If the velocity of the electron in Bohr’s first orbit is 2.19 x 106 m s-1, calculate the de Brogile wavelength associated with it.

ν = 2.19 x 106 m s-1As per de Brogile’s equation, λ= m/v = (6.626 x 10-34 kg m2 s-1) / (9.1 x 10-31 kg) x (2.19 x 106 m s-1)6.626/91 * 2.19= x 10-34+25 m = 0.33243 x 10-9 m = 332.43 pm

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Ncert Solutions Chemistry Class 11th Chemistry Class 11th Structure of Atoms

If the velocity of the electron in Bohr’s first orbit is 2.19 x 10⁶ m s^-1, calculate the de Brogile wavelength associated with it.

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Answered by

alok kumar singh | Contributor-Level 10

3 months ago

ν = 2.19 x 10⁶ m s^-1

As per de Brogile’s equation,

λ= m/v = (6.626 x 10^-34 kg m²s^-1) / (9.1 x 10^-31 kg) x (2.19 x 10⁶ m s^-1)

6.626/91 * 2.19= x 10^-34+25 m = 0.33243 x 10^-9 m = 332.43 pm

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