I The allowed energies of a simple atom are
a. Draw the atom's energy-level diagram. Label each level with the energy and the quantum number.
b. What wavelengths appear in the atom's emission spectrum?
c. What wavelengths appear in the atom's absorption spectrum?
We can start with expression for energy of the photon
(from atom's energy-level diagram)
Because of simplicity, we will continue to use the following tags:
On the same way we can find wavelengths in atom's absorption spectrum
A 100 W incandescent lightbulb emits about 5 W of visible light. (The other 95 W are emitted as infrared radiation or lost as heat to the surroundings.) The average wavelength of the visible light is about 600 nm, so make the simplifying assumption that all the light has this wavelength. How many visible-light photons does the bulb emit per second?
Consider a hydrogen atom in stationary state n.
a. Show that the orbital period of an electron in quantum state n is, and find a numerical value for
b. On average, an atom stays in the n = 2 state for 1.6 ns before undergoing a quantum jump to the n = 1 state. On average, how many revolutions does the electron make before the quantum jump?
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