Lecture 29B - UCSD Department of Physics
Transcription
Lecture 29B - UCSD Department of Physics
Physics 1C Lecture 29B "Nuclear powered vacuum cleaners will probably be a reality within 10 years. " --Alex Lewyt, 1955 http://chemwiki.ucdavis.edu/Textbook_Maps/Physical_Chemistry_Textbo ok_Maps/Blinder's_%22Quantum_Chemistry%22 CAPE Evaluations Extra credit problem if high participation rate (>75 %) Important for future course Important for my assignments Outline Last time – hydrogen atom atomic spectra quantized orbitals and energy levels This time - Bohr’s model continued principal and other quantum numbers periodic table EPR and MRI nuclear stability Problems with Bohr’s Model Bohr’s explanation of atomic spectra includes some features of the currently accepted theory. Bohr’s model includes both classical and nonclassical ideas. He applied Planck’s ideas of quantized energy levels to orbiting electrons and Einstein’s concept of the photon to determine frequencies of transitions. What would happen if atoms could be excited to same higher energy level and then emission could be induced? Laser An acronym for Light Amplification by Stimulated Emission of Radiation. A laser is a light source that produces a focused, collimated, monochromatic beam of light. The laser operates using the principle of stimulated emission of light. In 1917, Albert Einstein established the theoretic foundations for the laser. Problems with Bohr’s Model Discrete orbitals and energies come from solving the Schrödinger equation (wave equation) Another fundamental property of motion is angular momentum, from Bohr description angular momentum always value (not true in quantum mechanics) Improved spectroscopic techniques, however, showed that many of the single spectral lines were actually groups of closely spaced lines. Single spectral lines could be split into three closely spaced lines when the atom was placed in a magnetic field. Quantum Numbers n is considered the principal quantum number. n can range from 1 to infinity in integer steps. But other quantum numbers were added later on to explain other subatomic effects (such as elliptical orbits; Arnold Sommerfeld (1868-1951)) and the idea of 3D orbitals. The orbital quantum number, ℓ, was then introduced. ℓ can range from 0 to n-1 in integer steps. Historically, all states with the same principal quantum number n are said to form a shell. Shells are identified by letters: K, L, M, … All states with given values of n and ℓ are said to form a subshell. Subshells: s, p, d, f, g, h, … Quantum Numbers Largest angular momentum will be associated with: ℓ =n–1 ℓ = 0 corresponds to spherical symmetry with no axis of rotation. This corresponds to a circular orbit. spherical orbits associated with each value of n Describes shape Quantum Numbers Because angular momentum is a vector, its direction also must be specified. Suppose a weak magnetic field is applied to an atom and its direction coincides with z axis. Then direction of the angular momentum vector relative to the z axis is quantized! Lz = mℓ ħ Note that L cannot be aligned with the z axis. space quantization Quantum Numbers States with quantum numbers that violate the rules below cannot exist. They would not satisfy the boundary conditions on the wave function of the system. Quantum Numbers In addition, it becomes convenient to think of the electron as spinning as it orbits the nucleus. There are two directions for this spin (up and down). Another quantum number accounts for this, it is called the spin magnetic quantum number, ms. Spin up, ms = 1/2 Spin down, ms = –1/2. Pauli Exclusion Principle Wolgang Pauli proposed that the four quantum numbers identify the electron No two electrons in an atom can be in the same quantum state No two electrons can have the same set of quantum numbers This prevents all atoms from having all electrons in the ground state Explained the order of the periodic table. Periodic Table The atoms position reflects the n and l values of the last electron, the chemical electron. In a single column, the elements’ last electrons differ by the principle quantum number n, but have the same l values. Wave Functions for Hydrogen The simplest wave function for hydrogen is the one that describes the 1s state: 1s (r ) 1 a 3 o e r ao All s states are spherically symmetric. The probability density for the 1s state is: 1s 2 1 2r ao 3 e a o Wave Functions for Hydrogen The radial probability density for the 1s state: 4r 2r ao P1s (r ) 3 e ao 2 The peak at the Bohr radius indicates the most probable location. The atom has no sharply defined boundary. The electron charge is extended through an electron cloud. Wave Functions for Hydrogen The electron cloud model is quite different from the Bohr model. The electron cloud structure does not change with time and remains the same on average. The atom does not radiate when it is in one particular quantum state. This removes the problem of the Rutherford atom. Radiative transition causes the structure to change in time. Wave Functions for Hydrogen The next simplest wave function for hydrogen is for the 2s state n = 2; ℓ = 0. This radial probability density for the 2s state has two peaks. In this case, the most probable value is r 5a0. The figure compares 1s and 2s states. 3 1 2 r r 2ao 2s ( r ) 2 e ao 4 2 ao 1 Clicker Question 29B-2 Which of the following hydrogen atom series can emit a photon with a wavelength in the infrared part of the spectrum? A) Lyman B) Balmer C) Paschen D) All of the above series can emit a photon with a wavelength in the infrared region Problem • If a photon with energy 1.40 eV were absorbed by a hydrogen atom. What is the minimum n that can be ionized by the photon? • ANSWER: • Related to energy difference between energy in initial orbital and that upon ionization • Free electron is unbound so has energy = 0 • Thus, look for orbital that has its magnitude of energy closest to that of the photon (1.40 eV) Problem 2 1 e 13.6 eV E tot ke 2 2 2 n ao n • Use • and solve for n. • n2 = 13.6/1.40 = 9.71 => n = 3.12 • So does n = 3 work? • For n = 3, ionization requires 1.51 eV • Energy is not sufficient. Can we ionize n = 2? • Thus, we can ionize n = 4 or electrons with higher values of n Electron Paramagnetic Resonance Apply magnetic field to remove energy degeneracy of spin up and spin down electrons When “splitting” matches photon energy, get absorption Seen as a signal Such radicals are relatively rare in nature (Block & Purcell, 1952 Nobel Prize) Nuclear Magnetic Resonance Imaging Nuclei also have quantum numbers Detect nuclear magnetic moments similar to NMR Nuclear Magnetic Resonance Imaging magnetic moments of some of these protons change and align with the direction of the field radio frequency transmitter is briefly turned on, producing a further varying electromagnetic field photons of this field have just the right energy, known as the resonance frequency, to be absorbed and flip the spin of the aligned protons Nuclear Magnetic Resonance Angiography generates pictures of the arteries administration of a paramagnetic contrast agent (gadolinium) or using a technique known as "flow-related enhancement" For Next Time (FNT) Read Chapter 30 through page 1032 Chapter 30 homework due Wednesday