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Chapter 37: 3 - Excercises And Problems (page 1081)

The wavelengths in the hydrogen spectrum with m=1form a series of spectral lines called the Lyman series. Calculate the wavelengths of the first four members of the Lyman series.

Short Answer

Expert verified

(a) Wavelength of first member = 121.573nm

(b) Wavelength of second member = 102.577nm

(c) Wavelength of third member = 97.258nm

(d) Wavelength of fourth member = 94.979nm

Step by step solution

01

Given information

Lyman series in hydrogen spectrum starts when value ofm=1

We have to calculate the wavelengths of first four member of Lyman series.

02

Simplify 

(a)The first member of Lyman series is , m=1ton=2

By hydrogen emission spectrum wavelengths is given by,

λ=91.181m2-1n2nm

By substituting the value of m=1and n=2 in above formula , we get

λ=91.18112-122nm=91.1811-14nm=91.184-14nm=364.723nm=121.573nm

(b) The wavelength of second member of Lyman series is ,m=1ton=3

By substituting the value of m=1and n=3 in above wavelength formula

λ=91.18112-132nm=91.1811-19nm=91.189-19nm=820.628nm=102.577nm

(c) The wavelength of third member of Lyman series is ,m=1ton=4

By substituting the value of m=1and n=4 in above wavelength ,

λ=91.18112-142nm=91.1811-116nm=91.1816-116nm=1458.8815nm=97.258nm

(d) The wavelength of fourth member of Lyman series is ,m=1ton=5

By substituting the value of m=1 and n=5 in above wavelength ,

λ=91.18112-152=91.1811-125=91.1825-125=2279.524=94.979nm

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