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Two of the wavelengths emitted by a hydrogen atom are 102.6nmand1876nm.

a. What are the mand nvalues for each of these wavelengths?

b. For each of these wavelengths, is the light infrared, visible, or ultraviolet?

Short Answer

Expert verified

a. For λ=102.6nm,n=3and m=1.

Forλ=1876nm,n=4andm=3.

b. 1) Ultraviolet

2) Infrared

Step by step solution

01

Part (a) Step 1: Given Information

We have given that wavelengths λ1=102.6nmand λ2=1876nm.

02

Part (a) Step 2: Evaluation

Formula for calculating wavelength is given as:

λ=91.181m2-1n2nm

substituting λ1=102.6nm

1m2-1n2=91.18102.6=0.889

comparing we can see that m=1andn=3satisfies the above equation.

substituting λ2=1876nm

1m2-1n2=91.181876=0.0486

comparing we can see thatm=3andn=4satisfies the above equation.

03

Part (b) Step 1: Given information

We have given that wavelengths λ1=102.6nmandλ2=1876nm.

04

Part (b) Step 2: Evaluation

λ1has m=1which corresponds to lyman series and all lines in lyman series lie in ultraviolet region of electromagnetic spectrum.

λ2hasm=3which corresponds to paschen series and all in paschen series lie in infrared region of electromagnetic spectrum.

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