Quantum Chemistry Dr Ron Rusay Atomic Structure and
- Slides: 81
Quantum Chemistry Dr. Ron Rusay
Atomic Structure and Periodicity ð ð ð ð Electromagnetic Radiation (LIGHT) The Nature of Matter The Atomic Spectrum of Hydrogen The Bohr Model The Quantum Mechanical Model of the Atom Quantum Numbers Orbital Shapes and Energies Electron Spin and the Pauli Principle Polyelectronic Atoms The History of the Periodic Table The Aufbau Principles and the Periodic Table Periodic Trends in Atomic Properties The Properties of a Group: The Alkali Metals
Quantum Theory Based on experimental observations of light and particles ð Development progressed through rigorous mathematical computations ð It bridges physics and chemistry ð It is described generally as quantum mechanics ð
Electromagnetic Radiation (“Light”) Energy that exhibits wave-like behavior. ð In a vacuum, electromagnetic energy travels through space at the speed of light. ð It is described by the Electromagnetic Spectrum. ð
Nature of EM Energy
Demonstrating Light’s Wave Nature
Frequency & Wave length
Waves http: //chemistry. beloit. edu/Blue. Light/waves/index. html ð Waves have 4 primary characteristics: ð 1. Wavelength: distance between two peaks in a wave. ð 2. Frequency: number of waves per second that pass a given point in space. ð 3. Amplitude: the height of the wave. Speed: speed of light is 2. 9979 108 m/s. ð 4.
Waves http: //chemistry. beloit. edu/Blue. Light/waves/index. html Focus on 2 of the primary characteristics: ð 1. Wavelength: distance between two peaks in a wave. ð ð 2. Frequency: number of waves per second that pass a given point in space. ð 3. Amplitude: the height of the wave. ð 4. Speed: speed of light is 2. 9979 108 m/s.
Wavelength and frequency = c / ð = frequency (s 1) ð = wavelength (m) ð c = speed of light (m s 1)
QUESTION
ANSWER 5 – 1 B) 4. 12 ´ 10 s The smaller the frequency of light, the longer the wavelength.
Planck’s Constant Transfer of energy is quantized, and can only occur in discrete units, called quanta. ð E = change in energy, in J ð h = Planck’s constant, 6. 626 10 34 J s ð = frequency, in s 1 ð = wavelength, in m ð c = speed of light
Planck’s Equation (Interactive) http: //chemconnections. org/general/chem 120/Flash/plancks_equation_s. html
Electromagnetic Energy ðEM Spectrum : Chem Connections http: //chemistry. beloit. edu/Stars/EMSpectrum/index. html
Energy and Mass ð Energy has mass ðE ðE = energy ð m = mass ð c = speed of light = 2 mc
Energy and Mass ”Duality” (Hence the dual nature of light. )
Wavelength and Mass de Broglie’s Equation ð = wavelength, in m ð h = Planck’s constant, 6. 626 10 34. s ð ð = kg m 2 s 1 m = mass, in kg = frequency, in s 1 J
Atomic Spectrum of Hydrogen http: //chemistry. beloit. edu/Blue. Light/pages/color. html Continuous spectrum: Contains all the wavelengths of light. ð Absorbtion vs. Emission ð ð http: //chemistry. beloit. edu/Blue. Light/pages/elements. html ð Line (discrete) spectrum: Contains only some of the wavelengths of light.
http: //chemconnections. org/general/chem 120/Flash/atomic_absorption_s. html
Emissions: Flame Tests
Electromagnetic Energy ðVisible Light / Color : Chem. Connections ðhttp: //chemistry. beloit. edu/Stars/applets/emission/index. html ðThe Perception of Colors ðhttp: //chemconnections. org/organicchem 227/227 assign-06. html#vision
Atomic Emission Spectrum of H 2
The Bohr Model “The electron in a hydrogen atom moves around the nucleus only in certain allowed circular orbits. ” X E = energy of the levels in the H-atom ð z = nuclear charge (for H, z = 1) ð n = an integer ð
The Bohr Model Ground State: The lowest possible energy state for an atom (n = 1). ð
Energy Changes in the Hydrogen Atom ð E = Efinal state Einitial state
Heisenberg Uncertainty Principle ð The more accurately we know a particle’s position, the less accurately we can know its momentum or vice versa. Quantum Entanglement/Superposition Schrödinger’s Cat: Alive or Dead? Can something be in two places at the same time? In quantum microstates, YES. Science, 272, 1132 (1996)
Quantum Numbers (QN) for Electrons (Solutions for the Schrödinger Equation: = ) Where: = Wave function ð 1. Principal QN ( integer n = 1, 2, 3, . . . ) : relates to size and energy of the orbital. ð 2. Angular Momentum QN ( integer l or )= 0 to n 1) : relates to shape of the orbital. ð 3. Magnetic QN (integer m l or m = + l to l) : relates to orientation of the orbital in space relative to other orbitals. ð 4. Electron Spin QN : (ms = +1/2, 1/2) : relates to the spin state of the electron.
“ORBITAL”: Electron Probability = | |2 = (double integral of wave function )
Periodic Table Classifications Electron Configurations & Quantum Numbers Representative Elements (A Groups): s (l=0) and p (l=1) (N, C, Al, Ne, F, O) ð Transition Elements: d (l=2) orbitals (Fe, Co, Ni, etc. ) ð Lanthanide and Actinide Series (inner transition elements): f (l=3) orbitals (Eu, Am, Es) ð
Valence Electrons Valence electrons are the outermost electrons in the highest principal quantum level of an atom. They are found in the s- and p- orbitals and are the bonding electrons. Inner electrons are called core electrons.
QUESTION
ANSWER B) 4 Orbitals are designated by ml. For n = 2, ml has four values.
QUESTION
ANSWER A) 0 For n = 3, l can be 0, 1, or 2. An f orbital has an l = 3.
Quantum Numbers : l, ml Orbital Shape & Orientation
Magnetic Spin ms
Electron Probability = | |2 = (double integral of wave function )
Atomic Orbitals ð See the following Web page: http: //chemconnections. org/general/chem 120/atomic-orbitals/orbitals. html Identify the unknown orbitals by comparing their shapes to the known orbitals and assign quantum numbers to each orbital.
Multi-electron Atoms Electron Configuration
Aufbau Principle ð As protons are added one by one to the nucleus to build up the elements, electrons are similarly added to these hydrogen-like orbitals.
Full electron configuration (Spectroscopic notation) --->
QUESTION
ANSWER 2 B) [Xe] 6 s [Xe] denotes a shorthand version of the electron configuration for Xe. Noble-gas configurations are used to reduce writing time.
Pauli Exclusion Principle In a given atom, no two electrons can have the same set of four quantum numbers ( n, l, ml , ms ). ð Therefore, an orbital can hold only two electrons, and they must have opposite spins. ð
QUESTION
ANSWER C) 14 For l = 3, ml = – 3, – 2, – 1, 0, 1, 2, 3 and each of these orbitals can hold two electrons.
Hund’s Rule orbital diagrams ð The lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals. Orbital Diagram ->
Periodic Table Classifications Electron Configurations Representative Elements (A Groups): fill s and p orbitals (Na, Al, Ne, O) ð Transition Elements: fill d orbitals (Fe, Co, Ni) ð Lanthanide and Actinide Series (inner transition elements): fill 4 f and 5 f orbitals (Eu, Am, Es) ð
Valence Electrons Valence electrons are the outermost electrons in the highest principal quantum level of an atom. They are found in the s- and p- orbitals and are the bonding electrons. Inner electrons are called core electrons.
QUESTION
ANSWER E) none Atoms in the same group have the same number of valence electrons. None of the sets of atoms have members all from the same group.
QUESTION
ANSWER + 2+ B) K , Ca , Ar, S 2– All of the species in an isoelectronic series must have the same number of electrons with the same electron configurations.
Two ways of showing the formation of lithium fluoride: Li. F; [Li+ and F -] using electron configurations & diagrams
QUESTION
ANSWER E) – ¯ ¯ N ion has an extra electron that must be paired. It is isoelectronic with oxygen.
Paramagnetism & Diamagnetism Electron Configuration & Magnetic Properties • Diamagnetic materials have all electrons paired and are not attracted to a magnetic field. • Paramagnetic materials have unpaired electrons and the magnetic attraction (magnetism) is generally proportional to the number of unpaired electrons. (Note: not all metals follow this rule. )
Electron Diagrams Magnetic Properties #1 = H 2 O(l) # 2 = Fe 2 O 3(s) # 3 = Fe. O(s) #4= Fe(s)
Transition Metal Ions (B Groups) Oxidation Numbers (States)
Isoelectronic atoms and ions have the same electron configurations
Apparatus Used to Measure Paramagnetism NOTE: O 2 is paramagnetic, N 2 is not! Also, Ferromagnetic effects are much, much stronger than Paramagnetic
Electron Diagrams Magnetic Properties • Ground state configurations of nitrogen (N) and oxygen (O) have 3 and 2 unpaired electrons in their electron diagrams respectively, what can be going on in the video? • Ground state diagrams do work very well for the Transition metals but not many others because of bonding, which forms pairs of electrons. (molecular orbitals vs. atomic orbitals). Eg. water, nitrogen and oxygen.
Molecular Orbital Diagrams
Summary: Information from the Periodic Table 1. Can obtain Group A valence electron configurations ð 2. Can determine individual electron configurations. ð This information can be used to: a. Predict the physical properties and general chemical behavior of the elements. ð b. Identify metals and nonmetals. ð
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