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Chem 105 Ch 3
| 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 |
Created by:
ksheehy96
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