Study Chemistry Chapter 4:1-2 Flash Cards

 
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Chemistry Chapter 4:1-2

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orbital
main energy level; 3D region around nucleus in which an electron can be found
Schrodinger Wave Equation
Aplies to all atoms, treats electrons as eaves.
laid foundation for quantum theory
Heisenberg Uncertainty Prinicple
it is impossible to determine simultaneously bot hthe position and velocity of an electron
Interference
occurs when overlap
Diffraction
bending of a wave as it passes by edge of object
de Broglie
electrons may havve wave-particle nature
quantum model of atom
electrons ac as waves and particles
Spectroscopy
Study of light emitted by excited atoms
Bright Line Spectrum
Orbits
allowable paths where electrons are found
Who created the Bohr Model of H Atom
Niels Bohr
excited state
state of higher energy
Ground State
lowest energy state (closest to nucleus)
H Atoms Line-Emmission Spectrum
Ground State and Excited State
Photon
individual quantum of light "packet"
quantum equation
E=hv
quantum
minimum quantity of energy that can be lost or gained by an atom
Spectroscope
device that separates light into a spectrum that can be seen
Frequency equation
C=Yv
Hz
hertz
Frequency
number of waves that hpass a given point in a specifies time
Wavelength
distance between 2 corresponding pts on adjacent waves
Speed of light in a vacuum
3.0/10 to hte 8 m/s
Electromagnetic Spectrum
all the forms of electromagnetic radiation
Electromagnetic Radiation
form of energy that exhibits wave-like behavior as it travels through space
A dual nature
discovered that light a & electrons both wave-like and particle -like properties
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