| A | B |
|---|
| spectra | range of colors - each element has its own |
| emission spectrum | spectrum of bright lines from light being emitted |
| absorbsion spectrum | spectrum of dark lines created by certain frequencies being absorbed |
| simple spectrum | spectrum of a single element |
| complex spectrum | a combination of spectra from more than one element |
| universal physical law | a fact that is true everywhere in the universe |
| hydrogen spectrum | the frequencies absorbed or emitted by hydrogen ions |
| Johan Balmer | created a formula by trial and error that could calculate all the lines in the visible spectrum of hydrogen |
| Rydberg | found a formula for all the lines of hydrogen |
| rydeberg constant | Rh=1.097E7 1/m |
| quantum theory of light & atoms | atoms and light come in whole number bundles and/or whole number multiples of fundamental values |
| flaw in the planetary model of the atom | orbiting electrons would constantly radiate energy. Therefore they would run out of energy and atoms would collapse |
| Bohr model | nuclear model BUT states that electrons in certain special orbits do not radiate energy |
| EM radiation jumps | Bohr said that electrons can move from one quantum state to another by absorbing or emitting a quanta of energy. This explains the spectral lines. |
| Quantum theory of EM radiation | electrons move from one energy to another by absorbing or emitting photons of specific frequencies |
| ground state | the lowest possible energy an electron in a particular atom can have. This electron is in the energy level closest to the nucleus |
| 1 eV | 1.6E-19 J |
| energy of light (if frequency is known) | E = hf |
| energy of light (if wavelength is known) | E=hc/(lambda) |
| planck's constant | h=6.6e-34 Js |
| speed of light | c = 3.0E8 m/s |
| nf | final energy of an electron in the Bohr model |
| ni | initial energy level of an electron in the Bohr model |
| equation for the Bohr model | 1/(lamda) = Rh[(1/nf squared) - (1/ni squared)] |
| formula for speed of light | c=f(lambda) |
| what is a problem with the Bohr model | it really only works for hydrogen |
| spectroscopy | used to identify the composition of a substance by examining the lines of light emitted or absorbed by a material |
| spectroscope | instrument used to perform spectroscopy. Works by separating wavelengths using diffraction |
