Question

Which statement is correct for the emission spectrum of the hydrogen atom?

a. The lines converge at lower energies.
b. The lines are produced when electrons move from lower to higher energy levels.
c. The lines in the visible region involve electron transitions into the energy level closest to the nucleus.
d. The line corresponding to the greatest emission of energy is in the ultraviolet region.

Answer 1

The emission line corresponding to the greatest energy in the hydrogen spectrum is the Lyman series in the ultraviolet region. These are transitions to the ground state, while the Balmer series represents transitions to the second orbit and is visible.

Step-by-step explanation:

The correct statement for the emission spectrum of the hydrogen atom is 'd. The line corresponding to the greatest emission of energy is in the ultraviolet region'. The emission process involves an electron transitioning from a higher energy level to a lower one, releasing a photon. For hydrogen, transitions to the ground state (n=1) result in the ultraviolet Lyman series of spectral lines, which include the line corresponding to the greatest energy emission. The Balmer series, visible in the spectrum, are transitions from higher energy levels to the second orbit (n=2). The lines in this series include wavelengths at 656 nm (red), 486 nm (green), 434 nm (blue), and 410 nm (violet), with the transitions to n=2 emitting photons in the visible light range.