**Journal of Modern Physics**

Vol.05 No.14(2014), Article ID:49019,8 pages

10.4236/jmp.2014.514127

Bohr’s Spectrum of Quantum States in the Atomic Hydrogen Deduced from the Uncertainty Principle for Energy and Time

Stanisław Olszewski

Institute of Physical Chemistry, Polish Academy of Sciences, Warsaw, Poland

Email: olsz@ichf.edu.pl

Copyright © 2014 by author and Scientific Research Publishing Inc.

This work is licensed under the Creative Commons Attribution International License (CC BY).

Received 12 June 2014; revised 8 July 2014; accepted 1 August 2014

ABSTRACT

A modified uncertainty principle coupling the intervals of energy and time can lead to the shortest distance attained in course of the excitation process, as well as the shortest possible time interval for that process. These lower bounds are much similar to the interval limits deduced on both the experimental and theoretical footing in the era when the Heisenberg uncertainty principle has been developed. In effect of the bounds existence, a maximal nuclear charge Ze acceptable for the Bohr atomic ion could be calculated. In the next step the velocity of electron transitions between the Bohr orbits is found to be close to the speed of light. This result provides us with the energy spectrum of transitions similar to that obtained in the Bohr’s model. A momentary force acting on the electrons in course of their transitions is estimated to be by many orders larger than a steady electrostatic force existent between the atomic electron and the nucleus.

**Keywords:**

Uncertainty Principle for Energy and Time, Bohr’s Spectrum of Quantum levels in the Hydrogen Atom

1. Introduction

The Bohr model of the hydrogen atom [1] assumed circular trajectories for electrons circulating about the atomic nucleus and the motion along these trajectories has been quantized. In effect definite radii of the orbits

(1)

and electron velocities on these orbits

(2)

could be calculated. From the balance of the electron energy

(3)

in which and are substituted from (1) and (2), a well-known quantum formula

(4)

could be obtained. Later it became possible to derive the same formula on the basis of a quantum- mechanical approach [2] .

The classical Bohr model stimulated several questions concerning its validity, the main of which was perhaps how the electron―in course of its transition to another orbit―can choose that orbit and become limited in its further motion to it [3] [4] . In other words the problem was concerning not so much separate, but their differences

(5)

for some, and the way how (5) can define the atomic spectrum.

The present paper tends to meet this question in case when an approach to the energy spectrum is done on the basis of the uncertainty principle, the essence of which are the energy differences applied together with the time intervals

(6)

In fact the principle expressed in the form given by Heisenberg [5]

(7)

where is a difference of energy met in the quantum process, and has been next objected on many occasions [6] - [8] . The effect of that numerous textbooks on physics or quantum mechanics do not even mention the validity; see e.g. [9] . Nevertheless a modification of (7) into a new formula

(8)

could be performed [10] - [12] and we show below that this transformation makes the uncertainty principle suitable in obtainig the atomic spectrum; the Formula (7) is fully ineffective at that point.

But before the spectrum is demonstrated, our aim is to point out that (8) can give also the lower bounds of the space intervals, say that along the Cartesian coordinate which is

(9)

This result can give a similar lower bound of the time intervals (6) met in the quantum processes.

2. Lower Bounds of the Position and Time Intervals Derived from the Uncertainty Principle for Energy and Time

Heisenberg [5] has coupled the observables which are the intervals of the position coordinate and that of momentum in the uncertainty relations similar to that given in (7) for the energy and time. Mathematically this is expressed by the formula

(10)

on condition that only the -coordinates of the particle momentum and position are taken into account. Though the observables of a pair in (10) enter the formalism on an approximately equal footing, their experimental background can be much different. For example the momentum of a particle is usually much more accurately defined than its position. A similar property concerns the energy intervals which are easier accessible than those of time, but―contrary to (7)―the mutual position of and in (8) is evidently different.

The Relations (10) and (7) imply no limits for, , as well as and, excepting for their sign. This property comes out from the Formula [13]

(11)

(12)

in which the particle velocity is directed along the axis. Both and can rise up unlimitedly with an increase of

(13)

towards its limit of the light velocity. In effect, in order to satisfy (10) and (7) for arbitrarily large and, the intervals

(14)

and

(15)

entering the (10) and (7) should tend to zero.

But this property has been objected already very soon after the the birth of the Heisenberg uncertainty relations [5] . The objections denying the arbitrary small and have been raised on both the experimen- tal and theoretical footing [14] - [17] . In fact these references proposed that there exists a minimal equal to

(16)

and a minimal equal to

(17)

where is the rest mass of a particle.

In order to derive (16) from (8) let us assume that is the excitation energy of a free particle from the level at to the level of. In this case

(18)

where is the electron momentum.

On the other hand we have

(19)

which is the effect of one of the Hamilton equations:

(20)

A transformation of (19) gives

(19a)

This formula, substituted together with (18) into (8), gives:

(21)

or

(21a)

Therefore we obtain a condition for the smallest equal to

(22)

This expression differs from (16) solely by a factor of. The smallest, labelled by, is obtained from (22) by requirement that the distance is travelled with a maximal speed close to. Therefore

(23)

The result in (23) differs from that in (17) solely by the factor of.

It can be noted that in (23) is only a half of the time interval

(24)

required to transform the kinetic energy of a particle motion into the energy of the electromagnetic radiation [18] .

3. Discussion

The lower bounds of and obtained in (22) and (23) can lead―respectively with the aid of (10) and (8) to the upper bounds of the intervals and. In particular from (10) and (22) we obtain

(25)

and from (8) and (23):

(26)

If instead of (8) the Heisenberg uncertainty relation (7) together with (23) is applied, the result for the upper bound of is

(27)

We see that the Formulae (25)-(27) for the upper bounds of the intervals of momentum and energy approach the relations which are well known from the classical relativistic mechanics. In the present case, however, they are an effect of the quantum-mechanical uncertainty formulae.

If the limiting values and [see (23) and (26)] are substituted into (8), the uncer-

tainty Relation (8)―in order to be satisfied--should attain its certitude in the form

(8a)

for in this case holds the relation

(28)

If the energy change is a radiation transfer of energy, so

(29)

there should exist the formula

(30)

defining a maximal frequency.

For equal to the electron mass we obtain from (30):

(31)

Roughly a similar result for in a metal has been obtained in [10] .

Moreover, for we have from (22) and from (23). The lower limits for the free-electron path and electron transition time in metals calculated before [19] fit the and quoted above.

If the orbital radii of a hydrogen-like atom having the nucleus of charge are considered instead of charge alone, the orbital radii become [20] [21]

(32)

giving the smallest radius

(32a)

According to the result obtained in (22) the smallest possible radius (32) should satisfy the relation

(33)

This gives a limiting condition for the atomic number

(33a)

A similar condition can be obtained by considering the shortest time period acceptable for the orbit. In this case from [20] and the result in (22) it should be satisfied

(34)

By applying next the Formula (33a) in (34) we obtain the relation

(35)

from which, by multiplying the both sides of the last equation in (35) by and taking into account (32a), we have

(35a)

The sense of (35a) is that in order to obtain from (35a) the same limiting as in (33a) we should assume instead of in (32a) as a smallest acceptable distance. This is an expected result if we note that the time formula for involves necessarily the orbit length in calculations and not alone.

4. The Uncertainty Relation (8) Referred to the Energy Spectrum of the Hydrogen Atom

Till the present point the electron motion on the orbits has been mainly taken into account. But in calculating the electron transitions between orbits the electron velocity normal to the orbital trajectories has to be considered. Let the electron which is on a circular orbit labelled by, so its radius is defined in (1), be promoted to another orbit, for example. An effect of this transition is a change of the orbit radius by the amount

(36)

on condition we assume that

(37)

so the term can be henceforth neglected. In course of the electron transition we assume that radiation of velocity is emitted or absorbed. Roughly the time of transition from to can be estimated by the absolute value of the expression

(38)

The property that the time interval satisfies (38) can be derived from the uncertainty principle (8). In a limiting case of (8) the Formula (8a) is valid from which

(39)

In course of the transition process the electron energy on the orbit is changed by an absolute amount equal to [see (5)]:

(40)

If we put

(41)

we obtain from (39) and (40) the formula

(42)

For large the time interval is found to be a short amount of the electron circulation time period

(43)

on the orbit [20] ;. For from (43) and (42) we have:

(44)

where the factor of 137 is coming from the constant expression (33a).

A characteristic point is that a substitution of and from (36) and (42), respectively, to the expression of velocity roughly estimated in (38) gives

(45)

For and we obtain

(45a)

The largest velocity (45) coming from and is.

If an approximate time interval

(46)

is substituted in place of into the Formula (8a) we obtain

(47)

from which

(48)

This expression becomes equal to that obtained from the Bohr theory in (40) on condition

(49)

or

(50)

are satisfied.

In effect a proper choice of for a given provides us with the relation

(51)

Certainly, the can approach an integer number only at a special.

5. The Momentary Force Acting on an Electron in Case of Its Transition between the Orbits

A stationary force acting on the electron of the hydrogen atom is a well-known electrostatic force of the electron attraction by the nucleus. This force is assumed by Bohr to be compensated by the centrifugal force of the electron orbital motion, so on an orbit having the index the electron is submitted to the force

(52)

Evidently this force is of a stationary character. Our aim is to approach a momentary force acting in course of the electron transition between the orbits.

Since the electron velocity of transition is close to [see (45)], the electron momentum associated with transition is a product equal approximately to, where is the electron mass. The momentary force active in a transition from the orbit to another orbit is

(53)

where the transition time―assumed to be the time of the action of the force due to the momentum possessed approximately by the electron―is that calculated in (42). The force obtained in (53) is much larger than (52) because of the ratio

(54)

When the energy relations instead of the forces are taken into account, the force given in (53) is multiplied by the distance travelled upon it, so the energy of transition is

(55)

on condition the velocity property presented in (38) is unchanged. In this case the energy in (55) is much larger than associated with any transition between the electron orbits.

6. Summary

In the first step we have demonstrated on the basis of a modified uncertainty relation between the intervals of energy and time that both an interval of the particle position and that of time can attain some minimal values different than zero. These interval limits differ solely by a factor of from those predicted a long time ago on both the experimental and theoretical footing [5] -[7] . When applied to the hydrogen-like atom, the lower bounds of the intervals for the position interval and interval of time lead to an upper bound for the atomic number equal to 137. On the other hand the upper bounds of the intervals of momentum and energy, obtained from the lower bounds of and, approach the relations which are well known from the classical relativistic mechanics.

A separate attention has been attached to the velocity calculation for the electron transitions between the orbits. First, with the aid of the uncertainty principle, it has been demonstrated that―for the atomic levels having index equal to about 10―this velocity is very close to the light speed. Moreover, the energy changes which accompany the electron transitions become close to those known from the Bohr’s atomic theory. Such result cannot be obtained from the uncertainty Formula (7).

The ratio of the stationary electrostatic force acting on the atomic electron to a momentary force active only in course of the electron transition between the orbits has been estimated in (54).

Cite this paper

StanisławOlszewski, (2014) Bohr’s Spectrum of Quantum States in the Atomic Hydrogen Deduced from the Uncertainty Principle for Energy and Time. *Journal of Modern Physics*,**05**,1264-1271. doi: 10.4236/jmp.2014.514127

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