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Modern Physics 342 References : 1.Modern Physics by Kenneth S. Krane., 2 nd Ed. John Wiley & Sons, Inc. 2.Concepts of Modern Physics by A. Beiser, 6 th.

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Presentation on theme: "Modern Physics 342 References : 1.Modern Physics by Kenneth S. Krane., 2 nd Ed. John Wiley & Sons, Inc. 2.Concepts of Modern Physics by A. Beiser, 6 th."— Presentation transcript:

1 Modern Physics 342 References : 1.Modern Physics by Kenneth S. Krane., 2 nd Ed. John Wiley & Sons, Inc. 2.Concepts of Modern Physics by A. Beiser, 6 th Ed. (2002), McGraw Hill Com. 3.Modern Physics for Scientists and Engineers by J. Taylor, C. Zafiratos and M. Dubson, 2 nd Ed, 2003. Chapters: 5 (Revision), 6 (6.4), 7, 8, 10, 11 and 12

2 Ch. 5 (Revision) Schrödinger Equation

3 Schrödinger Equation Requirements 1.Conservation of energy is necessary: Kinetic energy Potential energy Total energy

4 The kinetic energy K is conveniently given by Where P is the momentum = m v

5 Schrödinger Equation Requirements (continued) 2.Consistency with de Broglie hypothesis Where, λ and k are, respectively, the wavelength and the wave number.

6 Schrödinger Equation Requirements (continued) 3.Validity of the equation The solution of this equation must be valid everywhere, single valued and linear. By linear we meant that the equation must allow de Broglie waves to superimpose properly. The following is a mathematical form of the wave associating the particle.

7 To make sure that the solution is continuous, its derivative must have a value everywhere.

8 Time-Independent Schrödinger Equation

9 Probability, Normalization and Average The probability density is given by Which is the probability of finding a particle in the space dx. The probability of finding this particle in a region between x 1 and x 2 is

10 By normalization we mean the total probability allover the space is 1, so that,

11 The mean value ( the expectation value) of x, If the wave function is normalized, therefore,

12 Applications The Free Particle ( a particle is moving with no forces acting on it ) U(x)= constant anywhere=0 (arbitrarily) The solution of such deferential equation is given in the form Ψ(x)=A sin(kx)+B cos(kx) (8)

13 Particle in a one dimensional box Finding A Ψ(0)=A sin(kx) + B cos(kx)=0 and for this, B=0 Therefore, ψ(x)=A sin(kx)(9)

14 Ψ(L)=0, therefore A sin(kL)=0 since A≠0, sin(kL)=0 kL=  n  Normalization condition (10)

15 The wave function is now given by, The energy is given by using (8) and (10) together, (11) (12)

16 The ground state (lowest ) energy E O is given by We used n=1 The allowed energies for this particle are

17 The wave function is shown here for n=1 and n=2 Ψ(x) x n=1 n=2

18 Example 5.2 P149 An electron is trapped in a one-dimensional region of length 1X10 -10 m. How much energy must be supplied to excite the electron from the ground state to the first excited state? In the ground state, what is the probability of finding the electron in the region from 0.09 X 10 -10 m to 0.11 X 10 -10 m? In the first excited state, what is the probability of finding the electron between x=0 and x=0.25 X 10 -10 m?

19 Example 5.3 P151 Show that the average value of x is L/2, for a particle in a box of length L, independent of the quantum state (not quantized). Since the wave function is And the average value is defined by

20 A particle in a two dimensional box The Schrödinger equation in two dimensions is U(x,y)=0 inside the box (0≤x≤L) & (0≤y≤L) U(x,y)=∞ outside the box

21 The wave function ψ(x,y) is written as a product of two functions in x and y, Since ψ(x,y) must be zero at the boundaries, ψ(0,y) =0ψ(L,y) =0ψ(x,0) =0ψ(x,L) =0

22 Therefore, A sin k x (0)+ B cos k x (0)=0 which requires B=0 In the same way For x=L, f(x)=0 and y=L, g(y)=0 This requires k x L=n x  with n=1,2,3 and

23 To find the constant A’, the wave function should be normalized This integration gives

24 The energy states of a particle in a two dimensional box Substituting about the wave function ψ(x,y) in Schrödinger equation, we find Which after simplification becomes

25 Chapter 7 The Hydrogen Atom Wave Functions The Schrödinger Equation in Spherical Coordinates The Schrödinger equation in three dimensions is The potential energy for the force between the nucleus and the electron is This form does not allow to separate wave function Ψ into functions in terms of x, y and z, so we have to express the whole equation of Schrödinger in terms of spherical coordinates, r, θ, and φ.

26 Cartesian and spherical coordinates θ φ r x y z electron r sin θ r sin θ cos φ r cos θ r sin θ sin φ

27 x= r sin θ cos φ y= r sin θ sin φ z= r cos θ And Schrödinger equation becomes This wave function can be written in terms of 3 functions in their corresponding variables, r, θ and φ

28 Hydrogen wave functions in spherical coordinates R(r) is called radial function Θ(θ ) is called polar function and Φ (φ) is called azimuthal function when solving the three differential equations in R(r), Θ(θ ) and Φ (φ), l and m l quantum numbers were obtained in addition to the previous principal quantum number n obtained before.

29 n 1 2 2 2 n the principal quantum number 1, 2, 3, … l angular momentum quantum number 0, 1, 2, ……±(n-1) m l magnetic quantum number0, ±1, ±2, ……± l

30 The energy levels of the hydrogen atom The allowed values of the radius r around the nucleus are given by Bohr radius (r at n=1) is denoted by a O and is given by

31 The Radial Probability Density P(r) The radial probability density of finding the electron at a given location is determined by The total probability of finding the electron anywhere around the nucleus is The limits of the integration depend on the conditions of the problem

32 Example 7.1 Prove that the most likely distance from the origin of an electron in the n=2, l= 1 state is 4a O. At n=2 and l =1, R 2,1 (r) is given by The most likely distance means the most probable position. The maximum value of the probability is obtained if r=4a O. To prove that, the first derivative of P(r) with respect to r is zero at this value.

33 Simplifying this result we get

34 Example 7.2 An electron in the n=1, l= 0 state. What is the probability of finding the electron closer to the nucleus than the Bohr radius a O ? The probability is given by 32.3 % of the time the electron is closer than 1 Bohr radius to the nucleus.

35 Angular Momentum We discussed the radial part R(r) of Schrodinger equation. In this section we will discuss the angular parts of the Schrodinger equation. The classical angular momentum vector is given by During the variables separation of wave functions in Schrodinger equation, angular momentum quantum number l was produced. The length of the angular momentum vector L is given by The z-components of L are given by where m l is the magnetic quantum number 0, ± l

36 The angular momentum vector components For l =2, m l = 0, ±1, ±2 The angle  is given by

37 Intrinsic Spin Angular momentum vector Magnetic moment due to electric current i Using q=-e the charge of the electron, and rp= L, we get The negative singe indicates that µ L and L work in opposite directions.

38 When the angular momentum vector L is inclined to the direction of the z-axis, the magnetic moment µ L has a z-component given by Remember, m l =0, ± l

39 An electric dipole in a uniform and non-uniform electric field A magnetic dipole in a non-uniform magnetic field The electric dipole has its moment p rotates to align with the direction of the electric field

40 Two opposite dipoles in the same non-uniform electric field are affected by opposite net forces that lead to displacing each dipole up and down according to their respective alignments.

41 Similarly, the magnetic dipoles are affected in the same way. When an electron with an angular momentum inclined to the magnetic filed, it may move up or down according to the direction of rotation around the nucleus.

42 A beam of hydrogen atoms is in the n=2, l = 1 state. The beam contains equal numbers of atoms in the m l = -1, 0, and +1 states. When the beam passes a region of non-uniform magnetic field, the atoms with m l =+1 experience a net upward force and are deflected upward, the atoms with m l =-1 are deflected downward, while the atoms with m l =0 are undeflected. Stern-Gerlach Experiment

43 After passing through the field, the beam strikes a screen where it makes a visible image. 1.When the filed is off, we expect to see one image of the slit in the center of the screen 2.When the field is on, three images of the slit on the screen were expected – one in the center, one above the center (m l =+1 ) and one below (m l =-1). The number of images is the number of m l values = 2 l +1= 3 in our example. In the Stern - Gerlach experiment, a beam, of silver atoms is used instead of hydrogen. While the field is off, and instead of observing a single image of the slit, they observed two separate images. A new quantum number is introduced, which is specifies the electron, the spin quantum number s. It may have two values ±½. The magnitude of its vector is given by Its z component to the magnetic field direction is

44 The experiment

45 Example 7.6 In a Stern – Gerlach type of experiment, the magnetic field varies with distance in the z direction according to The silver atoms travel a distance x=3.5 cm through the magnet. The most probable speed of the atoms emerging from the oven is v=750 m/s. Find the separation of the two beams as they leave the magnet. The mass of a silver atom is 1.8 X 10 -25 kg, and its magnetic moment is about 1 Bohr magneton.

46 3.5 cm v O =750 m/s. The force applied to the beam must be obtained

47 The force is the change of potential energy U with distance z. The potential energy U is given by This is the vertical force due to the effect of the magnetic field on the electron magnetic dipoles. Using the law of motion at constant acceleration,  z=v O t + ½ a t 2. The initial vertical speed was zero before the effect of the magnetic field. We can find the vertical deflection  z above the horizontal level of the beam.  z= ½ a t 2 =7.5X10 -6 m, the beam separation is 2(7.5X10 -5 m)=1.6X10 -4 m

48 Energy Levels and Spectroscopic Notation The notation for the quantum state of an electron is now described by the four quantum numbers n, l, m l and m s. For example, the ground state of the hydrogen is labeled as (n, l,m l,m s )=(1,0,0,±½) which means the are two quantum states that can be occupied by the electron; (1,0,0,+½) or (1,0,0,-½). Degeneracy of the atomic levels The ground state energy level is now degenerated into two quantum states. The 1 st excited state of the hydrogen atom has (n, l,m l,m s )= (2,1,1,+½), (2,1,1,-½), (2,1,0,+½), (2,1,0,-½), (2,1,-1,+½), (2,1,-1,-½), (2,0,0,+½), (2,0,0,-½). The degeneracy is 8, or 2n 2, where n is the principal quantum number.

49 Some degenerate states after spin quantum number n=1,2,.. l =0,1,2,..,n-1m l =0,± l m s =±½Degeneracy 2n 2 100 +½ 2 -½ 2 00 +½ 8 -½ 1 1 +½ -½ 0 +½ -½ +½ -½

50 Spectroscopic Notation Magnetic quantum numbers, m l and m s have no necessity to be mentioned unless a magnetic field is applied to the atom. In normal cases, a certain notation is used to specify the energy levels of the electron in the atom. Also, it is important to specify the number of electrons occupying such state. This notation depends on the l values as follows: Value of l 012345 notationspdfgh For the electron in the n=1 level, it is in the state s and the level occupied by this electron is denoted as (1s 1 )or generally (ns 1 )

51 Electronic configuration of some elements element Number of electrons n 123 l 001012 H11s 1 He21s 2 Li31s 2 2s 1 Be41s 2 2s 2 B51s 2 2s 2 2p 1 Ne61s 2 2s 2 2p 2 Na111s 2 2s 2 2p 6 3s 1 K181s 2 2s 2 2p 6 3s 2 3p 6

52 Selection rules Transitions between energy states of the atom are governed by the condition of  l =±1. The transition from 4s state is possible to the 3p state because  l =+1, but not possible between 4s and 3s, 2s or 1s. In addition to this condition, there is a rule against m l differences (  m l ).

53 n 4 3 2 1 l 0123 spdf

54 Zeeman Effect A hydrogen atom is prepared in a 2p ( l =1) level, and is placed in an external uniform magnetic field B. The orbital angular momentum magnetic moment  L interacts with the field and the potential energy of this interaction U is given by In addition to this, there is the energy of this level, E O, for example. So on turning the magnetic field on, the energy of this electron is given by Since m l in this example has the values +1, 0, and -1, there will be 3 energy values, 3 different wave lengths emitted.

55 Wavelength notation +10 0 0

56 Problem 22 p 233 A hydrogen atom is in an excited 5g state, from which it makes a series of transitions, ending in the 1s state. Show on an energy levels diagram the sequence of transitions that can occur. Repeat the last steps if the atom begins in the 5d state. 1s 2s 3s 5g5f5p5d5s 4f4d4s4p 3p3d 2p

57 1s 2s 3s 5g5f5p5d5s 4f4d4s4p 3p3d 2p

58 Problem 23 p 233 Consider the normal Zeeman effect applied to 3d to 2p transition. (a) sketch an energy-level diagram that shows the splitting of the 3d and 2p levels in an external magnetic field. Indicate all possible transitions from each m l state of the 3d level to each m l state of the 2p level. (b) which transitions satisfy the  m l =±1 or 0 selection rule? (c) Show that there are only three different transitions energies emitted. 3d 2p mlml +2 +1 0 -2 0 +1

59 Since there are three different values of  m l namely +1, 0 and -1, there will be three different energies emitted. Let the energy of the 2p state at m l =0 be denoted by E op and that of the 3d state at m l =0 be denoted by E od. The following equation can be used to calculate any energy released from allowed transitions. The difference E od –E op is constant, while  m l has 3 different values, therefore,  E has only three different values.

60 Many Electron Atoms Pauli Exclusion Principle It was believed that different atoms in the ground states have all their electrons dropped down in the 1s state. This means they all must have the same physical properties. This is not the case, in fact. A conclusion was drawn by Pauli that states that: No two electrons in a single atom can have the same set of quantum numbers (n, l, m l, m s ).



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