Physics 1202: Lecture 37 Today’s Agenda

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Presentation transcript:

Physics 1202: Lecture 37 Today’s Agenda Announcements: Extra credits Final-like problems Team in class Teams 8, 9 & 10 HW 10 due this sFriday Atomic Physics: finally ! 1

Atomic Physics

Pauli exclusion principle Wolfgang Pauli (1925): Nobel 1945 No electron can be in the same quantum state No more than 2 electrons in an orbital For a given n, l, m with ms = ± ½ Explains the periodic table Electronic configuration Shell structure of atoms

Periodic table Atomic structure and chemical properties Pauli principle: atomic shell model

X-ray emission from atoms X-ray tube Discovered by Wilheim Röntgen (1895) Accelerated electrons hit targets Large potentials kV to MV

X-ray emission from atoms Bremsstrahlung Continuous x-ray Electron loosing energy Minimal l When all initial K is lost

X-ray emission from atoms K, L, etc. shells and x-ray emission Fast electron kick inner electron out Higher electron falls in and fill the “hole” X-ray emitted

X-ray emission from atoms Each element has a specific spectra lmin

Nuclear Physics

The nucleus Ernest Rutherford (1909-1910) Discovered the nucleus (Nobel 1908 Chem.) Using alpha particles on gold film Large deflection: tiny but massive positive nucleus

The neutron Why mass & charge do not “fit” mHe ~ 4 mH but only qHe = 2 qH (ion) Rutherford in 1920 speculated Neutral particle with about mass of proton must exist James Chadwick (Nobel 1935) Discovered the neutron (1932) Neutral particles (mass about 0.14% larger than p) Not photon (pass through matter), but massive:kick proton

The nucleus Made of Size and shape A Z protons N neutrons Mass number A = Z + N A Z Size and shape Almost spherical Not always though 1.2 X 10-15 m =1.2 fm

The strong nuclear force A force must exist to compensate electric repulsion Nuclear force Always attractive The same between protons or neutrons 100 times stronger than electrostatic force Short-range: about only 3 fm

The strong nuclear force Neutron are essential Provide the “glue” to maintain protons together Meed more n as A grows

Binding energy “missing” mass = negative or binding energy The mass of an atom is less than its constituents 12C (m=12 u): used to defined the atomic mass unit u 6 protons + 6 neutrons + 6 electrons Adding = 12.09893 u “missing” mass = negative or binding energy E = mc2