Exam topics-- understand and be able to apply ideas like in
... 7. Quantization of energy in atoms, and how established experimentally. 8. Atomic spectra and connection with electron energy levels in atoms. 9. Atomic spectra as signature of atom. 10. Potential energy of electron in atom. 11. Atomic discharge lamps- how work and why so efficient at converting ele ...
... 7. Quantization of energy in atoms, and how established experimentally. 8. Atomic spectra and connection with electron energy levels in atoms. 9. Atomic spectra as signature of atom. 10. Potential energy of electron in atom. 11. Atomic discharge lamps- how work and why so efficient at converting ele ...
Chemistry 1000 Lecture 6: Quantum mechanics and spectroscopy
... move outside the positively charged nucleus. ...
... move outside the positively charged nucleus. ...
Document
... 1. Proved quantization of electron energies and is the basis for Quantum Theory a. Quantum theory describes mathematically the wave properties of electrons and other very small particles 2. Electrons do not move around the nucleus in "planetary orbits" 3. Electrons exist in regions called orbitals a ...
... 1. Proved quantization of electron energies and is the basis for Quantum Theory a. Quantum theory describes mathematically the wave properties of electrons and other very small particles 2. Electrons do not move around the nucleus in "planetary orbits" 3. Electrons exist in regions called orbitals a ...
Topic 1 Atomic Structure and Periodic Properties Atomic Structure
... The Radial Distribution Function • The radial part R(r) of a wavefunction ψ(r) is related to the probability [ψ(r)ψ(r)* or ψ2] of finding an electron at a specific point with distance r from the nucleus • The probability of finding an electron at a given distance r from the nucleus is described by t ...
... The Radial Distribution Function • The radial part R(r) of a wavefunction ψ(r) is related to the probability [ψ(r)ψ(r)* or ψ2] of finding an electron at a specific point with distance r from the nucleus • The probability of finding an electron at a given distance r from the nucleus is described by t ...
Transparancies for Atomic Structure Section
... Basics intro: Rutherford’s atom, blackbody radiation, photoelectric effect, wave particle duality, uncertainty principle, schrödingers equation, intro. to H atom. ...
... Basics intro: Rutherford’s atom, blackbody radiation, photoelectric effect, wave particle duality, uncertainty principle, schrödingers equation, intro. to H atom. ...
Quantum Theory and Atomic Structure
... the exact position and momentum (velocity) of a particle can not be known simultaneously ∆x⋅∆p ≥ h/4π ∆x and ∆p = m∆u – uncertainty in position and momentum, respectively – A consequence of the wave-particle duality of matter – The exact location of very small particles is not well known due to thei ...
... the exact position and momentum (velocity) of a particle can not be known simultaneously ∆x⋅∆p ≥ h/4π ∆x and ∆p = m∆u – uncertainty in position and momentum, respectively – A consequence of the wave-particle duality of matter – The exact location of very small particles is not well known due to thei ...
3. atomic structure
... In this class we will be performing an experiment called the “Flame Test”. We will be heating up metal powders in order to excite the electrons to jump from a lower energy level to a higher energy level. When an electron returns from a higher energy state to a lower energy state, it emits a specific ...
... In this class we will be performing an experiment called the “Flame Test”. We will be heating up metal powders in order to excite the electrons to jump from a lower energy level to a higher energy level. When an electron returns from a higher energy state to a lower energy state, it emits a specific ...
uncertainty, atom
... charge, and accelerating charges give off EM radiation (like an antenna), thus giving off energy. The electron would gradually lose all its energy. That doesn’t happen -- atoms are stable. ...
... charge, and accelerating charges give off EM radiation (like an antenna), thus giving off energy. The electron would gradually lose all its energy. That doesn’t happen -- atoms are stable. ...
Notes on Electron Configurations
... • An orbital is described by a set of three quantum An orbital is described by a set of three quantum numbers. • Quantum numbers can be considered to be Quantum numbers can be considered to be “coordinates” (similar to x, y, and z coodrinates g p ) which are related to where an for a graph) elec ...
... • An orbital is described by a set of three quantum An orbital is described by a set of three quantum numbers. • Quantum numbers can be considered to be Quantum numbers can be considered to be “coordinates” (similar to x, y, and z coodrinates g p ) which are related to where an for a graph) elec ...
ENT145/3 Materials Engineering Tutorial 1 (Answer) 1. Why is it
... (b) Two important quantum-mechanical concepts associated with the Bohr model of the atom are (1) that electrons are particles moving in discrete orbitals, and (2) electron energy is quantized into shells. (c) Two important refinements resulting from the wave-mechanical atomic model are (1) that ele ...
... (b) Two important quantum-mechanical concepts associated with the Bohr model of the atom are (1) that electrons are particles moving in discrete orbitals, and (2) electron energy is quantized into shells. (c) Two important refinements resulting from the wave-mechanical atomic model are (1) that ele ...
De Broglie waves
... • The Bragg equation for maxima in the diffraction pattern is: n 2d sin • In a particular case, a beam of 54eV electrons were directed perpendicularly at the nickel target and a sharp maximum in the electron distribution occurred at an angle of 50o with the original beam. Here θ=650, d=0.091nm, ...
... • The Bragg equation for maxima in the diffraction pattern is: n 2d sin • In a particular case, a beam of 54eV electrons were directed perpendicularly at the nickel target and a sharp maximum in the electron distribution occurred at an angle of 50o with the original beam. Here θ=650, d=0.091nm, ...
Physics 107 Exam #3 October 13, 1994 Your name: Multiple Choice
... 3. Molecules of a dilute gas which are identical, distinguishable particles obey statistics. (a) Maxwell-Boltzmann, (b) Bose-Einstein, (c) Fermi-Dirac, (d) Rayleigh-Jeans. 4. We cannot think of the electron as orbiting the nucleus in any conventional sense because (a) the Pauli exclusion principle p ...
... 3. Molecules of a dilute gas which are identical, distinguishable particles obey statistics. (a) Maxwell-Boltzmann, (b) Bose-Einstein, (c) Fermi-Dirac, (d) Rayleigh-Jeans. 4. We cannot think of the electron as orbiting the nucleus in any conventional sense because (a) the Pauli exclusion principle p ...
Covalent Bonds
... in the model (except Hydrogen). i. Electronegativity increases left to right and bottom to top. b. The central atom is often the 1st atom in the formula. c. Carbon is ALWAYS central. d. Hydrogen/halogens are always terminal (on end). ...
... in the model (except Hydrogen). i. Electronegativity increases left to right and bottom to top. b. The central atom is often the 1st atom in the formula. c. Carbon is ALWAYS central. d. Hydrogen/halogens are always terminal (on end). ...
Slide 1
... The attractive Coulomb force between the positive nucleus and the orbiting electron could provide the attractive force which keeps the electron in it’s orbit, much as the planets orbit the sun with gravity providing the centripetal force. ...
... The attractive Coulomb force between the positive nucleus and the orbiting electron could provide the attractive force which keeps the electron in it’s orbit, much as the planets orbit the sun with gravity providing the centripetal force. ...
PS#4
... 3. Use the Slater determinant to arrive at a wave function to describe the ground state of a two-electron system such as He. Express the resulting wave function in terms of the 1s spatial wave function for each electron [ 1s 1 and 1s 2 ], and of the spin wave functions for each electron 1, ...
... 3. Use the Slater determinant to arrive at a wave function to describe the ground state of a two-electron system such as He. Express the resulting wave function in terms of the 1s spatial wave function for each electron [ 1s 1 and 1s 2 ], and of the spin wave functions for each electron 1, ...
CHAPTER 4: Structure of the Atom
... The Rydberg constant for infinite nuclear mass is replaced by R. ...
... The Rydberg constant for infinite nuclear mass is replaced by R. ...
Atomic orbital
An atomic orbital is a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom. This function can be used to calculate the probability of finding any electron of an atom in any specific region around the atom's nucleus. The term may also refer to the physical region or space where the electron can be calculated to be present, as defined by the particular mathematical form of the orbital.Each orbital in an atom is characterized by a unique set of values of the three quantum numbers n, ℓ, and m, which respectively correspond to the electron's energy, angular momentum, and an angular momentum vector component (the magnetic quantum number). Any orbital can be occupied by a maximum of two electrons, each with its own spin quantum number. The simple names s orbital, p orbital, d orbital and f orbital refer to orbitals with angular momentum quantum number ℓ = 0, 1, 2 and 3 respectively. These names, together with the value of n, are used to describe the electron configurations of atoms. They are derived from the description by early spectroscopists of certain series of alkali metal spectroscopic lines as sharp, principal, diffuse, and fundamental. Orbitals for ℓ > 3 continue alphabetically, omitting j (g, h, i, k, …).Atomic orbitals are the basic building blocks of the atomic orbital model (alternatively known as the electron cloud or wave mechanics model), a modern framework for visualizing the submicroscopic behavior of electrons in matter. In this model the electron cloud of a multi-electron atom may be seen as being built up (in approximation) in an electron configuration that is a product of simpler hydrogen-like atomic orbitals. The repeating periodicity of the blocks of 2, 6, 10, and 14 elements within sections of the periodic table arises naturally from the total number of electrons that occupy a complete set of s, p, d and f atomic orbitals, respectively.