Term | Definition |
Electromagnetic radiation | any form of radiant energy in the electromagnetic spectrum |
Electromagnetic spectrum | spectrum of electromagnetic energy |
Wavelength | the distance from crest to crest or trough to trough |
Frequency | number of crests of a wave that pass a stationary point of reference per second |
Amplitude | height of wave from crest to midpoint or trough to midpoint |
Atomic emission spectra | characteristic patterns of bright lines on black background |
Atomic absorption spectra | characteristic patterns of dark lines produced when an external source of radiation passes through free, gaseous atoms |
Blackbody radiation | anything that acts as a perfect absorber and perfect emitter, wavelength depends on T |
Quantum/quantized | having values to whole number multiples of a specific base values, stairs |
E = hν = hc/λ | energy formula |
Planck's constant | 6.626x10^-34 |
Photons | quanta of electromagnetic radiation |
work function | amount of energy needed to dislodge an election from the surface of a material |
Photoelectric effect | shows light has both wave and particle like waves |
Atomic line spectra | all lines |
Bohr model | not a valid but it explains quantum energy levels and nucleus concept |
Rydberg equation | used to find energy needed to move one electron to a different level |
emission | giving energy |
absorption | taking in energy |
Energy level diagram | showing the energy to levels |
Ground state | n=1 |
Excited states | n>1 |
Electron transitions | movement from one level to another |
De Broglie equation | λ=h/mu |
Standing wave/nodes | where there is not waves, no amplitude |
Heisenberg uncertainty principle | can't know position and momentum Δx*mΔu≥h/4π |
Quantum mechanics/wave mechanics | mathematic description of the wavelike bejavior of electrons and other particles |
Schrödinger wave equation | description of how electron matter wave varies with location and time around the nucleus |
Wave functions | solution to Schrödinger wave equation, define how varies both time and location |
Quantum numbers | describe electrons |
Principal | n energy level |
Angular momentum | n-1, s, p, d, f, g |
Magnetic | from +l to -l |
Spin | positive one half or negative |
Pauli exclusion principle | no two electrons can have the same four quantum numbers |
Atomic orbitals | the areas of propable electron location according to energy level |
s, p, d | orbital names |
Nodes | curved planar nodes, point node |
Aufbau principle | fill electrons from lowest to highest |
Electron configurations/condensed electron configurations | 1s2s2p3s3p4s3d4p… [Ne]3s3p |
Atoms | smallest unit of an element that still has the properties of that element |
Anomalies | cromium group and copper group |
Ions | usually corresponding to group number, transition metals usually 2+ or 3+ |
Core | electrons electrons under the valence shell |
Valence electrons | not in core, anything higher than nearest noble gas |
Valence shell | outer shell where valence electrons probable location is |
Hund’s rule | fill all positive spin before negative spin |
Orbital diagrams | electron configuration with the little arrows representing spin |
Isoelectronic | same number of electrons (ions with noble gases) |
Periodic trends | trends presented by periodic table |
Atomic radii | decreases going left to right on a period, increases going down groups |
Ionic radii | cations < neutral, anions > neutral |
Ionization energy | increases going left to right on a period, decreases going down groups (anomalies between groups 2 and 13 and between N and O) |
Electron affinity | energy to add electron decreases as you go across a period |
infinity | true radius of an atom |