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Chem 2045 test 2

QuestionAnswer
Maxwell Theory of EM waves
Thomson Plum pudding model
Bohr Planetary model
Lenard Studied the photoelectric effect
Hertz Discovered the photoelectric effect
Heisenberg Uncertainty principle
Debroglie Proposed matter waves
Sommerfield Elliptical orbits in Bohr model
Schroedinger Wave mechanics
Foucault Speed of light in air> water
Becquerel Discovered radioactivity
Davisson, Germer Exp. confirmed wave side of electron
Newton Earliest particles theory of light
Einstein Explained the photoelectric effect
Huygens Earliest wave theory of light
Planck Introduced the idea of Quanta
Pauli Exclusion principle
Dirac Most abstract quantum theory
Rutherford Nuclear model of the atom
Young Interference of light
1st E.A. Energy change when a gaseous atom gains an electron
Quantum stability Half and completely filled sublevels are extra stable
Dispersion Different λ bend at different angles
Metastable state Excited state with long lifetime
Wavelength Peak to peak distance in a wave
Phosphorescence Absorption of high energy with a delayed release of lower energy
Quantum Particles of energy
Fluoresence Absorption of high energy followed by immediate release of lower energy
Frequency # waves passing a given pt in one S
Relativistic effect Energy change when a gaseous atom gains an electron
Ground state All e- are in lowest possible energy level
Valence e- S and P electrons in the outer level
Isoelectonic Having the same e- configurations
Ionization energy Energy required to remove outer e-
Excited state One or more e- are not in the lowest possible energy level
Order of discovery e-, p, n
Gold Foil experiment 1. Alpha particles were shot into a gold foil 2. Results were not exactly as expected 3. It was performed in 1909
Discovered by Newton Continuous Spectrum
Magnetic splitting of spectral lines Zeeman effect
Planck's quantum idea Used to explain blackbody radiation
Einstein's explanation of the photoelectric effect Extended the quantum idea to all forms of energy
Bohr principle of complementarity states Light sometimes behaves as a wave, sometimes as a particle, but never both at the same time
Original Bohr model The electron can jump from one orbit to another
The fully modified Bohr model failed in which way? Did not work for multi electron atoms
The fully modified Bohr model included 1. 4 quantum numbers 2. Selection rules 3.Elliptical orbits
Heisenberg uncertainty principle Allows for violation of matter energy conservation
For quantum teleportation to occur An end-run must be done around the uncertainty principle
The modern picture of empty space is that it Exists as a quantum foam
Have the smallest I.E. value Na 1+
The 1st I.E. of P is abnormally large because P has half filled p sublevel
Einstein was against Bohr's interpretation of quantum theory for each of the following reasons 1. "God does not play dice with the universe" 2. Was against copenhagen interpretation 3. Quantum theory is incomplete are hidden variables
In a many electron atom, n determines what about an orbital Energy and size
In a many electron atom what does, I, the orbital quantum #, determine about an orbital Energy and shape
The max # of electron in the n=3 level is 18
The max# of electron in the I=3 sublevel is 14
Configuration of Cu 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^1, 3d^10
In a many electron atom, n determines what about an orbital Energy and size
In a many electron atom, n determines what about an orbital Energy and size
In a many electron atom what does, I, the orbital quantum #, determine about an orbital Energy and shape
The max # of electron in the n=3 level is 18
The max# of electron in the I=3 sublevel is 14
Configuration of Cu 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^1, 3d^10
Which is true concerning the n+1 rule in determining the sublevel with the lower energy It will have lower n+I value and If n+I values are equal then it will have lower n value
Belongs to the Lyman series 4->1
Compare Sr, Vs, Ca As to metallic nature Sr is more metallic
Interpretation of the quantum theory that involves multiple universes Many Worlds
Even though atomic size gradually decreases across a period for transition elements, Hg is actually larger than Os because 1. Expansion of 5d orbital 2.e- repulsions 3.Relativistic effects
Densest element Osmium
The unusual properties of gold can be explained by The Relativistic effect
Not an unusual property of gold Highly reactive
Not one of the coinage metals Cr
Pair of metals have an abnormal yellow color Cu, Au
Correct short form configuration 77 Ir [Xe] 6s^2 4f^14 5d^7
Correct short form configuration for 97 Bk [Rn] 7s^2 5f^8 6d^1
Correct electron configuration of 62 Sm 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^10, 4p^6, 5s^2, 4d^10, 5p^6, 6s^2, 4f^5, 5d^1
Created by: nzambrano