Emission spectrum of hydrogen atom

Question 1

Describe how a series os achieved.

Answer 1

~Electrons within an atom can be excited to higher energy levels when heat or other forms of energy are applied. The excited state is not stable and short-lived. Thus the electron returns rapidly to its initial state simultaneously emitting energy in the form of a photon.
~The energy of the released photon equals the energy difference between the excited and initial states of the electron
~Since there are discrete values of electron energies only certain energies (frequencies, wavelengths) may be emitted by the atom.
~The different electrons within the atom will be excited to different energy levels and each will emit a photon characteristic of the energy transition it undergoes.
~Thus a line spectrum is produced with each line corresponding to a specific electron transition.
~Each element produces a unique emission spectrum that can serve as its fingerprint.
~The set of spectral lines observed during transitions from all higher levels into a certain energy level corresponding to the given n is called a series.

Question 2

What are the series of atomic emission spectra of hydrogen?

Answer 2

The atomic emission spectra of hydrogen is composed of several series:

Lyman Series: lines corresponding to e- transition from higher energy levels into the ground state (n = 1)
–observed in the ultraviolet region of light (high energy emission)

Balmer series: lines corresponding to e- transitions from higher energy levels into
n = 2
–observed in the region of visible light

Paschen series: lines corresponding to e- transitions from higher energy levels into
n = 3 (Paschen‘s series) and to higher values of n
–observed in the region of infrared light (low energy emission)

*The greatest energy emitted is in the Lyman series and corresponds to an electron falling from n = to n = 1