1. The energy of the electron in the lowest level of the hydrogen atom (n=1) is -2.179×10-18 J. What is the energy of the electron in level n=5? -8.716×10-20 J 2.The electron in a hydrogen atom moves from level n=6 to level n=4.
a) Is a photon emitted or absorbed?
b) What is the wavelength of the photon?
Energy of an electron in nth orbital is given by,
E= -(2.179x10-18)/n2 Joules
, therefore, we can write as,
E5 = (-2.179x10-18)(12/52)
E5 = -8.176x10-20
a) as the electron energy is directly proportional to the square of the orbit number,
when the electron moves from n=6 to n=4,
its energy decreases, so it must have emitted a photon so that the energy will decrease.
b) E6-E4 = (E1/n62) - (E1/n42) (From above equations)
E6-E4 = 7.5659 x 10-20 Joules
now this energy difference will be equal to (hc/)
where h = Planck's constant
c = velocity of light
= wavelength of photon
= hc / change in energy
=((6.634x10-34)x(3x108))/7.5659 x 10-20
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