Modern Physics
An electron in an atom moves from an energy level of -3.4 eV to -13.6 eV. What happens?
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 gas is heated and emits light. The spectrum of this light shows bright lines at specific wavelengths. What type of spectrum is this?
A photon with energy 8 eV strikes an atom and ejects an electron with kinetic energy 2 eV. What is the binding energy of the electron in the atom?
An atom transitions from a lower energy state to a higher energy state. What process must occur?
An electron transitions between energy levels in an atom, emitting a photon. Which of the following is true regarding the emitted photon's properties?
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A newly discovered gas is analyzed, and its spectrum shows absorption lines at 410 nm, 434 nm, 486 nm, and 656 nm. A known element has emission lines at 434 nm and 656 nm. What can be concluded?
An electron is removed from an atom. What is this process called?
What determines the specific, quantized energy levels in an atom?