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.

Question

Noe Golden

Chemistry

9 July, 22:57

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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Answers (1)

Know the Answer?

Sierra Warner · Answer 1

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