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The possible values for the angular
momentum of an electron orbiting a hydrogen nucleus could be given by
L = nh/2π
n is the principal quantum number, which can be any positive integer, and h
is Planck’s constant
He then related the permitted angular momentum values to the energy of the electrons
E =− RH/n2
RH is the experimentally determined Rydberg unit of energy,
2.18 × 10-18 J/electron. Therefore, like angular momentum, the energy of the electron changes in discrete amounts with respect to the quantum number. - A value of zero
energy was assigned to the state in which the proton and electron are separated
completely( no attractive force between them)- the
electron in any of its quantized states in the atom will have an attractive force toward
the proton, represented by the negative sign in the equation- the energy of an electron increases—
becomes less negative—the farther out from the nucleus that it is located (increasing n).
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