Question

Calculate the frequency and wavelength of an hydrogen electron when it jumps from third line of lymon series .

Answer fast and correctly​

Answer 1

The Bohr’s formula of finding the energy ‘n’th shell is

E = (-13.6)*(Z^2)/n^2 eV

where,

n = the shell from which the electron has to be radiated

Z = atomic number

Therefore, the energy required to radiate the electron corresponding to the Lyman series is:

E = (-13.6)*1/(1)

E= -13.6 eV

There is another formula for energy in terms of wavelength and frequency

E = hc/λ

h = Planck’s constant (6.63*10^-34)

λ = wavelength

c = speed of light in vacuum (3*10^8)

as c/λ = f

f = frequency

Answer 2

Answer:

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Your answer is...!!

The Bohr’s formula of finding the energy ‘n’th shell isE = (-13.6)*(Z^2)/n^2 eV

where,

n = the shell from which the electron has to be radiated

Z = atomic number

Therefore, the energy required to radiate the electron corresponding to the Lyman series is:E = (-13.6)*1/(1)E= -13.6 eV

There is another formula for energy in terms of wavelength and frequency

E = hc/λh = Planck’s constant (6.63*10^-34)λ = wavelengthc = speed of light in vacuum (3*10^8)as c/λ = ff = frequency

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