Hyrdogen Series
Energy Levels
Rydberg Constant
Emission and Absorption Spectra
Franck-Hertz Experiment
100
Transitions of electrons between n = 2 and higher in atomic hydrogen.
What is the Balmer series?
100
Why does an electron in the second energy level have more energy than one in the ground state, according to the Bohr model of the atom?
What is the electron in the ground state is a location that is closer to the nucleus, and therefore, more stable. Electrons in higher energy states are further from the nucleus and are therefore less tightly bound to the nucleus?
100
Using the Rydberg formula, calculate the wavelength when an electron transitions from n = 3 to n= 2 in a hydrogen atom.
What is 1/ʎ = 1.10 x 10^7/m(1/2^2 - 1/3^2) 1/ʎ = 1.10 x 10^7/m (0.25-0.111) 1/ʎ = 1.10 x 10^7/m(0.139) 1/ʎ = 0.153 x10^7/m ʎ = 6.50 x 10^-8 m
100
Continuous spectra, emission spectra, and absorption spectra.
What is the three types of spectra?
100
Where the electrons were accelerated and current collected.
What is the Franck-Hertz apparatus?
200
“H-alpha”, “H-beta”, “H-gamma” and so on where H is element hydrogen.
What are Balmer lines?
200
Visualize the different energy levels of an atom and the energy required for an electron to move from one energy level to the other.
What is an energy level diagram?
200
Used to predict wavelength of light resulting from electron moving between energy levels of atom.
What is the rydberg formula?
200
A magnetic field causes the spectral lines to split due to small changes in the energy associated with different spins of the electrons occupying each energy state.
What is the Zeeman Effect?
200
Accelerating voltage for mercury is 4.9V.
What is the lowest energy required by the mercury atom for excitation?
300
Series that is entirely in the UV.
What is the Lyman series?
300
E = h (Plank’s constant) x c (speed light) / wavelength
How to calculate the energy of a photon?
300
R = (1.0973731568539(55) x 107 m-1)
What is the Rydberg's constant?
300
Emitted when gases are at a high pressure. In general, solids, liquids and dense gases emit light at all wavelengths.
What is a continuous spectra?
300
As the electrons were accelerated at a voltage of 4.9 eV, the electrons underwent _________ _________ with the mercury
What are inelastic collisions?
400
1/λ = R(1/2^2 - 1/n^2) n = 3, 4, 5 ...
What is Balmer's formula?
400
Negative eV values represent _______________________
What is the energy bound to the nucleus?
400
Use the Rydberg equation to calculate the wavelength of the photon absorbed when a hydrogen atom undergoes a transition from n=4 to n=6.
What is 1/λ = RH · (1/(n1)² - 1/(n2)²) λ = 1/[ RH · (1/(n1)² - 1/(n2)²) ] = 1 / [ 1.096776×10+7m^-1 · (1/4² - 1/6²) ] = 2.6259×10-6m
400
Produced by cool gases illuminated by another source
What is the absorption sepctra?
400
Energy levels in atoms are _________
What is quantized?
500
1/λ = R(1/3^2 - 1/n^2) n = 4, 5, 6 ...
What is Paschen's series?
500
Electron can only exist in ________ __________ ________.
What are discrete energy levels?
500
Using the Rydberg formula, calculate the initial energy level when an electron in a hydrogen atom transitions into n= 2 and emits a photon at 410.1 nm. Note: the Rydberg constant = 1.097 x 107 m^–1
What is n = 6?
500
Produced by thin gases where the atoms do not experience many collisions.
What is emission spectra?
500
New wavelength can be calculated and also find the angle at which the photon emerges from the collision using this formula.
What is λ’ - λ = h/ mec (1-cosΘ)?
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