Topic 3 2/2 Flashcards
Describe:
Atomic spectra
Range of frequencies of EM radiation emitted/absorbed by matter. 3 types of spectra:
Continuous, Line emission (Colour lines), Line absorption (Black lines)
Describe:
Incandescence
All matter vibrates, charges do so and release EM radiation. Increased temperature, increases oscillations of vibrations, thus frequency of EM, which can result in visible light being emitted.
Describe:
the changes in the spectrum of a filament globe as the temperature of the filament increases.
Increase in temperature will cause higher frequency EM radiation to be released, closer to violet colour.
Describe:
characteristics of the line emission spectra of elements.
When atoms of pure gas is heated or subject to potential difference. Light emitted is viewed through spectrometer/diffraction grating, showing color lines on dark.
Specific to each gas, thus can identify them.
Explain:
the uniqueness of the spectra of elements can be used to identify the presence of an element.
Emission spectra is specific to each atom as electron shells are different for each. Thus, a known gass’s emission spectra can be used to define its presence via discrete frequencies of light absorbed.
Explain:
production of characteristic X-rays in an X-ray tube.
Produced through incident electrons colliding and removing electrons in lower energy levels of target metals. Higher energy level electrons drop down to fill place, releasing X-ray photon with energy equal to the energy difference between the energy levels.
Describe:
Energy levels
There are different states in an atom, each with their own energy, which can be represented in energy-lvl diagram. Can be raised to excited states through having one electron not in ground state.
Explain:
magnitude of the transitions on an energy-level diagram relation to the region in the electromagnetic spectrum of the emitted photons
From higher to lower, photons are emitted with energy equal to the difference of energy levels the electron passed. Units of energy in eV
Describe:
Ionisation energy of an atom
the minimum energy required to remove a single electron from the atom in its ground state.
Describe:
line absorption spectrum of atomic hydrogen.
Only one electron with series dependant on ending level from 5 up.
Lyman series. N = 1 [UV]
Balmer series. N = 2 [Visible]
Paschen series. N = 3 [IR]
Explain:
why there are no absorption lines in the visible region for hydrogen at room temperature.
At room temperature, electron is in ground state, meaning that any transitions that occur will be in the Lymans series, requiring UV light, not visible.
Explain:
presence of absorption lines (Fraunhofer lines) in the Sun’s spectrum.
Sun produces white light, spanning the visible spectrum. Electrons in atoms of the suns atmosphere absorb photons with energy equal to the gap between lower/higher energy states. These incident photos are removed from the total light, resulting in the dark lines.
Describe:
Fluorescence
process of converting high-energy photons into a larger number of lower-energy photons
Describe:
Stimulated emission
a photon with energy corresponding to a transition from a higher-energy state to a lower-energy state is incident on an atom in the higher state, it can stimulate a transition to the lower state. This results in two identical photons
Compare
process of stimulated emission with that of ordinary (or spontaneous) emission.
Stimulated emission occurs when a photon of energy corresponding to a transition of high->low energy states is incident on an atom in the energy state, resulting in an incident photon and emitted photon which have equal energy.
Spontanious emission results in only one photon release, is also immediate.