Final answer:
The Lyman series corresponds to electron transitions to the ground state (n=1) of the hydrogen atom. The energies involved in such transitions can be calculated using the provided wavelengths and Bohr's model.
Step-by-step explanation:
The correct statement about the Lyman series is that it corresponds to electron transitions to the n=1 energy level. The energy levels for a hydrogen atom are calculated using Bohr's model and constitute a series of transitions where the final state is the ground state (n=1). Bohr's model tells us that these energy levels are proportional to 1/n², meaning that the energy released during a transition is related to the difference between the initial and final energy levels. Each series represents different downward transitions, and for the Lyman series, all transitions end in the ground state.
To calculate the energies of the first five excited states using the wavelengths of the Lyman series provided, we have to apply the equation E₂ - E₁ = -13.6eV * (1/n₁² - 1/n₂²), where E2 is the excited state's energy and E1 is the ground state's energy (which is -13.6 eV). The change in energy ∆E corresponds to the photon energy involved in the transition (E₂ - E₁), which can be related to the wavelength (λ) using the equation ∆E=hc/λ, where h is Planck's constant and c is the speed of light.