Chapter 11: Atomic Phenomena Flashcards
At absolute zero (0 degrees Kelvin), what occurs:
all random atomic movement stops
Blackbody radiators are:
ideal radiators with set light-radiation profiles, dependent on their temperature; ideal radiators are also ideal absorbers and appear black because they absorb all wavelengths of light (when at temperatures lower than their surroundings)
The peak wavelength for a blackbody radiator is:
the wavelength at which the object radiates the greatest amount of energy; it is proportional to the blackbody’s absolute temperature
The intensity of energy being radiated by a blackbody is proportional to:
the fourth power of the body’s absolute temperature
Blackbody radiation is approximated by:
cavity radiation
Equation to determine the peak wavelength emitted by an object at a given temperature (Wien’s Displacement Law):
(λpeak)(T) = constant = 2.9 X 10-3 m•K
λpeak refers to:
the wavelength at which more energy is emitted than at any other wavelength; it does not refer to the maximum wavelength emitted
Equation to determine the total energy emitted by a blackbody (Stefan-Boltzmann Law):
ET = σT4
where σ is a constant, T is the temperature, and ET is the total energy emitted per unit of area
units = W/m2
The photoelectric effect is:
the ejection of an electron from the surface of a metal; it occurs in a vacuum when the metal is hit with incident light (a photon) that has a high enough energy to eject the electron
The threshold frequency is:
the minimum light frequency necessary to eject an electron from a given metal; depends on the type of metal exposed to radiation
Equation to determine the energy of a photon:
E = hf
where h is Planck’s constant and f is the frequency of the light. Once you know the frequency, you can find the wavelength using:
λ = c / f
The energy of a photon increases with:
increasing frequency
Equation to determine the maximum kinetic energy of an electron ejected by an incident photon:
Kmax = hf - W
where W is the work function of the metal in question
W = hft
The Work Function is:
the minimum energy required to eject an electron and is related to the threshold frequency of a given metal:
W = hft
Relationship between the frequency of the incident photon and the threshold frequency:
if the frequency of the incident photon is less than ft, no electron will be ejected
if the frequency of the incident proton is greater than ft, an electron will be ejected and the maximum kinetic energy will be the difference between hf and hft (the excess energy is converted into KE of the electron)
If the photoelectric effect is occuring, what do electrons do?
electrons leaving the surface of the metal will form a current; the magnitude of this current is proportional to the intensity of the incident beam of photons
The higher the principal quantum number, the higher the:
energy of an electron
The Bohr Model of the Hydrogen Atom is:
an early quantum mechanical model of one-electron systems that proposes a hydrogen atom is a dense nucleus orbited by an electron
For an electron to jump from a lower energy orbital to a higher energy orbital, it must:
absorb an amount of energy (hf) exactly equal to the difference between the two energy levels (in the form of a photon of light at the proper frequency)
For an electron to jump from a higher energy orbital to a lower energy orbital, it must:
emit an amount of energy (hf) exaclty equal to the difference between the two energy levels (in the form of a photon of light at the proper frequency)
Equation to estimate the energy of an electron with a given quantum number (n) in joules:
E = - Rh/n2
where R is Rydberg’s constant and n is the quantum level
Equation to estimate the energy of an electron with a given quantum number (n) in electron-volts (eV):
En = - 13.6 eV/n2
The energy of an electron increases the farther is is from:
the nucleus; the energy gets less negative as it moves farther from the nucleus. Once the energy becomes positive, the electron is no longer bound to the nucleus
In Bohr’s model, as n2 increases, what happens to the energy of the electron?
it increases
Ground state:
the small orbit an electron can be found; the lowest energy level; n = 1
An excited state is:
any orbit higher than the electron’s ground state, and, thus, has more energy than the ground state
Equation to determine the change in energy of an electron due to absorption or emission of a photon:
∆E = Ef - Ei
(both of these values will always be negative; if ∆E is negative, their was an emission of energy and the electron came down states)
units = joules
Equation to determine the change in energy of an electron due to absorption or emission of a photon:
hf = |∆E|
units = joules
Flourescence is a method by which:
absorbed high frequency light (usually UV) is emitted by a substance as lower frequency light (usually visible light); the electrons return to their ground state in multiple steps, releasing a lower-frequency photon than the absobed photon at each step
Equation to find the wavelength of a photon:
λ = c/f
where c = 3 X 108