum amount of energy that can be gained or lost by an atom | Quantum |
| Planck's relationship between the quantum and the frequency of emitted radiation | E=h(Planck's Constant-6.626 X 10^-34)v(frequency) |
| A particle of electromagnetic radiation with no rest mass that carries a quantum of energy | Photon |
| Only whole numbers of wavelengths are allowed in a circular orbit of a fixed radius; light has characteristics of both waves and particles; electrons move in wavelike motion with restricted circular orbits | De Broglie's Atomic Theory |
| Proposed quantum model; predicted frequencies of hydrogen's atomic emission spectrum; atoms have only certain allowable energy states; related energy states to the motion of electrons in circular orbits | Bohr's Atomic Theory |
| Can determine either the velocity or the position of an electron, cannot determine both | Heisenberg's Uncertainty Principle |
| Treats the hydrogen atom's electron as a wave; only limits the electron's energy values, does not attempt to describe the electron's path | Scrodinger's Equation |
| Terms to Describe the Location of an Electron | Energy Level(n), Sublevel(l), Orbitals(ml), Spin(ms) |
| Indicates relative sizes and energies of atomic orbitals; whole numbers, ranging from 1-7 | Energy Level |
| Number of sublevels present in each energy level is present to n; in order of increasing energy: s<p<d<f | Sublevels |
| Only one Orbital | S Sublevel |
| 3 Orbitals Present; Each Orbital can have only two electrons | P Sublevel |
| 5 Orbitals Present | D Orbital |
| 7 Orbitals Present | F Orbital |
| An electron will occupy the lowest energy orbital that can receive it | Aufbau Principle |
| Orbitals of equal energy must each contain one electron before electrons begin pairing | Hund's Principle |
| If two electrons are to occupy the same orbital, they must be spinning in opposite directions | Pauli Exclusion Principle |
| The Principle Quantum Number | n |
| The Azimuthal Quantum Number | l |
| Number used to describe s orbitals | 0 |
| Number used to describe p orbitals | 1 |
| Number used to describe d orbitals | 2 |
| Number used to describe f orbitals | 3 |
| The Magnetic Quantum Number | ml |
| The Electron Spin Quantum Number | ms |
