Chapter 2 Flashcards
Amplitude
The height of the wave, determines intensity and brightness, amount of photons
Wavelength
distance between crests, determines the color, longer wavelength equals less energy
frequency
number of cycles that pass through a stationary point in a given period of time, Hz, 1 cycle per second, 1/s, directly proportional to the speed at which the wave is traveling, inversely proportional to wavelength
Electromagnetic Spectrum from Lowest Energy to Highest Energy
Low Frequency/Long Wavelength
1. Radio
2. Microwave
3. Infrared
4. Visible Light
5. Ultraviolet
6. X-Ray
7. Gamma Ray
High Frequency/Short Wavelength
Quantized
contained in energetic specific amounts, not continuum
Photoelectric Effect
When light was shone on a metal surface, electrons are ejected from the surface of the metal which completed an electric circuit
ROYGBIV
BIV has shorter wavelength and more energy
Planck
He believed there were discrete and specific energy levels. He hypothesized that an oscillator must gain/lose energy in whole numbers, correspond to the difference between 2 levels
Quanta or Photons
light energy delivered to the atoms in packets, proposed by Einstein
Einstein’s second proposal
when an electron in the metal absorbs a photon of light, it gains the energy required to escape from the metal
Threshold Frequency
minimum frequency
Constructive Interference
same wavelength that lines up doubles amplitude
Destructive Interference
same wavelength that lines up opposite cancels out amplitude
White light
totality of wavelengths/frequencies in the visible portion of the EM spectrum
Emission Spectrum
black background with colored lines, shows which colors are emitted when the electron jumps down in energy, lines indicate that only certain energies are allowed for the electron in that atom
Absorption Spectrum
color background with black lines, colors blacked out are the colors that are absorbed when the electron jumps up in energy
Neils Bohr Model
energy in the atom is quantized, orbits are in stationary states, electrons emit radiation when the jump from an orbit of higher energy to an orbit of lower energy, distance between orbits are determined by energy of the photon of light produced
Wavelength v Atomic/Nuclear Dimensions
When the wavelengths are comparable to atomic or
nuclear dimensions, it is then that the wave-particle
duality is important
Heisenberg’s Uncertainty Principle
the more one knows about the location/position of the electron, the less one knows about the momentum/velocity of the electron, can be observed as either a wave or a particle, never both at the same time, limited by the choice in observation
Determinacy
definite, predictable future
