How does the Bohr model of the hydrogen atom explain the spectrum of hydrogen?

Bohr’s model explains the spectral lines of the hydrogen atomic emission spectrum. While the electron of the atom remains in the ground state, its energy is unchanged. When the atom absorbs one or more quanta of energy, the electron moves from the ground state orbit to an excited state orbit that is further away.

What correctly describes the relationship between the spectrum of one atom and the spectrum of another?

What correctly describes the relationship between the spectrum of one atom and the spectrum of another? The spectra are similar; however, the lines are offset by a certain wavelength either to higher or lower wavelengths due to the number of protons in the nucleus of the atoms.

How can the spectrum of hydrogen contain so many lines when hydrogen contains only one electron?

Though a hydrogen atom has only one electron, it contains a large number of shells, so when this single electron jumps from one shell to another, a photon is emitted, and the energy difference of the shells causes different wavelengths to be released… hence, mono-electronic hydrogen has many spectral lines.

How does his model explain atomic spectra?

The Bohr model suggests that the atomic spectra of atoms is produced by electrons gaining energy from some source, jumping up to a higher energy level, then immediately dropping back to a lower energy level and emitting the energy difference between the two energy levels.

What does the Bohr model explain?

The Bohr model shows that the electrons in atoms are in orbits of differing energy around the nucleus (think of planets orbiting around the sun). Bohr used the term energy levels (or shells) to describe these orbits of differing energy.

Why does each element have its own unique atomic line spectrum?

Each elements emission spectrum is distinct because each element has a different set of electron energy levels. The emission lines correspond to the differences between various pairs of the many energy levels. The lines (photons) are emitted as electrons fall from higher energy orbitals to lower energies.

What is the relationship between the atomic number and the number of spectral lines?

I think you are mixing two different n. If an atom has N=number of levels then the number of transitions and therefore number of spectral lines is N−1. However, for energy levels in an atom it is common to use three numbers to label each energy levels. This numbers are n,l,m.

How would you obtain the atomic spectrum of hydrogen?

Emission Spectrum of Hydrogen. When an electric current is passed through a glass tube that contains hydrogen gas at low pressure the tube gives off blue light. When this light is passed through a prism (as shown in the figure below), four narrow bands of bright light are observed against a black background.

Why might spectra of atoms with more than one electron be difficult to explain using Bohr’s model?

In Bohr’s model, electrons can only exist in certain orbits and thus, can only have certain energies. As a result, we say that the energies of the electrons are quantized. to predict the energy level of an electron in the nth energy level (or orbit) of a hydrogen atom.

How does the Bohr model explain that each element has a unique emission spectrum?

In the Bohr model, electrons can exist only in certain energy levels surrounding the atom. When electrons jump from a higher energy level to a lower one, they emit light at a wavelength that corresponds to the energy difference between the levels. The energy levels in each atom are unique.