Question

# Draw a neat labelled energy level diagram and explain the different series of spectral lines for hydrogen atom.

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Solution

## The energy level diagram of the hydrogen atom is shown in the figure above depicting different series line. There are four series namely 1. Lyman Series (U.V.) 2 Blamer Series (visible) 3. Psachen Series (infrared) 4. Brackett Series (infrared) 5. Pfund Series (infrared) n=principle quantum number whose values ranges from 1−∞ n=1represents the ground energy level n=∞is the highest energy level. 1. Lyman Series (U.V.) In this series the transition occur from n>1 to the first orbit that isn=1. This represents the Lyman Series of the Hydrogen atom. It is mainly observed in the ultraviolet region of the EM wave. 1λ=R(112−1n2) Wheren=2,3 This is further divided into sublevels as α−lymanfor n=2 and so on. 2 Blamer Series (visible) In this series the transition occur from n>2to the second orbit that isn=2. This represents the Balmer Series of the Hydrogen atom. It is mainly observed in the Visible region of the EM wave. 1λ=R(122−1n2) Where, n=3,4 This is further divided into sublevels as α−Balmerfor n=3and so on. 3. Psachen Series (infrared) In this series the transition occur from n>3 to the second orbit that isn=3. This represents the Paschen Series of the Hydrogen atom. It is mainly observed in the Infrared region of the EM wave. 1λ=R(132−1n2) Where n=4,5,6 4. Brackett Series (infrared) In this series the transition occur from n>4 to the second orbit that isn=4. This represents the Bracket Series of the Hydrogen atom. It is mainly observed in the Infrared region of the EM wave. 1λ=R(142−1n2) Where n=5,6, 5. Pfund Series (infrared) In this series the transition occur fromn>5to the second orbit that isn=5. This represents the Bracket Series of the Hydrogen atom. It is mainly observed in the Infrared region of the EM wave. 1λ=R(152−1n2) Where n=6,7

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