| A | B |
|---|
| James Maxwell | discovered that all light has an electric and magnetic fields |
| wavelength | crest to crest; "lambda" is the symbol |
| frequency | waves per second; sec -1, 1/sec, or Hz |
| Hertz | unit of frequency |
| node | area of no energy in a standing wave; between energy levels or outside of an orbital in an atom |
| amplitude | "rest" to crest |
| speed of a wave | depends on the media; = wavelength x frequency |
| 300,000,000m/s | speed of light; "c" |
| "quantized" | where only certain wavelengths or energies are possible |
| "quanta" | means "bundle" in Latin |
| continuous spectrum | shows ROYGBIV, like light from a fluorescent or incandescent lamp |
| incandescent | lamp or candle light; has more yellow/green light |
| fluorescent lamp | has more blue light |
| "h" in E = hv | Planck's constant |
| Albert Einstein | discovered the photoelectric effect |
| photoelectric effect | when light strikes a metal and causes electrons to be released |
| E = hv | Einstein's energy of a photon formula |
| line spectra | also called emission spectra; characteristic lines of color seen in a spectroscope for a particular element or compound |
| absorption spectra | when all colors are shown EXCEPT the line spectra, which appear as black lines |
| quantum leap | when an electron moves from an excited energy level to ground state |
| ground state | lowest state for an electron; most stable |
| E = - Rhc/n2 | formula for the energy of a particular energy level in an atom where n=1,2,3... |
| Louis de Broglie | stated that an electron with a particular velocity and mass would have an associated wavelength--that is, it IS a wave! |
| Werner Heisenburg | states that the momentum and position of an electron at the same time |
| Erwin Schrodinger | father of quantum mechanics; used a "wave equation" to produce 3D models of orbitals where electrons have a 90% probability of being found |
| Neil Bohr | discovered that line spectra correspond to quantum leaps by electrons within hydrogen |
| orbital | 3D model of where electrons are 90% likely to be found |
| quantum numbers | used to express the area where to find electrons |
| "n" | principal quantum number; represents energy & size of energy level |
| "l" | represents the shape of an orbital (s,p,d,f) |
| "m sub l" | represents the orientation of an orbital on the x,y, and z axes |
| s-orbital | spherical, l=0 |
| p-orbital | dumb-bell shaped, l =1 |
| d-orbital | clover-leaf shaped, l=2 |
| f-orbital | complex shapes; l=3 |
| cartesian coordinate system | used to locate a point in space; x,y, and z axes |
| magnetic quantum number | called m "sub" l, is the orientation in space of an orbital |
| Ernest Rutherford | discovered that the atom has a nucleus using his "gold foil experiment" |
| one | number of "s" orbitals |
| three | number of different "p" orbitals |
| five | number of different "d" orbitals |
| seven | number of different "f" orbitals |
| photon | a massless particle of light |
