explain the hydrogen spectrum with the …

Bohr Model of Hydrogen
The simplest example of the Bohr Model is for the hydrogen atom (Z = 1) or for a hydrogen-like ion (Z > 1), in which a negatively-charged electron orbits a small positively-charged nucleus. Electromagnetic energy will be absorbed or emitted if an electron moves from one orbit to another. Only certain electron orbits are permitted. The radius of the possible orbits increases as n2, where n is the principal quantum number. The 3 → 2 transition produces the first line of the Balmer series. For hydrogen (Z = 1) this produces a photon having wavelength 656 nm (red light).

Problems with the Bohr Model
It violates the Heisenberg Uncertainty Principle because it considers electrons to have both a known radius and orbit.
The Bohr Model provides an incorrect value for the ground state orbital angular momentum.
It makes poor predictions regarding the spectra of larger atoms.
It does not predict the relative intensities of spectral lines.
The Bohr Model does not explain fine structure and hyperfine structure in spectral lines.