Physics 102: Lecture 24. Heisenberg Uncertainty Principle & Bohr Model of Atom. Physics 102: Lecture 24, Slide 1

Transcription

1 Physics 10: Lecture 4 Heisenberg Uncertainty Principle & Bohr Model of Atom Physics 10: Lecture 4, Slide 1

2 Heisenberg Uncertainty Principle Recall: Quantum Mechanics tells us outcomes of individual measurements are uncertain Δ p Δ h y y Uncertainty in momentum (along y) Uncertainty in position (along y) Rough idea: if we know momentum very precisely, we lose knowledge of location, and vice versa. This uncertainty is fundamental: a it arises because quantum particles behave like waves! Physics 10: Lecture 4, Slide

3 Electron diffraction Electron beam traveling through h slit will diffract w electron beam y θ x λ psinθ sin θ screen Single slit diffraction pattern Number of electrons arriving at screen Recall single-slit diffraction 1 st minimum: sinθ = λ/w w = λ/sinθ = Δy Δp y Δy = Physics 10: Lecture 4, Slide 3 = λ p h θ Δp y = p sinθ = Using de Broglie λ = h/p

4 p y Number of electrons arriving at screen w electron beam y y Δp w= h x screen Electron entered slit with momentum along x direction and no momentum in the y direction. When it is diffracted it acquires a p y which can be as big as h/w. The Uncertainty in p y is Δp y h/w. An electron passed through the slit somewhere along the y direction. The Uncertainty in y is Δy w. Physics 10: Lecture 4, Slide 4 Δp Δy h y

5 p y Number of electrons arriving at screen electron beam w y Δp Δ y h y x screen If we make the slit narrower (decrease w =Δy) the diffraction peak gets broader (Δp y increases). If we know location very precisely, we lose knowledge of momentum, and vice versa. Physics 10: Lecture 4, Slide 5

6 to be precise... Δ p y y Δ h Of course if we try to locate the position of the particle along the x axis to Δx we will not know its x component of momentum better than Δp x, where Δ p h xδx and the same for z. Checkpoint 1 According to the H.U.P., if we know the x-position of a particle, we cannot know its: (1) y-position () x-momentum (3) y-momentum (4) Energy Physics 10: Lecture 4, Slide 6

7 Atoms Evidence for the nuclear atom Today Bohr model of the atom Spectroscopy of atoms Next lecture Quantum atom Physics 10: Lecture 4, Slide 7

8 Plum Pudding Early Model for Atom negative charges (electrons) in uniformly distributed cloud of positive charge like plums in pudding But how can you look inside an atom m across? Physics 10: Lecture 4, Slide 8 Light (visible) λ = 10-7 m Electron (1 ev) λ = 10-9 m Helium atom λ = m

9 Rutherford Scattering 1911: Scattering He ++ (an alpha particle ) atoms off of gold. Mostly go through, some scattered back! + + Plum pudding theory: + - electrons in cloud of - + uniformly distributed ib t d + charge - - electric field felt by alpha never gets too large To scatter at large angles, need positive charge concentrated in small + region (the nucleus) Atom is mostly empty space with a small (r = m) positively charged nucleus surrounded by cloud of electrons (r = m) Physics 10: Lecture 4, Slide 9

10 Nuclear Atom (Rutherford) Large angle scattering Nuclear atom Classic nuclear atom is not stable! Electrons orbit nucleus -> constant centripetal acceleration Accelerated charges radiate energy Electrons will radiate and spiral into nucleus! Physics 10: Lecture 4, Slide 10 Early quantum model: Bohr Need quantum theory

11 Bohr Model is Science fiction The Bohr model is complete nonsense. Electrons do not circle the nucleus in little planetlike orbits. The assumptions injected into the Bohr model have no basis in physical reality. BUT the model does get some of the numbers right for SIMPLE atoms Physics 10: Lecture 4, Slide 11

12 Hydrogen-Like Atoms single electron with charge -e nucleus with charge +Ze (Z protons) e = 1.6 x C Ex: H (Z=1), He (Z=), Li (Z=3), etc Physics 10: Lecture 4, Slide 1

13 The Bohr Model Electrons circle the nucleus in orbits Only certain orbits are allowed πr = nλ -e n=1 +Ze Physics 10: Lecture 4, Slide 13

14 The Bohr Model Electrons circle the nucleus in orbits Only certain orbits are allowed πr = nλ = nh/p L = pr = nh/π = nħ Angular momentum is quantized -e +Ze n= Physics 10: Lecture 4, Slide 14 v is also quantized in the Bohr model!

15 An analogy: Particle in Hole Let s define energy so that a free particle has E = 0 Consider a particle trapped in a hole To free the particle, need to provide energy mgh Relative to the surface, energy =-mgh a particle that is just free has 0 energy E=0 E=-mgh h Physics 10: Lecture 4, Slide 15

16 An analogy: Particle in Hole Quantized Energy: only fixed discrete heights of particle allowed Lowest energy (deepest hole) state is called the ground state E=0 h Physics 10: Lecture 4, Slide 16 ground state

17 For Hydrogen-like atoms: Energy levels (relative to a just free E=0 electron): E n 4 mk e Z 13.6 Z = ev where / h n n ( h h π ) Radius of orbit: r n h 1 n n = = ( nm ) π mke Z Z Physics 10: Lecture 4, Slide 17

18 Checkpoint = ( h 1 n ) π mke Z = n (0.059nm) Z r n Bohr radius If the electron in the hydrogen atom was 07 times heavier (a muon), the Bohr radius would be 1) 07 Times Larger h 1 Bohr Radius = ( ) ) Same Size π mke 3) 07 Times Smaller Physics 10: Lecture 4, Slide 18 This m is electron mass!

19 ACT/Checkpoint 3 A single electron is orbiting around a nucleus with charge +3. What is its ground state (n=1) energy? (Recall for charge +1, E= ev) 1) E = 9(-136eV) /1 = 9 ) E = 3 (-13.6 ev) 3) E = 1 (-13.6 ev) Physics 10: Lecture 4, Slide 19 Z E n = 13. 6eV n Note: This is LOWER energy since negative!

20 ACT: What about the radius? Z=3, n=1 1. larger than H atom. same as H atom 3. smaller than H atom h n r 1 = ( ) = (0.059 nm n mke Z ) π n Z Physics 10: Lecture 4, Slide 0

21 Summary Bohr s Model gives accurate values for electron energy levels... But Quantum Mechanics is needed to describe electrons in atom. Next time: electrons jump between states by emitting or absorbing photons of the appropriate energy. Physics 10: Lecture 4, Slide 1

22 Some (more) numerology 1 ev = kinetic energy of an electron that has been accelerated through a potential difference of 1 V 1 ev = qδv = 1.6 x J h (Planck s constant) = 6.63 x J s hc = 140 ev nm m = mass of electron = 9.1 x kg mc = 511,000 ev U = ke /r, so ke has units ev nm (like hc) πke /(hc) = 1/137 (dimensionless) fine structure t constant t Physics 10: Lecture 4, Slide