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Quantum Physics
Quantum TheoryMax Planck, examining heat radiation (ir light) proposes energy is quantized, or occurring in discrete small packets with a definite minimum value. (1901)All energy amounts were multiple of a certain constant, called Planck’s constant h with a value of 6.63 x 10-34 JsEnergy of radiation, E = hf
Max Planck1858-1947
The Photoelectric Effect
Hertz observed spark discharges improved with illumination (1898)
Illumination of metal by electromagnetic radiation causes emission of electrons
Could not be explained by wave theory
Frequency of e-m radiation determines if emission occurs, not intensity
The Photoelectric EffectEach metal has minimum energy that must be supplied by light before emission occurs: called the work function of the metal.Each metal found to have cutoff frequency of incident light below which no emission occurs, no matter how intense the lightOnly particle theory of light could explain this
Einstein’s Explanation
Light consists of stream of massless particles called photons having energy hf, moving along electromagnetic waves (1905)When photon strikes electron, it gives up all its energy to the electronIf hf > w (work function of metal), emission occurs
Einstein’s Explanation
Light intensity makes no difference if frequency is below a threshold frequency, ft
Work function of metal = h ft
Max. electron kinetic energy = hf - hft
Einstein won Nobel Prize for explanation
Albert Einstein
1879-1955
Laws of Photoelectric Emission
• Rate of emission is directly proportional to intensity of incident light
• Kinetic energy of photoelectrons is independent of intensity of incident light.
• Maximum kinetic energy of photoelectrons varies directly with difference between frequency of incident light and cutoff frequency of metal
Compton ShiftAurthur Compton sent X-rays into graphite
X-rays scattered by collisions with electrons showed longer wavelength and lower energy
Energy and momentum transferred from photon to electron
Further support for particle nature of light
The Compton Shift
Arthur Compton
1892-1962
The Quantized AtomRutherford’s discovery of nucleus (1911) led to “solar system” model of atom
Orbiting electrons contradicted e-m theory
Niels Bohr (1913) proposed model of atom with electron orbits based on quantized energy states
Difference between energy states always some multiple of Planck’s constant
Light EmissionElectrons can absorb energy and “jump” to higher energy levelWhen electrons fall to lower level, photon is emitted whose energy equals difference in the energy of the two levelsSince frequency depends on energy, different energy changes cause different colors (frequencies) of light emitted
Niels Bohr
1885-1962
Ernst Rutherford
1871-1937
Line Spectra
Unique structure of each element results in unique pattern of emission lines for each element allowing identification by spectroscopy
When light passes through the element (usually as a low pressure gas) same frequencies are absorbed from the spectrum
Continuous Spectrum
When atoms are crowded together in a solid or dense gas, available energy levels are so numerous, all light frequencies are emitted
White light is seen and when dispersed by a prism or diffraction grating, all colors are seen
The Hydrogen Spectrum
Hydrogen spectrum first to be analyzed
Visible emission lines predicted and observed by Balmer; called Balmer series.
6 uv emission lines (Lyman series) and 4 ir lines (Paschen series) discovered later.
Matter and Waves
de Broglie proposed wave-particle duality applied to matter particles, photons must have momentum
E = hf = mc2 ; so mc = h/ , photon momentum
h/mv , wavelength of particle with mass m and velocity v
Louis de Broglie
1892-1987
Matter and Waves
All matter has wave properties but for large objects, wavelength is too small to be observedWave nature of electron explains why only some orbits are stable: standing wave must fit in orbitWhole number of wavelengths must equal circumference of orbit
Matter Waves
X-Ray Production
Reverse of photoelectric effect
High energy electron beam strike metal causing emission of photons
EK = hfmax - w
Frequency of photon depends on speed of electron
Werner Heisenberg
1901-1976
The Uncertainty Principle (Heisenberg, 1927)
It is impossible to simultaneously measure particle’s position and momentum accurately
Measurement of one quantity changes the other
Electron’s location can only be described by probability
Erwin Schrödinger
1887-1961
The Wave Function
Schrödinger (1926) proposed wave function (Ψ) that describes subatomic particles
Probability of electron’s location can be found using the wave function
Electron orbitals are probability distributions called electron clouds