Why do a large number of lines appear in hydrogen spectrum?

A hydrogen atom contains only one electron, but this electron can be raised to higher energy states. The large number of spectral lines in hydrogen atom spectrum are due to the fact that a large number of transitions of the electron can take place between the different energy states.

Why is there more than one set of lines in the full emission spectrum?

Different types of atoms have different energy levels. As a result each produces photons with different energy and so the line spectra for different elements will be different.

Why do we only see 4 lines in the hydrogen emission spectrum?

Whilst hydrogen has only one electron, there are many shells or energy levels which that electron can transition between. The gaps between those levels are all different, so each has its own frequency resulting in different lines in the spectra.

Why is a line spectrum observed for metal atoms?

atoms is known as a line spectrum, because the radiation (light) emitted consists of a series of sharp lines. The wavelengths of the lines are characteristic of the element and may form extremely complex patterns.

How are the visible lines created in hydrogen?

In the simplified Rutherford Bohr model of the hydrogen atom, the Balmer lines result from an electron jump between the second energy level closest to the nucleus, and those levels more distant. For hydrogen (Z = 1) this transition results in a photon of wavelength 656 nm (red).

Why do elements have more than one spectral line?

Its because, elements have electrons in orbitals. In addition there will be infinite number of empty orbitals. So when transitions occur in the atoms of an element, they absorb/release energy in the form of spectral lines.

How many spectral lines are produced in the spectrum of hydrogen atom from 5th energy level?

Hence the final answer is three spectral lines lie in the visible region for the hydrogen atom when electrons jump from $ n_2 = 5\; $ to $ n_1 = 1\; $ in the visible region.

How many spectral lines are formed in hydrogen spectrum when excited electrons jump from 5th orbit to 1st in multiple steps?

So, the six spectral lines are, 5 → 4.

Why is there no yellow line in the hydrogen emission spectrum?

Each time an electron changes from a higher energy state to a lower one, a package of energy is emitted. Sometimes the energy emitted is visible. There is no transition in the hydrogen atom that results in the emission of yellow light.

Why is a line spectrum observed?

The presence of spectral lines is explained by quantum mechanics in terms of the energy levels of atoms, ions and molecules. Emission lines occur when the electrons of an excited atom, element or molecule move between energy levels, returning towards the ground state.