Final answer:
The true statements regarding atom behavior and electromagnetic radiation are: The energy of electromagnetic radiation increases with frequency; an electron can transition between energy levels by emitting radiation; and frequency and wavelength are inversely proportional.
Step-by-step explanation:
The statements concern the behavior of atoms and electromagnetic radiation upon excitation and de-excitation. Here is the clarification of each statement:
Statement 1: False. An excited atom returns to its ground state by emitting radiation, not absorbing it.
Statement 2: False. The energy of an atom decreases when electromagnetic radiation is emitted from it because the emission is a loss of energy.
Statement 3: True. The energy of electromagnetic radiation increases as its frequency increases.
Statement 4: True. An electron in a hydrogen atom can transition from the n=4 state to the n=2 state by emitting electromagnetic radiation at the appropriate frequency.
Statement 5: True. The frequency and wavelength of electromagnetic radiation are inversely proportional to each other.
Atomic Excitations and De-Excitations
When an atom is heated, such as in a sample of hydrogen gas, its electrons are excited to higher energy levels and, upon returning to the ground state, they emit light of specific colors based on the energy transition. This emission accounts for the discrete lines in the emission spectrum and explains the pale pink color observed. The best explanation for this behavior would be option b: As the gas heats up, the electrons within the hydrogen atoms are excited to high energy levels. As the electrons transition to lower energies, they emit light of specific colors, corresponding to the distinct wavelengths of the transitions.