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3 October, 08:38

A hydrogen atom requires a minimum energy of 2.18*10^-18 J atom to remove an electron from its ground state level. Determine whether a blueviolet light with a wavelength of 434.0 nm can affect this process.

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  1. 3 October, 11:46
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    Just find the energy of the blueviolet light with a wavelength of 434.0 nm using the formula:

    E = hc / lambda

    E = energy

    c = speed of light = 3 x 10^8 m/s

    h = planck's constant = 6.6 x 10^{-34} m^2 kg / s

    lambda = 434 nm = 434 x 10^{-9} m

    Putting these values (with appropriate units) in the above formula:

    we get: Energy, E = 4.5 x 10^{-19} J

    E = 0.45 x 10^{-18} J

    Now, the minimum energy is 2.18*10^-{18} J but our energy is 0.45 x 10^{-18} J which is less.

    Means the electron will not be removed
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