Modern Physics
An atom transitions from a lower energy state to a higher energy state. What process must occur?
What determines the specific, quantized energy levels in an atom?
An electron in an atom moves from an energy level of -3.4 eV to -13.6 eV. What happens?
An electron transitions between energy levels in an atom, emitting a photon. Which of the following is true regarding the emitted photon's properties?
A hydrogen atom in its ground state absorbs a photon of energy 12.09 eV. To what energy level does the electron transition? (The ground state energy of hydrogen is -13.6 eV, and the energy levels are given by eV)
What is the relationship between the frequency/wavelength and energy of a photon?
A photon with a wavelength of 600 nm is emitted during an atomic transition. Given that Planck's constant is and the speed of light is , what is the energy of the photon?
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An electron in a hypothetical atom transitions from an energy level of -2 eV to -5 eV, emitting a photon. This photon then strikes a metal with a work function of 2.5 eV. What is the maximum kinetic energy of the emitted electron from the metal?
What is a unique characteristic of each element's atomic spectra?
A gas is heated and emits light. The spectrum of this light shows bright lines at specific wavelengths. What type of spectrum is this?