| A | B |
|---|
| electromagnetic spectrum | Any "particle" which moves at the speed of light through space |
| crest | the highest point in a wave |
| amplitude | the distance from the median to the crest or median to the trough |
| wavelength | the distance from one point to the next identical point on the wave |
| frequency | the number of waves passing a fixed point in a one second period |
| hertz | the unit used to measure frequency or waves/second |
| lambda | the symbol for wavelength |
| nu | the symbol for frequency |
| Planck's constant | 6.63 x 10E-34 J/Hz |
| speed of light | 3.00 x10E8 m/s |
| ground state | electrons in the lowest energy state possible |
| excited state | when electrons are not in the lowest energy state possible |
| spectra | the set of lines of light formed by an excited atom |
| Rydberg equation | an equation relating wavelength and the change in energy levels according to the Bohr model. |
| E=hv | equation relating energy and frequency |
| c=lambda nu | equation relating wavelength and frequency |
| energy level | the average distance of a group of electrons from the nucleus |
| azimuthal quantum number | tells the type of subshell an electron occupies |
| magnetic quantum number | tells which orbital within a subshell an electron occupies |
| spin quantum number | tells if an electron is the first or second on in the orbital |
| Hund's Rule | one electron per orbital before doubling up |
| Pauli Exclusion Principle | no two electrons in the same atom can have the same set of quantum numbers |
| Quantum Numbers | a set of 4 numbers showing the most likely place to find an electron |
| aufbau principle | electrons fill the lowest energy orbitals before moving to higher energy orbitals |
| ionization energy | the amount of energy required to remove an electron from an atom/ion |
| first ionization energy | the amount of energy required to remove the most losely held electron from an atom |
| electron affinity | the amount of energy gained by gaining and electron |
| Lewis Electron Dot Structure | a symbol used to show only the valence electrons |
| valence electrons | electrons in the highest energy level |
| electron configuration | listing of all electrons in an atom in the order the subshells fill. Includes the number of electrons per subshell. |
| shielding effect | the cancellation of the effect of the nucleus by inner energy level electrons |
| s orbital | sphere shaped, one orbital per energy level, appears in all energy levels |
| p orbital | dumbbell shaped, 3/energy level, appears in energy levels 2 and greater |
| d orbital | double dumbbell, 5 orbital/energy level, appears in energy levels 3 and above |
| f orbital | flowery shaped, 7/ energy level, appears in energy level 4 and above |
| transition elements | last electron appears in the d subshell |
| alkaline earth metals | last electron completes the s subshell |
| alkali metals | one valence electron |
| noble gases | full set of s and p valence electrons |
| halogens | form a -1 ion by gaining an electron to complete the p subshell |
| photon/quanta | a small "packet" of energy |
| valence shells | orbitals in the highest energy level |
| effective nuclear charge | the amount of nuclear pull an electron feels. |
| atomic radius | the radius of an atom |
| ionic radius | the distance from the nucleus to the edge of the electron cloud in an ion. |
