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A simplified approach to the question of how lis related to angular momentum – due to P. W. Milonni and Richard Feynman – can be stated as follows: If can take on only those values mlh, whereml=0,±1,±l , then its square is allowed only valuesml2h2, and the average of localid="1659178449093" l2should be the sum of its allowed values divided by the number of values,2l+1 , because there really is no preferred direction in space, the averages of Lx2andLy2should be the same, and sum of all three should give the average of role="math" localid="1659178641655" L2. Given the sumrole="math" localid="1659178770040" 1Sn2=N(N+1)(2N+1)/6, show that these arguments, the average of L2 should be l(l+1)h2.

Short Answer

Expert verified

Given the sum 1Sn2=N(N+1)(2N+1)/6the average of L2isl(l+1)h2.

Step by step solution

01

Average of Lz2 :

The Azimuthal quantum number specifies the shape and angular momentum of the orbital in the space.

Given that,

If L2can take on only those values mlh, where ml=0,±1,±l, then its square is allowed only values ml2h2, and the average of l2 should be the sum of its allowed values divided by the number of values, 2l+1, because there really is no preferred direction in space, the averages of Lx2andLy2 should be the same, and sum of all three should give the average ofL2 .

Where, L is the Orbital angular momentum, Lx is the component of orbital angular momentum along x-axis, Ly is the component of orbital angular momentum along y-axis, Lz is the component of orbital angular momentum along z-axis, l is theAzimuthal quantum number,ml is theMagnetic quantum number.

role="math" localid="1659179529670" Lz2=12l+1ml=-llml2h2

Where, h is Planck’s constant.

Lz2=22l+1ml=-llml2h2=22l+1h2ll+12l+1/6=13h2ll+1

02

Average of  :

It is also given that,

Avg.ofLx2=Avg.ofLy2=Avg.ofLz2 ….. (1)

Hence,

Avg.ofL2=Avg.ofLy2=Avg.ofLz2=3×Avg.ofLx2+Avg.ofLy2+Avg.ofLz2=3×AvgofLz2=3×13h2ll+1=h2ll+1

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Most popular questions from this chapter

Question: The kinetic energy of hydrogen atom wave functions for which lis its minimum value of 0 is all radial. This is the case for the 1s and 2s states. The 2 p state has some rotational kinetic energy and some radial. Show that for very large n, the states of largest allowed lhave essentially no radial kinetic energy. Exercise 55 notes that the expectation value of the kinetic energy (including both rotational and radial) equals the magnitude of the total energy. Compare this magnitude with the rotational energy alone,L2/2mr2
,assuming that n is large. That lis as large as it can be, and thatrn2a0.

Calculate the electric dipole moment p and estimate the transition time for a hydrogen atom electron making an electric dipole transition from the

(n,l,m)=(3,2,0)to the (2,1,0) state.

Classically, an orbiting charged particle radiates electromagnetic energy, and for an electron in atomic dimensions, it would lead to collapse in considerably less than the wink of an eye.

(a) By equating the centripetal and Coulomb forces, show that for a classical charge -e of mass m held in a circular orbit by its attraction to a fixed charge +e, the following relationship holds

ω=er-3/24πε0m.

(b) Electromagnetism tells us that a charge whose acceleration is a radiates power P=e2a2/6ε0c3. Show that this can also be expressed in terms of the orbit radius as P=e696π2ε03m2c3r4. Then calculate the energy lost per orbit in terms of r by multiplying the power by the period T=2π/ωand using the formula from part (a) to eliminate .

(c) In such a classical orbit, the total mechanical energy is half the potential energy, or Eorbit=-e28πε0r. Calculate the change in energy per change in r : dEorbit/dr. From this and the energy lost per obit from part (b), determine the change in per orbit and evaluate it for a typical orbit radius of 10-10m. Would the electron's radius change much in a single orbit?

(d) Argue that dividing dEorbit/dr by P and multiplying by dr gives the time required to change r by dr . Then, sum these times for all radii from rinitial to a final radius of 0. Evaluate your result for rinitial=10-10m. (One limitation of this estimate is that the electron would eventually be moving relativistically).

A particular vibrating diatomic molecule may be treated as a simple harmonic oscillator. Show that a transition from that n=2state directly to n=0ground state cannot occur by electric dipole radiation.

Consider an electron in the ground state of a hydrogen atom. (a) Sketch plots of E and U(r) on the same axes (b) Show that, classically, an electron with this energy should not be able to get farther than 2a0from the proton. (c) What is the probability of the electron being found in the classically forbidden region?

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