Chemistry Comes Alive: Part A
... • Electrical energy—results from movement of charged particles • Mechanical energy—directly involved in moving matter • Radiant or electromagnetic energy—exhibits wavelike properties (i.e., visible light, ultraviolet light, and X-rays) Energy Form Conversions • Energy may be converted from one form ...
... • Electrical energy—results from movement of charged particles • Mechanical energy—directly involved in moving matter • Radiant or electromagnetic energy—exhibits wavelike properties (i.e., visible light, ultraviolet light, and X-rays) Energy Form Conversions • Energy may be converted from one form ...
Document
... Valence Bond Theory: A quantum mechanical model which shows how electron pairs are shared in a covalent bond. ◦ Bond forms between two atoms when the following conditions are met: ◦ Covalent bonds are formed by overlap of atomic orbitals, each of which contains one electron of opposite spin. ◦ Each ...
... Valence Bond Theory: A quantum mechanical model which shows how electron pairs are shared in a covalent bond. ◦ Bond forms between two atoms when the following conditions are met: ◦ Covalent bonds are formed by overlap of atomic orbitals, each of which contains one electron of opposite spin. ◦ Each ...
QM lecture - The Evergreen State College
... Spin - review • Hydrogen atom so far: 3D spherical solution to Schrödinger equation yields 3 new quantum numbers: l = orbital quantum number L l (l 1) ml = magnetic quantum number = 0, ±1, ±2, …, ±l ms = spin = ±1/2 • Next step toward refining the H-atom model: Spin with ...
... Spin - review • Hydrogen atom so far: 3D spherical solution to Schrödinger equation yields 3 new quantum numbers: l = orbital quantum number L l (l 1) ml = magnetic quantum number = 0, ±1, ±2, …, ±l ms = spin = ±1/2 • Next step toward refining the H-atom model: Spin with ...
Introduction to theoretical chemistry 2 semesters
... • What can we learn about the stability and properties of a material by analyzing its electronic orbitals? Such knowledge will allow more powerful prediction. What was known before? • Why is it necessary to consider quantum mechanics? Why does classical mechanics fail? • What is an electronic orbita ...
... • What can we learn about the stability and properties of a material by analyzing its electronic orbitals? Such knowledge will allow more powerful prediction. What was known before? • Why is it necessary to consider quantum mechanics? Why does classical mechanics fail? • What is an electronic orbita ...
Deconstructed HS-PS1-2
... Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.[Clarification Statement: Examples of chemical reactions could include the reaction of ...
... Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.[Clarification Statement: Examples of chemical reactions could include the reaction of ...
Slide 1
... which when operating upon the wavefunction associated with a definite value of that observable will yield that value times the wavefunction. 3. Any operator Q associated with a physically measurable property q will be Hermitian 4. The set of eigenfunctions of each Hermitian operator Q will form a co ...
... which when operating upon the wavefunction associated with a definite value of that observable will yield that value times the wavefunction. 3. Any operator Q associated with a physically measurable property q will be Hermitian 4. The set of eigenfunctions of each Hermitian operator Q will form a co ...
unit 102-10: quantum theory and the atom
... To understand the atomic spectra we studied in the first section of this Unit, we used the Bohr Model of the atom. Niels Bohr developed this semi-classical model of the atom which incorporated the work of Einstein and Planck. In particular, this model predicts that the energy states of electrons wit ...
... To understand the atomic spectra we studied in the first section of this Unit, we used the Bohr Model of the atom. Niels Bohr developed this semi-classical model of the atom which incorporated the work of Einstein and Planck. In particular, this model predicts that the energy states of electrons wit ...
Chemistry 521/421 Fall 2013 Atomic and Molecular Structure
... background is required, including but not limited to linear algebra, differential equations, and multi-dimensional calculus. All mathematical constructs and concepts will be defined, but students should have had prior exposure to the material. A list of such topics is given below. Prerequisite know ...
... background is required, including but not limited to linear algebra, differential equations, and multi-dimensional calculus. All mathematical constructs and concepts will be defined, but students should have had prior exposure to the material. A list of such topics is given below. Prerequisite know ...
Waves and Energy
... Recall that atomic emission spectrum is discontinuous; that is, it is made of only certain frequencies of light. Why are element's atomic emission spectra discontinuous rather than continuous? In 1913, Niels Bohr, a young Danish physicist proposed a quantum model for the hydrogen atom that seemed to ...
... Recall that atomic emission spectrum is discontinuous; that is, it is made of only certain frequencies of light. Why are element's atomic emission spectra discontinuous rather than continuous? In 1913, Niels Bohr, a young Danish physicist proposed a quantum model for the hydrogen atom that seemed to ...
“SUPERPOSITION” “interference term”
... In quantum mechanics, if state 1 → state 1’ and state 2 → 2’, then superposition of 1 and 2 → superposition of 1’ and 2’ . ...
... In quantum mechanics, if state 1 → state 1’ and state 2 → 2’, then superposition of 1 and 2 → superposition of 1’ and 2’ . ...
ppt
... ● The radius of an atom is about 100,000 times larger than the radius of the nucleus. ● Electrons are located around the nucleus in orbitals. ● Orbitals – not distinct like planetary orbits, but 3-D regions where electrons can probably be found (“electron clouds”). ● The position of the outermost el ...
... ● The radius of an atom is about 100,000 times larger than the radius of the nucleus. ● Electrons are located around the nucleus in orbitals. ● Orbitals – not distinct like planetary orbits, but 3-D regions where electrons can probably be found (“electron clouds”). ● The position of the outermost el ...
lect19-20
... reduces the repulsion and hence a lower energy solution results, ie. to take the electron from the state described by (y1+y2) and take it to infinite distance costs energy. It also follows that E+total < E-total The total energy is given by E+total = E+ + Up, where E+ is the energy of the electron i ...
... reduces the repulsion and hence a lower energy solution results, ie. to take the electron from the state described by (y1+y2) and take it to infinite distance costs energy. It also follows that E+total < E-total The total energy is given by E+total = E+ + Up, where E+ is the energy of the electron i ...
Quantum physics
... • Photocurrent I = (n/t)e, where (n/t) = rate of emission of electrons • Why rate of emission of electrons << rate of incidence of photons {for f>f0}: • Not every photon would collide with an electron; most are reflected by the metal or miss hitting any electron. • On the way out to the metal surfac ...
... • Photocurrent I = (n/t)e, where (n/t) = rate of emission of electrons • Why rate of emission of electrons << rate of incidence of photons {for f>f0}: • Not every photon would collide with an electron; most are reflected by the metal or miss hitting any electron. • On the way out to the metal surfac ...
Downlad - Inspiron Technologies
... If an attempt is made to determine experimentally which slit the electron goes through, the act of measuring destroys the ...
... If an attempt is made to determine experimentally which slit the electron goes through, the act of measuring destroys the ...
Chapter 2 Atomic structure and spectra
... where φj (qi ) = Rnj j (ri )Yj mj (θi , ϕi )σmsj represents a spin orbital with σmsj being the spin part of the orbital, either α for msj = 1/2 or β for msj = −1/2 . The electron wave function in Equation (2.16) gives the occupation of the atomic orbitals and represents a given electron configurat ...
... where φj (qi ) = Rnj j (ri )Yj mj (θi , ϕi )σmsj represents a spin orbital with σmsj being the spin part of the orbital, either α for msj = 1/2 or β for msj = −1/2 . The electron wave function in Equation (2.16) gives the occupation of the atomic orbitals and represents a given electron configurat ...
Atoms and Molecules - New Age International
... which revolve in defined shells or orbits. This model has been replaced by wave mechanical model, i.e., replaced by de-Broglies electron wave. These waves form stationary waves with their nodes and antinodes. Hence, instead of being localised at a point, the whole of electron mass and charge is spr ...
... which revolve in defined shells or orbits. This model has been replaced by wave mechanical model, i.e., replaced by de-Broglies electron wave. These waves form stationary waves with their nodes and antinodes. Hence, instead of being localised at a point, the whole of electron mass and charge is spr ...
PowerPoint 演示文稿
... If we have a hydrogen atom with its electron in an excited state (either by light absorption or by heating) the electron may fall down to a lower orbit by emission of light. The electron may fall into any lower orbit, and the energy it loses will be exactly equal to the energy difference between the ...
... If we have a hydrogen atom with its electron in an excited state (either by light absorption or by heating) the electron may fall down to a lower orbit by emission of light. The electron may fall into any lower orbit, and the energy it loses will be exactly equal to the energy difference between the ...
Chapter 6 Electronic Structure of Atoms
... phenomena in this way: 3. Energy is only absorbed or emitted in such a way as to move an electron from one “allowed” energy state to another; the energy is defined by E = h Electronic Structure of Atoms ...
... phenomena in this way: 3. Energy is only absorbed or emitted in such a way as to move an electron from one “allowed” energy state to another; the energy is defined by E = h Electronic Structure of Atoms ...
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.